Unit 1 Intro to Chem & Matter and Change 2011 - Reeths
Download
Report
Transcript Unit 1 Intro to Chem & Matter and Change 2011 - Reeths
Chapter One
Introduction to
Chemistry
What is Chemistry?
Define Chemistry -
• The study of the
composition of matter and
the changes it undergoes.
Define Matter -
• Anything that has mass
and occupies space.
What are the five branches of
Chemistry?
Organic Chemistry
Inorganic
Chemistry
Analytical
Chemistry
Physical Chemistry
Biochemistry
3.a. WHAT IS ORGANIC
CHEMISTRY?
STUDIES CARBON CONTAINING
COMPOUNDS.
• Hydrocarbons specifically
3.b. WHAT IS INORGANIC
CHEMISTRY?
STUDIES SUBSTANCES WITHOUT
CARBON.
• Mainly substances of nonliving
things.
3. c. WHAT IS ANALYTICAL
CHEMISTRY?
CONCERNED PRIMARILY WITH
IDENTIFYING UNKNOWN
SUBSTANCES.
• Lab based chemistry
• Forensic chemistry is an example
3. d. WHAT IS PHYSICAL
CHEMISTRY?
SPECIALIZES IN THEORIES AND
EXPERIMENTS THAT DESCRIBE THE
BEHAVIOR OF CHEMICALS.
• LOTS OF MATH
• DESCRIPTIVE CHEMISTRY: How and
why do materials behave the way
they do...
3.e. WHAT IS BIOCHEMISTRY?
STUDIES THE COMPOSITION OF
LIVING ORGANISMS.
• MEDICINES,
PHOTOSYNTHESIS/RESPIRATION,
CELL BIOLOGY, ETC.
IS THERE CLEAR DISTINCTION BETWEEN FIELDS?
NO!
OBVIOUSLY THE SUBDIVISIONS OF CHEMISTRY
OVERLAP.
• FOR EXAMPLE, YOU CAN’T MEASURE A CHANGE IN
SUBSTANCE WITHOUT SOME PROFICIENCY IN
ANALYTICAL CHEMISTRY.
4. Why study chemistry?
Your everyday life
involves chemistry,
how?
a. Food Industry
b. Environmental
Reasons
c. Medical Advances
d. Better products
means better lives
HOW DOES CHEMISTRY AFFECT YOUR
EVERYDAY LIFE?
VIDEO - “CHEMISTRY IN YOUR LIFE”
Directions are in the notepack.
Chapter 2 (pg. 5 in Notepack)
Matter and Change
2.1 Properties of matter
1. Matter –
• Anything that has a mass and takes up space.
2. Mass –
• The amount of matter the object contains.
3. Substance –
• Matter that has uniform and constant
composition. It is pure. Contains only one kind
of matter.
2.1 Properties of Matter
Continued
4. Physical Property –
• A quality or condition of a substance that can
be observed or measured without changing
the substance’s composition.
Write these examples in the left-hand margin
Examples: Color, solubility, odor, hardness,
density, melting point, boiling point.
States of Matter
5. Solid –
• Matter with a definite (“fixed”) shape and volume.
6. Liquid –
• Matter that flows, has a fixed volume, and takes the
shape of its container.
7. Gas –
• Matter that takes both the shape and volume of its
container. Gases are easily compressed.
8. Vapor –
• A gaseous form of matter that is usually a solid or
liquid at room temperature
Physical Change
9. A change that alters matter without
changing its composition.
• Cutting, grinding, bending, boiling, freezing,
melting, etc.
Things to think about…
Is every sample of matter a substance?
• Explain
Substance
If a substance only defines pure matter –
that is matter that is only made up of one
kind of matter NOT EVERY TYPE OF MATTER IS A SUBSTANCE.
In nature, we have mixtures – those forms
of matter that are made up of two or more
types of matter physically blended
together.
To review:
List 5-7 physical properties of matter
Answer:
Color,
solubility,
odor,
hardness,
density,
melting point,
boiling point
Which of the following are physical
changes?
a)
b)
c)
d)
Making caramel from sugar
Carving a wooden figurine
Freezing mercury
Dissolving salt in water
Answers:
a)
b)
c)
d)
Making caramel from sugar: Chemical
Carving a wooden figurine: Physical
Freezing mercury: Physical
Dissolving salt in water: Physical
2.2 Classifying Mixtures
pg. 6 in your Note pack
1. Mixture:
• Variable composition - 2 or
more things put together,
each retaining it’s own
identity.
2. Heterogeneous Mixture
> 2 or more things put together, each retains
it’s own identity, but looks different
throughout.
> Has distinct phases
3. Homogeneous Mixture
> 2 or more things put together, each retains it’s
own identity, but looks uniform
throughout.
4.
solution
• A solution is a homogeneous
mixture
5. Phase
Any part of a system with uniform (“same”)
composition and properties.
• Salt water = One Phase
• Sand and Iron Filings = Two Phases
6. Distillation
A process used to separate two liquids
from one another based on their boiling
point.
How do we separate mixtures?
What might be a way that we could separate a
mixture of sand and salt using only physical
changes?
Answer:
Add water to dissolve the salt.
Filter the saltwater through a funnel.
Boil the water out of the salt water.
Left with two separate piles of sand and
salt.
Your turn to Practice: Are the
following a Substance or a Mixture?
Silver
Alphabet soup
Textbook
Table salt (sodium chloride)
Answers:
Substance
Alphabet soup - Mixture
Textbook - Mixture
Silver -
Table salt (sodium chloride) -
Substance
Separate this mixture:
What physical properties could be used to
separate iron filings from salt?
Answer:
Iron is magnetic.
Use a magnet to pull out
the iron filings from the mixture.
Classify the following mixtures as either
Homogeneous or Heterogeneous?
Spaghetti sauce with meatballs
Glass
Muddy water
Cough syrup
Mixture of nitrogen gas and helium gas
Answers:
Spaghetti sauce with meatballs:
Glass:
Hetero
Homo
Hetero
Cough syrup: Homo
Muddy water:
Mixture of nitrogen gas and helium gas: Homo
(gases will diffuse to blend completely)
Texting 101 – this is NOT in your
notes
The following are shortened
representations of longer phrases. What
does each mean?
Lol
Ttyl
Bff
These are shorthand representations of a
longer meaning.
2.3 Element and Compounds
Note pack, pg. 7
Elements:
• The simplest form of matter
• Cannot be broken down further
• Found on the periodic table
• Represented by a chemical
symbol
–Sometimes from its English name,
sometimes from its Latin name
Compound
2 or more elements CHEMICALY bonded
together.
Still just one substance, but made of 2
or more kinds of atoms.
Represented by a chemical
FORMULA
Symbol vs Formula
Chemical symbol:
• One or two letter abbreviation for the elements
• Found on the periodic table
Chemical formula:
• Shorthand for a compound
• Comprised of two or more chemical symbols
• May contain subscripts to denote how many
atoms of each element present in the compound.
Chemical Change
To turn a compound into its elements, a
CHEMICAL CHANGE must occur.
The elements comprising a compound have
very different properties.
Water Hydrogen gas + Oxygen gas
Practice the Chemical Symbols
Copper
Oxygen
Phosphorus
Silver
Sodium
Helium
Practice Naming
Sn
Ca
S
Cd
P
Cl
K
Mg
Mn
Practice Classifying
element, compound or mixture
Spaghetti sauce
Glass
Table sugar
River water
Cough syrup
nitrogen
2.4 Chemical Reactions
CHEMICAL REACTION –
• shorthand for representing a
chemical change.
Reactants – Starting substances
Products – Ending substances
CH4 + O2 CO2 + H2O
Reactants Products
Chemical Reactions
Heating Iron and Sulfur strongly produces a
chemical change … iron sulfide is
produced.
see the reaction here
Chemical Property
The ability of a substance to undergo a
chemical reaction and to form new
substances.
• Iron metal has the ability to rust.
• Magnesium has the ability to react with acid.
Law of Conservation of Mass and
Energy
During a chemical change, the total amount
of mass and energy is a constant.
The mass and energy of the reactants
must equal the mass and energy of the
products.
Chemical Change vs Physical
Change
Chemical changes produces new substances.
Physical changes do not produce new substances.
Chemical changes can be observed by
things such as color changes,
•
•
•
•
heat changes (absorb heat = feel cold; release heat = feel warm),
formation of a gas (bubbles) ,
formation of a new solid (a precipitate solid suspended in a liquid) ,
mass changes, etc.
Practice
Classify each as a chemical or physical
change
•
•
•
•
•
•
Cookies are baked
Water boils
Salt dissolves in water
A firefly emits light
Milk spoils
Metal chair rusts
Practice
State several physical and chemical
properties that could be used to
distinguish between each of the following
pairs of substances and mixtures
•
•
•
•
Gasoline and water
Copper and silver
Water and salt water
Aluminum and steel
The Law of Conservation of Mass
In any physical change or chemical
change, mass is neither created nor
destroyed; it is conserved.
• Mass of the products must equal the mass of
the original reactants
Practice
Law of conservation of mass.
• Hydrogen and oxygen react chemically to form
water. How much water would be formed if 4.8
grams of hydrogen reacted with38.4 grams of
oxygen?
Practice
Law of conservation of mass.
• Hydrogen and oxygen react chemically to form
water. How much water would be formed if 4.8
grams of hydrogen reacted with38.4 grams of
oxygen?
Hydrogen + Oxygen Water
38.4 g
+
4.8 g 43.2 g
Summary
On the back of our notes in the space
provided, let’s draw in the classification of
matter pyramid together. (page 38)