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a) Almost every transition metal can exist as a cation with a 2+ charge. b) Square planar transition metal complexes do not follow the VSEPR model. c) The ligand field splitting energy for a tetrahedral complex is smaller than the ligand field splitting energy for an octahedral complex. d) Fe2* (aq) is light green and Zn²+ (aq) is colorless. e) Co(NH3)6* (aq) is yellow and Co(H2O)6³* (aq) is pale pink.

a) Almost every transition metal can exist as a cation with a 2+ charge. b) Square planar transition metal complexes do not follow the VSEPR model. c) The ligand field splitting energy for a tetrahedral complex is smaller than the ligand field splitting energy for an octahedral complex. d) Fe2* (aq) is light green and Zn²+ (aq) is colorless. e) Co(NH3)6* (aq) is yellow and Co(H2O)6³* (aq) is pale pink.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Explain why each statement is true. a) Almost every transition metal can exist as a cation with a 2+ charge. b) Square planar transition metal complexes do not follow the VSEPR model. c) The ligand field splitting energy for a tetrahedral complex is smaller than the ligand field splitting energy for an octahedral complex. d) Fe2* (aq) is light green and Zn²* (aq) is colorless. e) Co(NH3),* (aq) is yellow and Co(H2O)6³* (aq) is pale pink.
Transcribed Image Text:Explain why each statement is true. a) Almost every transition metal can exist as a cation with a 2+ charge. b) Square planar transition metal complexes do not follow the VSEPR model. c) The ligand field splitting energy for a tetrahedral complex is smaller than the ligand field splitting energy for an octahedral complex. d) Fe2* (aq) is light green and Zn²* (aq) is colorless. e) Co(NH3),* (aq) is yellow and Co(H2O)6³* (aq) is pale pink.
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