Warm-UpSeptember 13, 2013 (ODD)

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 Atom2. The Story of Chemistry

HOMEWORK- Read pages 73 – 78

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 Atom2. The Story of Chemistry

HOMEWORK- Read pages 73 – 78

Warm-Up September 17, 2013 (ODD)1. What is the difference between a law and theory2. 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 exam2. Finish The Story of Chemistry3. The sequel: The Story of the Atom

HOMEWORK

Warm-Up September 18, 2013 (EVEN)1. What is the difference between a law and theory2. 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 Chemistry2. The sequel: The Story of the Atom

HOMEWORK

Agenda September 19, 2013 (ODD)1. Lego Activity2. The sequel: The Story of the Atom

HOMEWORK

Warm-Up September 20, 2013 (E)1. Democritus came up with the concept of ________2. Robert Boyle came up with the concept of _______3. What are three important laws from the story so

far?4. Look up the terms “reactant” and “products.”

Agenda September 20, 2013 (E)1. Finish Lego Activity today2. 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 ray5. 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 homework2. Begin the “The Story of Atom”, the sequel to “The


HOMEWORK1. Worksheet

Agenda September 23, 2013 (O)1. Go over homework2. 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


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 ray5. If a metal has a density of 2.86 g/cm3, what is the

volume? The mass is 0.327g6. Turn homework in box

Agenda September 24, 2013 (E)1. Go over homework2. Begin the “The Story of Atom”, the sequel to “The



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 homework2. 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

HOMEWORK1. Worksheet2. 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 Proportion4. 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 homework2. 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


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 Proportion4. 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 homework2. Continue the “The Story of Atom”, the sequel to

“The Story of Chemistry”• Discovery of the Nucleus and the Proton



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


HOMEWORK1. Worksheet2. Section Review 3.2

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


HOMEWORK1. Worksheet2. Section Review 3.2

Warm-Up October 4, 2013 (E)1. Draw and label Thomson’s experimental setup.2. Milikan is important because he calculated…3. What two forces was Milikan trying to balance?4. 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

Agenda October 3, 2013 (E)1. 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

HOMEWORK1. 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 ChemistryA. Greek Beginnings



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.

Early human civilizations organized “stuff” into four categories: Earth, Air, Fire, Water




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


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.


ATOM = a Greek word


ATOM = a Greek word

Temnein = to cut or divide

A = prefix meaning not


ATOM = a Greek word



a + temnein =


ATOM = a Greek word



a + temnein = unable to cut




He called that “thing” an ATOM.


Democritus’ idea of the atom is…

An observation?A hypothesis?

An experiment?A law?

A theory?


Democritus’ idea of the atom is…

A hypothesis because his idea could not be tested.


IMPORTANT!!!

Democritus’ idea of atom =/=

1. The Story of ChemistryB. Foundational Ideas

1. Democritus2. Alchemists during the Middle Ages –

wanted to convert one element to another.


1. Democritus2. Alchemists during the Middle Ages –

wanted to convert one element to another.

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.



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.



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 Chemistry4. 18th century; 1700’s

Joseph Priestly – O2, Combustion, CO2


Antoine Lavoisier


Antoine Lavoisier – Refined Priestly’s understanding of combustion as involiving carbon-based substance plus oxygen results in CO2 and H2O.


Antoine Lavoisier – MORE IMPORTANT than that =



something cannot be made from nothing



something cannot be made from nothing, and

something cannot become nothing.


Antoine Lavoisier – saw that when a chemical change takes place, the mass does not change.


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.


“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?


“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


Antoine Lavoisier is important because he showed that mass/matter cannot be created or destoyed.


Joseph Proust -


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…


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

C6H12O6H2O will always be made up of 2 H and 1

O


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?


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


John Dalton


Compound Mass of Element(g)

A 133B 266



A 0.0839



A 0.0839B 0.1678



A 0.0839B 0.1678C 0.2520



A 0.0839B 0.1678C 0.2520D



A 0.0839B 0.1678C 0.2520D 0.336



A 0.59B 1.18



A 0.59B 1.18C



A 0.59B 1.18C 1.77D



A 0.59B 1.18C 1.77D 2.36



A 0.59B 1.18C 1.77D 2.36E

F



A 0.59B 1.18C 1.77D 2.36E 2.96F 3.54


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.


John Dalton

Proposed a theory that all matter is made up of indivisible things called ATOMs.


John Dalton


We call this theory,

THE ATOMIC THEORY OF MATTER


John Dalton


We call this theory,

THE ATOMIC THEORY OF MATTER

How is a law different from a theory?

1. The Story of ChemistryDalton’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, whole- number ratios to form compounds

5. In chemical reactions, atoms are combined, separated, or rearranged but never created, destroyed, or changed

1. The Story of ChemistryDalton’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, whole- number 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 ChemistryQUICKWRITE

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


Atom made up of smaller parts

These parts are called: SUBATOMIC Particles


SUBATOMIC PARTICLES

Atom made up of smaller parts

These parts are called: SUBATOMIC Particles

Three types of SUBATOMIC Particles

1. Proton2. Neutron3. Electron


SUBATOMIC PARTICLES

1. Proton

- Has a POSITIVE charge- Mass is similar to that of a Neutron- Located in the nucleus


SUBATOMIC PARTICLES

2. Neutron

- Has NO charge- Has the largest mass of the three- Located in the nucleus


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


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 likethis

What’s missing in this picture?

So how did we get

from to

J.J. Thomson

How does a person discover a particle so small that no one has seen?

Discovered Electron in 1897

2. The Story of AtomHow 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 connectedto a power source.





Then the metal plates were connectedto a power source.

This resulted in a beam of light thatstarted from the cathode (-) and went to the anode (+)


Because these beams started from the cathode (-), scientists called the beam a CATHODE RAY



But what are these CATHODE RAYs made of?



But what are these CATHODE RAYs made of?

Thomson was trying to answerthis 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



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 Conclusions0 Cathode rays must be made of stuff that is NEGATIVELY

charged


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.




2. Thomson applied an ELECTRIC and magnetic field to 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.


How Robert Milikan calculated the charge and mass of 1 electron in 1909


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


How Robert Milikan discovered the charge and mass of 1 electron in 1909



- Sprayed droplets of oil



- Sprayed droplets of oil- Used x-rays to negatively charge oil drops



- Sprayed droplets of oil- Used x-rays to negatively charge oil drops- Used charged plates to “suspend” oil drops






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?




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







Mass of one electron = 9.11 x 10-28 grams

Answer on your warmup paper“JJ. Thomson, Millikan and the Electron Review”

1. What tool did Thomson use in his discovery of the electron?2. Draw and label the parts of Thomson’s tools.3. What were Thomson’s three conclusions?4. Explain why Thomson concluded that the particles were

negatively charged. Your answer should state something about opposite charges.

5. Explain why Thomson included a POSITIVE cloud in his model of the atom.

6. What was the purpose of Milikan’s experiment? 7. Draw and label Milikan’s setup8. What two forces did Milikan balance to calculate the charge

of a electron? 9. Charge of one electron = 1.609 x 10-19C. Use data from

Thomson to calculate mass one of electron.

Where is the Nucleus???


E. Rutherford and the Nucleus

What would happen you threw a baseball at a plume of smoke?

http://www.google.com/url?sa=i&rct=j&q=&esrc=s&frm=1&source=images&cd=&cad=rja&docid=L0x9e__RhecpAM&tbnid=bXTj4_3gh8L1tM:&ved=&url=http://vimeo.com/42962109&ei=2h1DUvP6DOKIigLslIDABA&psig=AFQjCNFVpHXPDlewMqRbap2scviToPxeIg&ust=1380216666678181


E. Rutherford and the Nucleus

What would happen you threw a baseball at a plume of smoke?

What would you conclude if the baseball bouncedback to you

http://www.google.com/url?sa=i&rct=j&q=&esrc=s&frm=1&source=images&cd=&cad=rja&docid=L0x9e__RhecpAM&tbnid=bXTj4_3gh8L1tM:&ved=&url=http://vimeo.com/42962109&ei=2h1DUvP6DOKIigLslIDABA&psig=AFQjCNFVpHXPDlewMqRbap2scviToPxeIg&ust=1380216666678181

E. Rutherford

Discovered Nucleus in

1911

2. The Story of AtomHow 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.




One of them was Alpha Particles.

They were positively charged particlesThat were smaller than an atom.


Alpha Particles = positively charged particles



Alpha Particles = smaller than an atom.



Alpha Particles = smaller than an atom.

Alpha Particles = very dense


Rutherford’s Experiment

setup expected results


ACTUAL expected results


ACTUALThese 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!


ACTUALThese 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 ExperimentWHY did Rutherford think an atom is

NOTlike a plum pudding/chocolate chip?



Because that model could not explain his results!



But what about the electrons?



But what about the electrons?

Couldn’t those have made the alpha particles bounce and deflect?

Rutherford’s ExperimentNO

Rutherford’s ExperimentNO

Why not?

Think about the washer and hanger demo.

Rutherford’s ExperimentEven if the marble hit a washer, the

washer does not have enough___________

to deflect the marble

Rutherford’s ExperimentBecause of Milikan, we know the mass of

1 electron

0.000000000000000000000000000909 g

Rutherford’s ExperimentBecause of Milikan, we know the mass of

1 electron

0.000000000000000000000000000909 g

9.09 x 10-28 grams

Rutherford’s ExperimentMass of one alpha particle is

more than 3000 times larger than one 1 electron

Rutherford’s ExperimentMass of one alpha particle is

more than 3000 times larger than one 1 electron

Rutherford’s ExperimentRutherford’s Model

1. Atoms have something else besides an electron and empty space.



2. That “something” has to be very dense. Why?



2. That “something” has to be very dense. Why?

3. That “something” also has a positive charge. Why?


concluded

so an atom looks like…

from to


from to


from to

Nuclear Model


setup rethought atom’s structure


Rutherford and the discovery of the Nucleus

1. Draw and label Rutherford’s setup2. 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


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 angles4. 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

0The narrator’s name is….0Around the 19th century the people only new about

_____ different elements0Rutherford discovered the nucleus while working in

the city of ______________.0Rutherford wondered about the meaning of his

results for __________0Rutherford and his partner James ___________ later

discovered the _____________ and the _____________0_________ are the agents of change in the universe

Summary of ExperimentsThomson Milikan Rutherford

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?

concluded



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 AtomsTelling Atoms Apart

ATOMIC NUMBER = # of protons



Example:Atom with 2 protons is a Helium atom



Example:Atom with 2 protons is a helium atomAtom with 6 protons is a carbon atom



Each type of atom has its own ATOMIC NUMBER



Each type of atom has its own ATOMIC NUMBER

This number NEVER changes



Atomic number also tells us # of electrons



Atomic number also tells us # of electrons

WHY?


MASS NUMBER = # of protons AND neutrons

Mass number =/= Mass of element


MASS NUMBER = # of protons AND neutrons

Mass number =/= Mass of element

Mass Number- Atomic Number

Number of Neutrons

3. Numbering AtomsPractice 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?


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



1. How many protons is a copper atom?1. Atomic Number = Number of protons2. So answer = 29



2. How many electrons in a copper atom?



2. How many electrons in a copper atom?1. Atomic Number = Number of protons



2. How many electrons in a copper atom?1. Atomic Number = Number of protons2. Atoms are neutral, so number of protons = number of electrons



2. How many electrons in a copper atom?1. Atomic Number = Number of protons2. Atoms are neutral, so number of protons = number of electrons3. So answer = 29



3. How many neutrons in this copper atom?1. Mass Number – Atomic Number = Number of Neutrons



3. How many neutrons in this copper atom?1. Mass Number – Atomic Number = Number of Neutrons2. Mass Number = 64, and Atomic Number = 29



3. How many neutrons in this copper atom?1. Mass Number – Atomic Number = Number of Neutrons2. Mass Number = 64, and Atomic Number = 293. 64-29 = 35 Neutrons





Copper’s atomic number is 29, and the mass number is 64.1. How many protons in a copper atom?

1. Atomic Number = Number of protons2. So answer = 29




Copper’s atomic number is 29, and the mass number is 64.1. How many protons in a copper atom?

1. Atomic Number = Number of protons2. So answer = 29



3. Numbering Atoms

Atomic Symbol

Atomic Number

Mass Number

Number of Protons

Number of Neutrons

Number of Electrons

11 5

O 16

7 8

Pb 122

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



Atoms of the SAME element can have different number of NEUTRONS.



These types of atoms are called ISOTOPES




Iso = sameTope = place









3. Numbering AtomTelling Atoms Apart

ISOTOPES


Different atoms can have the same MASS NUMBER.


Draw models of the nuclei of two isotopes: carbon-12carbon-13


Different atoms can have the same MASS NUMBER.


Different atoms can have the same MASS NUMBER

They CANNOT have the same ATOMIC NUMBER




EX: CopperAtomic Number = 29Neutrons = 29 or 36




EX: CopperAtomic Number = 29Neutrons = 29 or 36Mass Number = 58 or 65




EX: Copper ZincAtomic Number = 29 Atomic Number = 30Neutrons = 29 or 36Mass Number = 58 or 65




EX: Copper ZincAtomic Number = 29 Atomic Number = 30Neutrons = 29 or 36 Neutrons = 30 or 35Mass Number = 58 or 65




EX: Copper ZincAtomic Number = 29 Atomic Number = 30Neutrons = 29 or 36 Neutrons = 30 or 35Mass Number = 58 or 65 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 eggs in one dozen?

3. Numbering Atoms

Counting Atoms


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 = 121 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 1023

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 Molein AMU in grams

3. Numbering Atoms

Counting Atoms


Example:Carbon: Atomic mass = 12.01 AMU

3. Numbering Atoms

Counting Atoms



so Molar Mass = 12. 01 g

3. Numbering Atoms

Counting Atoms



so Molar Mass = 12. 01 gso 12.01 g of Carbon = 1 mole of Carbon

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Warm-UpSeptember 13, 2013 (ODD)