CHEM 111A Chapter Notes - Chapter 8: Potential Energy, Covalent Radius, Pauli Exclusion Principle
4 May 2017
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Orbital blocks: groups 1 and 2: s block, groups 3a 8a: p block, transition metals: d block, lanthanides and actinides: f block, use the periodic table to determine orbitals of elements (6) Electron configuration of ions: when writing configurations for a cation: remove the electrons from the highest energy level. Isoelectronic: same e configuration: when writing configurations for anions: add electrons. P3 : [ne]3s23p6 [ar] (cl and p3 are isoelectronic to each other) Z is atomic number (number of protons), s is shielding electrons. Penetration: as the outer electron undergoes penetration into the region occupied by inner electrons, it experienced a greater zeff. So the energy becomes more negative (more stable) (13) So noble gases are not reactive: the elements with configuration closes to noble gases are most reactive. The more attractive a proton (aka the bigger the number of protons), the smaller the element/ion: ca2+, ar, cl (16) Ie1 has a different trend than ie2 or ie3.
