userdata-paziras-Chem101-Chap_09A

Groupvathroughgroupviia chargeofaniongroupnumber 8

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Unformatted text preview: harge of Cation = Group Number Ø Atoms lose all their valence electrons (“s” and “p” electrons) Ø Electronic Configuration o f cations = Preceding Noble Gas electronic Configurat ion 2. Group IIIA through Group VA Ø Charge of Cation = Group Number – 2 Atoms lose only their “p” valence electrons ( “s” electrons are kept) 2 Electronic Configuration of cations = Preceding Pseudo Noble Configuration + ns Sn – 2e 2 10 2 [Kr] 5s 4d 5p Sb – 3e 3 [Kr] 5s2 4d 0 5p 1 2 Sn + [Kr] 5s2 4d 0 1 3 Sb + [Kr] 5s2 4d 0 1 2 Similarly: Pb + 3 Similarly: Bi + 3. Group VA through Group VIIA Ø Charge of Anion = Group Number ­ 8 Atoms gain electrons to achieve stable octet (or doublet in the case o f H) Electronic Configuration o f anio ns = Noble Gas electronic Configurat ion fo llowing the element. 10 Chemistry 101 Chapter 9 CATIONS OF TRANSITION METALS · These io ns are very often co lored Loss of electrons Ionic Charge Examples 2+ 2 2 Zn + Cd + In some cases in addition to the “s” electrons, some “d” electrons from an inner shell (n­1) may be lost. + 2 and/or larger + than 2 2 3 Fe + Fe + Unusual charges are due to irregular electronic configurations associated with the stability of half­filled or filled subshells + 2 + and/or 1 2 + Cu + Cu + Ag The “ns” electrons are lost first (most common) 2+ Fe -¯ - [Ar] 4s - - - . - - . 3d 0 Fe [Ar] -¯ -¯ 4s Cu 2+ [Ar] 4s0 3d 9...
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This document was uploaded on 03/18/2014 for the course CHEM 101 at Los Angeles Mission College.

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