Mock Test 1 — Coordination Compounds

EDTA donates how many e⁻ pairs:

Oxidation state of Fe in $[Fe(CN)_6]^{4-}$:

Geometry of $[Ni(CO)_4]$ (Ni in 0 state, $d^{10}$):

Werner's secondary valence equals:

Hybridization of $[Fe(H_2O)_6]^{2+}$:

Most stable complex (chelate effect):

Linkage isomerism:

Color of $[Co(NH_3)_6]^{3+}$:

Coordination compound used in cancer treatment:

EDTA forms most stable complex with:

Coordination number in $[Cr(NH_3)_4Cl_2]^+$:

Charge on metal in $[Fe(CN)_6]^{3-}$ (Fe oxidation state):

Number of unpaired electrons in $[Mn(H_2O)_6]^{2+}$ (high spin $d^5$):

Assertion (A): $[Fe(CN)_6]^{4-}$ is diamagnetic while $[Fe(H_2O)_6]^{2+}$ is paramagnetic. Reason (R): $CN^-$ is a strong field ligand causing pairing of d-electrons; $H_2O$ is weak field.

Assertion (A): $[Ni(CN)_4]^{2-}$ is square planar but $[NiCl_4]^{2-}$ is tetrahedral. Reason (R): $CN^-$ is strong field forcing $d^8$ to pair, freeing one $d$-orbital for $dsp^2$; $Cl^-$ is weak field, keeping $d^8$ as is, using $sp^3$.