Chapter: Chemical Bonding and Molecular Structure

Which of the following compounds contain(s) no covalent bond(s) \(\begin{align}KCl,P{{H}_{3}},{{O}_{2}},{{B}_{2}}{{H}_{6}},{{H}_{2}}S{{O}_{4}}\end{align}\)?

Amongst LiCl, RbCl, \(\begin{align}BeC{{l}_{2}}\text{ }and\text{ }MgC{{l}_{2}}\end{align}\) the compounds with the greatest and the least ionic character, respectively are:

Which of these statements is not true?

Lattice energy of an ionic compound depends upon

ortho-Nitrophenol is less soluble in water than p- and m- nitrophenols because:

Among the following, the species having the smallest bond length is

Which one of the following pairs of species have the same bond order?

Which of the following hydrogen bonds is strongest?

The bond order in NO is 2.5 while that in \(\begin{align}N{{O}^{+}}\end{align}\) is 3. Which of the following statements is true for these two species?

An ether is more volatile than an alcohol having the same molecular formula. This is due to

The dipole moments of \(\begin{align}CC{{l}_{4}},\text{ }CHC{{l}_{{3\text{ }}}}and\text{ }C{{H}_{4}}\end{align}\) are in the order:

Which compound exhibits maximum dipole moment among the following?

Molecule AB has a bond length of 1.617Å and a dipole moment of 0.38 D. The fractional charge on each atom (absolute magnitude) is: (\(\displaystyle {{e}_{0}}=4.802\times {{10}^{{-10}}}esu\))

The correct order of bond dissociation energy among \(\begin{align}{{N}_{2}},~{{O}_{2}},\text{ }O_{2}^{-}\end{align}\) is shown in which of the following arrangements?

Which one of the following molecules is polar?

Bond distance in HF is m. Dipole moment of HF is Cm. The percentage ionic character in HF will be: (electron charge = C)

Among the following chloro-compound having the lowest dipole moment is

Although ion and \(\begin{align}{{N}_{2}}\end{align}\) molecule are isoelectronic, yet \(\begin{align}{{N}_{2}}\end{align}\) molecule is chemically inert because of

The charge/size ratio of a cation determines its polarizing power. Which one of the following sequences represents the increasing order of the polarizing power of the cationic species, \(\begin{align}{{K}^{+}},C{{a}^{{2+}}},M{{g}^{{2+}}},B{{e}^{{2+}}}\end{align}\)?

Which one of the following pairs of molecules will have permanent dipole moments for both members?

The compound that has the largest H – M – H bond angle (M = N, S, C), is:

The molecule in which hybrid MOs involve only one d-orbital of the central atom is:

If \(\begin{align}A{{B}_{4}}\end{align}\) molecule is a polar molecule, a possible geometry of \(\begin{align}A{{B}_{4}}\end{align}\) is:

The shape/ structure of and \(\begin{align}Xe{{O}_{3}}{{F}_{2}}\end{align}\), respectively, are:

The molecular geometry of \(\begin{align}S{{F}_{6}}\end{align}\) is octahedral. What is the geometry of \(\begin{align}S{{F}_{4}}\end{align}\) (including lone pair(s) of electrons, if any)?

The correct statement about \(\begin{align}IC{{l}_{5}}\end{align}\) and \(\begin{align}ICl_{4}^{-}\end{align}\) is:

The ion that has \(\begin{align}s{{p}^{3}}{{d}^{2}}\end{align}\) hydridisation for the central atom, is:

Total number of lone pair of electrons in \(\begin{align}I_{3}^{-}\end{align}\) ion is :

Which of the following conversions involves change in both shape and hybridisation?

The incorrect geometry is represented by __________.

Identify the pair in which the geometry of the species is Tshape and square pyramidal, respectively

The decreasing order of bond angles in \(\begin{align}B{{F}_{3}},\text{ }N{{H}_{3}},\text{ }P{{F}_{3}}\text{ }and~I~_{3}^{-}\end{align}\) is:

\(\begin{align}s{{p}^{3}}{{d}^{2}}\end{align}\) Hybridisation is not displayed by:

The group having triangular planar structures is:

The species in which the N atom is in a state of sp hybridisation is:

The group of molecules having identical shape is:

The bond angle H–X–H is the greatest in the compound:

The number and type of bonds in \(\begin{align}C_{2}^{{2-}}\end{align}\) ion in \(\begin{align}Ca{{C}_{2}}\end{align}\) are:

Which of the following molecules has two sigma (\(\begin{align}\sigma \end{align}\)) and two pi (\(\begin{align}\pi \end{align}\)) bonds?

The shape of \(\begin{align}IF_{6}^{-}\end{align}\) is:

In which of the following sets, all the given species are isostructural?

In which of the following pairs, the two species are not isostructural?

The formation of molecular complex results in a change in hybridisation of boron

Which of the following has the square planar structure?

Among the following species which two have trigonal bipyramidal shape?
(I) \(\begin{align}N{{I}_{3}}\end{align}\)
(II) \(\begin{align}I_{3}^{-}\end{align}\)
(III) \(\begin{align}SO_{3}^{{2-}}\end{align}\)
(IV) \(\begin{align}NO_{3}^{-}\end{align}\)

The bond dissociation energy of B – F in \(\begin{align}B{{F}_{3}}\end{align}\) is 646 kJ \(\begin{align}mo{{l}^{{-1}}}\end{align}\), whereas that of C – F in \(\begin{align}C{{F}_{4}}\end{align}\) is 515 kJ \(\begin{align}mo{{l}^{{-1}}}\end{align}\). The correct reason for higher B – F bond dissociation energy as compared to that of C – F bond is

In which of the following molecules/ions are all the bonds not equal?

The decreasing values of bond angles from \(\begin{align}N{{H}_{{3\text{ }}}}\left( {106{}^\text{o}} \right)\text{ }to~Sb{{H}_{{3\text{ }}}}\left( {101{}^\text{o}} \right)\end{align}\) down group-15 of the periodic table is due to

The correct order of bond angles (smallest first) in \(\begin{align}{{H}_{2}}S,~N{{H}_{3}},\text{ }B{{F}_{3}}\text{ }and\text{ }Si{{H}_{4}}\end{align}\) is

The states of hybridization of boron and oxygen atoms in boric acid (\(\begin{align}{{H}_{3}}B{{O}_{3}}\end{align}\)) are respectively

Which one of the following has the regular tetrahedral structure?

The maximum number of 90º angles between bond pairbond pair of electrons is observed in

Which one of the following compounds has the smallest bond angle in its molecule?

The pair of species having identical shapes for molecules of both species is

In which of the following species the interatomic bond angle is 109° 28’?

Hybridisation of the underline atom changes in:

The potential energy curve for the H2 molecule as a function of internuclear distance is:

The structure of PCl₅ in the solid state is:

Of the species, the one with minimum bond strength is:

If the magnetic moment of a dioxygen species is 1.73 B.M, it may be:

The bond order and the magnetic characteristics of are:

During the change of \(\begin{align}{{O}_{2}}\text{ to }O_{2}^{-}\end{align}\), the incoming electron goes to the orbital:

Among the following, the molecule expected to be stabilised by anion formation is: \(\begin{align}{{C}_{2}},\text{ }{{O}_{2}},\text{ }NO,\text{ }{{F}_{2}}~\end{align}\)

Among the following species, the diamagnetic molecule is:

Among the following molecules/ions,
\(\begin{align}C_{2}^{{2-}},N_{2}^{{2-}},O_{2}^{{2-}},{{O}_{2}}\end{align}\)
Which one is diamagnetic and has the shortest bond length?

Two pi and half sigma bonds are present in:

According to molecular orbital theory, which of the following is true with respect to \(\begin{align}L{{i}_{2}}^{+}\end{align}\) and \(\begin{align}L{{i}_{2}}^{-}\end{align}\)?

In which of the following processes, the bond order has increased and paramagnetic character has changed to diamagnetic?

According to molecular orbital theory, which of the following will not be a viable molecule?

\(\begin{align}\begin{array}{l}\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,(I)\,\,\,\,(II)\\H-N—N—N~\end{array}\end{align}\)
In hydrogen azide, the bond orders of bonds (I) and (II) are _________.

Which of the following best describes the diagram of molecular orbital?

In the molecular orbital diagram for the molecular ion, \(\begin{align}N_{2}^{+}\end{align}\), the number of electrons in the \(\begin{align}{{\sigma }_{{2p}}}\end{align}\) molecular orbital is:

Which of the following is paramagnetic?

Which of the following species is not paramagnetic?

After understanding the assertion and reason, choose the correct option.
Assertion: In the bonding molecular orbital (MO) of H2, electron density is increased between the nuclei.
Reason: The bonding MO is \(\begin{align}{{\psi }_{A}}+{{\psi }_{B}}\end{align}\), which shows destructive interference of the combining electron waves.

Which one of the following properties is not shown by NO?

Which one of the following molecules is paramagnetic?

Which of the following has unpaired electron(s)?

In which of the following pairs of molecules/ions, both the species are not likely to exist?

Which one of the following molecules is expected to exhibit diamagnetic behaviour?

Which of the following is the wrong statement

Stability of the species \(\begin{align}L{{i}_{2}},\text{ }Li_{2}^{-}\text{ }and\text{ }Li_{2}^{+}\end{align}\) increases in the order of:

In which of the following ionization processes the bond energy has increased and also the magnetic behaviour has changed from paramagnetic to diamagnetic?

Bond order normally gives idea of stability of a molecular species. All the molecules viz. \(\begin{align}{{H}_{2}},\text{ }L{{i}_{2}}\text{ }and\text{ }{{B}_{2}}\end{align}\)have the same bond order yet they are not equally stable. Their stability order is

The internuclear distances in O – O bonds for \(\begin{align}O_{2}^{+},{{O}_{2}},O_{2}^{-}\end{align}\) and \(\begin{align}O_{2}^{{2-}}\end{align}\) respectively are:

The number of types of bonds between two carbon atoms in calcium carbide is:

Using MO theory, predict which of the following species has the shortest bond length?

Which of the following species exhibits the diamagnetic behaviour?

In which of the following ionization processes, the bond order has increased and the magnetic behaviour has changed?

Which of the following molecules/ions does not contain unpaired electrons?

Which of the following species is diamagnetic in nature?

Which of the following are arranged in an increasing order of their bond strength?