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Coordination Compounds Chemistry - Coordination Compounds

Rajasthan Board (RBSE) - STD 12 Science - Chemistry (Rajasthan - English Medium). 352 questions in this chapter.

Question types

Coordination Compounds question types

352 questions across 6 question groups — pick any mix to generate a Chemistry paper with step-by-step answer keys.

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5
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Sample Questions

Coordination Compounds questions

One sample from each question group in this chapter. Select any group above to see the full set with answer keys.

Q 6Assertion (A) & Reason (B) MCQ1 Mark
Two statements are given$-$ one labelled Assertion $(A)$ and the other labelled Reason $(R).$ Select the correct answer to these questions from the codes $(a), (b), (c)$ and $(d)$ as given below: Assertion $(A):$ Linkage isomerism arises in coordination compounds because of ambidentate ligand.
Reason $(R):$ Ambidentate ligand like $NO_2$ has two different donor atoms i.e., $N$ and $O.$
  • ✓
    Both Assertion $(A)$ and Reason $(R)$ are correct statements, and Reason $(R)$ is the correct explanation of the Assertion $(A).$
  • B
    Both Assertion $(A)$ and Reason $(R)$ are correct statements, but Reason $(R)$ is not the correct explanation of the Assertion $(A).$
  • C
    Assertion $(A)$ is correct, but Reason $(R)$ is incorrect statement.
  • D
    Assertion $(A)$ is incorrect, but Reason $(R)$ is correct statement.

Answer: A.

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Q 7Assertion (A) & Reason (B) MCQ1 Mark
Two statements are given$-$ one labelled Assertion $(A)$ and the other labelled Reason $(R)$. Select the correct answer to these questions from the codes $(a), (b), (c)$ and $(d)$ as given below:
Assertion $(A)$ : Linkage isomerism arises in coordination compounds because of ambidentate ligand.
Reason $(R)$ : Ambidentate ligand like $NO_2$ has two different donor atoms i.e., $N$ and $O$.
  • ✓
    Both Assertion $(A)$ and Reason $(R)$ are correct statements, and Reason $(R)$ is the correct explanation of the Assertion $(A)$.
  • B
    Both Assertion $(A)$ and Reason $(R)$ are correct statements, but Reason $(R)$ is not the correct explanation of the Assertion $(A).$
  • C
    Assertion $(A)$ is correct, but Reason $(R)$ is incorrect statement.
  • D
    Assertion $(A)$ is incorrect, but Reason $(R)$ is correct statement.

Answer: A.

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Q 8Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
Assertion: $\ce{[Cu(NH_3)_4]^{2+}}$ is coloured while $\ce{[Cu(CN)_4]^{3-}}$ ion is colourless.
Reason: $\ce{[Cu(NH_3)_4]^{2+}}$ has $dsp^2$ hybridisation.
  • A
    Assertion and reason both are correct statements and reason is correct explanation for assertion.
  • ✓
    Assertion and reason both are correct statements but reason is not correct explanation for assertion.
  • C
    Assertion is correct statement but reason is wrong statement.
  • D
    Assertion is wrong statement but reason is correct statement.

Answer: B.

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Q 9Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
  1. Assertion and reason both are correct statements and reason is correct explanation for assertion.
  2. Assertion and reason both are correct statements but reason is not correct explanation for assertion.
  3. Assertion is correct statement but reason is wrong statement.
  4. Assertion is wrong statement but reason is correct statement.
Assertion: The ligands nitro and nitrito are called ambidentate ligands.
Reason: An ambidentate ligand can attach to metal through two different atoms.
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Q 10Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
Assertion: $\ce{[Pt(NH_3)_2Cl_2]}$ is square planar.
Reason: The oxidation state of platinum is $+2.$
  • ✓
    Assertion and reason both are correct statements and reason is correct explanation for assertion.
  • B
    Assertion and reason both are correct statements but reason is not correct explanation for assertion.
  • C
    Assertion is correct statement but reason is wrong statement.
  • D
    Assertion is wrong statement but reason is correct statement.

Answer: A.

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Q 131 Marks Question1 Mark
Amongst the following, the most stable complex is :
  • A
    $[\ce{Fe(H2O)6]^{3+}}$
  • B
    $[\ce{Fe(NH3)6]^{3+}}$
  • ✓
    $[\ce{Fe(C2O4)3]^{3–}}$
  • D
    $[\ce{FeCl6]^{3–}}$

Answer: C.

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Q 163 Marks Question3 Marks
  1. Using valence bond theory, predict the shape and magnetic character of
  1. $\ce{[Ni(CO)_4]. [Ni = 28]}.$
  2. Give one example of application of coordination compounds$-$in medicine.
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Q 173 Marks Question3 Marks
  1. For the complex $\ce{[Fe(H_2O)_6]^3}^+,$ write the hybridization, magnetic character and spin of the complex. $($At. number: $\ce{Fe = 26)}$
  2. Draw one of the geometrical isomers of the complex $\ce{[Pt(en)_2Cl_2]^{2+}}$ which is optically inactive.
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Q 183 Marks Question3 Marks
  1. What type of isomerism is shown by $\ce{[Co(NH_3)_5ONO]Cl_2}$?
  2. On the basis of crystal field theory, write the electronic configuration for $d^{4 }$ ion if $\Delta _o< P.$
  3. Write the hybridization and shape of $\ce{[Fe(CN)_6]^{_{3-}}}.$
$($Atomic number of $\ce{Fe = 26)}$
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Q 193 Marks Question3 Marks
  1. What type of isomerism is shown by the complex $\ce{[Co(NH_3)_5 (SCN)]^{2+}}$?
  2. Why is $\ce{[NiCl_4]^{2-}}$ paramagnetic while $\ce{[Ni(CN)_4]^{2-}}$ is diamagnetic? $($Atomic number of $Ni = 28)$
  3. Why are low spin tetrahedral complexes rarely observed?
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Q 203 Marks Question3 Marks
  1. Write the $\text{IUPAC}$ name of the complex $\ce{[Cr(NH_3)_4 Cl_2]Cl}.$
  2. What type of isomerism is exhibited by the complex $\ce{[Co(en)_3]^{3+}}$?
$($en $=$ ethane $-1,2-$ diamine$)$
  1. Why is $\ce{[NiCl_4]^{2–}}$ paramagnetic but $\ce{[Ni(CO)_4]}$ is diamagnetic?
$($At. nos.: $Cr= 24, Co=27, Ni= 28)$
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Q 21Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions:
Coordination compounds are formulated and named according to the $\text{IUPAC}$ system.
Few rules for naming coordination compounds are:
  1. In ionic complex, the cation is named first and then the anion.
  2. In the coordination entity, the ligands are named first and then the central metal ion.
  3. When more than one type of ligands are present, they are named in alphabetical order of preference without any consideration of charge.
The following questions are multiple choice questions. Choose the most appropriate answer:
  1. The $\ce{[Pt(NH_3)_3Br(NO_2)Cl]Cl}$ name of the complex $\ce{[Pt(NH_3)_3Br(NO_2)Cl]Cl}$ is:
  1. Triamminechlorobromonitroplatinum $(IV)$ chloride.
  2. Triamminebromonitrochloroplatinum $(IV)$ chloride.
  3. Triamminebromidochloridonitroplatinum $(IV)$ chloride.
  4. Triamminenitrochlorobromoplatinum $(IV)$ chloride.
  1. The $\text{IUPAC}$ name of $\ce{[Ni(CO)_4]}$ is:
  1. Tetracarbonylnickel $(II).$
  2. Tetracarbonylnickel $(0).$
  3. Tetracarbonylnickelate $(II).$
  4. Tetracarbonylnickelate $(0).$
  1. As per $\text{IUPAC}$ nomenclature, the name of the complex $\ce{[Co(H_2O)_4(NH_3)_2]Cl_3}$ is:
  1. Tetraaquadiamminecobalt $(II)$ chloride.
  2. Tetraaquadiamminecobalt $(III)$ chloride.
  3. Diamminetetraaquacobalt $(II)$ chloride.
  4. Diamminetetraaquacobalt $(III)$ chloride.
  1. Which of the following represents correct formula of dichloridobis $($ethane $-1, 2-$diamine$)$ cobalt $(III)$ ion?
  1. $\ce{[CoCl_2(en)]^{2+}}$
  2. $\ce{[CoCl_2(en)_2]^{2+}}$
  3. $\ce{[CoCl_2(en)]^+}$
  4. $\ce{[CoCl_2(en)_2]^+}$
  1. Correct formula of pentaamminenitro$-O-$cobalt $(III)$ sulphate is:
  1. $\ce{[Co(NO_2)(NH_3)_5]SO_4}$
  2. $\ce{[Co(ONO)(NH_3)_5]SO_4}$
  3. $\ce{[Co(NO_2)(NH_3)_4](SO_4)_2}$
  4. $\ce{[Co(ONO)(NH_3)_4](SO_4)_2}$
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Q 22Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions :
Valence bond theory considers the bonding between the metal ion and the ligands as purely covalent. On the other hand, crystal field theory considers the metal$-$ligand bond to be ionic arising from electrostatic interaction between the metal ion and the ligands. In coordination compounds, the interaction between the ligand and the metal ion causes the five $d-$orbitals to split$-$up. This is called crystal field splitting and the energy difference between the two sets of energy level is called crystal field splitting energy. The crystal field splitting energy $(\Delta_0)$ depends upon the nature of the ligand. The actual configuration of complexes is divided by the relative values of $\Delta_0$ and $P\ ($pairing energy$)$.
If $\Delta_0<\text{P},$ then complex will be high spin.
If $\Delta_0>\text{P},$ then complex will be low spin
The following questions are multiple choice questions. Choose the most appropriate answer :
  1. Which of the following ligand has lowest $\Delta_0$ value?
  1. $CN^-$
  2. $CO$
  3. $F^-$
  4. $NH_3$
  1. The crystal field splitting energy for octahedral $(\Delta_0)$ and tetrahedral $(\Delta_t)$ complex is related as :
  1. $\Delta_\text{t}=\frac{1}{2}\Delta_0$
  2. $\Delta_\text{t}=\frac{4}{9}\Delta_0$
  3. $\Delta_\text{t}=\frac{3}{5}\Delta_0$
  4. $\Delta_\text{t}=\frac{2}{5}\Delta_0$
  1. On the basis of crystal field theory, the electronic configuration of $d_4$ in two situations : $(i)\ t.0 > P$ and $(ii)\ t.0$
  $(i)$ $(ii)$
$(a)$ $\text{t}^4_{2\text{g}}\text{e}^0_\text{g}$ $\text{t}^3_{2\text{g}}\text{e}^1_\text{g}$
$(b)$ $\text{t}^3_{2\text{g}}\text{e}^1_\text{g}$ $\text{t}^4_{2\text{g}}\text{e}^0_\text{g}$
$(c)$ $\text{t}^3_{2\text{g}}\text{e}^1_\text{g}$ $\text{t}^3_{2\text{g}}\text{e}^1_\text{g}$
$(d)$ $\text{t}^4_{2\text{g}}\text{e}^0_\text{g}$ $\text{t}^4_{2\text{g}}\text{e}^0_\text{g}$
  1. Using crystal field theory, calculate magnetic moment of central metal ion of $[FeF_6]^{4-}.$
  1. $1.79B.M.$
  2. $2.83B.M.$
  3. $3.85B.M.$
  4. $4.9B.M.$
  1. Electronic configuration of $d-$orbitals in $[Ti(H_2O)_6]^{3+}$ ion in an octahedral crystal field is:
  1. $\text{t}^1_{2\text{g}}\text{e}^0_\text{g}$
  2. $\text{t}^2_{2\text{g}}\text{e}^0_\text{g}$
  3. $\text{t}^0_{2\text{g}}\text{e}^1_\text{g}$
  4. $\text{t}^1_{2\text{g}}\text{e}^1_\text{g}$
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Q 23Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions:
To explain bonding in coordination compounds various theories were proposed. One of the important theory was valence bond theory. According to that, the central metal ion in the complex makes available a number of empty orbitals for the formation of coordination bonds with suitable ligands. The appropriate atomic orbitals of the metal hybridise to give a set of equivalent orbitals of definite geometry.
The $d-$orbitals involved in the hybridisation may be either inner $d-$orbitals i.e.$, (n - 1)d$ or outer $d-$orbitals i.e.$, nd.$
For example, $Co^{3+}$ forms both inner orbital and outer orbital complexes, with ammonia it forms $[\ce{Co(NH3)6]^{3+}}$ and with fluorine it forms $[\ce{CoF6]^{3-}}$ complex ion.
The following questions are multiple choice questions. Choose the most appropriate answer :
  1. Which of the following is not true for $[\ce{CoF6}]^{3-}$?
  1. It is paramagnetic.
  2. It has coordination number of $6.$
  3. It is outer orbital complex.
  4. It involves $d^2sp^3$ hybridisation.
  1. $[\ce{Cr(H2O)6]Cl3}\ ($at. no. of $Cr = 24)$ has a magnetic moment of $3.83\ B.M.$ The correct distribution of $3d-$electrons in the central metal of the complex is :
  1. $3\text{d}^1_\text{xy},3\text{d}^1_{\text{x}^2-\text{y}^2},3\text{d}^1_\text{yz}$
  2. $3\text{d}^1_\text{xy},3\text{d}^1_{\text{yz}},3\text{d}^1_\text{zx}$
  3. $3\text{d}^1_\text{xy},3\text{d}^1_{\text{zy}},3\text{d}^1_{\text{z}^2}$
  4. $3\text{d}^1_{\text{x}^2-\text{y}^2},3\text{d}^1_{\text{z}^2},3\text{d}^1_\text{xz}$
  1. Which of the following is true for $[\ce{Co(NH3)6}]^{3+}$?
  1. It is an octahedral, di magnetic and outer orbital complex.
  2. It is an octahedral, paramagnetic and outer orbital complex.
  3. It is an octahedral, paramagnetic and inner orbital complex.
  4. It is an octahedral, di magnetic and inner orbital complex.
  1. The paramagnetism of $[\ce{CoF6}]^{3-}$ is due to.
  1. $3$ electrons.
  2. $4$ electrons.
  3. $2$ electrons.
  4. $1$ electron.
  1. Which of the following is an inner orbital or low spin complex?
  1. $[\ce{Ni(H2O)6}]^{3+}$
  2. $[\ce{FeF6}]^{3-}$
  3. $[\ce{Co(CN)6}]^{3-}$
  4. $[\ce{NiCl4}]^{2-}$
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Q 24Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions: Werner, a Swiss chemist in $1892$ prepared and characterised a large number of coordination compounds and studied their physical and chemical behaviour. He proposed that, in coordination compounds, metals possess two types of valencies, viz. primary valencies, which are normally ionisable and secondary valencies which are non $-$ ionisable. ln a series of compounds of cobalt $(III)$ chloride with ammonia, it was found that some of the chloride ions could be precipitated as $\text{AgCl}$ on adding excess of $\ce{AgNO_3}$ solution in cold, but some remained in solution. The number ofions furnished by a complex in a solution can be determined by precipitation reactions. The measurement of molar conductance of solutions of coordination compounds helps to estimate the number of ions furnished by the compound in solution. In these questions $(Q$. No. $i-iv),$ a statement of assertion followed by a statement ofreason is given. Choose the correct answer out of the following choices.
  1. Assertion and reason both are correct statements and reason is correct explanation for assertion.
  2. Assertion and reason both are correct statements but reason is not correct explanation for assertion.
  3. Assertion is correct statement but reason is wrong statement.
  4. Assertion is wrong statement but reason is correct statement.
The following questions are multiple choice questions. Choose the most appropriate answer:
  1. Assertion : The complex $[\ce{Co(NH_3)_3Cl_3]}$ does not give precipitate with silver nitrate solution.
Reason : The given complex is non-ionisable.
  1. Assertion : The complex $\ce{[Co(NH_3)_4Cl_2]Cl}$ gives precipitate corresponding to $2$ mol of $\ce{AgCl}$ with $\ce{AgNO_3}$ solution.
Reason : It ionises as $\ce{[Co(NH_3)_4Cl_2]^+ + Cl}^-.$
  1. Assertion : $\ce{CoCl_3. 4NH_3}$ gives $1$ mol of $\ce{AgCl}$ on reacting with $\ce{AgNO_3},$ its secondary valency is $6$.
Reason : Secondary valency corresponds to coordination number.
  1. Assertion : $1$ mol of $\ce{[CrCl_2(H_2O)_4]Cl· 2H_2O}$ will give $1$ mol of $\ce{AgCl}$ on treating with $\ce{AgNO_3}.$
Reason : $ Cl^-$ ions satisfying secondary valanceis will not be precipitated.
  1. Assertion : $\ce{CoCl_3. 3NH_3}$ is not conducting while $\ce{CoCl_3. 5NH_3}$ is conducting.
Reason : The complex of $\ce{CoCl_3. 3NH_{3 }}$ is $\ce{[CoCl_3(NH_3)_3]}$ while that of $\ce{CoCl_3· 5NH_3}$ is $\ce{[CoCl(NH_3)_5]Cl_3}.$
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Q 25Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions: For understanding the structure and bonding in transition metal complexes, the magnetic properties are very helpful. Low spin complexes are generally diamagnetic because of pairing of electrons, whereas high spin complexes are usually paramagnetic because of presence of unpaired electrons. Larger the number of unpaired electrons, stronger will be the paramagnetism. However magnetic behaviour of a complex can be confirmed from magnetic moment measurement. Magnetic moment $\mu=\sqrt{\text{n(n+2)}}\text{B.M.}$ where $n =$ number of unpaired electrons. Greater the number of unpaired electrons, more will be the magnetic moment. In these questions $(Q$. No. $i-iv),$ a statement of assertion followed by a statement ofreason is given. Choose the correct answer out of the following choices.
  1. Assertion and reason both are correct statements and reason is correct explanation for assertion.
  2. Assertion and reason both are correct statements but reason is not correct explanation for assertion.
  3. Assertion is correct statement but reason is wrong statement.
  4. Assertion is wrong statement but reason is correct statement.
The following questions are multiple choice questions. Choose the most appropriate answer:
  1. Assertion : Both $\ce{[Cr(H_2O)_6]^{2+}}$ and $\ce{[Fe(H_2O)_6]^{2+}}$ have same magnetic moment.
Reason : Number of unpaired electrons in $Cr^{2+}$ and $Fe^{2+}$ are same.
  1. Assertion : $\ce{ [Fe(H_2O)_5NO]SO_4}$ is paramagnetic.
Reason : The $Fe$ in $\ce{[Fe(H_2O)_5NO]SO_4}$ has three unpaired electrons.
  1. Assertion : $\ce{[Co(en)_3]^{3+}}$ is paramagnetic.
Reason : It is an inner orbital complex.
  1. Assertion : $\ce{[Ni(CO)_4]}$ is diamagnetic and tetrahedral in shape.
Reason : $ \ce{[Ni(CO)_4]} $ contains no unpaired electrons and involves $\text{dsp}^2$ hybridisation.
  1. Assertion : $\ce{[Ni(CN)_4]^{2-}​​​​​​​}$ is diamagnetic complex.
Reason : It involves $\text{dsp}^2$ hybridisation and there is no unpaired electron.
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Q 275 Marks Questions5 Marks
Match the complex ions given in Column $I$ with the hybridisation and number of unpaired electrons given in Column $II$ and assign the correct code:
 
Column $I ($Complex ion$)$
 
Column $II ($Hybridisation, number of unpaired electrons$)$
$a.$ $\ce{[Cr(H_2O)_6]^{3+}}$ $1.$ $dsp^2, 1$
$b.$ $\ce{[Co(CN)_4]^{2-}}$ $2.$ $sp^3d^2, 5$
$c.$ $\ce{[Ni(NH_3)_6]^{2+}}$ $3.$ $d^2sp^3, 3$
$d.$ $\ce{[MnF_6]^{4-}}$ $4.$ $sp^3, 4$
 
 
$5.$
 $sp^3d^2, 2$
  • A
    $\ce{A (3), B (1), C (5), D (2)}.$
  • ✓
    $\ce{A (4), B (3), C (2), D (1)}.$
  • C
    $\ce{A (3), B (2), C (4), D (1)}.$
  • D
    $\ce{A (4), B (1), C (2), D (3)}.$

Answer: B.

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Q 285 Marks Questions5 Marks
Give the electronic configuration of the following complexes on the basis of Crystal Field Splitting theory. $\ce{[CoF_6]^{3-}, [Fe(CN)_6]^{4-}}$ and $\ce{[Cu(NH_3)_6]^{2+}}$
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Q 295 Marks Questions5 Marks
Match the complex ions given in Column $I$ with the colours given in Column $II$ and assign the correct code:
 
Column $I ($Complex ion$)$
 
Column $II ($Colour$)$
$a.$ $[Co(NH_3)_6]^{3+}$ $1.$
Violet
$b.$ $[Ti(H_2O)_6]^{3+}$ $2.$
Green
$c.$ $[Ni(H_2O)_6]^{2+}$ $3.$
Pale blue
$d.$ $[Ni(H_2O)_4(en)]^{2+} (aq)$ $4.$
Yellowish orange
 
 
 $5.$
Blue
Code:
  • A
    $\text{A (1), B (2), C (4), D (5).}$
  • B
    $\text{A (4), B (3), C (2), D (1).}$
  • C
    $\text{A (3), B (2), C (4), D (1).}$
  • ✓
    $\text{A (4), B (1), C (2), D (3).}$

Answer: D.

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Q 305 Marks Questions5 Marks
Match the coordination compounds given in Column $I$ with the central metal atoms given in Column $II$ and assign the correct code:
 
Column $I ($Coordination Compound$)$
 
Column $II ($Central metal atom$)$
$a.$
Chlorophyll
 $1.$
Rhodium
$b.$
Blood pigment
 $2.$
Cobalt
$c.$
Wilkinson catalyst
 $3.$
Calcium
$d.$
Vitamin $B_{12}$
 $4.$
Iron
 
 
 $5.$
Magnesium
Code:
  • ✓
    $\text{A (5), B (4), C (1), D (2).}$
  • B
    $\text{A (3), B (4), C (5), D (1).}$
  • C
    $\text{A (4), B (3), C (2), D (1).}$
  • D
    $\text{A (3), B (4), C (1), D (2).}$

Answer: A.

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