period 7.. pre-socratic philosopher born in abdera, elea, or miletus in the 5th century b.c....
TRANSCRIPT
•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.
QuickTime™ and a decompressor
are needed to see this picture.
• 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
QuickTime™ and a decompressor
are needed to see this picture.
• 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
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
Significance of Concept
Significance of Concept
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.biographybase.com/biography/Lavoisier_Antoine_Laurent.html
Joseph Proust: Law of Definite ProportionsJoseph Proust: Law of Definite Proportions
By: Simir and KatieBy: Simir and Katie
QuickTime™ and a decompressor
are needed to see this picture.
-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,
QuickTime™ and a decompressor
are needed to see this picture.
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
QuickTime™ and a decompressor
are needed to see this picture.
QuickTime™ and a decompressor
are needed to see this picture.
QuickTime™ and a decompressor
are needed to see this picture.
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
QuickTime™ and a decompressor
are needed to see this picture.
QuickTime™ and a decompressor
are needed to see this picture.
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
QuickTime™ and a decompressor
are needed to see this picture.
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
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
Dalton’s Law of Multiple Proportions
Dalton’s Law of Multiple Proportions
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
QuickTime™ and a decompressor
are needed to see this picture.
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
QuickTime™ and a decompressor
are needed to see this picture.
The DiscoveryThe Discovery
-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
QuickTime™ and a decompressor
are needed to see this picture.
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.
QuickTime™ and a decompressor
are needed to see this picture.
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
QuickTime™ and a decompressor
are needed to see this picture.
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
QuickTime™ and a decompressor
are needed to see this picture.
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
QuickTime™ and a decompressor
are needed to see this picture.
The DiscoveryThe Discovery
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
QuickTime™ and a decompressor
are needed to see this picture.
The ExperimentThe Experiment
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)
QuickTime™ and a decompressor
are needed to see this picture.
The ExperimentThe Experiment
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
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
QuickTime™ and a decompressor
are needed to see this picture.
Significance of Experiment
Significance of Experiment
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
QuickTime™ and a decompressor
are needed to see this picture.
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
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/
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
Sources Sources 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
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
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