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Chem 101
Exam 2
| Term | Definition |
|---|---|
| Atomic Size | Distance from the nucleus of an atom to the outermost e Increases down a group due to the addition of electron shells. It tends to decrease across a period from left to right because the increasing nuclear charge pulls the electrons closer to the nucleus. |
| Ionization Energy | The amount of energy required to remove the outermost e from a neutral atom in the gas phase. Increases across a period due to increased Zeff, which makes it harder to remove an e. Decreases down a group outer e are farther from the nucleus, more shield |
| Electron Affinity | Energy change that occurs when an electron is added to a neutral atom in the gas phase. Pos. EA value indicates that energy is released when an e is added, while a neg. val. indicates that energy is required. |
| Effective Nuclear Charge | Pull exerted on a specific electron by the nucleus. Increases across a period due to increased nuclear charge without significant additional shielding, leading to stronger attraction between the nucleus and the outer electrons. |
| Octet Rule | How atoms tend to bond in order to achieve a stable electron configuration, typically resembling that of the noble gases, which have full outer electron shells. |
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