Solutions for [Co(NH3)6]2+, [Co(H2O)6]2+, and [COC14]2-. The solutions present as pink, yellow, and blue. Which solution is which color? Explain your reasoning
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![Solutions for [Co(NH3)6]2+, [Co(H2O)6]2+, and [COC14]2-. The solutions present as pink,
yellow, and blue. Which solution is which color? Explain your reasoning](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7537e5cb-7da0-4f3a-91d1-6480122a4c34%2F3072954d-1003-4d3e-9868-5fe6df9378d9%2Fwkew8co_processed.jpeg&w=3840&q=75)
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- Solutions of [Co(NH3)6]2+, [Co(H2O)6]2+ (both octahedral) and [CoCl4]2– (tetrahedral) are colorful. One is pink, one is blue and the other is Based on the spectrochemical series, assign a color for each complex.explain why [CoBr4]^-2 is green while [Co(NH3)6]^2+ is orangeSolutions of [Co(NH3)6]2+, [Co(H2O)6]2+ (both octahedral), and [CoCl4]2- (tetrahedral) are colored. One is pink, one is blue, and one is yellow. Based on the spectrochemical series and remembering that the energy splitting in tetrahedral complexes is normally much less than that in octahedral ones, assign a color to each complex.
- [Co(H2O)6]2+ (aq) + 4 Cl-(aq )⇆ [CoCl4]2-(aq) + 6 H2O 3. Does the value of the equilibrium constant (K) for this reaction increase, decrease, or remain the same as the concentration of chloride increases? Explain your answer incorporating the definition of an equilibrium constant.[Co(H2O)6]3+ has how many unpaired electrons? the answer was 4 but I don't know how I get to the answer.Would you expect [Co(CN)6] 3- to be a powerful or weak oxidizing agent? Explain.
- When water ligands in [Ti(H2O)6]3+ are replaced by CN- ligands to give [Ti(CN)6]3-, the maximum absorption shifts from 500 nm to 450 nm. Is this shift in the expected direction? Explain.Explain why [FeF6]³- is colorless whereas [COF6]- is colored but exhibits only a single band in the visible.[CoF6]3- absorbs 700 nm (red) radiation whereas [Co(H2O)6]3+ absorbs 600 nm (orange) radiation. Please draw the crystal field splitting of the above two complexes. Clearly label the orbitals and show the electron occupation.