Co-ordination compounds practice · Easy

Option B (Potassium ferricyanide) is correct because the EAN of Fe in K3[Fe(CN)6] is 35, which does not satisfy the EAN rule (next inert gas configuration).

Option D ($\mathrm{W}$) is correct because manganese typically forms polynuclear carbonyls, not mononuclear carbonyls.

Option A (${CO}$) is correct because ${CO}$ can accept d-electrons from the metal in its antibonding orbitals, leading to synergic bonding.

Option A (Complex salts) is correct because complex salts contain complex ions that do not dissociate completely in solution, thus giving tests for only one of the metallic elements.

Option C (6 and 3) is correct because the coordination number is the number of ligands attached to the metal, and the oxidation number is calculated based on the charges of the ligands and counter-ion.

Option C, [ Fe( η ⁵ - C₅H₅ )₂ ]$\left[ {\mathrm{Fe}{{\left( {{{\mathrm{\eta }^5} - {\mathrm{C}_5}{\mathrm{H}_5}} \right)}_2}} \right]$, is correct because ferrocene exhibits both sigma and pi bonding between the iron center and the cyclopentadienyl rings.

Option D (Linear) is correct because the complex ion ${\left[ {\mathrm{Ag}{{\left( {\mathrm{N}{\mathrm{H}_3}} \right)}_2}} \right]^ + }$ has a coordination number of 2, resulting in a linear geometry.

Option D (The number of ligands around a metal ion bonded by sigma bonds) is correct because the coordination number is determined by the number of sigma bonds formed between the ligands and the central metal atom.

Option A is the correct example of coordination isomerism because it involves the exchange of ligands between the cationic and anionic coordination complexes.

Option D is correct because the complex has a coordination number of 4 and no lone pairs on the central metal atom, indicating a square planar geometry.

Option A (+6 and +3) is correct because the coordination number of Cr is 6 (three bidentate ligands) and its oxidation state is +3.

Option D is correct. [Cr(SCN)₂(NH₃)₄]⁺ exhibits both geometrical (cis-trans) and linkage isomerism, leading to a maximum number of isomers.

Option A ($\mathrm{Al(OC_2H_5)_3}$) is correct because in aluminum ethoxide, the aluminum atom is bonded to oxygen atoms, not directly to carbon.

Option A is correct because, according to Werner's theory, primary valencies (oxidation state) are ionizable, corresponding to the counter ions in the coordination complex.

Option B (If both (A) and (R) are correct but (R) is not correct explanation for (A)) is correct because both the assertion and reason are true, but the hybridization doesn't directly explain the diamagnetic nature.

Option C ($e_{\mathrm{g}}=t_{2 \mathrm{~g}}$) is correct because in a spherically symmetrical field, all d-orbitals remain degenerate, meaning they have the same energy.

Option C (Zero) is correct because ${\left[ {Co{{\left( {{H_2}O} \right)}_6}} \right]^{3 + }}$ is a low spin complex with no unpaired electrons.

Option B ($Mg$) is correct because Chlorophyll is a coordination compound with Magnesium ($Mg$) as its central atom.

Option B is correct because it follows IUPAC naming conventions: dichloro (two chloride ligands), bis (two methylamine ligands), copper(II) (copper with a +2 oxidation state).

Option C (34) is correct because the Effective Atomic Number (EAN) is calculated by subtracting the oxidation state of the metal from its atomic number and adding twice the coordination number.

Option A (Primary valencies are ionizable) is correct because, according to Werner's theory, primary valencies are ionizable and correspond to the oxidation state of the metal.

Option A ($\mathrm{Ni(CO)_4}$) is correct because nickel tetracarbonyl is a colorless liquid.

Option B (Complex compound) is correct because ${K}_4\left[{Fe}({CN})_6\right]$ is a coordination complex, which does not fully dissociate into its constituent ions in solution.

Option A (Complex salt) is correct because potassium ferrocyanide contains a complex ion, $[Fe(CN)_6]^{4-}$, which does not dissociate into simple ions in solution.

Option C (Lewis base) is correct because ligands donate electron pairs to the central metal atom/ion, which is the definition of a Lewis base.

Option A ($\left[{PtCl}_2({en})_2\right]\left({NO}_3\right)_2$) is correct because it accurately represents the given name, with platinum(IV), two chloride ligands, two ethylenediamine ligands, and two nitrate counterions.

Option B (2) is correct because the complex can exist as cis and trans isomers.

Option D ($\mathrm{Ti}{\left( {{\mathrm{C}_2}{\mathrm{H}_5}} \right)_4}$) is correct because it contains a direct bond between the metal (Ti) and carbon (from the ethyl group).

Option B is the correct answer because ${\left[ {\mathrm{Co}{{\left( {\mathrm{N}{\mathrm{H}_3}} \right)}_6}} \right]^{3 + }}$ has a coordination number of 6, requiring six hybridized orbitals, hence ${d^2}s{p^3}$ hybridization, not ${d^2}s{p^2}$.