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Chemistry Webquest

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on 21 October 2014

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Transcript of Chemistry Webquest

Chemistry Web-quest!
Niels Bohr
H.G.J Moseley
John Dalton
Marcel Proust
JJ Thomson
James Chadwick
Dmitri Mendeleev
Antonie Lavoiser
Gold Foil Experiment
Bohr Model
Rutherford Model
Law of definite proportions
Dalton's Atomic Theory
Law of conservation and mass
Plum pudding Atomic Model
Quantum Mechanical Model
Cathode Ray Tube Experiment
Antonie Lavoisier
In 1789 he proved the Law of Conservation Mass
Law of Conservation of Mass
Mass is neither created or destroyed in any ordinary reaction
In the greek era believed:

1) Atoms are indestructible
2) Atoms are solid but invisible
3) Atoms are homogeneous
4) Atoms differ in size, shape, mass, position, and arrangement
In 1922, Bohr developed an explanation of atomic structure that underlines regularities of periodic table of elements. His atomic model had atoms built up of sucessive orbital shells of electrons
Neils Bohr
In 1914 using x-ray tubes, determined the change on the nuclei of most atoms. "The atomic of an element is equal to the number of protons in the nucleus" This was used to reorganize the periodic table based upon the atomic number instead o the atomic mass.
H.G.J Moseley
Rutherford contributed in two ways. In 1898 he studied the radiations emitted from uranium. In 1911 using particles as a atomic bullet, probed the atom in a piece of thin gold foil.
In 1803 Dalton proposed a atomic theory with spherical solid atoms based upon measurable properties of mass.
John Dalton
In 1932 using alpha particles he discovered a neutral atomic particle with a mass close to a proton. Thus was discovered the "Neutron"
James Chadwick
In 1869 Medeleev, arranged elements into 7 groups with similar properties
He discovered the properties of elements were periodic functions of their atomic weight this became known as the periodic law
Dmitri Medeleev
In 1898 she studied Uranium and Thorium and called their spontaneous decay process" Radioactivity"
She and her husband Pierre also discovered the radioactive elements Polonium and Radium
Marie Curie
Discovered in 1911
An Atom was much more than empty space & scattered electrons an atom must have a positively charged center that contains most of the atoms.
Gold Foil Experiment
Discovered in 1931
Theory proposing that electrons travel in only certain successively larger orbits.
Bohr Model
Discovered in 1911
The atom is 99.9% empty space
Nucleus is 100,000 times smaller than the atom
Rutherford Model
A compound is composed of exact proportions of elements by mass regardless of how the compound was created.
Law of Definite Proportion
The "Plum Pudding Atomic Model" discovered in 1904 that atoms are made of pieces with positive and negative charge and that the negatively charged electrons within the atom were very small compared to the entire atom
Plum Pudding Atomic Model
In 1794 Proust came up with the "Law of Definite Proportions"
In 1930 he viewed electrons as continuous clouds and introduced "wave mechanics" as a mathematical model of the atom
Erwin Schrodinger
Created by Erwin Schrodinger the "Quantum Mechanical Model" introduced the concept of sub-energy levels and also predicts the odds of the location of the electron portrayed as nucleus surrounded by an electron cloud
Quantum Mechanical Model
1) All matter is made of atoms. Atoms are indivisible and indestructible
2) All atoms of a given element are identical in mass and properties
3) Compounds are formed by a combination of 2 or more of different kind of atoms
4) A chemical reaction is a rearrangement of atoms
Dalton's Atomic Theory
Discovered in 1859 the "Cathode Ray Tube Experiment" indicated that the stream crossing the vacuum was composed of particles rather than rays
Cathode Ray Tube Experiment
In 1909 the "Oil Drop Experiment" determined the size of the charge and the mass of an electron
Millikan Oil Drop Experiment
In 1897 he used CRT to experimentally determine the charge to ratio of an electron also studied "Canal Rays" and found they were associated with the proton H+
J.J. Thomson
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