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CuSO_4 (aq.)$\stackrel{{\mathrm{H}}_2\mathrm{S}\uparrow }{\to }$M$\downarrow$$\underset{\mathrm{of}<mspace\; width="1em"></mspace>\mathrm{KCN}}{\overset{\mathrm{Excess}}{\to }}$N+O
Then final products N and O are respectively.
1. [Cu(CN)₄]^3-,(CN)₂
2. CuCn,(CN)₂
3. [Cu(CN)₄]^2-,(CN)₂
4. Cu(CN)₂,K₂S

At pH = X, \(\text{CrO}_4^{2-}\)​ (yellow) changes to \(\text{Cr}_2\text{O}_7^{2-}\) (orange), and vice versa at pH = Y.
What are the values of X and Y, respectively?
1. 6, and 8
2. 6, and 5
3. 8, and 6
4. 7, and 7

When steam is passed over red hot iron , the substances formed are:
1. Fe₂O₃ +H₂
2. Fe₃O₄ +H₂
3. FeO +H₂
4. FeO+ H₂ +O₂

Which of the following solid salt on heating with K₂Cr₂O₇ and Conc. H₂SO₄ orange,red vapours are evolved which turn aquous NaOH solution yellow?
1. NaBr
2. NaCl
3. NaNO₃
4. NaI

Consider the following transformation:
2CuX₂$\stackrel{\mathrm{room}<mspace\; width="1em"></mspace>\mathrm{temperature}}{\to }$2CuX+X₂$\uparrow$
Then X^- can be :
1. F^-,Br^-
2. Cl^-,Br^-
3. CN^-
4. Cl^-,F^-

The iron salt used in blue prints is:
1. FeC₂O₄
2. Fe₂(C₂O₄)₃
3. K₄Fe(CN)₆
4. FeSO₄

Which element among the following has the highest melting point?
1. Cr
2. Fe
3. Cu
4. Mo

The colour of KMnO₄ is due to  :
1. d-d transition
2. Charge transfer spectra
3. Polarisation of ion
4. p-d transition

Which of the following element does not show the variable oxidation state?
1. Fe
2. Mn
3. Cu
4. Zn

With F highest stable oxidation state of Mn is
1. +6
2. +4
3. +7
4. +3

Cr₂O₇^2-+X$\stackrel{{\mathrm{H}}^{+}}{\to }$Cr³⁺+H₂O + oxidized product of X. X in the above reaction cannot be
1. C₂O₄^2-
2. Fe²⁺
3. SO₄^2-
4. S^2-

A pair of ions having similar magnetic moments is:
1. Ti³⁺,V³⁺
2. Cr³⁺,Mn²⁺
3. Mn²⁺,Fe³⁺
4. Fe²⁺,Mn²⁺

The main reason for a larger number of oxidation states exhibited by the actinoids than the corresponding lanthanoids is
1. The lesser energy difference between 5f and 6d orbitals than 4f and 5d orbitals
2. Larger atomic size of actinoids than the lanthanoids
3. More energy difference between 5f and 6d orbitals than between 4f and 5d orbitals
4. Greater reactive nature of the actinoids than the lanthanoids

In the dichromate ion Cr₂O₇^2-,
1. 4 Cr-O bonds are equivalent
2. 6 Cr-O bonds are equivalent
3. All Cr-O bonds are equivalent
4. None of Cr-O bonds are equivalent
 

The electronic configuration of a transition element X in +3 Oxidation state is [Ar]3d⁵.
The atomic number of X is :
1. 25
2. 26
3. 27
4. 24

Magnetic moment of K₃[Fe(CN)₅(H₂O)] is
1. 0
2. 4.92
3. 3.87
4. 2.83

HgCl₂ and I₂ both when dissolved in water containing I^- ions the pair of species formed is
(a) HgI₂, ${\mathrm{I}}_3^{-}$                              (b) HgI₂, I^-
(c) ${\mathrm{HgI}}_4^{2-},<mspace\; width="1em"></mspace>{\mathrm{I}}_3^{-}$                             (d) Hg₂I₂, I^-

The incorrect statement regarding the lanthanons is ;

The correct electronic configuration of Gadolinium(Atomic number = 64)  is :
1. [Xe]4f⁸6d²                   
2. [Xe]4f⁹5s¹
3. [Xe]4f⁷5d¹6s²                   
4. [Xe]4f⁶5d²6s²

Assuming complete ionisation, same moles of which of the following compounds will
require the least amount of acidified KMnO₄ for complete oxidation?
1. FeSO₄
2. FeSO₃
3. FeC₂O₄
4. Fe(NO₂)₂

The reason for lanthanoid contraction is:
1. Negligible screening effect of 'f' orbitals
2. Increasing nuclear charge
3. Decreasing nuclear charge
4. Decreasing screening effect

A diamagnetic lanthanoid ion among the following is :
(At. numbers:  Ce = 58, Sm = 62, Eu = 63, Yb = 70)
1. Ce²⁺
2. Eu²⁺
3. Sm²⁺
4. Yb²⁺

KMnO₄ can be prepared from K₂MnO₄ as per reaction
$3{\mathrm{MnO}}_4^{2-}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{\mathrm{H}}_2\mathrm{O}\rightleftharpoons 2{\mathrm{MnO}}_4^{-}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{MnO}}_2<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>4{\mathrm{OH}}^{-}$
The reaction can go to completion by removing OH^- ions by adding
1. HCl
2. KOH
3. CO₂
4. SO₂

Identify the mixture of metals that contain a non-metal as a constituent in it.
1. lnvar
2. Steel
3. Bell metal
4. Bronze

Which of the following ions will exhibit colour in aqueous solutions ?
1. La³⁺ (Z=57)
2. Ti³⁺ (Z=22)
3. Lu³⁺ (Z=71)
4. Sc³⁺ (Z=21)

In which of the following pairs are both the ions coloured in aqueous solution?
(1) Ni²⁺, Ti³⁺             
(2) Sc³⁺, Ti³⁺
(3) Sc³⁺, Co²⁺           
(4) Ni²⁺, Cu⁺
(At. no : Sc =21, Ti = 22, Ni = 28, Cu = 29, Co = 27)

Which of the following order of CFSE is incorrect?
$\left(\mathrm{a}\right)<mspace\; width="1em"></mspace>\left[\mathrm{Co}\right(\mathrm{en}{)}_3{]}^{3+<mspace\; width="1em"></mspace>}>\left[\mathrm{Co}\right({\mathrm{NH}}_3{)}_6{]}^{3+}>\left[\mathrm{Co}\right({\mathrm{H}}_2\mathrm{O}{)}_6{]}^{3+}$
(b) $[{\mathrm{PtCl}}_4{]}^{2-}>[{\mathrm{PdCl}}_4{]}^{2-}>[{\mathrm{NiCl}}_4{]}^{2-}$
(c) $\left[\mathrm{Ni}\right(\mathrm{DMHH}{)}_2]<[\mathrm{Ni}(\mathrm{en}{)}_2{]}^{2+}$
(d) $\left[\mathrm{Co}\right(\mathrm{ox}{)}_3{]}^{3-}<\left[\mathrm{Co}\right(\mathrm{en}{)}_3{]}^{3+}$

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 is called Wilkinson's catalyst:
(a) $\left[\mathrm{RhCl}\right({\mathrm{PPh}}_3{)}_3]$             (b) ${\mathrm{TiCl}}_4+({\mathrm{C}}_2{\mathrm{H}}_5{)}_3\mathrm{Al}$
(c) $({\mathrm{C}}_2{\mathrm{H}}_5{)}_4\mathrm{Pb}$                  (d) $\left[{\mathrm{PtCl}}_2\right({\mathrm{NH}}_3{)}_2]$

$\left(\mathrm{X}\right)+{\mathrm{K}}_2{\mathrm{CO}}_3+\mathrm{Air}\stackrel{\mathrm{heat}}{\to }\left(\mathrm{Y}\right)$
$\left(\mathrm{Y}\right)+{\mathrm{Cl}}_2\stackrel{}{\to }\left(\mathrm{Z}\right)\mathrm{Pink}$
Which of the following is correct?
(a) X= black, ${\mathrm{MnO}}_2$,Y=Blue, ${\mathrm{K}}_2{\mathrm{CrO}}_4$, Z = ${\mathrm{KMnO}}_4$
(b) X= green, ${\mathrm{Cr}}_2{\mathrm{O}}_3$, Y=Yellow ,${\mathrm{K}}_2{\mathrm{CrO}}_4$, Z = ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$
(c) X= black, ${\mathrm{MnO}}_2$, Y = green, ${\mathrm{K}}_2{\mathrm{MnO}}_4$, z = ${\mathrm{KMnO}}_4$
(d) x = black, ${\mathrm{Bi}}_2{\mathrm{O}}_3$, Y = Colourless, ${\mathrm{KBiO}}_2$, z = ${\mathrm{KBiO}}_3$

Acidified permanganate solution does not oxidize:
(1) ${\mathrm{C}}_2{\mathrm{O}}_4^{2-}\left(\mathrm{aq}\right)$                   
(2) ${\mathrm{NO}}_2^{-}\left(\mathrm{aq}\right)$
(3) ${\mathrm{S}}^{2-}\left(\mathrm{aq}\right)$                         
(4) ${\mathrm{F}}^{-}\left(\mathrm{aq}\right)$

Which of the following solid salt on heating with solid ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ and  conc.${\mathrm{H}}_2{\mathrm{SO}}_4$ orange red vapours are evolved which turn aqueous NaOH solution yellow?
(a)NaBr               (b) NaCl
(c) ${\mathrm{NaNO}}_3$           (d) NaI

Which of the following is true for the species $3{\mathrm{d}}^4$ configuration ?
(1) ${\mathrm{Cr}}^{2+}$ is reducing in nature                               
(2) ${\mathrm{Mn}}^{3+}$ is oxidising in nature.
(3) Both (A) and (B)                                             
(4) None of these

In which compound does vanadium have an oxidation number of +4?
(A) ${\mathrm{NH}}_4{\mathrm{VO}}_2$                                 
(B) ${\mathrm{K}}_4\left[\mathrm{V}{\left(\mathrm{CN}\right)}_6\right]$
(C) ${\mathrm{VSO}}_4$                                     
(D) ${\mathrm{VOSO}}_4$

Arrange the following species in the increasing order of their magnetic properties.
${\mathrm{VCl}}_3$    ${\mathrm{VOSO}}_4$    ${\mathrm{Na}}_3{\mathrm{VO}}_4$       $\left[\mathrm{V}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]{\mathrm{SO}}_4.{\mathrm{H}}_2\mathrm{O}$
  I              II                  III                      IV
 
(1) III<II<I<IV                                         
(2) III<IV<II<I
(3) II<III<I<IV                                         
(4) IV<I<II<III

Which of the following increasing order of oxidising power is correct for the following species?
           ${{\mathrm{VO}}_2}^{+},<mspace\; width="1em"></mspace>{{\mathrm{MnO}}_4}^{-},<mspace\; width="1em"></mspace>{\mathrm{Cr}}_2{{\mathrm{O}}_7}^{2-}$
(A) ${{\mathrm{VO}}_2}^{+}<{\mathrm{Cr}}_2{{\mathrm{O}}_7}^{2-}<{{\mathrm{MnO}}_4}^{-}$                           
(B) ${{\mathrm{VO}}_2}^{+}<{{\mathrm{MnO}}_4}^{-}<{\mathrm{Cr}}_2{{\mathrm{O}}_7}^{2-}$
(C) ${\mathrm{Cr}}_2{{\mathrm{O}}_7}^{2-}<{{\mathrm{VO}}_2}^{+}<{{\mathrm{MnO}}_4}^{-},$                           
(D) ${\mathrm{Cr}}_2{{\mathrm{O}}_7}^{2-}<{{\mathrm{MnO}}_4}^{-}<{{\mathrm{VO}}_2}^{+}$

At $300°\mathrm{C},<mspace\; width="1em"></mspace>{\mathrm{FeCl}}_3<mspace\; width="1em"></mspace>:$
1. Decomposes into ${\mathrm{FeCl}}_2<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>{\mathrm{Cl}}_2.$               
2. Decomposes into $\mathrm{Fe}<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>{\mathrm{Cl}}_2.$
3. Sublimes go give liquid ${\mathrm{FeCl}}_3$                         
4. Sublimes to give gaseous dimmer ${\left({\mathrm{FeCl}}_3\right)}_2.$

Anhydrous ferric chloride is prepared by
(1) Heating hydrated ferric chloride at a high temperature in a stream of air.
(2) Heating metallic iron in a stream of dry chlorine gas.
(3) Reaction of ferric oxide with HCl (aq).
(4) Reaction of metallic iron with HCl (aq).

Select the correct statement :
(1) ${\mathrm{PH}}_3$ reduces ${\mathrm{AgNO}}_3$ to metallic Ag.
(2) Organic tissues turn ${\mathrm{AgNO}}_3$ black by reducing it to Ag.
(3) $\mathrm{AgCN}<mspace\; width="1em"></mspace>$is soluble in $\mathrm{KCN}$.
(4) All are correct statements.

Which of the following products are formed when potassium bromide reacts with potassium permanganate in alkaline pH?
1. ${{\mathrm{BrO}}_3}^{‐},<mspace\; width="1em"></mspace>{\mathrm{MnO}}_2$                                     
2. ${{\mathrm{BrO}}_4}^{‐},<mspace\; width="1em"></mspace>{\mathrm{Mn}}^{2+}$
3. ${\mathrm{Br}}_2,<mspace\; width="1em"></mspace>{\mathrm{MnO}}_2$                                         
4. ${\mathrm{Br}}_2{\mathrm{O}}^{‐},<mspace\; width="1em"></mspace>{{\mathrm{MnO}}_4}^{2‐}$

Which of the following pairs of compounds are more stable
(A) $K_2\left[NiC{l}_6\right],\left[Pt\right(CN{)}_4{]}^{2-}$
(B) NiCl₄, PtCl₄
(C) $\left[Ni\right(CN{)}_4{]}^{2-},<mspace\; width="1em"></mspace>K_2\left[Pt\right(C{l}_6\left)\right]$
(D) PtCl₂, NiCl₂

Which of the following species has the highest number of unpaired electrons?
1. Fe²⁺
2. Fe³⁺
3. Co³⁺
4. Co²⁺

Heating of Ag with dil. HNO₃ give
1. NO
2. NO₂
3. N₂O
4. N₂O₃

When excess of SnCl₂ is added to HgCl₂, the substance formed is
1. Hg₂Cl₂
2. Sn
3. Hg
4. Cl₂

Which of the following elements form stable dinuclear ions
1. Zn
2. Cd
3. Hg
4. Fe