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प्रश्न
An aqueous pink solution of cobalt (II) chloride changes to deep blue on addition of excess of HCl. This is because:
(i) \[\ce{[Co(H2O)6]^{2+}}\] is transformed into \[\ce{[CoCl6]}^{4-}\]
(ii) \[\ce{[Co(H2O)6]^{2+}}\] is transformed into \[\ce{[CoCl4]}^{2-}\]
(iii) tetrahedral complexes have smaller crystal field splitting than octahedral complexes.
(iv) tetrahedral complexes have larger crystal field splitting than octahedral complex.
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उत्तर
(ii) \[\ce{[Co(H2O)6]^{2+}}\] is transformed into \[\ce{[CoCl4]}^{2-}\]
(iii) tetrahedral complexes have smaller crystal field splitting than octahedral complexes.
Explanation:
Aqueous pink solution of cobalt (II) chloride is due to electronic transition of electron from t2g to eg energy level of \[\ce{[Co(H2O)6]^{2+}}\] complex. When excess of HCl is added to this solution
(i) \[\ce{[Co(H2O)6]^{2+}}\] is transformed into \[\ce{[CoCl4]^{2-}}\].
(ii) Tetrahedral complexes have smaller crystal field splitting than octahedral complexes because Δr = `4/9` Δ0
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| A. \[\ce{[Cr(H2O)6]^{3+}}\] | 1. dsp2, 1 |
| B. \[\ce{[Co(CN)4]^{2-}}\] | 2. sp3d2, 5 |
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Choose the correct answer from the options given below:
