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**The Quantum Mechanical Model**

Energy is quantized. It comes in chunks. A quanta is the amount of energy needed to move from one energy level to another. Since the energy of an atom is never “in between” there must be a quantum leap in energy. Erwin Schrodinger derived an equation that described the energy and position of the electrons in an atom

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**The Quantum Mechanical Model**

The quantum mechanical model is a mathematical solution It is not like anything you can see.

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**The Quantum Mechanical Model**

Has energy levels for electrons. Orbits are not circular. It can only tell us the probability of finding an electron a certain distance from the nucleus.

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**QM model - Modern View The atom is mostly empty space Two regions**

1. Nucleus- protons and neutrons 2. Electron cloud- region where you might find an electron

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Other particles Proton - positively charged pieces 1840 times heavier than the electron – by E. Goldstein Neutron - no charge but the same mass as a proton – by J. Chadwick

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**Subatomic particles Relative mass Actual mass (g) Name Symbol Charge**

Electron e- -1 1 9.11 x 10-28 Proton p+ +1 1840 1.67 x 10-24 Neutron n0 1840 1.67 x 10-24

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**Size of an atom Nucleus tiny compared to atom**

If the atom was the size of a football stadium, the nucleus would be the size of a marble.

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