Unit 1 – Chemical Basis of Life Important introductory terminology: biochemistry - the chemistry of living things - - atom the most basic particle of matter,
Download ReportTranscript Unit 1 – Chemical Basis of Life Important introductory terminology: biochemistry - the chemistry of living things - - atom the most basic particle of matter,
Slide 1
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 2
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 3
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 4
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 5
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 6
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 7
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 8
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 9
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 10
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 11
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 12
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 13
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 14
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 15
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 16
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 17
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 18
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 19
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 2
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 3
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 4
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 5
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 6
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 7
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 8
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 9
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 10
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 11
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 12
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 13
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 14
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 15
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 16
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 17
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 18
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.
Slide 19
Unit 1 – Chemical Basis of Life
Important introductory terminology:
biochemistry
- the chemistry of living things
-
-
atom
the most basic particle of matter, consisting of a nucleus and electron(s) –
e.g. hydrogen atom
element
a substance made up of the same type of atom – e.g. gold
molecule
a particle composed of two or more atoms (atoms can be of the same type
or different type) – e.g. water molecule – H2O, nitrogen gas – N2
compound
- substance made up of different type of atoms – e.g. carbon dioxide – CO2
-
Chemical bonds
hold atoms together, some are stronger than
others
3 main types of chemical bonds present in living
things – covalent, ionic and hydrogen bond:
1. covalent bond
strongest bond of three types
electrons are shared (e.g. H2)
Covalent bond Animation
2.
-
-
-
ionic bond
weaker bond than covalent
electrons are not shared
one atom takes one or more electrons from
another atom to create ions (anion – a
negative ion, cation – a positive ion)
change in charge of these atoms (positive and
negative charge) creates an ionic attraction (e.g.
NaCl – salt)
Ionic Bond animation
3.
-
-
-
-
hydrogen bond
weakest of the three bonds discussed (5% of the
strength of a covalent bond), happens because of
hydrogen’s poor attraction to electrons
in water, the electrons collect more at the oxygen
end of the molecule, giving this end a partial
negative charge and the hydrogen end a partial
positive charge.
positive end of one water molecule has a weak
attraction to the negative end of another water
molecule
Give water it’s unique properties, such it’s ability
to stay a liquid at a wide range of temperatures,
and it’s high boiling point.
+
+
-
hydrogen bonds
+
+
-
+
-
+
+
+
+
hydrogen bonds also hold together the two
rungs of the DNA ladder
hydrogen bonds
Entropy
the natural progress from order to disorder in
living things (sometimes thought of as
randomness)
Constant supply of energy is needed to combat
entropy (in form of food for heterotrophic
organisms, or sunlight for autotrophic
organisms)
Without a constant supply of energy, living
things die and become more random
This energy originates from the sun
chemical reaction
-when chemicals react to create new substances
reactants
- chemicals used up in a chemical reaction
products
-chemicals produced in a chemical reaction
anabolism – building of more complex molecules using simpler
molecules
catabolism – breaking down of more complex molecules into
simpler ones
two
types of chemical reactions exist:
exothermic and endothermic
exothermic reaction
- release energy into the surroundings when the chemicals react
- 2 H2 + O2 2 H2O + energy (heat & light) – Hindenburg
reaction
- C6H12O6 (glucose) + 6 O2 6 CO2 + 6 H2O + energy (in the
form of ATP, this famous exothermic reaction is called cellular
respiration)
endothermic reaction
- absorb energy from the surroundings when the chemicals react
- e.g. - cold pack containing urea and ammonium chloride – mixed
together causes reaction to absorb heat and the chemicals feel cold
- e.g. 6 CO2 + 6 H2O + energy (light) C6H12O6 (glucose) + 6 O2
this famous endothermic reaction is called photosynthesis)
Synthesis and Decomposition
Reactions
Synthesis Reactions - is when there is a
combination of two or more substances and a
compound results (also called anabolism) . An
example of a synthesis reaction is as follows:
A + B --> AB
a special type of synthesis reactions occur in
living systems, called dehydration synthesis
(we will discuss later)
Decomposition Reactions is the opposite of
synthesis. It is when a compound is broken
down into simpler substances (sometimes called
catabolism). An example of decomposition is
as follows:
AB --> A + B
a special type of decomposition reaction occur
in living systems, called hydrolysis (we will
also discuss later)
Chapter 2 - Question 1-3, page 39
1. What distinguishes one element from another?
The number of protons in the nucleus
2. Describe the formation of an ionic compound.
In sodium chloride, a sodium atom loses an electron to
a chlorine atom.
The opposite charged ions are attracted to each other
and form an ionic bond.
3. What is the difference between and ionic bond and a
covalent bond?
An ionic bond is formed due to the electrical attraction
between oppositely charged ions.
A covalent bond is formed by atoms that share
electrons.
Questions 4-6
4. Compare and contrast – How does a molecule differ from an atom?
A molecule is made up of two or more atoms held together by a
covalent bond.
5. Apply – Explain why a hydrogen atom can become either an ion or
part of a molecule.
A hydrogen atom has one unpaired electron in its outer energy level.
The electron can be lost to form an ion or shared to form a covalent
bond.
6. Chemistry – A sodium atom has one outer electron, and a carbon
atom has four outer electrons. How might this difference be related
to the types of compounds formed by atoms of these two elements?
An atom that has a nearly full or nearly empty outer energy level
(such as sodium) tends to form ions. An atom in between (such as
carbon) tends to share electrons.
Questions 1-3, page 43
How do polar molecules form hydrogen bonds?
1.
-
2.
The oppositely charged regions of a polar molecule attract
other polar molecules, allowing a positively charged
hydrogen atom to bond to a negatively charged atom.
What determines whether a compound will dissolve
in water?
- Compounds that have charges, such as ionic compounds and
polar molecules, will dissolve in water
3.
Make a chart that compares acids and bases.
- acids donate protons (hydrogen ions) and bases
accept them
- acids have a pH less than 7, bases have a pH greater
than 7
Questions 4-5
4.
Compare and Contrast – How do polar molecules
differ from non-polar molecules? How does this
affect their interactions?
- Polar molecules have charged regions due to an unequal
sharing of electrons. Non-polar molecules do not have
charged regions because electrons are shared more
equally. The charge differences tend to keep the
molecules separate.
5.
Connect – Describe an example of cohesion or
adhesion that you might observe during your daily
life.
- Water beading on the surface, water sticking to the side of
a glass
Question 6
Cellular Respiration – When sugars are broken
down to produce usable energy for cells, a
large amount of heat is released. Explain how
the water inside the cell helps keep the cell’s
temperature constant.
6.
-
Water has a high specific heat.
Water in a cell can absorb a large amount of
energy before its temperature increases.