L38_TransMetals5

L38_TransMetals5 - Colors of coordination complexes Crystal field theory Crystal field theory magnetic properties and colors of coordination

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Unformatted text preview: Colors of coordination complexes: Crystal field theory Crystal field theory: magnetic properties and colors of coordination compounds Octahedral field splittings of d-orbitals: D o d z2 d x2-y2 (e g ) d zy d yz d xz (t 2g ) Filling in electrons: Aufbau principle and Hund’s rule Strength of splitting ( D o or D t ): Spectrochemical series CN- > NO 2- > en > NH 3 > H 2 O > OH- > F- > Cl- > Br- > I- Also, charge on the metal, e.g., splitting in Fe 3+ > Fe 2+ Which is the most accurate explanation for the fact that an octahedral complex ion containing Ti 3+ is always paramagnetic, but an octahedral complex ion containing Fe 2+ could end up being either paramagnetic or diamagnetic? 1 . T i 3 + . . . 2 . T i 3 + i o . . 3 . T i 3 + i o . . 4 . T i 3 + i o . . 11% 39% 42% 8% 1. Ti 3+ ions only bond to ligands that cause paramagnetism, while Fe 2+ ions are capable of bonding to ligands that can cause both paramagnetic and diamagnetic characteristics. 2. Ti 3+ ions always correspond to weak field bonding....
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This note was uploaded on 07/22/2008 for the course CHEM 115b taught by Professor Reisler during the Spring '08 term at USC.

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L38_TransMetals5 - Colors of coordination complexes Crystal field theory Crystal field theory magnetic properties and colors of coordination

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