Electrons

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Unformatted text preview: s Group 4A Atomic number = 6 1s2 2s2 2p2 ---> 2s 2p 6 total electrons total Here we see for the first time Here HUND’S RULE. When When HUND’S placing electrons in a set of orbitals having the same energy, we place them singly as long as possible. as Lanthanide Element Lanthanide Configurations Configurations 65 4f orbitals used for Ce 4f orbitals used for Ce - Lu and 5f for Th - Lr - Lu and 5f for Th - Lr 66 Draw these orbital diagrams! • Oxygen (O) • Chromium (Cr) • Mercury (Hg) Ion Configurations Ion Configurations 67 To form anions from elements, add 1 or more To e- from the highest sublevel. eP [Ne] 3s2 3p3 + 3e- ---> P3- [Ne] 3s2 3p6 or [Ar] 3p 3p 3s 3s 2p 2p 2s 2s 1s 1s General Periodic Trends • Atomic and ionic size • Ionization energy • Electronegativity Higher effective nuclear charge Electrons held more tightly Larger orbitals. Electrons held less tightly. 68 69 Atomic Size Atomic Size •• Size goes UP on going down a group. Size goes UP on going down a group. •• Because electrons a...
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This note was uploaded on 05/14/2013 for the course CHEM AP CHEM taught by Professor Dvg during the Fall '12 term at Wellesley Sr High.

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