Group4

Group 4: Mitch, Chloe, Max, Shawnna

(PEREZ) RUTHERFORD MODEL:

===Ernest Rutherford’s model describes that all the positive charges (protons), the neutrons (neutral) and all the atom’s mass is in the middle of the atom, known as the nucleus. The electrons in the atom surround the nucleus, as this picture shows: ===

===﻿The first Rutherford Model was just the nucleus, which contained just the proton and electon surrounding the nucleus. He did not include the nuetron. This picture shows the improved model which was suggested by James Chadwick.===

===In 1911 Rutherford suggested Hans Geiger, and Ernest Marsden to shoot positively charged particles at a thin foil of gold. Every positive particles went through the gold except a few. About 1 in 10000 of the positively charged particles bounced back from the foil. A nucleus is what deflected the the particles. Rutherford explained through his model that this is because all the mass in an atom is concentrated in the center, which is the nucleus. ===

Hans Geiger is one of the scientists who helped Ernest Rutherford with his model. At first they believed that it was just the nucleus, which had the protons in it, and the electrons in an atom. James Chadwick, one of Rutherford’s students, in 1932 suggested to Rutherford that the nucleus doesn’t only have protons, but they also contain neutral particles- neutrons. He says that the mass in a neutron is the same as the mass in a proton in one atom.

===The Rutherford Model was improved by scientist Niels Bohr because Rutherford did not have these shells that surround the nucleus- which is what Bohr discovered. ===

CARBON- RUTHERFORD MODEL:




 * __John Dalton:__ ** discovered that all matter is made up of particles called atoms.

The purpose of the theory is to learn about contribution of particular scientists to the atomic theory  John Dalton is now known as the father of modern atomic theory for all of his efforts. All of matter is made up atoms. Atoms are invisible and are indestructible. All atoms of the same element look identical and have very similar properties. Atoms that are made up of different elements will have different properties. Atoms with different elements are able to combine to create new substances. Atoms of the same element have similar masses and atom with different elements are different in masses.

Evidence supporting Dalton`s theory Dalton had reconsidered the ancient idea that different kind of element is composed of a different atom. All of his experiments and research led him to believe that all atoms were small spheres but each atom could have different properties. How his theory came to be John was a scientific chemists who focused on the behavior of gasses. John used his theory and understanding elements and gases he could determine the weight of atomic elements (meaning his theory is that you can tell different elements apart by there weight). Basic Ideas Johns Model proposed All matter is made up of atoms Atoms are not able to be destroyed All atoms with the same elements are identical Different atoms contain different elements When atoms are rearranged they cause a chemical reaction Dalton's Model was based off of Joseph Louis Proust`s law. His law is that when compounds are analysed into different parts they always contain the same amount of proportions of elements by weight.

References Dalton's atomic theory. (n.d.). Indiana University Northwest. Retrieved September 14, 2011, from [|__http://www.iun.edu/~cpanhd/C101w__] John Dalton's Model. (n.d.). The Peking Man. Retrieved September 16, 2011, from [|__http://northspringer.tripod.com/H__] <span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 14px; text-decoration: none; vertical-align: baseline;">Saskatchewan science 9 (Book, 2011) [WorldCat.org]. (n.d.). WorldCat.org: <span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 14px; text-decoration: none; vertical-align: baseline;">The World's Largest Library Catalog. Retrieved September 16, 2011, from <span style="background-color: transparent; color: #000099; font-family: Arial; font-size: 14px; vertical-align: baseline;">[|__http://www.worldcat.org/title/saskatchewan-science-9/oclc/726939717__] <span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 14px; text-decoration: none; vertical-align: baseline;"> (page 152, 153,156) John Dalton’s Atomic Theory. (n.d.). <span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 14px; text-decoration: none; vertical-align: baseline;">Universe Today — Space and astronomy news. Retrieved September 16, 2011, from <span style="background-color: transparent; color: #000099; font-family: Arial; font-size: 14px; vertical-align: baseline;">[|__http://www.google.com/url?q=http%3A%2F%2Fwww.universetoday.com%2F38193%2Fjohn-daltons-atomic-theory%2F&sa=D&sntz=1&usg=AFQjCNGv-DlPXWBUzWl6zXvU_7Uyr2tUxQ__]

<span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 19px; text-decoration: none; vertical-align: baseline;"> When Thomson discoverd electrons it meant that there were smaller particals making atoms up.This disproved Daltons model was wrong, because the electrons had a negative charge, Thomson knew that there must be something positive in the atom to balance out the electrons. <span style="background-color: transparent; color: #000000; font-family: arial; font-size: 19px; text-decoration: none; vertical-align: baseline;"><span style="font-family: 'Arial','sans-serif'; font-size: 10pt; line-height: 115%;"> <span style="font-family: 'arial','sans-serif'; font-size: 10pt; line-height: 115%; margin: 0in 0in 10pt;">Through his investigation of cathode rays. Thomson discovered that the rays could be deflected by an electric field. Using that he was able to find out the particles mass. This showed the cathode rays were made up of matter, but he found the particles to be 2000 times lighter than the lightest known atom, which is hydrogen. He concluded that the cathode rays were made up of very light negatively charged particles call corpuscles or electrons. <span style="background-color: transparent; color: #000000; font-family: arial; font-size: 19px; line-height: 0px; overflow: hidden; text-decoration: none; vertical-align: baseline;">
 * <span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 19px; vertical-align: baseline;">__J.J Thomson :__ **<span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 19px; text-decoration: none; vertical-align: baseline;">said that the atom is made up of even smaller particles that are scattered through out the atom- protons and electrons.


 * <span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 19px; vertical-align: baseline;">__Ernest Rutherford:__ **<span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 19px; text-decoration: none; vertical-align: baseline;"> discovered that the atom is not scattered protons and electrons, but there is a point in the middle of the atom called the nucleus- which is positively charged with protons and that the electrons surround the nucleus. Later, the neutrons were added to the nucleus by James Chadwick.


 * <span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 19px; vertical-align: baseline;">__Neils Bohr (Chloe):__ **<span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 19px; text-decoration: none; vertical-align: baseline;"> discovered these shells of electrons that surround the nucleus in pairs and in specific energy levels.

Bohr's theory that electrons being found in a particular set of orbits circling the nucleus. Through his research he believed it was key to the periodic table, memorization of the properties of the elements. Several shells, in which the electrons exsist have different quantum numbers and contain different amounts of energy. The first orbit contains NO more than two, the second up to eight. The third, ten. The fourth, fourteen. Atoms with less than the highest amount of numbers in their shells are less stable. Other than the one's with the "correct" amount of energy. Elements that contain the same amount of energy in the outermost shells appear in the exact column in the periodic table of elements.


 * <span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 19px; text-decoration: none; vertical-align: baseline;">All these scientists helped the modern day model become what it is now **

=__REFERENCES__=
 * =<span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 15px; text-decoration: none; vertical-align: baseline;">Google Images. (n.d.). Google. Retrieved September 19, 2011, from <span style="background-color: transparent; color: #000099; font-family: Arial; font-size: 15px; vertical-align: baseline;">__[]__ =
 * <span style="background-color: transparent; color: #000099; font-family: Arial; font-size: 15px; vertical-align: baseline;">__[]__ <span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 15px; text-decoration: none; vertical-align: baseline;">Molecular Expressions: Electricity and Magnetism: Interactive Java Tutorial - The Rutherford Experiment. (n.d.). Molecular Expressions: Images from the Microscope. Retrieve
 * <span style="background-color: transparent; color: #000000; font-family: Arial; font-size: 15px; text-decoration: none; vertical-align: baseline;">Google Images. (n.d.). Google. Retrieved September 19, 2011, from http://www.google.ca/imgres?q=Carbon-+Rutherford+Model&um=1&hl=en&safe=active&rls=com.microsoft:en-us&tbm=isch&tbnid=vuxUSksqlRA1nM:&imgrefurl=http://www.universetoday.comm/56469/atom-diagram/&docid=pLFhEw4LPin0gM

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=Bohr: (Kraus)=

Bohr's theory that electrons found in a particular set of orbits circling the nucleus was key to the periodic table. Memorizing the properties of the elements. The shells in which electrons orbit have several quantum numbers and contain certain numbers of electrons. The first shell holds NO more than two, as for the second up to eight. The third, to ten and the fourth to fourteen. Atoms with less than the "correct" number in their outermost shells are less stable than the ones with the "right" amount.Elements that have the same total of energy in their outermost shells appear in the exact column in the periodic table of elements. References:

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