The electronic arrangement of an octahedral complex with a ${\mathrm{d}}^4$ configuration, if ∆₀ < pairing energy is:

1. ${\mathrm{t}}_{2\mathrm{g}}^4{\mathrm{e}}_{\mathrm{g}}^0$                       

2. ${\mathrm{e}}_{\mathrm{g}}^4{\mathrm{t}}_{2\mathrm{g}}^0$               

3. ${\mathrm{t}}_{2\mathrm{g}}^3{\mathrm{e}}_{\mathrm{g}}^1$           

4. ${\mathrm{e}}_{\mathrm{g}}^2{\mathrm{t}}_{2\mathrm{g}}^2$

Which of the following statement is not correct ?

(a) Bis(glycinato)Zinc(II) is optically active

(b) $[{\mathrm{NiCl}}_4{]}^{2- }\mathrm{and} [{\mathrm{PtCl}}_4{]}^{2-}$ have different shape

(c) $\left[\mathrm{Ni}\right(\mathrm{CN}{)}_4{]}^{4-}$ is square planar complex

(d) $\left[\mathrm{Ni}\right(\mathrm{CN}{)}_4{]}^{2- }\mathrm{and} \left[\mathrm{Ni}\right(\mathrm{CO}{)}_4]$ have the same magnetic moment

Give the correct of initial T or F for following statements. Use T is statement is true and F if it is false

(I) Co(III) is stabilised in presence of weak ligands , while Co(II) is stabilised in presence of strong field ligand.

(II) Four coordinated complexes of Pd(II) and Pt(II) are diamagnetic and square planar.

(III) $\left[\mathrm{Ni}\right(\mathrm{CN}{)}_4{]}^{4-}$ ion and $\left[\mathrm{Ni}\right(\mathrm{CO}{)}_4]$ are diamagnetic tetrahedral and square planar.

(IV) ${\mathrm{Ni}}^{2+}$ ion does not form inner orbital octahedral complexes.

(1) TFTF                                   

(2) TTTF

(3) TTFT                                   

(4) FTFT

Match List-I with List-II and select the correct answer using the codes given below :

                      List-I                                              List-II

(I) $[{\mathrm{FeF}}_6{]}^{3-}$                                                   (A) 1.73 BM

(II) $\left[\mathrm{Ti}\right({\mathrm{H}}_2\mathrm{O}{)}_6{]}^{3+}$                                             (B) 5.93 BM

(III) $\left[\mathrm{Cr}\right({\mathrm{NH}}_3{)}_6{]}^{3+}$                                            (C) 0.00 BM

(IV) $\left[\mathrm{Ni}\right({\mathrm{H}}_2\mathrm{O}{)}_6{]}^{2+}$                                             (D) 2.83 BM

(V)  $\left[\mathrm{Fe}\right(\mathrm{CN}{)}_6{]}^{4-}$                                               (E) 3.88 BM

          (I)    (II)   (III)   (IV)   (V)                       (I)    (II)   (III)   (IV)   (V) 

(a)      B      A       C       D      E                  (b)    B      A       E       D      C

(c)       B     C       D       E      A                 (d)     D     E       A       B       C  

Set of d-orbitals which is used by central metal during formation of ${\mathrm{MnO}}_4^{-}$?

(1) ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2 },{\mathrm{d}}_{{\mathrm{z}}^{2 }},{\mathrm{d}}_{\mathrm{xy}}$                   

(2) ${\mathrm{d}}_{\mathrm{xy}} , {\mathrm{d}}_{\mathrm{yz}} , {\mathrm{d}}_{\mathrm{xz}}$

(3) ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2} , {\mathrm{d}}_{\mathrm{xy}} , {\mathrm{d}}_{\mathrm{xz}}$                   

(4) ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2} , {\mathrm{d}}_{z^2} , {\mathrm{d}}_{\mathrm{xz}}$

${\mathrm{FeSO}}_4$ is a very good absorber for NO, the new compound formed by this process is found to contain number of unpaired electrons:

(1) 4         

(2) 5           

(3) 3         

(4) 6

$\mathrm{A}\left[\mathrm{M}\right({\mathrm{H}}_2\mathrm{O}{)}_6{]}^{2+}$ complex typically absorbs at around 600 nm. It is allowed to react with ammonia to form a new complex $\left[\mathrm{M}\right({\mathrm{NH}}_3{)}_6{]}^{2+}$ that should have absorption at :

(1) 800 nm         (2) 580 nm       (3) 620 nm      (4)  320 nm

The CFSE for $\left[\right(\mathrm{Cocl}{)}_6{]}^{4-}$ complex is 18000 ${\mathrm{cm}}^{-1}$. The $∆$ for $\left[\right(\mathrm{Cocl}{)}_4{]}^{2-}$ will be:

(a) 18000 ${\mathrm{cm}}^{-1}$                    (b) 16000 ${\mathrm{cm}}^{-1}$

(c) 8000 ${\mathrm{cm}}^{-1}$                       (d) 2000 ${\mathrm{cm}}^{-1}$

Which of the following order of CFSE is incorrect?

$\left(\mathrm{a}\right) \left[\mathrm{Co}\right(\mathrm{en}{)}_3{]}^{3+ }>\left[\mathrm{Co}\right({\mathrm{NH}}_3{)}_6{]}^{3+}>\left[\mathrm{Co}\right({\mathrm{H}}_2\mathrm{O}{)}_6{]}^{3+}$

(b) $[{\mathrm{PtCl}}_4{]}^{2-}>[{\mathrm{PdCl}}_4{]}^{2-}>[{\mathrm{NiCl}}_4{]}^{2-}$

(c) $\left[\mathrm{Ni}\right(\mathrm{dmgH}{)}_2]<[\mathrm{Ni}(\mathrm{en}{)}_2{]}^{2+}$

(d) $\left[\mathrm{Co}\right(\mathrm{ox}{)}_3{]}^{3-}<\left[\mathrm{Co}\right(\mathrm{en}{)}_3{]}^{3+}$

For which of the following ${\mathrm{d}}^{\mathrm{n}}$ configuration of octahedral complexes, can not exist in both high spin and slow spin forms:

(I) ${\mathrm{d}}^3$                  (II) ${\mathrm{d}}^5$               (III) ${\mathrm{d}}^6$             (IV) ${\mathrm{d}}^8$

(1) I,II and III                                 

(2) II,III & IV

(3) I & IV                                         

(4) None of these