$Ag _2SO _4$

$CuF _2$

$ZnF _2$

$Cu _2Cl _2$

$[Ti(H _2O) _6]^{3+}$

$[Cu(NH _3) _4]^{2+}$

$[CoF _6]^{3-}$

$CrO _4^{2-}$

(A) - (iii), (B) - (iv), (C) - (i), (D) - (ii), (E) - (v)

(A) - (ii), (B) - (iii), (C) - (iv), (D) - (i), (E) - (v)

(A) - (v), (B) - (ii), (C)-(iii), (D) - (iv), (E) - (i)

(A) - (iii), (B)-(i), (C)-(ii), (D) - (iv), (E).- (v)

Only $Zn^{2+}$ is colourless and $Ni^{2+}$, $Cu^{2+}$ and $Cr$ are coloured

All the ions are coloured

All the ions are colourless

$Zn^{2+}$and $Cu^{2+}$ are colourless while $Ni^{2+}$ and $Cr^{2+}$ are coloured

$1,4$

$3,4$

$2,3$

$1,2$

$CoF _6^{3-}$and $NiCl _4^{2-}$

$TiF _6^{2-}$and $Cu _2Cl _2$

$Cu _2Cl _2$ and $NiCl _4^{2-}$

$TiF _6^{2-}$ and $CoF _6^{ 3-}$

$d-f$ transition

$s-s$ transition

$s-d$ transition

$d-d$ transition

${ VCl } _{ 3 }$

${ VOSO } _{ 4 }$

${ Na } _{ 3 }{ VO } _{ 4 }$

$[{ V(H } _{ 2 }O) _{ 6 }]{ SO } _{ 4 }{ H } _{ 2 }O$

${K} _{2}{Cr} _{2}{O} _{7}$

$KMn{O} _{4}$

$Cu{SO} _{4}.5{H} _{2}O$

Both a and b

$Ni^{2+}$

$Sc^{3+}$

$Cu^{2+}$

$Mn^{3+}$

due to s being filled before d (Aufbau principle)

Due to presence of unpaired electron

unfilled d orbital

d-d transition

Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

Both the Statement 1 and Statement 2 are correct, but Statement 2 is NOT the correct explanation of Statement 1.

Statement 1 is correct, but Statement 2 is not correct.

Statement 1 is not correct, but Statement 2 is correct.

Cu

Zn

Fe

Cr

blue

light green

very dark green

yellow

d-d transition of electrons

charge transfer

polirisation of halid${Ag}^{+}$ by

both (b) and (c)

$ Na _{2}[CuCl _{4}] $

$ Na _{2}[CdCl _{2}] $

$ [Cr(H _{2}O) _{6}]Cl _{3} $

all of the above

L-> M charge transfer transition

$\sigma -{ \sigma }^{ * }$ transition

M-> L charge transfer transition

d-d transition

Only few transition metal complexes are coloured

d-orbital are degenerated hence, they form complexes

Transition metal complexes reflect the complimentary colour of absorbed colour

Energy difference between ${ t } _{ 2(g) }$ and ${ t } _{ g }$ level is very large

${ Ni }^{ 2+ }$

${ Cu }^{ + }$

${ Ti }^{ 3+ }$

${ Fe }^{ 3+ }$

$Cu _{2}Cl _{2},\ NiCl _{4}^{2-}$

$TiF _{6}^{2-},\ Cu _{2}Cl _{2}$

$CoF _{6}^{3-},\ NiCl _{4}^{2-}$

$TiF _{6}^{2-},\ CiF _{6}^{3-}$

$\,{\text{AgN}}{{\text{O}} _3}$

$\,{\text{CuS}}{{\text{O}} _4}$

${\text{CuCl}}$

${\text{ZnC}}{{\text{l}} _{\text{2}}}$

pink

yellow

violet

blue

$d-d$ transition

$L\rightarrow M$ charge transfer transition

$\sigma-\sigma^{*}$ transition

$M\rightarrow L$ charge transfer transition

$V^{+4}, Cu^{+2}$

$Co^{+2}, Ni^{+2}$

$Fe^{+3}, Ti^{+3}$

$Co^{+2}, Fe^{+3}$

${K} _{2}{Cr} _{2}{O} _{7}$

$KMn{O} _{4}$

$Cu{SO} _{4}.5{H} _{2}O$

Both (1) and (2)

${\text{TiC}}{{\text{l}} _{\text{4}}}$ is a colourless compound.

$\left[ {{\text{Cr}}{{\left( {{\text{N}}{{\text{H}} _{\text{3}}}} \right)} _{\text{6}}}} \right]{\text{C}}{{\text{L}} _{\text{3}}}$ is a coloured compound

${{\text{K}} _{\text{3}}}\left[ {{\text{V}}{{\text{F}} _{\text{6}}}} \right]$ is a colourless compound

$\;\left[ {{\text{Cu}}{{\left( {{\text{NCC}}{{\text{H}} _{\text{3}}}} \right)} _{\text{4}}}} \right]\left[ {{\text{B}}{{\text{F}} _{\text{4}}}} \right]$ is a colourless compound

green

deep blue

yellow

red

${Ni}^{2+}$

${Fe}^{2+}$

${Cu}^{2+}$

${Cu}^{+}$

$d-d$ transition

charge transfer

change in the geometry

none

${Fe}^{3+}$ gives brown color with potassium ferricyanide

${Fe}^{2+}$ gives blue precipitate with potassium ferricyanide

${Fe}^{3+}$ gives red color with potassium thiocyanate

${Fe}^{2+}$ gives brown color with ammonium thiocyanate

${Ti}^{4+}$

${Cu}^{+}$

${Zn}^{2+}$

${Cr}^{3+}$

$V{Cl} _{3}$

$VO{SO} _{4}$

${Na} _{3}{VO} _{4}$

$\left[ V{ \left( { H } _{ 2 }O \right) } _{ 6 }{ SO } _{ 4 } \right] .{ H } _{ 2 }O$

$Zn{({NO} _{3})} _{2}$

$Li{NO} _{3}$

$Co{({NO} _{3})} _{2}$

$Cr{Cl} _{3}$

Ions of $d$-block elements are colored due to $d-d$ transition

Ions of $f$-block elements are colored due to $f-f$ transtition

${ \left[ Sc{ \left( { H } _{ 2 }O \right) } _{ 6 } \right] }^{ 3+ },{ \left[ Ti{ \left( { H } _{ 2 }O \right) } _{ 6 } \right] }^{ 4+ }$ are colored complexes.

${Cu}^{+}$ is colorless ion.

$Zn{({NO} _{3})} _{2}$

$Li{NO} _{3}$

$Co{({NO} _{3})} _{2}$

$Cr{Cl} _{3}$

Potash alum

$Sc^{+3}$

$V^{+3}$

$Cr^{+3}$

All of these

$Mn^{+3}, CO^{+3}$

$Fe^{3+}, Cr^{+3}$

$Zn^{2+}, Sc^{3+}$

$Ti^{2+}, Cu^{2+}$

$Ag^+$

$Co^{2+}$

$Ti^{4+}$

None of these

presence of low oxidation state of copper

completely filled d-level in $Cu(I)$

diamagnetic nature of the compound

high polarizability of $Cu(I)$ ion

$Cu^{2+}$

$Mn^{2+}$

$Co^{2+}$

$Ni^{2+}$

$C{ r }^{ +4 }$

$Sc^{ +3 }$

$Ti^{ +3 }$

${ V }^{ +3 }$

$K _{2}MnO _{4}$, dark green

$KMnO _{4}$, purple

$Mn _{2}O _{3}$, brown

$Mn _{3}O _{4}$, black.

Magnesium

Aluminium

Iron

Chromium

${Na} _{2}Cu{Cl} _{4}$

${Na} _{2}Cd{Cl} _{4}$

${Na} _{3}[Fe{(CN)} _{6}]$

${K} _{3}[Fe{(CN)} _{6}]$

$Ni^{2+}$

$Fe^{3+}$

$Ti^{4+}$

$Cu^{2+}$

$d _{x^2-y^2},d _{xy}$

$d _{xy},d _{yz}$

$d _{x^2-y^2},d _{yz}$

$d _{z^2},dxy$

$Cr{O} _{3}$

${Cr} _{2}{O} _{3}$

$Cr$

$CrO ({O} _{2})$

${Cr}^{3+}$

${Ti}^{3+}$

${Sc}^{3+}$

${V}^{3+}$