Transcript The Atom - cloudfront.net

Warm-Up
September 13, 2013 (ODD)
1. Draw a picture of an atom, and label the different
particles.
2. What is an atom?
3. What is a compound?
4. What does it mean to conserve?
5. What is a proportion?
Agenda September 13, 2013 (ODD)
1. Begin New Unit: The Atom
2. The Story of Chemistry
-
Read pages 73 – 78
HOMEWORK
Warm-Up
September 16, 2013 (EVEN)
1. Draw a picture of an atom, and label the different
particles.
2. What is an atom?
3. What is a compound?
4. What does it mean to conserve?
5. What is a proportion?
Agenda September 16, 2013 (EVEN)
1. Begin New Unit: The Atom
2. The Story of Chemistry
-
Read pages 73 – 78
HOMEWORK
Warm-Up
September 17, 2013 (ODD)
1. What is the difference between a law and theory
2. What does the prefix “sub” mean as in “submerge” or
“subscript” or “subordinate”
3. In a cell, where is the DNA found?
4. What word describes amount of space taken up by an
object?
5. What word describes amount of “stuff” in an object.
6. Density is the relationship between insert phrase___
over insert phrase____
Agenda September 17, 2013 (ODD)
1. Go over exam
2. Finish The Story of Chemistry
3. The sequel: The Story of the Atom
HOMEWORK
Warm-Up
September 18, 2013 (EVEN)
1. What is the difference between a law and theory
2. What does the prefix “sub” mean as in “submerge” or
“subscript” or “subordinate”
3. In a cell, where is the DNA found?
4. What word describes amount of space taken up by an
object?
5. What word describes amount of “stuff” in an object.
6. Density is the relationship between insert phrase___
over insert phrase____
Agenda September 18, 2013 (EVEN)
1. Finish The Story of Chemistry
2. The sequel: The Story of the Atom
HOMEWORK
Agenda September 19, 2013 (ODD)
1. Lego Activity
2. The sequel: The Story of the Atom
HOMEWORK
Warm-Up
1.
2.
3.
4.
September 20, 2013 (E)
Democritus came up with the concept of ________
Robert Boyle came up with the concept of _______
What are three important laws from the story so far?
Look up the terms “reactant” and “products.”
Agenda
September 20, 2013 (E)
1. Finish Lego Activity today
2. Begin the “The Story of Atom”, the sequel to “The
Story of Chemistry”
Warm-Up
September 23, 2013 (O)
1. What does the prefix “sub” mean?
2. What are the three subatomic particles discussed?
3. What happens when the + side of a magnet is placed
next to a - side of a magnet? What happens when the
+ side is placed next to another + side?
4. Draw a line, a line segment, and a ray
5. If a metal has a density of 2.86 g/cm3, what is the
volume of a 0.327g block of that metal?
Agenda
September 23, 2013 (O)
1. Go over homework
2. Begin the “The Story of Atom”, the sequel to “The
Story of Chemistry”
1. Worksheet
HOMEWORK
Agenda
September 23, 2013 (O)
1. Go over homework
2. Begin the “The Story of Atom”, the sequel to “The
Story of Chemistry”
• Discovery of the Electron
• Discovery of the Nucleus and the Proton
• Discovery of the Neutron
2. Atomic Number and Atomic Mass
1. Worksheet
HOMEWORK
Warm-Up
September 24, 2013 (E)
1. What does the prefix “sub” mean?
2. What are the three subatomic particles discussed?
3. What happens when the + side of a magnet is placed
next to a - side of a magnet? What happens when the
+ side is placed next to another + side?
4. Draw a line, a line segment, and a ray
5. If a metal has a density of 2.86 g/cm3, what is the
volume? The mass is 0.327g
6. Turn homework in box
Agenda
September 24, 2013 (E)
1. Go over homework
2. Begin the “The Story of Atom”, the sequel to “The
Story of Chemistry”
1. Worksheet
HOMEWORK
Warm-Up
September 25, 2013 (O)
1. Most of an atom is _________.
2. Most of the mass of an atom is located _________
3. What would happen if you shined a flashlight at the
object below?
4. What would you throw to make the object rotate?
5. A package of Skittles has a mass of 28.8 grams. One
Skittle has a mass of 1.7 grams. How can I find out the
number of Skittles for each package?
Agenda
September 25, 2013 (O)
1. Go over homework
2. Continue the “The Story of Atom”, the sequel to “The
Story of Chemistry”
• Review Discovery of the Electron
• Discovery of the Nucleus and the Proton
• Discovery of the Neutron
3. Atomic Number and Atomic Mass
HOMEWORK
1. Worksheet
2. Read and outline 3.2
Warm-Up
September 26, 2013 (E)
1. Most of an atom is _________.
2. Most of the mass of an atom is located _________
3. What would happen if you shined a flashlight at the
object below?
4. What would you throw to make the object rotate?
5. A package of Skittles has a mass of 28.8 grams. One
Skittle has a mass of 1.7 grams. How can I find out the
number of Skittles for each package?
Warm-Up
September 27, 2013 (O)
1. What are the three important laws from our first
story?
2. You did not create or destroy any Lego blocks in the
Lego activity. Which law is related to this?
3. Use a McDonald’s cheeseburger to explain the Law of
Definite Proportion
4. If 1 gallon = 3.94 liters, how many liters of gas goes
into a car with a 15 gallon tank?
5. If 1 liter costs $1.39, how much to fill up the tank?
Agenda
September 27, 2013 (O)
1. Go over homework
2. Continue the “The Story of Atom”, the sequel to “The
Story of Chemistry”
• Discovery of the Nucleus and the Proton
3.
•
•
•
•
Atomic Number and Mass Number
Calculating number of protons and neutrons
Discovery of Neutron
What are isotopes?
Discovery of isotopes
1. Worksheet
HOMEWORK
Warm-Up
September 30, 2013 (E)
1. What are the three important laws from our first
story?
2. You did not create or destroy any Lego blocks in the
Lego activity. Which law is related to this?
3. Use a McDonald’s cheeseburger to explain the Law of
Definite Proportion
4. If 1 gallon = 3.94 liters, how many liters of gas goes
into a car with a 15 gallon tank?
5. If 1 liter costs $1.39, how much to fill up the tank?
Agenda
September 30, 2013 (E)
1. Go over homework
2. Continue the “The Story of Atom”, the sequel to “The
Story of Chemistry”
• Discovery of the Nucleus and the Proton
3.
•
•
•
•
Atomic Number and Mass Number
Calculating number of protons and neutrons
Discovery of Neutron
What are isotopes?
Discovery of isotopes
1. Worksheet
HOMEWORK
Warm-Up
October 1, 2013 (O)
1. Compound A has a mass of 2.77 g and compound B has a
mass of 5.54 g. Does this data support the law of
multiple proportion?
2. Order the five main characters from the first story
from earliest to latest: Boyle, Dalton, Democritus,
Lavoisier, and Proust.
3. San Francisco is 384 miles away. A train leaves Los
Angeles and travels 88 km in one hour. How long is the
train ride if 1 mile = 1.6 km?
4. A train leaves Los Angeles and heads east to
Washington D.C. The train travels 75 km in one hour.
Hoover Dam is 280 miles away. How many minutes until
the train arrives at Hoover Dam?
5. At what time will the train pass Hoover Dam if the train
left Los Angeles at 3:30pm?
Agenda
October 1, 2013 (O)
1. Review and finish the “The Story of Atom”, the sequel
to “The Story of Chemistry”
• Discovery of the Nucleus and the Proton
2.
•
•
•
•
Atomic Number and Mass Number
Calculating number of protons and neutrons
Discovery of Neutron
What are isotopes?
Discovery of isotopes
1. Worksheet
2. Section Review 3.2
HOMEWORK
Warm-Up
October 2, 2013 (E)
1. Compound A has a mass of 2.77 g and compound B has a
mass of 5.54 g. Does this data support the law of
multiple proportion?
2. Order the five main characters from the first story
from earliest to latest: Boyle, Dalton, Democritus,
Lavoisier, and Proust.
3. A train travels 35 km in 1 hour. How long will it take to
94.5 km?
4. San Francisco is 384 miles away. A train leaves Los
Angeles and travels 88 km in one hour. How long is the
train ride if 1 mile = 1.6 km?
5. A train leaves Los Angeles and heads east to
Washington D.C. The train travels 55 km in one hour.
Hoover Dam is 280 miles away. When will the train
reach Hoover Dam?
Agenda
October 2, 2013 (E)
1. Review and finish the “The Story of Atom”, the sequel
to “The Story of Chemistry”
• Discovery of the Nucleus and the Proton
2.
•
•
•
•
Atomic Number and Mass Number
Calculating number of protons and neutrons
Discovery of Neutron
What are isotopes?
Discovery of isotopes
1. Worksheet
2. Section Review 3.2
HOMEWORK
Warm-Up
October 4, 2013 (E)
Draw and label Thomson’s experimental setup.
Milikan is important because he calculated…
What two forces was Milikan trying to balance?
Rutherford concluded that atoms have a dense and
positively charged nucleus. Explain why the nucleus is
dense and positively charged.
5. A football field is 100 yards in distance. Usain Bolt runs
200 meters in 19.66 seconds. How many seconds will it
take him to run the length of a football field? 1 meter =
1.09 yards
1.
2.
3.
4.
Agenda
1.
•
•
•
•
October 3, 2013 (E)
Atomic Number and Mass Number
Calculating number of protons and neutrons
Discovery of Neutron
What are isotopes?
Discovery of isotopes
2. Counting Atoms
• Mole
• Converting grams to mole
• Converting grams to mole to number of atoms
1.
•
•
•
HOMEWORK
Make index cards for:
The 3 laws
Democritus, Boyle, Dalton, Proust, Lavoisier
Thomson, Milikan, Rutherford
How is Accuracy different from
Precision?
Accuracy is how close the data is to the
actual recorded number or
measurement. Precision is how close the
data are to one another. For example,
2.67g, 2,59g, 2.60g, and 2.64g are
precise but not accurate because it is
not close to the actual mass of 3.45.
Differentiate between Law and Theory
Both theory and a law are part of the scientific method,
but a theory describes WHY something happens; why
something is the way it is, why it works in a certain way. A
law describes WHAT/HOW something happens. For
example, “ice always floats on water” is a law because it
states WHAT. If you say “ice floats on water because it’s
density is less than the density of water,” then you are
stating a theory because you are describing why
something happens.
Differentiate between Pure Substance
and Homogeneous Mixture
A pure substance can either be a compound or an
element. An element is made up of one type of
atom. A compound is made up of two or more
different types of atoms that are chemically
joined. A homogeneous mixture is physically
mixed. It is a mixture that is evenly distributed. An
example of a pure substance can be gold or water.
An example of a homogeneous mixture can be like
a chocolate bar or food coloring in water.
Differentiate between Mass and Weight
Mass is the amount of “stuff” in
something and weight is the amount
of gravitational pull exerted by the
thing. If you were to go on the
moon, your weight would change
but your mass would not.
Accuracy vs. Precision
The measured masses are examples of
precision because when compared to the
mass of 3.45, none of them are accurate or
close to the number. They are a cluster of
numbers that aren’t near the actual number.
An accurate answer would be 3.44 g, 3.46 g,
and 3.43 g.
1. The Story of Chemistry
How we know what we know
about the Atom
OBJECTIVE: Understand the development of
how the idea of an “atom” came about
1. The Story of Chemistry
A. Greek Beginnings
1. The Story of Chemistry
1. The Story of Chemistry
In order to understand WHY we know and HOW we know
this is what an atom looks like, we need to learn about the
story of the atom.
1. The Story of Chemistry
Early human civilizations organized “stuff” into
four categories: Earth, Air, Fire, Water
1. The Story of Chemistry
1. The Story of Chemistry
The first known writing that has the word
“ATOM” is from Greece.
It was written around 400 B.C. by a
philosopher named Democritus, Δημόκριτος
1. The Story of Chemistry
Democritus’ idea was…
Everything that exists is made up of this
“thing” that cannot be broken, separated, or
divided into something smaller.
1. The Story of Chemistry
Democritus’ idea was…
Everything that exists is made up of this
“thing” that cannot be broken, separated, or
divided into something smaller.
He called that “thing” an ATOM.
1. The Story of Chemistry
ATOM = a Greek word
1. The Story of Chemistry
ATOM = a Greek word
Temnein = to cut or divide
A = prefix meaning not
1. The Story of Chemistry
ATOM = a Greek word
Temnein = to cut or divide
A = prefix meaning not
a + temnein =
1. The Story of Chemistry
ATOM = a Greek word
Temnein = to cut or divide
A = prefix meaning not
a + temnein = unable to cut
1. The Story of Chemistry
Democritus’ idea was…
Everything that exists is made up of this
“thing” that cannot be broken, separated, or
divided into something smaller.
He called that “thing” an ATOM.
1. The Story of Chemistry
Democritus’ idea of the atom is…
An observation?
A hypothesis?
An experiment?
A law?
A theory?
1. The Story of Chemistry
Democritus’ idea of the atom is…
A hypothesis because his idea could not be
tested.
1. The Story of Chemistry
IMPORTANT!!!
Democritus’ idea of atom =/=
1. The Story of Chemistry
B. Foundational Ideas
1. Democritus
2. Alchemists during the Middle Ages –
wanted to convert one element to
another.
1. The Story of Chemistry
1. Democritus
2. Alchemists during the Middle Ages –
wanted to convert one element to
another.
3. 16th and 17th century; 1500’s – 1600’s
1. The Story of Chemistry
3. 16th and 17th century; 1500’s – 1600’s
Robert Boyle – worked with gases, and
looked at pressure and volume.
Robert Boyle is important because came up
with the idea that some things CANNOT be
further separated.
1. The Story of Chemistry
3. 16th and 17th century; 1500’s – 1600’s
Robert Boyle – worked with gases, and
looked at pressure and volume.
Robert Boyle is important because he came
up with the idea, the concept, of an
ELEMENT.
1. The Story of Chemistry
3. 16th and 17th century; 1500’s – 1600’s
Robert Boyle is important because he came
up with the idea, the concept, of an
ELEMENT.
Now that we knew about ELEMENTS, people
began to identify many things as elements,
largely elements.
1. The Story of Chemistry
4. 18th century; 1700’s
Joseph Priestly – O2, Combustion, CO2
1. The Story of Chemistry
4. 18th century; 1700’s
Antoine Lavoisier
1. The Story of Chemistry
4. 18th century; 1700’s
Antoine Lavoisier – Refined Priestly’s
understanding of combustion as involiving
carbon-based substance plus oxygen
results in CO2 and H2O.
1. The Story of Chemistry
4. 18th century; 1700’s
Antoine Lavoisier – MORE IMPORTANT
than that =
1. The Story of Chemistry
4. 18th century; 1700’s
Antoine Lavoisier – MORE IMPORTANT
than that =
something cannot be made from nothing
1. The Story of Chemistry
4. 18th century; 1700’s
Antoine Lavoisier – MORE IMPORTANT
than that =
something cannot be made from nothing,
and
something cannot become nothing.
1. The Story of Chemistry
4. 18th century; 1700’s
Antoine Lavoisier – saw that when a
chemical change takes place, the mass does
not change.
1. The Story of Chemistry
4. 18th century; 1700’s
Antoine Lavoisier – saw that when a
chemical change takes place, the mass does
not change.
So he concluded, mass cannot be created or
destroyed during a chemical or physical
change.
1. The Story of Chemistry
4. 18th century; 1700’s
“mass cannot be created or destroyed
during a chemical or physical change.”
Is this an observation?
Is this a hypothesis?
Is this an experiment?
Is this a law?
Is this a theory?
1. The Story of Chemistry
4. 18th century; 1700’s
“mass cannot be created or destroyed
during a chemical or physical change.”
It is a law because it is a statement
about WHAT nature does.
Law of Conservation of Mass/Matter
1. The Story of Chemistry
4. 18th century; 1700’s
Antoine Lavoisier is important because he
showed that mass/matter cannot be
created or destoyed.
1. The Story of Chemistry
4. 18th century; 1700’s
Joseph Proust -
1. The Story of Chemistry
4. 18th century; 1700’s
Joseph Proust – glucose is the same,
C6H12O6, and it doesn’t matter it if is from
grapes, honey, oranges, or apples because
glucose will ALWAYS have 6 C, 12 H, and
O6.
Or, to summarize this in your notes…
1. The Story of Chemistry
4. 18th century; 1700’s
Joseph Proust – Joseph Proust – a compound
always contains the same elements, and
exactly the same amount in mass.
Example
Glucose will always be made up of C6H12O6
H2O will always be made up of 2 H and 1 O
1. The Story of Chemistry
4. 18th century; 1700’s
Joseph Proust – a compound always contains
the same elements, and exactly the same
amount in mass. Example H2O will always be
made up of 2 H and 1 O
Which part of the S.M. does this belong?
1. The Story of Chemistry
4. 18th century; 1700’s
Joseph Proust – a compound always contains
the same elements, and exactly the same
amount in mass. Example H2O will always be
made up of 2 H and 1 O
Which part of the S.M. does this belong?
It is a law.
Law of Definite Proportions
1. The Story of Chemistry
4. 18th century; 1700’s
John Dalton
1. The Story of Chemistry
Compound
A
B
Mass of Element(g)
133
266
1. The Story of Chemistry
Compound
A
Mass of Element(g)
0.0839
1. The Story of Chemistry
Compound
A
B
Mass of Element(g)
0.0839
0.1678
1. The Story of Chemistry
Compound
A
B
C
Mass of Element(g)
0.0839
0.1678
0.2520
1. The Story of Chemistry
Compound
A
B
C
D
Mass of Element(g)
0.0839
0.1678
0.2520
1. The Story of Chemistry
Compound
A
B
C
D
Mass of Element(g)
0.0839
0.1678
0.2520
0.336
of Element(g)
Compound
1. The Story ofMass
Chemistry
A
B
0.59
1.18
of Element(g)
Compound
1. The Story ofMass
Chemistry
A
B
C
0.59
1.18
of Element(g)
Compound
1. The Story ofMass
Chemistry
A
B
C
D
0.59
1.18
1.77
of Element(g)
Compound
1. The Story ofMass
Chemistry
A
B
C
D
0.59
1.18
1.77
2.36
of Element(g)
Compound
1. The Story ofMass
Chemistry
A
B
C
D
E
F
0.59
1.18
1.77
2.36
of Element(g)
Compound
1. The Story ofMass
Chemistry
A
B
C
D
E
F
0.59
1.18
1.77
2.36
2.96
3.54
1. The Story of Chemistry
John Dalton
Law of Multiple Proportion – when elements
form two or more compounds, the mass of
one element that combines with a mass of
the other is in the ration of small whole
numbers.
1. The Story of Chemistry
John Dalton
Proposed a theory that all matter is made up of indivisible
things called ATOMs.
1. The Story of Chemistry
John Dalton
Proposed a theory that all matter is made up of indivisible
things called ATOMs.
We call this theory,
THE ATOMIC THEORY OF MATTER
1. The Story of Chemistry
John Dalton
Proposed a theory that all matter is made up of indivisible
things called ATOMs.
We call this theory,
THE ATOMIC THEORY OF MATTER
How is a law different from a theory?
1. The Story of Chemistry
Dalton’s Atomic Theory of Matter
1. All matter is composed of extremely small particles called
ATOMs, which cannot be subdivided
2. Atoms of a given element (compound) are identical in their
physical and chemical properties, does not matter where
they are from.
3. Atoms of the same elements are identical, and different
elements have different types of atoms
4. Atoms of different elements combine in simple, wholenumber ratios to form compounds
5. In chemical reactions, atoms are combined, separated, or
rearranged but never created, destroyed, or changed
1. The Story of Chemistry
Dalton’s Atomic Theory of Matter
1. All matter is composed of extremely small particles called
ATOMs, which cannot be subdivided - DEMOCRITUS
2. Atoms of a given element are identical in their physical and
chemical properties – LAW OF DEFINITE PROPORTIONS
3. Atoms of the same elements are identical, and different
elements have different types of atoms – BOYLE
4. Atoms of different elements combine in simple, wholenumber ratios to form compounds – LAW OF MULTIPLE
PROPORTIONS
5. In chemical reactions, atoms are combined, separated, or
rearranged but never created, destroyed, or changed – LAW
OF CONSERVATION OF MASS
1. The Story of Chemistry
QUICKWRITE
1. Democritus is important because………
2. Robert Boyle is important because…
3. Law of Conservation of Mass means…
4. Law of Definite Proportions means…
When a log completely burns in a campfire, the mass of the
ass is much less than the mass of the log. What happened
to the “missing” mass?
The question above is related to which of the three laws?
H and O can react to form either H2O or H2O2. In H2O,
the mass of H is 0.125 g. In H2O2, the mass of H is 0.250
g. If the masses of H are set as a proportion, it is equal
to…
This is related to which of the three laws?
QUICKWRITE
1. The purpose of the Lego Activity was…
2. How did the Lego activity help you to
better understand the laws?
2. The Story of Atom
The Sequel: The Story of How
we know what an atoms looks like
OBJECTIVE: To be able to state how we
went from a theory of atom, to actually
knowing what an atom looks like
2. The Story of Atom
Atom made up of smaller parts
These parts are called: SUBATOMIC Particles
2. The Story of Atom
SUBATOMIC PARTICLES
Atom made up of smaller parts
These parts are called: SUBATOMIC Particles
Three types of SUBATOMIC Particles
1. Proton
2. Neutron
3. Electron
2. The Story of Atom
SUBATOMIC PARTICLES
1. Proton
- Has a POSITIVE charge
- Mass is similar to that of a Neutron
- Located in the nucleus
2. The Story of Atom
SUBATOMIC PARTICLES
2. Neutron
- Has NO charge
- Has the largest mass of the three
- Located in the nucleus
2. The Story of Atom
SUBATOMIC PARTICLES
3. Electron
- Has a NEGATIVE charge
- Is the smallest of the three subatomic particles
- Has the least amount of mass of the subatomic particles
- NOT in the nucleus
2. The Story of Atom
Write these questions on your
warmup paper , and answer while
watching the video. Label “Video on
Atoms”
1. If the atoms of a grapefruit are the size of a
blueberry, then how big would the grapefruit be?
2. If an atom is the size of a football stadium, the nucleus
is the size of a ______.
3. What is in between the nucleus and the electrons?
4. _____ many cars packed into a box would equal the
density of the nucleus of one Nitrogen atom
An Atom looks like…
Dalton’s atom looked like
this
Dalton’s atom looked like
this
What’s missing in this picture?
So how did we get
from
to
Discovered Electron
in 1897
How does a
person
discover a
particle so
small that no
one has seen?
J.J. Thomson
2. The Story of Atom
How JJ Thomson discovered the Electron
In the 1850’s, a scientist created a CATHODE RAY TUBE.
2. The Story of Atom
How JJ Thomson discovered the Electron
In the 1850’s, a scientist created a CATHODE RAY TUBE.
Metal plates were placed inside a glass tube.
2. The Story of Atom
How JJ Thomson discovered the Electron
In the 1850’s, a scientist created a CATHODE RAY TUBE.
Metal plates were placed inside a glass tube.
The air was then removed.
2. The Story of Atom
How JJ Thomson discovered the Electron
In the 1850’s, a scientist created a CATHODE RAY TUBE.
Metal plates were placed inside a glass tube.
The air was then removed.
Then the metal plates were connected
to a power source.
2. The Story of Atom
How JJ Thomson discovered the Electron
In the 1850’s, a scientist created a CATHODE RAY TUBE.
Metal plates were placed inside a glass tube.
The air was then removed.
Then the metal plates were connected
to a power source.
This resulted in a beam of light that
started from the cathode (-) and went to
the anode (+)
2. The Story of Atom
How JJ Thomson discovered the Electron
Because these beams started from the cathode (-), scientists
called the beam a CATHODE RAY
2. The Story of Atom
How JJ Thomson discovered the Electron
Because these beams started from the cathode (-), scientists
called the beam a CATHODE RAY
But what are these CATHODE RAYs made of?
2. The Story of Atom
How JJ Thomson discovered the Electron
Because these beams started from the cathode (-), scientists
called the beam a CATHODE RAY
But what are these CATHODE RAYs made of?
Thomson was trying to answer
this question.
J.J. Thomson’s Experiment
normal
J.J. Thomson’s Experiment
normal
with magnet
Thomson’s Conclusions
0 Cathode rays must be made of stuff that is
NEGATIVELY charged
Thomson’s Conclusions
0 Cathode rays must be made of stuff that is
NEGATIVELY charged
0 Particles that make up cathode rays are 1000 times
smaller than a Hydrogen atom
Thomson’s Conclusions
0 Cathode rays must be made of stuff that is
NEGATIVELY charged
0 Particles that make up cathode rays are 1000 times
smaller than a Hydrogen atom
0 All different metals give off cathode rays
Thomson’s Conclusions
0 Cathode rays must be made of stuff that is NEGATIVELY
charged
0 Particles that make up cathode rays are 1000 times smaller
than a Hydrogen atom
0 All different metals give off cathode rays
0 1.72 x 108 Coulombs for every one gram of the negatively
charged particles.
1. The name of the device
Thomson used to discover the
electron was the….
2. Thomson applied an __________
and magnetic field to the
cathode ray tube.
3. Thomson concluded that the
cathode ray has negatively
charged particles because….
4. What other food items besides a
muffin or mint ice cream are
similar to Thomson’s model of
the atom?
1. The name of the device
Thomson used to discover the
electron was the CATHODE RAY
TUBE
2. Thomson applied an __________
and magnetic field to the
cathode ray tube.
3. Thomson concluded that the
cathode ray has negatively
charged particles because….
4. What other food items besides a
muffin or mint ice cream are
similar to Thomson’s model of
1. The name of the device
Thomson used to discover the
electron was the CATHODE RAY
TUBE
2. Thomson applied an ELECTRIC
and magnetic field to the
cathode ray tube.
3. Thomson concluded that the
cathode ray has negatively
charged particles because….
4. What other food items besides a
muffin or mint ice cream are
similar to Thomson’s model of
1. The name of the device
Thomson used to discover the
electron was the CATHODE
RAY TUBE
2. Thomson applied an
ELECTRIC and magnetic field
to the cathode ray tube.
3. Thomson concluded that the
cathode ray has negatively
charged particles because the
ray was attracted to the
positively charged plate.
2. The Story of Atom
How Robert Milikan calculated the charge
and mass of 1 electron in 1909
2. The Story of Atom
How Robert Milikan calculated the charge and
mass of 1 electron in 1909
Purpose: to calculate charge of ONE electron
Discovered charge of 1 electron = 1.6 x 10-19 Coulombs
2. The Story of Atom
How Robert Milikan discovered the charge
and mass of 1 electron in 1909
2. The Story of Atom
How Robert Milikan discovered the charge
and mass of 1 electron in 1909
- Sprayed droplets of oil
2. The Story of Atom
How Robert Milikan discovered the charge
and mass of 1 electron in 1909
- Sprayed droplets of oil
- Used x-rays to negatively charge oil drops
2. The Story of Atom
How Robert Milikan discovered the charge and
mass of 1 electron in 1909
- Sprayed droplets of oil
- Used x-rays to negatively charge oil drops
- Used charged plates to “suspend” oil drops
2. The Story of Atom
How Robert Milikan discovered the charge
and mass of 1 electron in 1909
2. The Story of Atom
How Robert Milikan discovered the charge
and mass of 1 electron in 1909
Discovered charge of 1 electron = 1.6 x 10-19 Coulombs
If we know from Thomson’s experiment that electrons have a
charge to mass ratio of 1.76 x 108 Coulombs per gram of
electrons, what is the mass of one electron?
2. The Story of Atom
How Robert Milikan discovered the charge
and mass of 1 electron in 1909
Discovered charge of 1 electron = 1.6 x 10-19 Coulombs
If we know from Thomson’s experiment that electrons have a
charge to mass ratio of 1.76 x 108 Coulombs per gram of
electrons, what is the mass of one electron?
Mass of one electron = 9.11 x 10-28 grams
2. The Story of Atom
How Robert Milikan discovered the charge
and mass of 1 electron in 1909
Discovered charge of 1 electron = 1.6 x 10-19 Coulombs
2. The Story of Atom
How Robert Milikan discovered the charge
and mass of 1 electron in 1909
Discovered charge of 1 electron = 1.6 x 10-19 Coulombs
Mass of one electron = 9.11 x 10-28 grams
Answer on your warmup paper
“JJ. Thomson, Millikan and the Electron Review”
1.
2.
3.
4.
5.
6.
7.
8.
9.
What tool did Thomson use in his discovery of the electron?
Draw and label the parts of Thomson’s tools.
What were Thomson’s three conclusions?
Explain why Thomson concluded that the particles were
negatively charged. Your answer should state something
about opposite charges.
Explain why Thomson included a POSITIVE cloud in his
model of the atom.
What was the purpose of Milikan’s experiment?
Draw and label Milikan’s setup
What two forces did Milikan balance to calculate the charge
of a electron?
Charge of one electron = 1.609 x 10-19C. Use data from
Thomson to calculate mass one of electron.
Where is the Nucleus???
2. The Story of Atom
E. Rutherford and the Nucleus
What would happen you threw a baseball
at a plume of smoke?
2. The Story of Atom
E. Rutherford and the Nucleus
What would happen you threw a baseball at a
plume of smoke?
What would you
conclude if the
baseball bounced
back to you
E. Rutherford
Discovered
Nucleus in
1911
2. The Story of Atom
How Rutherford discovered the Nucleus
Was originally researching radiation and Uranium.
2. The Story of Atom
How Rutherford discovered the Nucleus
Was originally researching radiation and Uranium.
Identified three different types of particles that was “radiating”
from Uranium.
2. The Story of Atom
How Rutherford discovered the Nucleus
Was originally researching radiation and Uranium.
Identified three different types of particles that was “radiating”
from Uranium.
One of them was Alpha Particles.
2. The Story of Atom
How Rutherford discovered the Nucleus
Was originally researching radiation and Uranium.
Identified three different types of particles that was “radiating”
from Uranium.
One of them was Alpha Particles.
They were positively charged particles
That were smaller than an atom.
2. The Story of Atom
How Rutherford discovered the Nucleus
Alpha Particles = positively charged particles
2. The Story of Atom
How Rutherford discovered the Nucleus
Alpha Particles = positively charged particles
Alpha Particles = smaller than an atom.
2. The Story of Atom
How Rutherford discovered the Nucleus
Alpha Particles = positively charged particles
Alpha Particles = smaller than an atom.
Alpha Particles = very dense
2. The Story of Atom
Rutherford’s Experiment
setup
expected results
Rutherford’s Experiment
ACTUAL
expected results
Rutherford’s Experiment
ACTUAL
These results are
crazy! Why?
0 Because it is like throwing a
baseball into a plume of
smoke and having it
rebound and hit you in the
face!
Rutherford’s Experiment
ACTUAL
These results are
crazy! Why?
0 Because it is like throwing a
baseball into a plume of
smoke and having it
rebound and hit you in the
face!
0 So Rutherford
hypothesized that the atom
is NOT like a chocolate chip
cookie.
Rutherford’s Experiment
WHY did Rutherford think an atom is
NOT
like a plum pudding/chocolate chip?
Rutherford’s Experiment
WHY did Rutherford think an atom is
NOT
like a plum pudding/chocolate chip?
Because that model could not explain his
results!
Rutherford’s Experiment
WHY did Rutherford think an atom is
NOT
like a plum pudding/chocolate chip?
But what about the electrons?
Rutherford’s Experiment
WHY did Rutherford think an atom is
NOT
like a plum pudding/chocolate chip?
But what about the electrons?
Couldn’t those have made the alpha
particles bounce and deflect?
Rutherford’s Experiment
NO
Rutherford’s Experiment
NO
Why not?
Think about the washer and hanger
demo.
Rutherford’s Experiment
Even if the marble hit a washer, the
washer does not have enough
___________
to deflect the marble
Rutherford’s Experiment
Because of Milikan, we know the mass of
1 electron
0.000000000000000000000000000909 g
Rutherford’s Experiment
Because of Milikan, we know the mass of
1 electron
0.000000000000000000000000000909 g
9.09 x 10-28 grams
Rutherford’s Experiment
Mass of one alpha particle is
more than 3000 times
larger than one 1 electron
Rutherford’s Experiment
Mass of one alpha particle is
more than 3000 times
larger than one 1 electron
Rutherford’s Experiment
Rutherford’s Model
1. Atoms have something else besides an
electron and empty space.
Rutherford’s Experiment
Rutherford’s Model
1. Atoms have something else besides
an electron and empty space.
2. That “something” has to be very
dense. Why?
Rutherford’s Experiment
Rutherford’s Model
1. Atoms have something else besides
an electron and empty space.
2. That “something” has to be very
dense. Why?
3. That “something” also has a positive
charge. Why?
Rutherford’s Experiment
concluded
so an atom looks like…
from
to
so an atom looks like…
from
to
so an atom looks like…
from
to
Nuclear Model
Rutherford’s Experiment
setup
rethought atom’s structure
2. The Story of Atom
Rutherford and the discovery of the Nucleus
1. Draw and label Rutherford’s setup
2. What did Rutherford expect to see?
3. Why did he expect those results?
4. What did he actually see?
5. Explain how his results led him to propose the
existence of a nucleus
2. The Story of Atom
Rutherford and the discovery of the Nucleus
1. Draw and label Rutherford’s setup.
2. What did Rutherford expect to see? Alpha
particles to pass through the “positive cloud”
3. What did he actually see? Alpha particles
deflecting off at various angles
4. Explain how his results led him to propose the
existence of a nucleus. Rutherford explained that
something dense and positive must be at the
center to deflect and repel the alpha particles.
Just like baseball and plume of smoke
Write these questions on your warm up,
then answer it as you watch the video
0 The narrator’s name is….
0 Around the 19th century the people only new about
_____ different elements
0 Rutherford discovered the nucleus while working in
the city of ______________.
0 Rutherford wondered about the meaning of his
results for __________
0 Rutherford and his partner James ___________ later
discovered the _____________ and the _____________
0 _________ are the agents of change in the universe
Summary of Experiments
Thomson
Milikan
Important because…
Write name and draw
proposed model of atom
SKIP
Draw and label
experimental setup
For Thomson and
Rutherford only What
did they see?
FOR MILIKAN
ONLY:
What two forces was
he trying to balance?
For Thomson and
Rutherford only.
EXPLAIN WHY they
reached their conclusion.
FOR MILIKAN
ONLY:
On what does each
force depend?
Rutherford
Rutherford’s Experiment
concluded
so an atom looks like…
from
to
3. Numbering Atoms
How to study and work with
atoms using numbers
OBJECTIVE: To be able to understand atoms by
using quantitative data.
3. Numbering Atoms
Telling Atoms Apart
3. Numbering Atoms
Telling Atoms Apart
What makes a gold atom different from a
silver atom?
3. Numbering Atoms
Telling Atoms Apart
What makes a gold atom different from a
silver atom?
Answer: the number of subatomic
particles
3. Numbering Atoms
Telling Atoms Apart
The most important number to the
IDENTITY
of an atom is
3. Numbering Atoms
Telling Atoms Apart
The most important number to the
IDENTITY
of an atom is
the number of PROTONS
3. Numbering Atoms
Telling Atoms Apart
ATOMIC NUMBER = # of protons
3. Numbering Atoms
Telling Atoms Apart
ATOMIC NUMBER = # of protons
Example:
Atom with 2 protons is a Helium atom
3. Numbering Atoms
Telling Atoms Apart
ATOMIC NUMBER = # of protons
Example:
Atom with 2 protons is a helium atom
Atom with 6 protons is a carbon atom
3. Numbering Atoms
Telling Atoms Apart
ATOMIC NUMBER = # of protons
Each type of atom has its own ATOMIC
NUMBER
3. Numbering Atoms
Telling Atoms Apart
ATOMIC NUMBER = # of protons
Each type of atom has its own ATOMIC
NUMBER
This number NEVER changes
3. Numbering Atoms
Telling Atoms Apart
ATOMIC NUMBER = # of protons
Atomic number also tells us # of
electrons
3. Numbering Atoms
Telling Atoms Apart
ATOMIC NUMBER = # of protons
Atomic number also tells us # of
electrons
WHY?
3. Numbering Atoms
Telling Atoms Apart
MASS NUMBER = # of protons AND neutrons
Mass number =/= Mass of element
3. Numbering Atoms
Telling Atoms Apart
MASS NUMBER = # of protons AND neutrons
Mass number =/= Mass of element
Mass Number
- Atomic Number
Number of Neutrons
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
1. How many protons is a copper atom?
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
1. How many protons is a copper atom?
1. Atomic Number = Number of protons
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
1. How many protons is a copper atom?
1. Atomic Number = Number of protons
2. So answer = 29
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
2. How many electrons in a copper atom?
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
2. How many electrons in a copper atom?
1. Atomic Number = Number of protons
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
2. How many electrons in a copper atom?
1. Atomic Number = Number of protons
2. Atoms are neutral, so number of protons = number of electrons
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
2. How many electrons in a copper atom?
1. Atomic Number = Number of protons
2. Atoms are neutral, so number of protons = number of electrons
3. So answer = 29
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
3. How many neutrons in this copper atom?
1. Mass Number – Atomic Number = Number of Neutrons
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
3. How many neutrons in this copper atom?
1. Mass Number – Atomic Number = Number of Neutrons
2. Mass Number = 64, and Atomic Number = 29
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
3. How many neutrons in this copper atom?
1. Mass Number – Atomic Number = Number of Neutrons
2. Mass Number = 64, and Atomic Number = 29
3. 64-29 = 35 Neutrons
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
3. How many neutrons in this copper atom?
1. Mass Number – Atomic Number = Number of Neutrons
2. Mass Number = 64, and Atomic Number = 29
3. 64-29 = 35 Neutrons
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
1. How many protons in a copper atom?
1.
2.
Atomic Number = Number of protons
So answer = 29
2. How many electrons in a copper atom?
1. Atomic Number = Number of protons
2. Atoms are neutral, so number of protons = number of electrons
3. So answer = 29
3. How many neutrons in this copper atom?
1. Mass Number – Atomic Number = Number of Neutrons
2. Mass Number = 64, and Atomic Number = 29
3. 64-29 = 35 Neutrons
3. Numbering Atoms
Practice using Atomic and Mass Numbers
Copper’s atomic number is 29, and the mass number is 64.
1. How many protons in a copper atom?
1.
2.
Atomic Number = Number of protons
So answer = 29
2. How many electrons in a copper atom?
1. Atomic Number = Number of protons
2. Atoms are neutral, so number of protons = number of electrons
3. So answer = 29
3. How many neutrons in this copper atom?
1. Mass Number – Atomic Number = Number of Neutrons
2. Mass Number = 64, and Atomic Number = 29
3. 64-29 = 35 Neutrons
3. Numbering Atoms
Atomic
Symbol
Atomic
Number
O
Number of
Protons
11
5
Number of
Neutrons
16
7
Pb
Mass
Number
8
122
Number of
Electrons
3. Numbering Atoms
Atomic
Symbol
Atomic
Number
Mass
Number
Number of
Protons
Number of
Neutrons
Number of
Electrons
B
5
11
5
6
5
O
8
16
8
8
8
N
7
15
7
8
7
Pb
82
204
82
122
82
3. Numbering Atoms
Telling Atoms Apart
3. Numbering Atoms
Telling Atoms Apart
Atoms of the SAME element can have different number of
NEUTRONS.
3. Numbering Atoms
Telling Atoms Apart
Atoms of the SAME element can have different number of
NEUTRONS.
These types of atoms are called ISOTOPES
3. Numbering Atoms
Telling Atoms Apart
Atoms of the SAME element can have different number of
NEUTRONS.
These types of atoms are called ISOTOPES
Iso = same
Tope = place
3. Numbering Atoms
Telling Atoms Apart
Atoms of the SAME element can have different number of
NEUTRONS.
These types of atoms are called ISOTOPES
Iso = same
Tope = place
3. Numbering Atoms
Telling Atoms Apart
Atoms of the SAME element can have different number of
NEUTRONS.
These types of atoms are called ISOTOPES
Iso = same
Tope = place
3. Numbering Atom
Telling Atoms Apart
ISOTOPES
3. Numbering Atom
Telling Atoms Apart
Different atoms can have the same MASS NUMBER.
3. Numbering Atoms
Telling Atoms Apart
Draw models of the nuclei of two isotopes:
carbon-12
carbon-13
3. Numbering Atom
Telling Atoms Apart
Different atoms can have the same MASS NUMBER.
3. Numbering Atom
Telling Atoms Apart
Different atoms can have the same MASS NUMBER
They CANNOT have the same ATOMIC NUMBER
3. Numbering Atoms
Telling Atoms Apart
Different atoms can have the same MASS NUMBER
They CANNOT have the same ATOMIC NUMBER
EX:
Copper
Atomic Number = 29
Neutrons = 29 or 36
3. Numbering Atoms
Telling Atoms Apart
Different atoms can have the same MASS NUMBER
They CANNOT have the same ATOMIC NUMBER
EX:
Copper
Atomic Number = 29
Neutrons = 29 or 36
Mass Number = 58 or 65
3. Numbering Atoms
Telling Atoms Apart
Different atoms can have the same MASS NUMBER
They CANNOT have the same ATOMIC NUMBER
EX:
Copper
Atomic Number = 29
Neutrons = 29 or 36
Mass Number = 58 or 65
Zinc
Atomic Number = 30
3. Numbering Atoms
Telling Atoms Apart
Different atoms can have the same MASS NUMBER
They CANNOT have the same ATOMIC NUMBER
EX:
Copper
Atomic Number = 29
Neutrons = 29 or 36
Mass Number = 58 or 65
Zinc
Atomic Number = 30
Neutrons = 30 or 35
3. Numbering Atoms
Telling Atoms Apart
Different atoms can have the same MASS NUMBER
They CANNOT have the same ATOMIC NUMBER
EX:
Copper
Atomic Number = 29
Neutrons = 29 or 36
Mass Number = 58 or 65
Zinc
Atomic Number = 30
Neutrons = 30 or 35
Mass Number = 60 or 65
3. Numbering Atoms
Scientific Notation
3.0 x 108 meter per second
0.000000000000000000000000000909 g
3. Numbering Atoms
Counting Atoms + Mole
3. Numbering Atoms
Counting Atoms
How many donuts in one dozen?
3. Numbering Atoms
Counting Atoms
How many donuts in one dozen?
How many flowers in one dozen?
3. Numbering Atoms
Counting Atoms
How many donuts in one dozen?
How many flowers in one dozen?
How many eggs in one dozen?
3. Numbering Atoms
Counting Atoms
How many donuts in one dozen?
How many flowers in one dozen?
How many eggs in one dozen?
Does it matter?
3. Numbering Atoms
Counting Atoms
Dozen = unit of measurement
Mole is also a unit of measurement
3. Numbering Atoms
Counting Atoms
Just like 1 dozen = 12
1 mole = 6.02 x 1023
602 000 000 000 000 000 000 000
3. Numbering Atoms
Counting Atoms
1 mole = 6.02 x 1023
1 mole of donuts = 602 000 000 000 000
000 000 000 donuts
3. Numbering Atoms
Counting Atoms
1 mole = 6.02 x 1023
1 mole of donuts = 602 000 000 000 000
000 000 000 donuts
1 mole of flowers = 602 000 000 000 000
000 000 000 flowers
3. Numbering Atoms
Counting Atoms
1 mole = 6.02 x 1023
We use MOLE to count number of atoms
3. Numbering Atoms
Counting Atoms
1 mole = 6.02 x 1023
Example: 1 mole of Copper atoms = 602 000
000 000 000 000 000 000 atoms
6.02 x 1023 copper atoms
3. Numbering Atoms
Counting Atoms
6.02 x 1023 = Avogadro’s Number
3. Numbering Atoms
Counting Atoms
6.02 x 1023 = Avogadro’s Number
C.F. 1 mole = 6.02 x 1023 atoms
3. Numbering Atoms
C.F. 1 mole = 6.02 x
23
10
1. Convert 3.27 moles of Fe into
number of atoms.
3. Numbering Atoms
Counting Atoms
How do we get moles?
3. Numbering Atoms
Counting Atoms
How do we get moles?
We get moles from MOLAR MASS
3. Numbering Atoms
Counting Atoms
Where do we get Molar Mass?
3. Numbering Atoms
Counting Atoms
Where do we get Molar Mass?
We get Molar Mass from Atomic Mass
3. Numbering Atoms
Counting Atoms
Where do we get Atomic Mass?
We get Molar Mass from Atomic Mass
3. Numbering Atoms
Counting Atoms
Where do we get Atomic Mass?
We get Atomic Mass from Periodic Table
3. Numbering Atoms
Counting Atoms
Atomic Mass = Molar Mass = 1 Mole
in AMU
in grams
3. Numbering Atoms
Counting Atoms
Atomic Mass = Molar Mass = 1 Mole
in AMU
in grams
Example:
Carbon: Atomic mass = 12.01 AMU
3. Numbering Atoms
Counting Atoms
Atomic Mass = Molar Mass = 1 Mole
in AMU
in grams
Example:
Carbon: Atomic mass = 12.01 AMU
so Molar Mass = 12. 01 g
3. Numbering Atoms
Counting Atoms
Atomic Mass = Molar Mass = 1 Mole
in AMU
in grams
Example:
Carbon: Atomic mass = 12.01 AMU
so Molar Mass = 12. 01 g
so 12.01 g of Carbon = 1 mole of Carbon