Exam – Chemistry – Flashcards
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Pauli exclusion principle |
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two electrons per orbital |
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Aufbau |
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electrons occupy the lowest level or energy |
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Hund’s Rule |
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- electrons occupy equal energy orbital’s so that a minimum number of unpaired electrons |
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Newlands |
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based his table on music |
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Mendeleev |
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arranged the table by atomic mass |
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Bohr |
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proposed the existence of energy levels |
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Rutherford |
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couldn’t explain the chemical properties of elements |
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Dobenreiner |
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arranged elements into triads |
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Ground |
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1s^2 2s^2 2p^6 3s^2 |
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Excited- |
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1s^2 2s^2 3s^1 3p^1 |
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Impossible |
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1s^2 2s^3 2p^6 3s^1 |
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In the forth quantum there are four sublevels called |
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S,P,D,F |
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The lowest sublevel that can be found within an electron is called |
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the s sublevel |
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The maximum number of electrons that can go into the f sublevel is |
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14 |
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The quantum number |
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= the number of sublevels |
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Quantum mechanical model |
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determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus |
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Atomic orbital |
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often thought of as a region of space in which there is a high probability of finding an electron |
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Quantum |
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the amount of energy required needed to move an electron from one energy level to another |
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Energy levels |
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fixed energies that an electron can have |
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Atomic mass
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weighted average mass of the atomic atoms in a naturally occurring sample or element |
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Isotopes |
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atoms that have the same number of protons but different number of neutrons also have different saggy assed mass numbers |
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# of neutrons |
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mass # – atomic # |