A) \[s{{p}^{3}}{{d}^{2}},4.89\,BM\]
B) \[{{d}^{2}}s{{p}^{3}},4.89\,BM\]
C) \[ds{{p}^{2}},5.89\,BM\]
D) \[s{{p}^{3}}{{d}^{2}},3.39\,BM\]
Correct Answer: A
Solution :
\[Cr\]is in \[+2\] oxidation state in\[[Cr{{({{H}_{2}}O)}_{6}}C{{l}_{2}}\]. The electronic configuration of |
\[C{{r}^{2+}}\] is \[3{{d}^{4}}4{{s}^{0}}\] |
As \[{{H}_{2}}O\]is a weak field ligand, so pairing will not occur. |
Thus, the hybridisation of \[{{\left[ Cr\left( {{H}_{2}}O \right)6 \right]}^{2+}}\] \[s{{p}^{3}}{{d}^{2}}\] |
Magnetic moment \[=\sqrt{n\left( n+2 \right)}\] |
For this complex, \[n=4\] |
\[\mu =\sqrt{4\left( 4+2 \right)}\] |
\[=\sqrt{24}\] |
\[=4.89BM\] |
You need to login to perform this action.
You will be redirected in
3 sec