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10 Cards in this Set
- Front
- Back
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N = ? |
Principal number and Orbital energy(size) (1, 2, 3, ...) |
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l = ? |
Orbital shape (0 to n-1). Also corresponds to s, p, d, and f orbitals respectively. |
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Mi = ? |
Orbital orientation (-l to 0 to +l) |
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Ms=? |
Spin (+1/2 or -1/2) |
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Exclusion principle |
No two electrons in the same atom can have the same four quantum numbers. |
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Shielding |
Reduces the full nuclear charge to an effective nuclear charge, the nuclear charge an electron actually experiences, and this lower nuclear charge makes the electron easier to remove. |
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Effects of penetration |
It increases the nuclear attraction for a 2s electron over that of for a 2p electron. It decreases the shielding of a 2s electron by the 1s electron. |
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Electron configuration vs orbital diagram. |
Electron configuration involves n, l, ml, ms. Orbital diagram involves boxes with arrows drawn in. |
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Special rule for 3d orbitals. |
Best examples are chromium and copper, though this applies to other elements too. |
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Valence electrons |
For main-group elements, the valence electrons are the outer electrons. For transition elements, in addition to the outer ns electron, the (n-1)d electrons are also valence electrons. |
