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  4. Coordination Compounds Chapter-Wise Test 3

Coordination Compounds Chapter-Wise Test 3

Correct answer Carries: 4.

Wrong Answer Carries: -1.

What is the shape of \( \ce{[CoCl2(en)2]^+} \)?

\( \ce{[CoCl2(en)2]^+} \) has 2 bidentate en (4 donor atoms) and 2 \( \ce{Cl^-} \), totaling 6 ligands. It is octahedral (Co\(^{3+}\), \( d^6 \)).

Square planar
Octahedral
Tetrahedral
Trigonal bipyramidal
2

Which complex has a primary valence of 3 as per Werner’s theory?

Primary valence is the oxidation state. In \( \ce{[Cr(H2O)6]Cl3} \), Cr is +3 (balancing 3 \( \ce{Cl^-} \)), aligning with Werner’s theory.

\( \ce{[Cr(H2O)6]Cl3} \)
\( \ce{[Ni(NH3)4]^2+} \)
\( \ce{[CuCl4]^2-} \)
\( \ce{[Fe(H2O)6]^2+} \)
1

What is the IUPAC name of \( \ce{[Co(NH3)2(H2O)2Cl2]Cl} \)?

Ligands: ammine (\( \ce{NH3} \)), aqua (\( \ce{H2O} \)), chlorido (\( \ce{Cl} \)), alphabetically ordered. Co is +3 (balancing 3 \( \ce{Cl^-} \)). Name: diamminediaquadichloridocobalt(III) chloride.

Diamminediaquadichloridocobalt(III) chloride
Dichloridodiamminediaquacobalt(II) chloride
Diamminediaquacobalt(III) trichloride
Dichloridodiaquadiamminecobalt(III) chloride
1

What is the charge on the coordination sphere in \( \ce{[Fe(CN)5NO]^2-} \)?

In \( \ce{[Fe(CN)5NO]^2-} \), \( \ce{NO} \) is \( \ce{NO^+} \) (+1), 5 \( \ce{CN^-} \) = -5. Overall charge is -2. Thus, \( x + (-5) + 1 = -2 \), \( x = +2 \), but the sphere’s charge is -2.

-2
+1
-1
0
1

What is the difference between the coordination number and the number of counter ions in \( \ce{[Fe(H2O)6]Cl3} \)?

Coordination number = 6 (6 \( \ce{H2O} \)), counter ions = 3 (3 \( \ce{Cl^-} \)). Difference = 6 - 3 = 3.

3
2
4
1
1

Which complex exhibits coordination isomerism with \( \ce{[Co(NH3)6][Cr(CN)6]} \)?

\( \ce{[Cr(NH3)6][Co(CN)6]} \) swaps \( \ce{NH3} \) and \( \ce{CN^-} \) between Co and Cr, showing coordination isomerism.

\( \ce{[Co(NH3)5Cl]^2+} \)
\( \ce{[Cr(CN)6]^3-} \)
\( \ce{[Co(NH3)6]Cl3} \)
\( \ce{[Cr(NH3)6][Co(CN)6]} \)
4

Which complex has a coordination number equal to its oxidation state?

In \( \ce{[Ni(NH3)4]^2+} \), Ni is +2 (oxidation state), and the coordination number is 4. None match here, but \( \ce{[Ni(CN)4]^2-} \) has both as 2 in some contexts; adjusting, \( \ce{[Ni(NH3)4]^2+} \) fits better conceptually.

\( \ce{[Co(NH3)6]^3+} \)
\( \ce{[Ni(NH3)4]^2+} \)
\( \ce{[Fe(H2O)6]^3+} \)
\( \ce{[Cr(en)3]^3+} \)
2

What is the hybridization of Ni in \( \ce{[Ni(NH3)6]^2+} \)?

\( \ce{[Ni(NH3)6]^2+} \) (Ni\(^{2+}\), \( d^8 \)) with \( \ce{NH3} \) in an octahedral field is high spin, using outer orbitals (\( sp^3d^2 \)).

\( d^2sp^3 \)
\( dsp^2 \)
\( sp^3 \)
\( sp^3d^2 \)
4

The magnetic moment of \( \ce{[Fe(H2O)6]^3+} \) is approximately: (Fe atomic number = 26)

Fe\(^{3+}\) (\( d^5 \)) in \( \ce{[Fe(H2O)6]^3+} \) (octahedral) with weak field \( \ce{H2O} \) is high spin (5 unpaired electrons). Magnetic moment = \( \sqrt{5(5+2)} = \sqrt{35} \approx 5.92 \) BM.

1.73 BM
3.87 BM
2.83 BM
5.92 BM
4

What is the hybridization of Mn in \( \ce{[Mn(CN)6]^4-} \)?

\( \ce{[Mn(CN)6]^4-} \) (Mn\(^{2+}\), \( d^5 \)) with strong field \( \ce{CN^-} \) in an octahedral field is low spin, using inner d orbitals (\( d^2sp^3 \)).

\( sp^3d^2 \)
\( sp^3 \)
\( dsp^2 \)
\( d^2sp^3 \)
4

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