Slide 1

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 2

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 3

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 4

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 5

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 6

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 7

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 8

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 9

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 10

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 11

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 12

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 13

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 14

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 15

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 16

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 17

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 18

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 19

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 20

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 21

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 22

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 23

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 24

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 25

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 26

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31


Slide 27

UNIT 1
• Significant figures
• Uncertainty in measurement
• Percent error
• Separation Techniques for
Mixtures (Lab activities once I
open the Flinn boxes!)

Class Groups
Explain the distribution of class groups.
Groups of Eight
4 Groups will perform lab and remaining 4
will study in their groups
Switch around next day!

Atomic Structure

Image courtesy of www.lab-initio.com

Chemistry Timeline #1

B.C.
400 B.C. Demokritos and Leucippos use the term "atomos”



2000 years of Alchemy

1500's
 Georg Bauer: systematic metallurgy
 Paracelsus: medicinal application of minerals

1600's
Robert Boyle:The Skeptical Chemist. Quantitative experimentation, identification of
elements

1700s'
 Georg Stahl: Phlogiston Theory
 Joseph Priestly: Discovery of oxygen
 Antoine Lavoisier: The role of oxygen in combustion, law of conservation of
mass, first modern chemistry textbook

Chemistry Timeline #2
1800's
Joseph Proust: The law of definite proportion (composition)
 John Dalton: The Atomic Theory, The law of multiple proportions
Joseph Gay-Lussac: Combining volumes of gases, existence of diatomic molecules
Amadeo Avogadro: Molar volumes of gases
Jons Jakob Berzelius: Relative atomic masses, modern symbols for the elements
 Dmitri Mendeleyev: The periodic table
 J.J. Thomson: discovery of the electron
 Henri Becquerel: Discovery of radioactivity
1900's
 Robert Millikan: Charge and mass of the electron
 Ernest Rutherford: Existence of the nucleus, and its relative size
 Meitner & Fermi: Sustained nuclear fission
 Ernest Lawrence: The cyclotron and trans-uranium elements

Dalton’s Atomic Theory (1808)

John Dalton

 All matter is composed of extremely
small particles called atoms
 Atoms of a given element are
identical in size, mass, and other
properties; atoms of different
elements differ in size, mass, and
other properties

 Atoms cannot be subdivided, created, or destroyed
 Atoms of different elements combine in simple
whole-number ratios to form chemical compounds
 In chemical reactions, atoms are combined,
separated, or rearranged

Modern Atomic Theory
Several changes have been made to Dalton’s theory.

Dalton said:
Atoms of a given element are identical
in size, mass, and other properties;
atoms of different elements differ in
size, mass, and other properties
Modern theory states:
Atoms of an element have a
characteristic average mass which is
unique to that element.

Modern Atomic Theory #2
Dalton said:
Atoms cannot be subdivided, created, or
destroyed

Modern theory states:
Atoms cannot be subdivided, created, or
destroyed in ordinary chemical reactions.
However, these changes CAN occur in
nuclear reactions

Discovery of the Electron
In 1897, J.J. Thomson used a cathode ray tube
to deduce the presence of a negatively charged
particle.

Cathode ray tubes pass electricity through a gas
that is contained at a very low pressure.

Link to Animations
• http://highered.mcgrawhill.com/sites/0072512644/student_view0/chapt
er2/animations_center.html

Thomson’s Atomic Model

J.J. Thomson

Thomson believed that the
electrons were like plums embedded
in a positively charged “pudding,”
thus it was called the “plum
pudding” model.

Mass of the Electron
1909 – Robert Millikan
determines the mass of the
electron.

The oil drop apparatus

Mass of the
electron is
9.109 x 10-31 kg

Conclusions from the Study of
the Electron
 Cathode rays have identical properties regardless
of the element used to produce them. All elements
must contain identically charged electrons.
Atoms are neutral, so there must be positive
particles in the atom to balance the negative
charge of the electrons
 Electrons have so little mass that atoms must
contain other particles that account for most of
the mass

Questions for Homework

• Write a paragraph to explain
the Millikan’s experiment.
• What all did he calculate from
his experiment?
• How did he calculate the charge
on an electron.
• Why is oil drop used in
Millikan's oil drop experiment
instead of water drop?

Rutherford’s Gold Foil Experiment

 Alpha particles are helium nuclei
 Particles were fired at a thin sheet of
gold foil
 Particle hits on the detecting screen
(film) are recorded

Try it Yourself!
In the following pictures, there is a target hidden by
a cloud. To figure out the shape of the target, we
shot some beams into the cloud and recorded where
the beams came out. Can you figure out the shape of
the target?

The Answers
Target #1

Target #2

Rutherford’s Findings
 Most of the particles passed right through
 A few particles were deflected
 VERY FEW were greatly deflected
“Like howitzer shells bouncing off
of tissue paper!”

Conclusions:
 The nucleus is small
 The nucleus is dense
 The nucleus is positively charged

Atomic Particles
Particle
Electron

Proton
Neutron

Charge
Mass (kg)
-1
9.109 x 10-31

+1

1.673 x 10-27

Location
Electron
cloud
Nucleus

0

1.675 x 10-27

Nucleus

The Atomic
Scale

Helium-4

 Most of the mass of

the atom is in the
nucleus (protons and
neutrons)
 Electrons are found
outside of the nucleus
(the electron cloud)
 Most of the volume
of the atom is empty
space

Image: User Yzmo Wikimedia Commons

.

QUARKS

About Quarks…
Protons and neutrons are NOT fundamental particles.

Protons are made of two “up” quarks and
one “down” quark.

Neutrons are made of one “up” quark
and two “down” quarks.
Quarks are held together by “gluons”
Images: Arpad Horvath, Wikimedia Commons

.

GOD PARTICLE
• One year ago, several hours before cities across the
United States started their annual fireworks displays, a
different type of fireworks were set off at the European
Center for Nuclear Research (CERN) in Switzerland. At
9:00 a.m., physicists announced to the world that they
had found something they had been searching for nearly
50 years: the elusive Higgs boson.
• Today, on the anniversary of its discovery, are we any
closer to figuring out what that particle's true identity is?
• What exactly is the Higgs boson?

Isotopes
Isotopes are atoms of the same element having
different masses due to varying numbers of neutrons.
Isotope

Protons

Electrons

Neutrons

Hydrogen–1
(protium)

1

1

0

Hydrogen-2
(deuterium)

1

1

1

Hydrogen-3
(tritium)

1

1

2

Nucleus

Atomic Masses

Atomic mass is the average of all the naturally
isotopes of that element.
Isotope

Symbol

Composition of
the nucleus

% in nature

Carbon-12

12C

6 protons
6 neutrons

98.89%

Carbon-13

13C

6 protons
7 neutrons

1.11%

Carbon-14

14C

6 protons
8 neutrons

<0.01%

Carbon = 12.011

Atomic Number
Atomic number (Z) of an element is
the number of protons in the nucleus
of each atom of that element.
Element
Carbon
Phosphorus
Gold

# of protons Atomic # (Z)
6
6
15
15
79

79

Mass Number
Mass number is the number of
protons and neutrons in the nucleus
of an isotope.
Mass # = p+ + n0
Nuclide

p+

n0

e-

Mass #

Oxygen - 18

8

10

8

18

Arsenic - 75
Phosphorus - 31

33

42

33

75

15

16

15

31