Hybridisation of the central metal in a given complex (valence bond theory)

1. A.
   $dsp^2$
2. B.
   $sp^3d^2$
3. C.
   $d^2sp^3$
4. D.
   $sp^3$

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1. A.
   $\text{sp}^3$
2. B.
   $\text{dsp}^2$
3. C.
   $\text{d}^2\text{sp}^3$
4. D.
   $\text{sp}^3\text{d}^2$

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1. A.
   $sp^3d^2$
2. B.
   $dsp^2$
3. C.
   $sp^3$
4. D.
   $d^2sp^3$

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1. A.
   $d^2sp^3$
2. B.
   $sp^3d^2$
3. C.
   $sp^3$
4. D.
   $dsp^3$

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1. A.
   ${sp}^{3}$
2. B.
   ${dsp}^{2}$
3. C.
   ${sp}^{3}\text{ }d$
4. D.
   ${sp}^{3}{\text{ }d}^{2}$

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1. A.
   $dsp^3$
2. B.
   $sp^3d^2$
3. C.
   $d^2sp^3$
4. D.
   $sp^3$

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1. A.
   It is $sp^3d^2$ hybridised and tetrahedral.
2. B.
   It is $d^2sp^3$ hybridised and octahedral.
3. C.
   It is $dsp^2$ hybridised and square planar
4. D.
   It is $sp^3d^2$ hybridised and octahedral.

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1. A.
   $sp^3$
2. B.
   $sp^3d^2$
3. C.
   $d^2sp^3$
4. D.
   $dsp^2$

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1. A.
   $d^2sp^3$ and diamagnetic
2. B.
   $d^2sp^3$ and paramagnetic
3. C.
   $sp^3d^2$ and diamagnetic
4. D.
   $sp^3d^2$ and paramagnetic

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1. A.
   $d^2sp^3$
2. B.
   $sp^3d^2$
3. C.
   $dsp^2$
4. D.
   $sp^3$

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