By: Caleb VanderWal. Began to look for a description of matter more 2400 thousand years ago. His Theory Matter could not be divided into smaller and smaller.

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Presentation transcript:

By: Caleb VanderWal

Began to look for a description of matter more 2400 thousand years ago. His Theory Matter could not be divided into smaller and smaller pieces forever, eventually the smallest possible piece would be obtained. Democritus thought that atoms were small, hard particles that were all made of the same material but were different shapes and sizes. Atoms were infinite in number, always moving and capable of joining together.

Dalton was so smart that he became a school teacher at the age of 12. His theory was based on his experimental observations. His theory All matter is made of atoms. Atoms are indivisible and indestructible. All atoms of a given element are identical in mass and properties. Compounds are formed by a combination of two or more different kinds of atoms. A chemical reaction is a rearrangement of atoms. Atoms can be neither created nor destroyed.

Thomson discovered electrons. His theory: An atom consists of a sphere of positive charge with negatively charged electron embedded in it. The positive and the negative charges in an atom are equal in magnitude, due to which an atom is electrically neutral. It has no over all negative or positive charge.

100 years ago, on March 7, 1911, Ernest Rutherford presented a paper to the Manchester Literary and Philosophical Society accurately describing the structure of the atom. Based on an experiment he had performed he realized that the atom must have almost all of its mass concentrated at its center, in a nucleus, with the vast majority of the atom consisting chiefly of empty space. Two years earlier, in 1909, he had conducted an experiment with two other scientists, in which they studied the deflection angles of "alpha particles" that they shot through a microscopically thin layer of gold. Alpha particles are just helium atoms stripped of their 2 electrons. He showed that while the nucleus contains virtually all of the mass of the atom, it only takes up one-billionth of the volume of the atom, an inconceivably tiny amount. Much smaller particles orbit the nucleus at a great distance, relatively speaking.

Neils Bohr refined Rutherford's model in 1913 by proposing that electrons: orbit the nucleus without losing energy; could move only in fixed orbits of specific energies. Electrons with low energy would orbit closer to the nucleus while electrons with high energy orbit further from the nucleus.

Schrodinger came up with a set of equations or wave functions in 1926 for electrons. According to Schrodinger, electrons confined in their orbits would set up standing waves and you could describe only the probability of where an electron could be.

Heisenberg's theory was “To view an electron in its orbit, you must shine a wavelength of light on it that is smaller than the electron's wavelength. This small wavelength of light has a high energy. The electron will absorb that energy. The absorbed energy will change the electron's position.”

In 1932 Chadwick identified the neutron. With the discovery of the neutron three subatomic particles were identified that would help explain observations made at the atomic level. One observation was the existence of radioactive variances of the same element.

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