CHEM-UA 109 Lecture Notes - Lecture 3: Ionic Compound, Roman Numerals, Lewis Structure
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23 Aug 2016
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Added electrons go to inner d orbitals, increasing the screening effect. Size of atoms vary depending on the electron screening effect. Ionization energy (ie): energy required to remove an electron from a gaseous atom. Ie increases down a row, decreases down a group. It requires more energy to remove a successive electron. When all valance electrons have been removed, the ionization energy takes a quantum leap. Cations are smaller than the original atom zeff increases and n stays the same. The energy change associated with the addition of an electron to a gaseous atom isolated. Must be gaseous because it has a lot of energy, changing its matter. The larger the amount of energy release, the higher the electron affinity. The higher the negative value, the more stable the ion. Noble gases have positive electron affinity because they do not form ions. Electron affinities decrease down a group and increase across a period (many.
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