Period 7.. Pre-Socratic philosopher Born in Abdera, Elea, or Miletus in the 5th Century B.C....

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Period 7.

•Pre-Socratic philosopher

•Born in Abdera, Elea, or Miletus in the 5th Century B.C.

•Pre-Socratic philosopher

•Born in Abdera, Elea, or Miletus in the 5th Century B.C.



• Lived from 460-370 B.C

• Ancient Greek philosopher

• His mentor was Leucippus

• The two of them worked together on atoms

•He was more of a scientists than other Greek philosophers

•Leucippus and Democritus realized that the world consisted of myriads of

indivisible particles, called atoms which were the smallest particles of

matter possible•Upon further speculation, they came up

with the idea that the observable properties of common materials are because of the different shapes of

atoms which they contain, or different motions of atoms

•Leucippus and Democritus realized that the world consisted of myriads of

indivisible particles, called atoms which were the smallest particles of

matter possible•Upon further speculation, they came up

with the idea that the observable properties of common materials are because of the different shapes of

atoms which they contain, or different motions of atoms

• Lived from 384 to 322 BC

• He was a Greek philosopher

• A student of Plato and a teacher of Alexander the Great

• Had ideas referring to many different subjects



• Aristotle’s Theory of the Elements: A piece of matter could be divided an infinite number of times and one would never

find a piece of matter that could be further divided

• He believed in the four elements: earth, fire, water, and air

• According to him, everything in the world was made up of some combination of these four elements

•At this time this was the most popular theory.

•The atomic theories that were created at this time were not 100% accurate; however, they provided insight in an area never explored

before•The central ideas of Leucippus and Democritus have remained

unchanged

•The atomic theories that were created at this time were not 100% accurate; however, they provided insight in an area never explored

before•The central ideas of Leucippus and Democritus have remained

unchanged

Antoine Lavoisier & The Law of

Conservation of Matter

Antoine Lavoisier & The Law of

Conservation of Matter

By: Jin Shin & Taylor Seeman By: Jin Shin & Taylor Seeman

Born: August 26, 1743

Died: May 8, 1794

“Father of Modern Chemistry”

Attended the College Mazarin at the request of his aunt

College Mazarin had an excellent mathematics and science program

Lavoisier was a brilliant student, and earned numerous awards

He conducted his first few experiments individually or while aiding professors.

Attended the College Mazarin at the request of his aunt

College Mazarin had an excellent mathematics and science program

Lavoisier was a brilliant student, and earned numerous awards

He conducted his first few experiments individually or while aiding professors.

Educational Background

ExperimentExperiment

Lavoisier burnt phosphorous and sulfur in air and proved the products weighed more than the reactants but the weight gained was lost from the air.

Lavoisier burnt phosphorous and sulfur in air and proved the products weighed more than the reactants but the weight gained was lost from the air.

ExperimentExperiment

When you heat a piece of copper metal in air, it comes together with oxygen in the air. If you weigh it, it is found to have a greater mass that the original piece. However, the mass of the oxygen of the air is combined with the mass of copper, the mass of the product is equal to the sum of the masses of the copper and oxygen that were combined.

When you heat a piece of copper metal in air, it comes together with oxygen in the air. If you weigh it, it is found to have a greater mass that the original piece. However, the mass of the oxygen of the air is combined with the mass of copper, the mass of the product is equal to the sum of the masses of the copper and oxygen that were combined.

Significance of Concept


Showed that the quantity of matter is the same in the beginning and end of every chemical reaction, though matter may change its state.

Though matter may change form, it can neither be created nor destroyed

Mass of reactants always equal the mass of products

Showed that the quantity of matter is the same in the beginning and end of every chemical reaction, though matter may change its state.

Though matter may change form, it can neither be created nor destroyed

Mass of reactants always equal the mass of products



Law demonstrates understanding of the properties of movement and energy.

It is a fundamental principle of physics.

Law demonstrates understanding of the properties of movement and energy.

It is a fundamental principle of physics.

Sources: http://www.iscid.

org/encyclopedia/Law_of_Conservation_of_Mass

http://www.biographybase.com/biography/Lavoisier_Antoine_Laurent.html

Sources: http://www.iscid.

org/encyclopedia/Law_of_Conservation_of_Mass


http://www.iscid.org/encyclopedia/Law_of_Conservation_of_Mass






















Joseph Proust: Law of Definite ProportionsJoseph Proust: Law of Definite Proportions

By: Simir and KatieBy: Simir and Katie



-born in France (1754-1826)

-son of a pharmacist

-chief apothecary at Saltpetriere Hospital

-became the director of Royal Laboratory under Charles IV

-laboratory was destroyed by the invasion of Spanish Army by Napoleon so he returned to France

Joseph Proust Joseph Proust

-Lived in poverty before being awarded pension by Louis XVIII

-He taught at the Chemistry school at Segovia and the University of Salamanca at Spain

-He was the chair of this school and was proposed in 1784 to to train artillery cadets with the latest scientific knowledge

-He worked with Antoine Lavosier

-He also taught chemistry at Musee, a private school in Paris,

-Lived in poverty before being awarded pension by Louis XVIII

-He taught at the Chemistry school at Segovia and the University of Salamanca at Spain

-He was the chair of this school and was proposed in 1784 to to train artillery cadets with the latest scientific knowledge

-He worked with Antoine Lavosier

-He also taught chemistry at Musee, a private school in Paris,



ExperimentExperiment Proust prepared a copper carbonate

compound He heated it, getting rid of the water

and then the carbonic acid, or what was left of the copper oxide

- From the 180 lbs of "copper carbonate" (it was actually carbon dioxide) he took away 10 lbs of water and 46 of the carbon dioxide

- The copper oxide left had 100 lbs of copper and 25 of oxygen

Proust prepared a copper carbonate compound

He heated it, getting rid of the water and then the carbonic acid, or what was left of the copper oxide

- From the 180 lbs of "copper carbonate" (it was actually carbon dioxide) he took away 10 lbs of water and 46 of the carbon dioxide

- The copper oxide left had 100 lbs of copper and 25 of oxygen

ExperimentExperimentDecomposition of CuCO3 into

Cu, C and OProust found that the ratio of

the masses of Cu to C to O was always the same no matter what size sample of CuCO3 he started with.

He formed his theory by dividing to find the ratios

Decomposition of CuCO3 into Cu, C and O

Proust found that the ratio of the masses of Cu to C to O was always the same no matter what size sample of CuCO3 he started with.

He formed his theory by dividing to find the ratios







Example Set of DataExample Set of Data

SignificanceSignificance

Law of Definite ProportionsCopper carbonate must always be made

from the same fixed proportions of copper, carbon, and oxygen

All compounds contain elements in certain definite proportions

Ex) Nitric Oxide- 8:7 oxygen to nitrogenEx2) Water- 8:1 oxygen to hydrogen

Law of Definite ProportionsCopper carbonate must always be made

from the same fixed proportions of copper, carbon, and oxygen

All compounds contain elements in certain definite proportions

Ex) Nitric Oxide- 8:7 oxygen to nitrogenEx2) Water- 8:1 oxygen to hydrogen

Significance in the Scientific CommunitySignificance in the

Scientific Community Initially not accepted by all chemists ie) Claude-Louis Berthollet

argued that elements could combine in many different proportions (actually thinking of solutions/mixtures- Proust was thinking of compounds)

Law of Definite Proportions was the basis for John Dalton’s atomic theory and multiple proportions

Initially not accepted by all chemists ie) Claude-Louis Berthollet

argued that elements could combine in many different proportions (actually thinking of solutions/mixtures- Proust was thinking of compounds)

Law of Definite Proportions was the basis for John Dalton’s atomic theory and multiple proportions





Significance in Scientific Community

cont

Significance in Scientific Community

contProust expanded upon Lavoisier’s Law of Conservation of Mass

Law of Conservation of Mass-mass of reactants was always equal to mass of products (matter cannot be created or destroyed)

Proust measured each individual substance instead of the total mass for reactants and products



John Dalton Early Life

John Dalton Early Life

From Cumberland, England

Birth date is unknown

Family were Quakers Worked in the

fields and in the family cloth shop

Relatively poor Did not get formal

education Did get basic

lessons in reading, writing, and arithmetic

From Cumberland, England

Birth date is unknown

Family were Quakers Worked in the

fields and in the family cloth shop

Relatively poor Did not get formal

education Did get basic

lessons in reading, writing, and arithmetic

John Dalton Adult Life

John Dalton Adult Life

Dalton and his brother ran a school in Kendal

Dalton recorded the weather patterns each day (for his entire life) in a journal

Originally wanted to be a physician, decided on scientist instead

Tutored students at Manchester University

Dalton and his brother ran a school in Kendal

Dalton recorded the weather patterns each day (for his entire life) in a journal

Originally wanted to be a physician, decided on scientist instead

Tutored students at Manchester University

Dalton’s Law of Multiple Proportions


If 2 elements formmultiple compounds,the ratios of themasses of the secondelement combiningwith a fixed mass ofthe first element willbe in ratios of smallwhole numbers

If 2 elements formmultiple compounds,the ratios of themasses of the secondelement combiningwith a fixed mass ofthe first element willbe in ratios of smallwhole numbers



For Example Elements Y and Z

The weight of Element Z, when combined with the fixed weight of element Y, will compute to a ratio of small integral numbers (2:1, 3:1, etc.)

ORCarbon + Oxygen = CO,

CO2, but not CO1.3

For Example Elements Y and Z

The weight of Element Z, when combined with the fixed weight of element Y, will compute to a ratio of small integral numbers (2:1, 3:1, etc.)

ORCarbon + Oxygen = CO,

CO2, but not CO1.3

Importance of Dalton’s Law of

Multiple Proportions

Importance of Dalton’s Law of

Multiple Proportions One of the fundamental laws of stoichiometry

Basis for other Atomic Theories Law of Conservation of Mass

Law of Definite Proportions

One of the fundamental laws of stoichiometry

Basis for other Atomic Theories Law of Conservation of Mass

Law of Definite Proportions

Dalton’s Modern Atomic Theory

Dalton’s Modern Atomic Theory

All matter is made of atoms

Atoms are invisible and indestructible

All atoms of a given element are identical in mass and properties

Compounds are formed by a combinations of two or more different kinds of atoms

A chemical reaction is a rearrangement of atoms

All matter is made of atoms

Atoms are invisible and indestructible

All atoms of a given element are identical in mass and properties

Compounds are formed by a combinations of two or more different kinds of atoms

A chemical reaction is a rearrangement of atoms

The DiscoveryThe Discovery

Dalton studied gases Discovered the partial

pressures of gases Lead to formulation of

working theory of the atom

*Noticed that certain gases maintained the same ratios of mixture regardless of amount

Realized that Ratios remain the same because they were consistent down to the smallest particle or atom

Dalton studied gases Discovered the partial

pressures of gases Lead to formulation of

working theory of the atom

*Noticed that certain gases maintained the same ratios of mixture regardless of amount

Realized that Ratios remain the same because they were consistent down to the smallest particle or atom

Significance of Dalton’s Atomic

Theory

Significance of Dalton’s Atomic

Theory First understanding

of the atom Prior to, it was

an abstract philosophical concept

The essence of Dalton’s theory remains valid

Led to great expansion of theoretical thought in chemistry

First understanding of the atom Prior to, it was

an abstract philosophical concept

The essence of Dalton’s theory remains valid

Led to great expansion of theoretical thought in chemistry

JJ ThomsonJJ Thomson

-Discovered the electron and also invented the mass spectrometer

-Interested in sciences as a child and later on his life showed a large interest in atomic structure

-Graduated and taught at Trinity College after a brief stay at Owens College

-Was an author of many non-fiction science books



Personal LifePersonal Life

-Born in Cheetham Hill, Manchester on Decemeber 18, 1856

-Full name Sir Joseph John Thomson-Father died when he was only 16-In 1890 he married Rose Elizabeth-He had one son named Sir George Paget Thomson

-Born in Cheetham Hill, Manchester on Decemeber 18, 1856

-Full name Sir Joseph John Thomson-Father died when he was only 16-In 1890 he married Rose Elizabeth-He had one son named Sir George Paget Thomson




-A century ago discovered the electron while using a Cathode Ray Tube

-Cathode Ray Tube is a glass tube that has wiring attached to its two sides.

-The air is taken out and in order to try and form a vacuum.

-An electric charge goes from one end to the other and produces a glow that looks fluorescent.

-A cathode ray or electron gun is attached to the glass contraption

-A century ago discovered the electron while using a Cathode Ray Tube

-Cathode Ray Tube is a glass tube that has wiring attached to its two sides.

-The air is taken out and in order to try and form a vacuum.

-An electric charge goes from one end to the other and produces a glow that looks fluorescent.

-A cathode ray or electron gun is attached to the glass contraption



The ExperimentThe Experiment

-Used his Cathode Ray Tube made a unique tube to probe that the rays shot in had a negative charge.

-Almost perfect vacuum and he put the fluorescent layer on a specific side.

- Had an electric plate, this gave a positive charged electrode to the negative cathode. The ray would be deflected.

-Shot a ray got deflected by the opposite positive charge. This showed that the ray was made up of charged, negatively particles.

-Used his Cathode Ray Tube made a unique tube to probe that the rays shot in had a negative charge.

-Almost perfect vacuum and he put the fluorescent layer on a specific side.

- Had an electric plate, this gave a positive charged electrode to the negative cathode. The ray would be deflected.

-Shot a ray got deflected by the opposite positive charge. This showed that the ray was made up of charged, negatively particles.



The Third ExperimentThe Third Experiment

-Figured out that the charge to mass ratio could have been very large or extremely small

-Chose correctly that they were very small

-Figured out that the charge to mass ratio could have been very large or extremely small

-Chose correctly that they were very small



SignificanceSignificance

-Later Devices, helps with electronic devices, making impulses so a screen can run and one can see a display.

-Cathode-Ray Tube can produce an image on a screen with electrical impulses.

-It can primarily help with TV screens and computer screens.

-Disproved Plum-Pudding theory

-Later Devices, helps with electronic devices, making impulses so a screen can run and one can see a display.

-Cathode-Ray Tube can produce an image on a screen with electrical impulses.

-It can primarily help with TV screens and computer screens.

-Disproved Plum-Pudding theory



Robert Andrews Millikan-born in 1868 in Illinois

-grew up in Iowa

-worked on Oil Drop Experiment in University of Chicago (professor)

-1923: Nobel Prize for Physics




At University of Chicago

Performed a series of experiments

Wanted to find the charge of an election

Worked off Thomson’s experiments

At University of Chicago

Performed a series of experiments

Wanted to find the charge of an election

Worked off Thomson’s experiments






The atomizer produces fine oil dropletsOil droplets fall through a hole in the first chamber as a stream of tiny droplets

X-rays negatively charge the oil dropletsAn applied voltage on two plates surrounding the oil drops creates an electric field. The electric force pull some drop upward.

The rate at which the oil droplets are falling and rising between the two charged plates is measured through the microscope.

The atomizer produces fine oil dropletsOil droplets fall through a hole in the first chamber as a stream of tiny droplets

X-rays negatively charge the oil dropletsAn applied voltage on two plates surrounding the oil drops creates an electric field. The electric force pull some drop upward.

The rate at which the oil droplets are falling and rising between the two charged plates is measured through the microscope.

The ExperimentThe Experiment Some oil droplets fell, and some did not This depended on the forces acting upon it: electric

force, gravitational force, and air resistance He found… 1. When a large electric field is applied, but the

electric force on the droplet is larger, then the gravitation force acts in the opposite direction: it moves upward

2. Net force of a droplet=sum of the gravitational force, the air resistance, and electrical force

V1=k(Eq-mq)

Some oil droplets fell, and some did not This depended on the forces acting upon it: electric

force, gravitational force, and air resistance He found… 1. When a large electric field is applied, but the

electric force on the droplet is larger, then the gravitation force acts in the opposite direction: it moves upward

2. Net force of a droplet=sum of the gravitational force, the air resistance, and electrical force

V1=k(Eq-mq)




In simpler terms… When there was no voltage applied, the droplet would fall down to the bottom

Voltage applied, droplets with negative charge drop more slowly, stop altogether, or even go up (depending on the voltage given)

Charges of the droplets were all multiples of the smallest value

e-=1.6 x 10 to the -19 coulombs

In simpler terms… When there was no voltage applied, the droplet would fall down to the bottom

Voltage applied, droplets with negative charge drop more slowly, stop altogether, or even go up (depending on the voltage given)

Charges of the droplets were all multiples of the smallest value

e-=1.6 x 10 to the -19 coulombs

Significance of Experiment


Calculated charge of electron

Showed that charge on electron was smallest possible amount of charge

Total amount of electric charge must always be an integer multiple of this electric charge

Calculated charge of electron

Showed that charge on electron was smallest possible amount of charge

Total amount of electric charge must always be an integer multiple of this electric charge





Now that the charge of an electron is discovered, further advancements in science can be made on the atom

An atom is the basic unit of an element

With the discovery of an electron, we can find out more on the states of substances, elements, etc.

Without him, chemistry would not have advanced much

Now that the charge of an electron is discovered, further advancements in science can be made on the atom

An atom is the basic unit of an element

With the discovery of an electron, we can find out more on the states of substances, elements, etc.

Without him, chemistry would not have advanced much

Earnest RutherfordEarnest Rutherford

As well as Marsden and Geiger and their gold foil

experiment

As well as Marsden and Geiger and their gold foil

experiment



Background InfoBackground Info

Ernest Rutherford, 1st Baron Rutherford of Nelson was a British-New Zealand chemist and physicist. In his early work he discovered the concept of radioactive half and also differentiated and named alpha and beta radiation. He was awarded the Nobel Prize in Chemistry in 1908 "for his investigations into the disintegration of the elements, and the chemistry of radioactive substances”.

Ernest Rutherford, 1st Baron Rutherford of Nelson was a British-New Zealand chemist and physicist. In his early work he discovered the concept of radioactive half and also differentiated and named alpha and beta radiation. He was awarded the Nobel Prize in Chemistry in 1908 "for his investigations into the disintegration of the elements, and the chemistry of radioactive substances”.

Before his Experiment

Before his Experiment

Before his experiment people though that the particles in an atom were randomly arranged according to the plum pudding model. See diagram below.

Before his experiment people though that the particles in an atom were randomly arranged according to the plum pudding model. See diagram below.

HypothesisHypothesis

Rutherford thought that if the plum pudding model was correct then a beam of alpha particles would go though matter with very little deflection. See diagram below.

Rutherford thought that if the plum pudding model was correct then a beam of alpha particles would go though matter with very little deflection. See diagram below.

ExperimentExperimentRutherford’s experiment consisted of a block of radium to generate alpha particles, gold foil for the particles to pass trough and a florescent screen that he could use to determine where the alpha particles ended up. See diagram below.

Rutherford’s experiment consisted of a block of radium to generate alpha particles, gold foil for the particles to pass trough and a florescent screen that he could use to determine where the alpha particles ended up. See diagram below.

ConclusionsConclusions

The Gold Foil experiment showed that the plum pudding model of the atom was not accurate. This is because the experiment showed how there had to be a piece of the atom with a large mass in the center of the atom. The realization that things were not just loosely "hanging out" around an atom but instead are arranged in a specific way around a center led him to discover the Atomic Nucleus. See diagram below

The Gold Foil experiment showed that the plum pudding model of the atom was not accurate. This is because the experiment showed how there had to be a piece of the atom with a large mass in the center of the atom. The realization that things were not just loosely "hanging out" around an atom but instead are arranged in a specific way around a center led him to discover the Atomic Nucleus. See diagram below

More ConclusionsMore Conclusions

Without this discovery, much of what we know about atoms would not be possible. If not for the discovery of the nucleus, we could not know about the important parts that it consists of (protons and neutrons). Also, the periodic table of elements that we all know so well (from intense memorization for Chemistry tests), the elements would not be ordered the same way, because Atomic number is the number of protons in the nucleus of an atom. Also, we can also identify different atoms by mass number. This is the number of protons and neutrons added together in the nucleus. All these things, and many more, that are the basis of our knowledge of atoms would not be possible without the information from Rutherford's Gold Foil Experiment.

Without this discovery, much of what we know about atoms would not be possible. If not for the discovery of the nucleus, we could not know about the important parts that it consists of (protons and neutrons). Also, the periodic table of elements that we all know so well (from intense memorization for Chemistry tests), the elements would not be ordered the same way, because Atomic number is the number of protons in the nucleus of an atom. Also, we can also identify different atoms by mass number. This is the number of protons and neutrons added together in the nucleus. All these things, and many more, that are the basis of our knowledge of atoms would not be possible without the information from Rutherford's Gold Foil Experiment.

James Chadwick Background Info

James Chadwick Background Info

•Chadwick was born in Cheshire, England in 1891.•He went to Manchester University in 1908.•After college, he spent his time studying under Professor Rutherford.•Professor Rutherford created the first artificial nuclear transformation.•This is where he made studies on atomic nuclei.•In 1921, he became Assistant Director of Research of the Cavendish Laboratory.•In 1927, he was elected a Fellow of the Royal Society.

Background Info (con’t) In 1932, he discovered the

existence of neutrons. For this he was awarded the

Hughes Medal of the royal society.

He was later awarded the Nobel Peace Prize in 1935 for physics.

From 1943 to 1946, he worked in the United States on the Manhattan Project for the development of the atomic bomb.

He retired in England in 1948.

He died in 1974.

• http://nobelprize.org/nobel_prizes/physics/laureates/1935/chadwick-bio.html

Neutron Discovery Rutherford discovered the proton in the nucleus

Noticed it was not the only particle in the nucleus Atomic mass could not only be the mass of protons

(e.g. Helium has an atomic mass of 4, but the number of protons is 2

Chadwick went further in trying to discover the neutron, and kept on trying, even as he failed.

Walter Bothe and Herbert Becker did experiments with beryllium where it emitted radiation to penetrate 200 mLs of lead. They thought this was high energy gamma rays, but Chadwick noticed it was something else

Without the clues and inspirations of Rutherford, Bothe, and Becker, Chadwick would not have been able to discover the neutron.

Neutron Discovery (Cont.)

Two other scientists, Federic and Irlene Joliot-Curry, tracked particle radiation by putting paraffin wax in front of the rays (thought to be gamma rays) coming from the beryllium. During this, they observed high-speed protons coming out the paraffin.

Chadwick recognized the rays from the beryllium were not gamma rays because they were too strong. He concluded that they were neutrons. He did his own experiments to back this up.

Since neutrons are neutral, they can penetrate thick layers of different substances because they are not disturbed by positive or negative charges.

Chadwick also discovered that the mass of a neutron is 1.0067

http://www.helium.com/items/216709-james-chadwick-and-his-discovery-of-the-neutron

The Neutron Experiment

Significance By knowing about the

neutron, scientists could use atomic number and atomic mass because they were no longer extremely similar.

Also, knowing about neutrons was important in the creation of nuclear weapons and nuclear reactors.

In addition, the creation of plutonium-235 and uranium-235 is caused by their absorption of neutrons.

Significance (Cont.) At extremely high pressure and temperature, neutrons and

electrons collapse into neutronic matter, known as neutronium.

This is what happens in neutron stars Neutron capture results in neutron activation, which

creates radioactivity Used to excited delayed and prompy gamma rays from

elements in materials Neutron emitters can detect light in the nuclei,

especially hydrogen found in water molecules.

http://en.wikipedia.org/wiki/Neutron

Niels BohrNiels Bohr

Born: Copenhagen, Denmark, in 1885Died: Copenhagen, Denmark, in 1962 of

heart failure

A Doctor of Physics

Born: Copenhagen, Denmark, in 1885Died: Copenhagen, Denmark, in 1962 of

heart failure

A Doctor of Physics

Background Info.Background Info.

Awarded Nobel Prize for his work in the structure of atoms in 1922

Worked under J.J. Thomson in Cambridge, and later with Ernest Rutherford in Manchester University, in the field of physics

Awarded Nobel Prize for his work in the structure of atoms in 1922

Worked under J.J. Thomson in Cambridge, and later with Ernest Rutherford in Manchester University, in the field of physics

The Bohr ModelThe Bohr Model

Developed model of atom in which electrons orbited the nucleus in certain energy levels. Called the Bohr Model.

Conducted the Liquid Drop Experiment.

Developed model of atom in which electrons orbited the nucleus in certain energy levels. Called the Bohr Model.

Conducted the Liquid Drop Experiment.

The Shell ModelThe Shell Model

Developed Shell Model in which the outermost orbit of electrons determined the chemical properties of the element.

Developed Shell Model in which the outermost orbit of electrons determined the chemical properties of the element.

Significance of Bohr and Shell Model

Significance of Bohr and Shell Model

Shell Model is used as a basis for Chemistry, since Chemistry is about the RXNS and interactions between elements/chemicals

The Bohr Model gave a more accurate model of an atom. The fact that electron movement was not applicable in classical mechanics caused the introduction of quantum mechanics into modern science.

Shell Model is used as a basis for Chemistry, since Chemistry is about the RXNS and interactions between elements/chemicals

The Bohr Model gave a more accurate model of an atom. The fact that electron movement was not applicable in classical mechanics caused the introduction of quantum mechanics into modern science.

Contributions, cont.Contributions, cont. Helped develop the Atomic Bomb (part of Manhattan Project/Atomic Energy Project)

Began work in Theoretical Quantum Physics (Old Quantum Physics)

Identified isotope of Uranium responsible for slow-neutron fission

Helped develop the Atomic Bomb (part of Manhattan Project/Atomic Energy Project)

Began work in Theoretical Quantum Physics (Old Quantum Physics)

Identified isotope of Uranium responsible for slow-neutron fission

• http://en.wikipedia.org/wiki/Democritus

•http://www.nndb.com/people/790/000087529/democritus-1-sized.jpg

•http://mrsvesseymathematicians.wikispaces.com/file/view/aristotle_stone.jpg/122672537/aristotle_stone.jpg

•http://en.wikipedia.org/wiki/Aristotle

•http://killashandra.tripod.com/Page2.html

•http://ancienthistory.about.com/od/gm/g/Leucippus.htm

•http://farside.ph.utexas.edu/teaching/sm1/lectures/node5.htmll

•http://www.nndb.com/people/021/000094736/

http://en.wikipedia.org/wiki/Democritus

http://www.nndb.com/people/790/000087529/democritus-1-sized.jpg

http://www.nndb.com/people/790/000087529/democritus-1-sized.jpg

http://mrsvesseymathematicians.wikispaces.com/file/view/aristotle_stone.jpg/122672537/aristotle_stone.jpg



http://en.wikipedia.org/wiki/Aristotle

http://killashandra.tripod.com/Page2.html

http://ancienthistory.about.com/od/gm/g/Leucippus.htm

http://farside.ph.utexas.edu/teaching/sm1/lectures/node5.htmll

http://farside.ph.utexas.edu/teaching/sm1/lectures/node5.htmll

http://www.nndb.com/people/021/000094736/

Works Cited ProustWorks Cited Proust

http://www.britannica.com/EBchecked/topic/480555/Joseph-Louis-Proust

htttp://www.answers.com/topic/joseph-prousthttp://www.amityregion5.org/jlaliberte/adobe/

4DefiniteMultipleProportions.pdf http://web.lemoyne.edu/~giunta/classicalcs/proust.html

http://www.britannica.com/EBchecked/topic/480555/Joseph-Louis-Proust

htttp://www.answers.com/topic/joseph-prousthttp://www.amityregion5.org/jlaliberte/adobe/

4DefiniteMultipleProportions.pdf http://web.lemoyne.edu/~giunta/classicalcs/proust.html

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theory-part-6 http://www.hcc.mnscu.edu/chem/V.07/page_id_7029.html http://swift.tahoma.wednet.edu/tjhs/kmchenry/index.php?

section=links

http://www.iun.edu/~cpanhd/C101webnotes/composition/dalton.html http://www.jstor.org/pss/2103296 http://www.universetoday.com/38193/john-daltons-atomic-theory/ http://en.citizendium.org/wiki/Law_of_multiple_proportions_(chemist

ry http://en.wikipedia.org/wiki/Law_of_multiple_proportions#Law_3:_Law

_of_Multiple_Proportions http://mechanical01.blogspot.com/2008/10/chemical-equation.html http://ritter.tea.state.tx.us/student.assessment/resources/online/

2006/grade10/science/10science.htm http://chemistry.learnhub.com/lesson/3763-history-of-the-atomic-

theory-part-6 http://www.hcc.mnscu.edu/chem/V.07/page_id_7029.html http://swift.tahoma.wednet.edu/tjhs/kmchenry/index.php?

section=links

Ricki Harris and Jodi Lefkowitz

http://www.iun.edu/~cpanhd/C101webnotes/composition/dalton.html

http://www.jstor.org/pss/2103296

http://www.universetoday.com/38193/john-daltons-atomic-theory/

http://en.citizendium.org/wiki/Law_of_multiple_proportions_(chemistry


http://en.wikipedia.org/wiki/Law_of_multiple_proportions#Law_3:_Law_of_Multiple_Proportions


http://www.iun.edu/~cpanhd/C101webnotes/composition/dalton.html

http://www.jstor.org/pss/2103296

http://www.universetoday.com/38193/john-daltons-atomic-theory/





Thomson sourcesThomson sources

-nobleprize.org/noble_prizes/physics/laureates/1906/thomson-bio.html

-Wikipedia

-www.aip.org/history/electron/jjhome.htm

-http://www.experiment-resources.com/cathode-ray.htm

-http://en.wikipedia.org/wiki/J._J._Thomson

-nobleprize.org/noble_prizes/physics/laureates/1906/thomson-bio.html

-Wikipedia

-www.aip.org/history/electron/jjhome.htm

-http://www.experiment-resources.com/cathode-ray.htm

-http://en.wikipedia.org/wiki/J._J._Thomson

CitationsCitations http://www.suite101.com/content/millikan-

oil-drop-experiment-a124624 http://sdsu-physics.org/physics180/

physics180B/Chapters/phys180Bch18.htm http://www.eskom.co.za/nuclear_energy/

fuel/fuel.html http://imglib.lbl.gov/ImgLib/COLLECTIONS/

BERKELEY-LAB/index/pg08_Millikan.html http://www.wired.com/science/discoveries/

news/2008/04/dayintech_0430 http://www.wwnorton.com/college/

chemistry/gilbert2/tutorials/interface.asp?chapter=chapter_02&folder=millikan

http://www.suite101.com/content/millikan-oil-drop-experiment-a124624

http://sdsu-physics.org/physics180/physics180B/Chapters/phys180Bch18.htm

http://www.eskom.co.za/nuclear_energy/fuel/fuel.html

http://imglib.lbl.gov/ImgLib/COLLECTIONS/BERKELEY-LAB/index/pg08_Millikan.html

http://www.wired.com/science/discoveries/news/2008/04/dayintech_0430

http://www.wwnorton.com/college/chemistry/gilbert2/tutorials/interface.asp?chapter=chapter_02&folder=millikan

Work citedWork cited

Wikipedia contributors. "Ernest Rutherford." Wikipedia, The Free Encyclopedia. Wikipedia, The Free Encyclopedia, 11 Sep. 2010. Web. 22 Sep. 2010.

"Ernest Rutherford - Biography". Nobelprize.org. 21 Sep 2010 http://nobelprize.org/nobel_prizes/chemistry/laureates/1908/rutherford-bio.html

http://www.wwnorton.com/college/chemistry/gilbert2/tutorials/interface.asp?chapter=chapter_02&folder=rutherford_experiment

Wikipedia contributors. "Ernest Rutherford." Wikipedia, The Free Encyclopedia. Wikipedia, The Free Encyclopedia, 11 Sep. 2010. Web. 22 Sep. 2010.

"Ernest Rutherford - Biography". Nobelprize.org. 21 Sep 2010 http://nobelprize.org/nobel_prizes/chemistry/laureates/1908/rutherford-bio.html

http://www.wwnorton.com/college/chemistry/gilbert2/tutorials/interface.asp?chapter=chapter_02&folder=rutherford_experiment

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Period 7.. Pre-Socratic philosopher Born in Abdera, Elea, or Miletus in the 5th Century B.C....

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