CHEM 1A Lecture Notes - Lecture 16: Electron Configuration, Nonmetal, Ion

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Parent atoms: + charge of nucleus = # of e- in orbitals. E- in valence shell removed stable electron configuration of noble gasses strongly attracted to nucleus reduction in cation size. Remove 1+ e- from metal atoms reduce electron-electron repulsions e- cloud smaller. Isoelectronic- ions with same # of e- and e- configuration. Atomic radii of parent atoms across period. Electrons less attracted to nucleus e- cloud expand increase in size of. Adding 1+ electrons to nonmetal atom electron-electron repulsions e- anion cloud larger. Across period: anion is bigger than cations. Size when moving down column http://scientifictutor. org/569/chem-college-ionic-radius/ https://www. quora. com/why-are-the-cations-always-smaller-than-the-corresponding-atoms. Ionization energy- amount of energy to remove electrons. Requires energy because e- is attracted to nucleus (+ charge) need to have enough energy to overcome attraction. Magnitude of ionization energy = how strong e- is bound to nucleus. Greater ionization energy = more difficult to remove electron. Noble gases have highest ionization energy b/c they want their shells to remain complete.

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