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18 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Periodic table according to valences |
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Energy level |
Specific amount of energy an electron in an atom can posses -different electrons, depending on their energies, are found in certain areas |
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Orbital |
Region of space occupied by an electron in a particular energy level |
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S- orbitals |
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P- orbitals |
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D-orbitals |
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F-orbitals |
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s, p, d, f refer to |
The 4 different types of orbitals |
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Shell |
Set of all orbitals having the same n-value |
3rd consists of 3s, 3p and 3d orbitals |
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Subshell |
Set of orbitals of the same type |
2nd shell: 1 orbital of the 2s subshell 3 orbitals of the 2p subshell |
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Name the 3 rules electrons have to follow for electron configuration |
1. Aufbau principle 2. Hund's rule 3. Pauli exclusion principle |
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Aufbau principle |
Electrons added to the lowest energy level possible |
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Hund's rule |
Electrons will occupy orbitals of each subshell singly before filling orbitals in pairs. |
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Pauli exclusion principle |
A maximum of 2 electrons can be placed in each orbital and must spin in opposite directions. directions. . |
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Order of orbitals for polyelectronic atoms |
1s, 2s, 2p, 3s, 3p, 4s, (3d), 4p, 5s, (4d), 5p, 6s, (4f), (5d) |
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Valence electrons |
Are the electrons outside the core taking part in reactions. |
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Exceptions to e configuration up to strontium |
1. Chromium: (Ar) 4s1 3d5 2. Copper: (Ar) 4s1 3d10 |
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Why are there exceptions (what is the cause)? |
A filled or 1/2 (so 5e) filled d-subshell is especially stable. |
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