Chapter 13

The common features among the species \(\mathrm{CN}^{-}, \mathrm{CO}\) and \(\mathrm{NO}^{+}\)are (a) bond order three and isoelectronic (b) bond order three and weak field ligands (c) bond order two and \(\pi\)-acceptors (d) isoelectronic and weak field ligands.

The correct order of increasing \(\mathrm{C}-\mathrm{O}\) bond length of \(\mathrm{CO}, \mathrm{CO}_{3}^{2-}, \mathrm{CO}_{2}\) is (a) \(\mathrm{CO}_{3}^{2-}<\mathrm{CO}_{2}<\mathrm{CO}\) (b) \(\mathrm{CO}_{2}<\mathrm{CO}_{3}^{2^{2}}<\mathrm{CO}\) (c) \(\mathrm{CO}<\mathrm{CO}_{3}^{2-}<\mathrm{CO}_{2}\) (d) \(\mathrm{CO}<\mathrm{CO}_{2}<\mathrm{CO}_{2}^{2-}\)

KF combines with HF to form \(\mathrm{KHF}_{2}\). The compound contains the species (a) \(\mathrm{K}^{+}, \mathrm{F}\) and \(\mathrm{H}^{\prime}\) (b) \(\mathrm{K}^{+}, \mathrm{F}^{-}\)and \(\mathrm{HF}\) (c) \(\mathrm{K}^{\prime}\) and \(\left[\mathrm{HF}_{2}\right]\) (d) \([\mathrm{KHF}]^{+}\)and \(\mathrm{F}_{2}\)

The following compounds are to be arranged in order of their increasing thermal stabilities. Identify the correct order. 1\. \(\mathrm{K}_{2} \mathrm{CO}_{3}\) 2\. \(\mathrm{MgCO}_{3}\) 3. \(\mathrm{CaCO}_{3}\) 4\. \(\mathrm{BeCO}_{3}\) (a) \(1<2<3<4\) (b) \(4<2<3<1\) (c) \(4<2<1<3\) (d) \(2<4<3<1\)

Among the following species, identify the isostructural pairs \(\mathrm{NF}_{3}, \mathrm{NO}_{3}^{-}, \mathrm{BF}_{3}, \mathrm{H}_{3} \mathrm{O}^{+}, \mathrm{HN}_{3}\) (a) \(\left[\mathrm{NF}_{3}, \mathrm{NO}_{3}^{-}\right]\)and \(\left[\mathrm{BF}_{3}, \mathrm{H}_{3} \mathrm{O}^{+}\right]\) (b) \(\left[\mathrm{NF}_{3}, \mathrm{HN}_{3}\right]\) and \(\left[\mathrm{NO}_{3}^{-}, \mathrm{BF}_{3}\right]\) (c) \(\left[\mathrm{NF}_{3}, \mathrm{H}_{3} \mathrm{O}^{+}\right]\)and \(\left[\mathrm{NO}_{3}^{-}, \mathrm{BF}_{3}\right]\) (d) \(\left[\mathrm{NF}, \mathrm{H}_{3} \mathrm{O}^{+}\right]\)and \(\left[\mathrm{HN}_{3}, \mathrm{BF}_{3}\right]\)

9\. Which type of bond is not present in HNO \(_{2}\) molecule? (a) covalent (b) coordinate (c) ionic (d) ionic as well as coordinate

The molecules that will have dipole moment (1) 2,2 -dimethylpropane (2) trans-1-pent-2-ene (3) cis-hex-3-ene (4) \(2,2,3,3\)-tetramethylbutane (a) 2,3 (b) 1,3 (c) \(1,2,3\) (d) all of these

The linear structure is seen in (i) \(\mathrm{SnCl}_{2}\) (ii) \(\mathrm{NCO}^{-}\) (iii) \(\mathrm{NO}_{2}\) (iv) \(\mathrm{CS}_{2}\) (a) (i), (ii) and (iii) (b) (ii), (iii) and (iv) (c) (i), (iii) and (iv) (d) none of these

Which bond angle \(\theta\), would result in the maximum dipole moment for the triatomic molecule \(\mathrm{XY}_{2}\) shown below? (a) \(\theta=120^{\circ}\) (b) \(\theta=90^{\circ}\) (c) \(\theta=145^{\circ}\) (d) \(\theta=175^{\circ}\)

Which bond angle \(\theta\), would result in the maximum dipole moment for the triatomic molecule \(\mathrm{XY}_{2}\) shown below? (a) \(\theta=120^{\circ}\) (b) \(\theta=90^{\circ}\) (c) \(\theta=145^{\circ}\) (d) \(\theta=175^{\circ}\)

Match the following: \(\begin{array}{ll}\text { List I } & \text { List II }\end{array}\) (Hydridization) \(\quad\) (Geometry of the molecule) 1\. \(\mathrm{sp}^{2}\) (i) trigonal bipyramidal 2\. \(\mathrm{sp}^{3}\) (ii) planar trigonal 3\. sp (iii) octahedral 4. (iv) tetrahedral (v) linear The correct matching is: \(\begin{array}{lll}1 & 2 & 3\end{array}\) 4 (a) (ii) (iv) (v) (i) (b) (iii) (v) (i) (vi) (c) (iv) (iii) (i) (ii) (d) (vi) (ii) (v) (iii)

Consider the following statements: 1\. the bond order of \(\mathrm{NO}\) is \(2.5\) 2\. the bond order of \(\mathrm{NO}^{+}\)is 3 3\. the bond order of \(\mathrm{O}_{2}\) is \(1.5\) 4\. the bond order of \(\mathrm{CO}\) is 3 Which of these statements are correct? (a) 1,2 and 3 (b) 2,3 and 4 (c) 1,3 and 4 (d) 1,2 and 4

Match the following: \(\begin{array}{ll}\text { List I } & \text { List II }\end{array}\) (Species) (Hybridization) 1\. \(\mathrm{BCI}_{3}\) (i) \(\mathrm{sp}^{3}\) 2\. \(\mathrm{NH}_{3}\) (ii) \(\mathrm{sp}^{3} \mathrm{~d}^{2}\) 3\. \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\) (iii) \(\mathrm{sp}^{2}\) 4\. \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (iv) \(\mathrm{sp}^{2} \mathrm{~d}\) The correct matching is: \(\begin{array}{lll}1 & 2 & 3\end{array}\) 4 (a) (iii) (i) (iv) (ii) (b) (i) (iii) (ii) (iv) (c) (i) (iii) (iv) (ii) (d) (iii) (i) (ii) (iv)

Match the following: \(\begin{array}{ll}\text { List I } & \text { List II }\end{array}\) (Compounds) (Structures) 1\. \(\mathrm{CS}_{2}\) (i) Bent 2\. \(\mathrm{SO}_{2}\) (ii) Linear 3\. \(\mathrm{BF}_{3}\) (iii) Trigonal planar 4\. \(\mathrm{NH}_{3}\) (iv) Tetrahedral (v) Trigonal pyramidal The correct matching is: 1 \(2 \quad 3 \quad 4\) (a) (i) (ii) (iv) (v) (b) (ii) (i) (iii) (v) (c) (i) (ii) (v) (iv) (d) (ii) (i) (v) (iv)

Which of the following types of bonds are present in \(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O} ?\) (1) electrovalent (2) covalent (3) coordinate Select the correct answer using the code given below. (a) 1 and 2 only (b) 1 and 3 only (c) 1,2 and 3 (d) 2 and 3 only

In which one of the following pairs, molecules/ions have similar shape? (a) \(\mathrm{CCl}_{4}\) and \(\mathrm{PtCl}_{4}\) (b) \(\mathrm{NH}_{3}\) and \(\mathrm{BF}_{3}\) (c) \(\mathrm{BF}_{3}\) and t-butyl carbonium ion (d) \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\)

Which of the following are non-polar? (1) \(\mathrm{SiF}_{4}\) (2) \(\mathrm{XeF}_{4}\) (3) \(\mathrm{SF}_{4}\) (4) \(\mathrm{BF}_{3}\) (5) \(\mathrm{NF}_{3}\) Select the correct answer using the code given below: (a) 1,2 and 4 (b) 3,4 and 5 (c) 2,3 and 4 (d) 1,3 and 4

Consider the following type of bonds: (1) ionic (2) covalent (3) coordinate (4) hydrogen bond Which type of bonds are present in \(\mathrm{NaHCO}_{3}\) ? (a) 1 and 3 (b) 2 and 4 (c) 1 and 2 (d) 1,2 and 3

Match the following: List I (Molecule) List II (Bond angle) 1\. \(\mathrm{BF}_{3}\) (i) \(88^{\circ}\) 2\. \(\mathrm{NF}_{3}\) (ii) \(96^{\circ}\) 3\. \(\mathrm{PF}_{3}\) (iii) \(103^{\circ}\) 4\. \(\mathrm{ClF}_{3}\) (iv) \(110^{\circ}\) (v) \(120^{\circ}\) The correct matching is: \(1 \quad 2\) \(\begin{array}{ll}3 & 4\end{array}\) (a) (iv) (iii) (ii) (i) (b) (v) (iii) (ii) (i) (c) (iv) (iii) (v) (ii) (d) (iii) (iv) (i) (ii)

Which are the species in which sulphur undergoes \(\mathrm{sp}^{3}\) hybridization? (1) SF \(_{4}\) (2) \(\mathrm{SCl}_{2}\) (3) \(\mathrm{SO}_{4}^{2-}\) (4) \(\mathrm{H}_{2} \mathrm{~S}\) Select the correct answer using the code given below: (a) 1 and 2 (b) 2,3 and 4 (c) 1,3 and 4 (d) 1,2 and 3

Which of the following species have undistorted octahedral structures? (1) \(\mathrm{SF}_{6}\) (2) \(\mathrm{PF}_{6}^{-}\) (3) \(\mathrm{SiF}_{6}^{2-}\) (4) \(\mathrm{XeF}_{6}\) Select the correct answer using the codes given below: (a) 1,3 and 4 (b) 1,2 and 3 (c) 1,2 and 4 (d) 2,3 and 4

Consider the given statements about the molecule \(\left(\mathrm{H}_{3} \mathrm{C}\right)_{2} \mathrm{CH}-\mathrm{CH}=\mathrm{CH}-\mathrm{C} \equiv \mathrm{C}-\mathrm{CH}=\mathrm{CH}_{2}\) 1\. Three carbon atoms are sp \(^{3}\) hybridized 2\. Three carbon atoms are sp \(^{2}\) hybridized 3\. Two carbon atoms are sp hybridized Of three statements (a) \(\mathrm{I}\) and 2 are correct (b) \(\mathrm{I}\) and 3 are correct (c) 2 and 3 are correct (d) 1,2 and 3 are correct

Consider the following molecules or ions. (i) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) (ii) \(\mathrm{NH}_{4}^{+}\) (iii) \(\mathrm{SO}_{4}^{2}-\) (iv) \(\mathrm{ClO}_{4}^{-}\) (v) \(\mathrm{NH}_{3}\) sp \(^{3}\) hybridization is involved in the formation of (a) (i), (ii), (v) only (b) (i), (ii) only (c) (i), (ii), (iii), (iv) (d) (i), (ii), (iii), (iv), (v)

Consider the following halogen containing compounds (i) \(\mathrm{CHCl}_{3}\) (ii) \(\mathrm{CCl}_{4}\) (iii) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) (iv) \(\mathrm{CH}_{3} \mathrm{Cl}\) (v) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{Cl}_{2}\) The compounds with a net zero dipole moment are (a) (ii) and (v) only (b) (iii) only (c) (iii) and (iv) only (d) (iv) only

According to molecular orbital theory which of the following statement about the magnetic character and bond order is correct regarding \(\mathrm{O}_{2}^{1}\) ? (a) paramagnetic and bond order \(<\mathrm{O}_{2}\) (b) paramagnetic and bond order \(>\mathrm{O}_{2}\) (c) diamagnetic and bond order \(<\mathrm{O}_{2}\) (d) diamagnetic and bond order \(>\mathrm{O}_{2}\)

Pick out the isoelectronic structures from the following: 1\. \(\mathrm{CH}_{3}\) 2\. \(\mathrm{H}_{3} \mathrm{O}^{+}\) 3\. \(\mathrm{NH}_{3}\) 4\. \(\mathrm{CH}_{3}^{-}\) (a) 1 and 2 (b) 3 and 4 (c) 1 and 3 (d) 2,3 and 4

Arrange the following compounds in order of increasing dipole moment 1\. Toluene, 2\. m-dichlorobenzene 3\. o-dichlorobenzene, 4\. p-dichlorobenzene (a) \(1<4<2<3\) (b) \(4<1<2<3\) (c) \(4<1<3<2\) (d) \(4<2<1<3\)

Species having the same bond order are (a) \(\mathrm{N}_{2}\) (b) \(\mathrm{N}_{2}^{+}\) (c) \(\mathrm{N}_{2}^{-}\) (d) \(\mathrm{N}_{2}^{2-}\)

Mark out the incorrect match of shape for a given molecule/ion. (a) \(\mathrm{ICl}_{4}^{-}-\)square planar (b) \(\mathrm{NH}_{2}^{-}-\)Pyramidal (c) \(\mathrm{SF}_{4}-\) See \(-\) saw shape (d) \(\mathrm{XeOF}_{2}-\) Trigonal planar

Which of the pairs have identical values of bond order? (a) \(\mathrm{F}_{2}\) and \(\mathrm{Ne}_{2}\) (b) \(\mathrm{N}_{2}^{+}\)and \(\mathrm{O}_{2}^{+}\) (c) \(\mathrm{O}_{2}^{2-}\) and \(\mathrm{B}_{2}\) (d) \(\mathrm{C}_{2}\) and \(\mathrm{N}_{2}\)

Isostructural group of molecule is (a) \(\mathrm{XeO}_{4}, \mathrm{NH}_{4}^{+}, \mathrm{CH}_{4}\) (b) \(\mathrm{CH}_{3}^{-}, \mathrm{NH}_{3}, \mathrm{NF}_{3}\) (c) \(\mathrm{NH}_{3}, \mathrm{NF}_{3}, \mathrm{BF}_{3}\) (d) \(\mathrm{NO}_{3}, \mathrm{NO}_{2}, \mathrm{SF}_{4}\)

The correct statements if the following are: (a) The bond angle of hybrid bonds increases as \(\mathrm{sp}^{3}<\) \(\mathrm{sp}^{2}<\mathrm{sp}\) (b) For hydrogen halides, bond length increases as \(\mathrm{HF}<\mathrm{HCl}<\mathrm{HBr}<\mathrm{HI} .\) (c) Increasing order of bond energy : Single bond \(<\) Double bond \(<\) Triple bond.

In \(\mathrm{O}_{2}\) molecule which of the following molecular orbitals are lower in energy than \(\sigma 2 \mathrm{p}_{z}\) orbital (a) \(\sigma 2 \mathrm{~s}\) (b) \(\pi_{2 p x}\) (c) \(\pi_{2 p y}\) (d) \(\sigma^{*} 2 \mathrm{~s}\)

Which combination of the compound and their shapes are correct? (a) \(\mathrm{ClF}_{3}-\) see saw (b) \(\mathrm{ICl}_{4}^{-}-\)square planar (c) \(\mathrm{ICl}_{3}-\mathrm{T}-\) shaped (d) \(\mathrm{I}_{3}^{-}\)- linear

The magnitude of polarization depends upon a number of factors. These factors were suggested by Fajan and are known as Fajan's rule. (a) Greater is the polarization in a molecule, more is covalent character. (b) As the charge on cation increases, its tendency to polarize the anion increases (c) As the size of the cation decreases or size of the anion increases, the polarization increases. (d) All of these.

Considering \(\mathrm{BeCl}_{2}, \mathrm{MgCl}_{2}, \mathrm{CaCl}_{2}\) and \(\mathrm{BaCl}_{2}\), predict which of the following statement is true? (a) Covalent character increases as the atomic number of the metal atom increases (b) \(\mathrm{BeCl}_{2}\) is least ionic out of the given chlorides. (c) \(\mathrm{BeCl}_{2}\) has the highest melting point among the given chlorides. (d) All are highly ionic compound.

In which of the halides, there is maximum polarization ? (a) \(\mathrm{AlBr}_{3}\) (b) \(\mathrm{AlF}_{3}\) (c) \(\mathrm{AlI}_{3}\) (d) \(\mathrm{AlCl}_{3}\)

Which one of the following compounds shows most covalent character? (a) \(\mathrm{MgCl}_{2}\) (b) \(\mathrm{AlCl}_{3}\) (c) \(\mathrm{NaCl}\) (d) All are equally covalent

The compound having highest dipole moment is (a) \(\mathrm{H}_{2} \mathrm{~S}\) (b) \(\mathrm{SO}_{2}\) (c) \(\mathrm{NH}_{3}\) (d) \(\mathrm{H}_{2} \mathrm{O}\)

The dipole moment of \(\mathrm{LiH}\) is \(1.964 \times 10^{-29} \mathrm{C} . \mathrm{m} .\) and the interatomic distance between \(\mathrm{Li}\) and \(\mathrm{H}\) in this molecule is \(1.596 \AA\). What is the \% ionic character in \(\mathrm{LiH} ?\) (a) \(76.8 \%\) (b) \(60.25 \%\) (c) \(15.5 \%\) (d) \(26.2 \%\)

Match the following \begin{tabular}{ll} \hline Column-I & Column-II \\ \hline (a) \(\mathrm{NH}_{4}^{+}\) & (p) O.N. is \(+6\) \\ (b) \(\mathrm{CCl}_{4}\) & (q) O.N. is \(-1\) \\ (c) \(\mathrm{CaOCl}_{2}\) & (r) \(\mu=0.0 \mathrm{D}\) \\ (d) \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) & (s) Coordinate covalent bond \\ & (t) O.N. is \(+1\) \end{tabular}

Match the following Column-I \(\quad\) Column-II (a) \(\mathrm{NH}_{2}^{-}\) (p) Bent shape (b) \(\mathrm{XeF}_{4}\) (q) \(\mathrm{AB}_{2} \mathrm{E}_{2}\) (c) \(\mathrm{CH}_{3}^{-}\) (r) \(\mathrm{sp}^{3}\) hybridization (d) \(\mathrm{NO}_{2}^{-}\) (s) square planar (t) lone pair

Match the following Column-I Column-II (a) \(\mathrm{KHF}_{2}\) (p) Compound can exist (b) \(\mathrm{KHCl}_{2}\) (q) Compound is electrolyte in nature (r) Compound shows hydrogen (c) \(\mathrm{NF}_{3}\) bonding (d) \(\mathrm{PH}_{5}\) (s) Compound is non electrolyte (t) Compound can not exist.

\begin{tabular}{ll} \hline Match the following & \\ \hline Column-I & Column-II \\ \hline (a) Electrovalent bond & (p) \(\mathrm{NH}_{4} \mathrm{Cl}\) \\ (b) Covalent bond & (q) \(\mathrm{CaOCl}_{2}\) \\ (c) Co-ordinate bond & (r) \(\mathrm{KHF}_{2}\) \\ (d) Hydrogen bond & (s) \(\mathrm{N}_{2} \mathrm{O}_{5}\) \\ & (t) \(\mathrm{CuSO}_{4} .5 \mathrm{H}_{2} \mathrm{O}\) \\ \hline \end{tabular}

Of the following, the number of species having two and more than two electrons in the antibonding molecular orbital is \(\mathrm{He}_{2}, \mathrm{He}_{2}^{\prime}, \mathrm{B}_{2}, \mathrm{O}_{2}^{-}, \mathrm{N}_{2}\)

Number of lone pairs of electrons present in central atom of \(\mathrm{ClF}\), is

Among \(\mathrm{BF}_{3}, \mathrm{NF}_{3}, \mathrm{PH}_{3}, \mathrm{IF}_{3}, \mathrm{IF}_{5}\) and \(\mathrm{SF}_{4}\), the number of species having the same number of lone pair of electrons on the central atom is

How many lone pairs are there at xenon in XeOF \(_{4}\) ?

Of the following the number of species having unpaired electron are \(\mathrm{B}_{2}, \mathrm{KO}_{2}, \mathrm{BaO}_{2}, \mathrm{NO}_{2}, \mathrm{O}_{2}, \mathrm{ClO}_{2}, \mathrm{O}_{2}\left[\mathrm{AsF}_{6}\right]\)

Find the total number of \(\mathrm{p} \pi-\mathrm{d} \pi\) bonds present in \(\mathrm{XeO}_{4}^{.}\)