Chapter 13

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) \(\theta=175^{\circ}\)

Correct order of dipole moment is Clc1ccccc1Cl Cc1ccccc1C Oc1ccccc1O (1) (2) (3) (a) \(1=2=3\) (b) \(3<2<1\) (c) \(1<2<3\) (d) \(2<3<1\)

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: List I List II 1\. CIF \(_{3}\) (i) planar 2\. \(\mathrm{NF}_{3}\) (ii) pyramidal 3\. \(\mathrm{BF}_{3}\) (iii) T-shaped 4\. \(\left[\mathrm{CrF}_{3}\right] \mathrm{x}\) The correct matching is: 1 2 3 4 (a) (-) (iii) (ii) (i) (b) (iii) (ii) (i) (-) (c) (iii) (i) (ii) (iv) (d) (iii) (ii) (i) (ii)

Match the following: List I List II (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: \(1 \quad 2\) \(3 \quad 4\) (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 \(\mathrm{CuSO}_{4} .5 \mathrm{H}_{2} \mathrm{O} ?\) (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) \(\mathrm{l}\) and 3 (b) 2 and 4 (c) 1 and 2 (d) 1,2 and 3

Match the following: List I (Molecule) \(\quad\) 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\. ClF \(_{3}\) (iv) \(110^{\circ}\) (v) \(120^{\circ}\) The correct matching is: 1 2 34 (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) \(\mathrm{SF}_{4}\) (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

Consider the following type of energies and decide the correct order of magnitude. 1\. covalent single bond energy 2\. average translational kinetic energy of gases at room temperature 3\. rotational barrier energy in ethane between eclipsed and staggered forms 4\. ionization energy of hydrogen atom (a) \(4>1>3>2\) (b) \(4>1>2>3\) (c) \(2>1>4>3\) (d) \(4>3>2>1\)

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) 1 and 2 are correct (b) 1 and 3 are correct (c) 2 and 3 are correct (d) 1,2 and 3 are correct

Match the following: List I List II (Species) (Bond order) 1\. \(\mathrm{O}_{2}^{2+}\) (i) \(1.0\) 2\. \(\mathrm{O}_{2}\) (ii) \(2.0\) 3\. \(\mathrm{F}_{2}\) (iii) \(2.5\) 4\. \(\mathrm{O}_{2}^{+}\) (iv) \(3.0\) The correct matching is: \(\begin{array}{llll}1 & 2 & 3 & 4\end{array}\) (a) (iv) (i) (ii) (ii) (b) (ii) (iii) (i) (iv) (c) (iv) (ii) (i) (iii) (d) (iii) (iv) (i) (ii)

The halogen form compound among themselves with the formula \(\mathrm{AA}, \mathrm{AA}_{3}, \mathrm{AA}_{5}\) and \(\mathrm{AA}_{5}\), where \(\mathrm{A}\) is the heavier halogen. Which of the following pairs representing their structures and being polar and non-polar are correct? 1\. AA, linear, polar 2\. \(\mathrm{AA}_{3}\), T-shaped, polar 3\. \(\mathrm{AA}_{5}\), square pyramidal, polar 4\. AA \(_{7}\), pentagonal bipyramidal, non-polar (a) 1 and 3 are correct (b) 1,2 and 3 are correct (c) 2,3 and 4 are correct (d) \(1,2,3\) and 4 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) \(\mathrm{NH}_{3}\) \(\mathrm{sp}^{3}\) 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) \(\mathrm{C}_{6} \mathrm{H}_{3} \mathrm{Cl}_{2}\) 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

The electronegativity difference between \(\mathrm{N}\) and \(\mathrm{F}\) is greater than that between \(\mathrm{N}\) and \(\mathrm{H}\), yet the dipole moment of \(\mathrm{NH}_{3}(1.5 \mathrm{D})\) is larger than that of \(\mathrm{NF}_{3}\) \((0.2 \mathrm{D})\) This is because (a) in \(\mathrm{NH}_{3}\) as well as \(\mathrm{NF}_{3}\) the atomic dipole and bond dipole are in opposite directions (b) in \(\mathrm{NH}_{3}\) the atomic dipole and bond dipole are in the opposite directions whereas in \(\mathrm{NF}_{3}\) these are in the same direction (c) in \(\mathrm{NH}_{3}\) as well as in \(\mathrm{NF}_{3}\) the atomic dipole and bond dipole are in same direction (d) in \(\mathrm{NH}_{3}\) the atomic dipole and bond dipole and in the same direction whereas in \(\mathrm{NF}_{3}\) these are in opposite directions

According to molecular orbital theory which of the following statement about the magnetic character and bond order is correct regarding \(\mathrm{O}_{2}^{+}\)? (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\. \(\mathrm{m}\)-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 \(\leq\) Double bond \(<\) Triple bond.

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

Which of the following species have bond order \(3 ?\) (a) \(\mathrm{CN}^{-}\) (b) \(\mathrm{O}_{2}^{-}\) (c) \(\mathrm{NO}^{+}\) (d) \(\mathrm{CO}\)

When anions and cations approach each other, the valence shell of anions are pulled towards cation nucleus and thus, shape of anion is deformed. The phenomenon of deformation of anion by a cation is known as polarization and the ability of the cation to polarize the anion is called as polarizing power of cation. Due to polarization, sharing of electrons occurs between two ions to some extent and the bond shows some covalent character. 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.

When anions and cations approach each other, the valence shell of anions are pulled towards cation nucleus and thus, shape of anion is deformed. The phenomenon of deformation of anion by a cation is known as polarization and the ability of the cation to polarize the anion is called as polarizing power of cation. Due to polarization, sharing of electrons occurs between two ions to some extent and the bond shows some covalent character. 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.

When anions and cations approach each other, the valence shell of anions are pulled towards cation nucleus and thus, shape of anion is deformed. The phenomenon of deformation of anion by a cation is known as polarization and the ability of the cation to polarize the anion is called as polarizing power of cation. Due to polarization, sharing of electrons occurs between two ions to some extent and the bond shows some covalent character. In which of the halides, there is maximum polarization ? (a) \(\mathrm{AlBr}_{3}\) (b) \(\mathrm{AlF}_{3}\) (c) \(\mathrm{AlI}_{3}\) (d) \(\mathrm{AlCl}_{3}\)

When anions and cations approach each other, the valence shell of anions are pulled towards cation nucleus and thus, shape of anion is deformed. The phenomenon of deformation of anion by a cation is known as polarization and the ability of the cation to polarize the anion is called as polarizing power of cation. Due to polarization, sharing of electrons occurs between two ions to some extent and the bond shows some covalent character. Which is most volatile in nature? (a) \(\mathrm{AlCl}_{3}\) (b) \(\mathrm{CaCl}_{2}\) (c) \(\mathrm{NaCl}\) (d) \(\mathrm{MgCl}_{2}\)

When two oppositely charged ions approach each other, the ion smaller in size attracts outermost electrons of the other ion and repels its nuclear charge. The electron cloud of anion no longer remains symmetrical but is elongated towards the cation. Due to that, sharing of electrons occur between the two ions to some extent and the bond shows some covalent character. The value of dipole moment can be used for determining the amount of ionic character in a bond. Thus, percentage ionic character \(=\) \(\frac{\text { Experimental value of dipole moment }}{\text { Theoretical value of dipole moment }} \times 100\) 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) \(\mathrm{O} \cdot \mathrm{N}\), is \(+6\) \\\ (b) \(\mathrm{CCl}_{4}\) & (q) \(\mathrm{O} \cdot \mathrm{N}\). 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 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) sp \(^{3}\) hybridization (d) \(\mathrm{NO}_{2}^{-}\) (s) square planar (t) lone pair

Match the following \begin{tabular}{ll} \hline Column-I & Column-II \\ \hline \(\begin{aligned}&\text { (a) Aqueous solution is acidic } & \text { (p) } \mathrm{S}_{3} \mathrm{O}_{9} \\ &\text { (b) Detection of carbon monoxide } & \text { (q) } \mathrm{N}_{2} \mathrm{O}_{5} \\ &\text { (c) Having } \mathrm{M}-\mathrm{O}-\mathrm{M} \text { bond }(\mathrm{M} \text { is } \\ &\text { central atom) } & \text { (r) } \mathrm{P}_{4} \mathrm{O}_{10}\end{aligned}\) \\ \(\begin{array}{ll}\text { (d) On cooling form blue coloured } \\ \text { liquid } & \text { (s) } \mathrm{N}_{2} \mathrm{O}_{3} \\ \text { (t) } \mathrm{I}_{2} \mathrm{O}_{5}\end{array}\) \\ \hline \end{tabular}

Match the following \begin{tabular}{ll} \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}

Match the following Column-I Column-II (a) \(\mathrm{O}_{2}^{2+}\) (p) Paramagnetic (b) \(\mathrm{O}_{2}^{+}\) (q) Diamagnetic (c) \(\mathrm{O}_{2}^{-}\) (r) Bond order \(=1\) (d) \(\mathrm{O}_{2}^{2-}\) (s) Bond order \(=1.5\) (t) Stable ion under appropriate conditions in the gas or liquid phase.

Match the following Column-I (a) Oc1ccc(O)cc1 (b) CC=CC (c) \(\mathrm{CS}_{2}\) (d) \(\mathrm{PH}_{3}\) Column-II (p) \(\mu=0\) (q) sp \(^{2}\) hybridised atoms (r) sp \(^{3}\) hybridised atoms (s) sp hybridization (t) \(\mu \neq 0\)

The number of \(\sigma\) bonds in 1 -buten- 3 -yne is

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

Number of lone pairs of electrons present in central atom of \(\mathrm{ClF}_{2}\) 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 \(\mathrm{XeO}_{4}^{\circ}\)

The number of sp hybridized atoms in pseudohalogen cyanogens is /are