The solubility of ${\rm{KCl}}$ is relatively more in (where $D$ is dielectric constant):

${\rm{C}}{{\rm{H}}_3}{\rm{OH}}\left( {{\rm{D}} = 32} \right)$

${{\rm{C}}_6}{{\rm{H}}_6}({\rm{D}} = 0)$

${\left( {{\rm{C}}{{\rm{H}}_3}} \right)_2}{\rm{CO}}\left( {{\rm{D}} = 2} \right)$

${\rm{CC}}{{\rm{l}}_4}\left( {{\rm{D}} = 0} \right)$

${\rm{C}} - {\rm{Cl}}$ bond is stronger than ${\rm{C}}-{\rm{I}}$ bond, because

${\rm{C}} - {\rm{Cl}}$ bond is more ionic than ${\rm{C}}-{\rm{I}}$

${\rm{C}} - {\rm{Cl}}$ bond is polar covalent bond

${\rm{C}} - {\rm{Cl}}$ bond is more covalent than ${\rm{C}}-{\rm{I}}$

${\rm{C}} - {\rm{Cl}}$ bond length is longer than ${\rm{C}}-{\rm{I}}$

Correct order of bond angles in ${\rm{N}}{{\rm{H}}_3}$, ${\rm{PC}}{{\rm{l}}_3}$ and ${\rm{BC}}{{\rm{l}}_3}$ is

${\rm{BC}}{{\rm{l}}_3} > N{{\rm{H}}_3} > PC{{\rm{l}}_3}$

${\rm{PC}}{{\rm{l}}_3} > N{{\rm{H}}_3} > BC{{\rm{l}}_3}$

${\rm{N}}{{\rm{H}}_3} > BC{{\rm{l}}_3} > PC{{\rm{l}}_3}$

${\rm{N}}{{\rm{H}}_3} > PC{{\rm{l}}_3} > BC{{\rm{l}}_3}$

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Chemical bonding & molecular structure practice · Mixed difficulty

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211 Easy

211 of 579

Application +4 | -1

Which has

s{p^2}

-hybridisation?

View answer and explanation

Correct option: B

\mathrm{S}{\mathrm{O}_2}

Option B (

\mathrm{S}{\mathrm{O}_2}

) is correct because sulfur has one lone pair and two bond pairs, resulting in

sp^2

hybridization.

212 Medium

212 of 579

Remembering +4 | -1

The shape of carbon dioxide is

View answer and explanation

Correct option: D

linear

Option D (linear) is correct because carbon dioxide (

CO_2

) has a linear shape due to the

sp

hybridization of the central carbon atom and two double bonds to oxygen atoms.

213 Medium

213 of 579

Understanding +4 | -1

Which molecule is planar?

View answer and explanation

Correct option: C

{\mathrm{C}_2}{\mathrm{H}_4}

Option C (

{\mathrm{C}_2}{\mathrm{H}_4}

) is correct because ethylene (

C_2H_4

) has a planar structure due to the double bond between the two carbon atoms, forcing all atoms to lie in the same plane.

214 Easy

214 of 579

Application +4 | -1

In which of the following set all molecules have equal bond order?

View answer and explanation

Correct option: C

{H_2},L{i_2},{B_2}

Option C (

{H_2},L{i_2},{B_2}

) is correct because all three molecules have a bond order of 1.

215 Medium

215 of 579

Understanding +4 | -1

The solubility of

\mathrm{KCl}

is relatively more in (where

D

is dielectric constant):

View answer and explanation

Correct option: C

\mathrm{C}{\mathrm{H}_3}\mathrm{OH}\left( {\mathrm{D} = 32} \right)

Option C (

\mathrm{CH}_3\mathrm{OH}(\mathrm{D} = 32)

) is correct because KCl, being an ionic compound, dissolves more in polar solvents with higher dielectric constants.

216 Medium

216 of 579

Application +4 | -1

The bond order is not three for

View answer and explanation

Correct option: A

{N}_2^{+}

Option A (

{N}_2^{+}

) is correct because its bond order is 2.5, while the bond order of the other options is 3.

217 Medium

217 of 579

Analyzing +4 | -1

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

View answer and explanation

Correct option: C

\mathrm{N}{\mathrm{O}_2}

and

{\mathrm{O}_3}

Option C (

\mathrm{N}{\mathrm{O}_2}

and

{\mathrm{O}_3}

) is correct because both nitrogen dioxide (

\mathrm{N}{\mathrm{O}_2}

) and ozone (

{\mathrm{O}_3}

) have bent structures, leading to a non-zero net dipole moment.

218 Easy

218 of 579

Analyzing +4 | -1

Assertion : lonic reactions are not instantaneous.

Reason : Oppositely charged ions exert strong forces.

View answer and explanation

Correct option: D

If assertion is false but reason is true

Option D is correct because ionic reactions are generally very fast (instantaneous), so the assertion is false, but the reason is true because oppositely charged ions do exert strong electrostatic forces.

219 Medium

219 of 579

Understanding +4 | -1

Strongest bond is formed by the head on overlapping of:

View answer and explanation

Correct option: B

2p

and

2p

-orbitals

Option B (

2p

and

2p

-orbitals) is correct because head-on overlapping of p-orbitals forms a sigma bond, which is stronger than bonds formed by s-orbitals.

220 Hard

220 of 579

Understanding +4 | -1

The minimum number of

90^\circ

angle between hybrid orbitals is observed in

View answer and explanation

Correct option: C

ds{p^2}

Option C (dsp2) is correct because dsp2 hybridization results in a square planar geometry, which has four 90° angles.

221 Easy

221 of 579

Analyzing +4 | -1

Assertion : The bond between two identical nonmetal atoms has a pair of electrons with identical spin.

Reason : Electrons are transferred fully from one atom to another.

View answer and explanation

Correct option: D

If the assertion and reason both are false.

Option D (If the assertion and reason both are false) is correct because the bond between two identical nonmetal atoms has electrons with opposite spins, and electrons are not fully transferred in covalent bonds.

222 Easy

222 of 579

Application +4 | -1

Hybridisation state of chlorine in

{ClF}_3

View answer and explanation

Correct option: B

s p^3 d

Option B (

s p^3 d

) is correct because chlorine in

ClF_3

has three bond pairs and two lone pairs, resulting in a steric number of 5 and

sp^3d

hybridization.

223 Hard

223 of 579

Understanding +4 | -1

Which of the following is drawback of the octet theory?
I. It is clear that octet rule is based upon the chemical inertness of noble gases. However, some noble gases (for example xenon and krypton) also combine with oxygen and fluorine to form a number of compounds like

\mathrm{XeF}_2, \mathrm{KrF}_2, \mathrm{XeOF}_2

etc.
II. This theory does not account for the shape of molecules.
III. It does not explain the relative stability of the molecules being totally silent about the energy of a molecule.
Choose the correct statements

View answer and explanation

Correct option: D

All of these

Option D (All of these) is correct because all three statements accurately describe the limitations and drawbacks of the octet theory.

224 Easy

224 of 579

Understanding +4 | -1

The molecule that has linear structure

View answer and explanation

Correct option: A

C{O_2}

Option A (

CO_2

) is correct because carbon dioxide has a linear structure with carbon double-bonded to two oxygen atoms.

225 Easy

225 of 579

Understanding +4 | -1

\mathrm{Xe}{\mathrm{F}_6}

is:

View answer and explanation

Correct option: B

Pentagonal pyramidal

Option B (Pentagonal pyramidal) is correct because XeF6 has a distorted octahedral structure due to the lone pair, resulting in a pentagonal pyramidal shape.

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226 Easy

226 of 579

Remembering +4 | -1

\pi

-bond is formed by sideways overlapping of:

View answer and explanation

Correct option: B

p-p orbitals

Option B (p-p orbitals) is correct because pi bonds are formed by the sideways or lateral overlapping of p-orbitals.

227 Medium

227 of 579

Application +4 | -1

Which has triangular planar shape?

View answer and explanation

Correct option: A

\mathrm{CH}_3^ +

Option A (

\mathrm{CH}_3^ +

) is correct because the central carbon atom in

CH_3^+

has three bond pairs and no lone pairs, resulting in a triangular planar shape.

228 Hard

228 of 579

Application +4 | -1

The molecule having permanent dipole moment is:

View answer and explanation

Correct option: A

\mathrm{S}{\mathrm{F}_4}

Option A (

\mathrm{S}{\mathrm{F}_4}

) is correct because its seesaw geometry results in a net dipole moment due to the lone pair.

229 Medium

229 of 579

Remembering +4 | -1

The O-H bond distance in water molecule is:

View answer and explanation

Correct option: C

0.96\,{A^0}

Option C (

0.96\,{A^0}

) is correct because the O-H bond distance in a water molecule is approximately 0.96 Angstroms, a known experimental value.

230 Medium

230 of 579

Analyzing +4 | -1

The correct increasing bond angles order is:

View answer and explanation

Correct option: B

\mathrm{Cl}{\mathrm{F}_3} < P{\mathrm{F}_3} < N{\mathrm{F}_3} < B{\mathrm{F}_3}

Option B (

\mathrm{Cl}{\mathrm{F}_3} < P{\mathrm{F}_3} < N{\mathrm{F}_3} < B{\mathrm{F}_3}

) is correct because it correctly orders the bond angles based on the number of lone pairs and electronegativity differences.

231 Medium

231 of 579

Analyzing +4 | -1

Among the following isostructural compounds, identify the compound which has the highest lattice energy

View answer and explanation

Correct option: D

MgO

Option D (

MgO

) is correct because lattice energy is directly proportional to the product of charges and inversely proportional to the distance between ions;

Mg^{2+}

and

O^{2-}

have higher charges than the other options.

232 Easy

232 of 579

Understanding +4 | -1

Two electrons of one atom

A

and two electrons of another atom

B

are utilized to form a compound

A B

. This is an example of

View answer and explanation

Correct option: A

Polar covalent bond

Option A is correct because if atoms A and B have different electronegativities, the bond formed will be a polar covalent bond.

233 Easy

233 of 579

Remembering +4 | -1

Polar covalent compounds are soluble in:

View answer and explanation

Correct option: A

Polar solvents

Option A (Polar solvents) is correct because polar covalent compounds dissolve best in solvents with similar polarity due to intermolecular forces.

234 Medium

234 of 579

Application +4 | -1

The bond order in

{N}_2{ }^{+}

View answer and explanation

Correct option: C

2.5

Option C (2.5) is correct because the bond order in

{N}_2{ }^{+}

is calculated using the molecular orbital configuration and the formula (bonding electrons - antibonding electrons)/2.

235 Easy

235 of 579

Analyzing +4 | -1

The increasing order of bond angle among

\mathrm{BeCl}_2(\mathrm{I})

\mathrm{NH}_3(\mathrm{II}), \mathrm{CH}_4(\mathrm{III}), \mathrm{BF}_3 \mathrm{(IV})

will be:

View answer and explanation

Correct option: B

<

III

<

<

Option B (II

<

III

<

<

I) is correct because it represents the increasing order of bond angles based on molecular geometry and VSEPR theory.

236 Hard

236 of 579

Understanding +4 | -1

\mathrm{C} - \mathrm{Cl}

bond is stronger than

\mathrm{C}-\mathrm{I}

bond, because

View answer and explanation

Correct option: A

\mathrm{C} - \mathrm{Cl}

bond is more ionic than

\mathrm{C}-\mathrm{I}

Option A (

\mathrm{C} - \mathrm{Cl}

bond is more ionic than

\mathrm{C}-\mathrm{I}

) is correct because the electronegativity difference between C and Cl is greater than that between C and I, leading to a more polar and thus stronger bond.

237 Hard

237 of 579

Analyzing +4 | -1

Correct order of bond angles in

\mathrm{N}{\mathrm{H}_3}

\mathrm{PC}{\mathrm{l}_3}

and

\mathrm{BC}{\mathrm{l}_3}

View answer and explanation

Correct option: D

\mathrm{BC}{\mathrm{l}_3} > N{\mathrm{H}_3} > PC{\mathrm{l}_3}

Option D (

\mathrm{BC}{\mathrm{l}_3} > N{\mathrm{H}_3} > PC{\mathrm{l}_3}

) is correct because bond angle depends on hybridization and lone pairs.

238 Medium

238 of 579

Remembering +4 | -1

For the formation of covalent bond, the difference in the value of electronegativities should be:

View answer and explanation

Correct option: A

Equal to or less than

1.7

Option A is correct because a difference in electronegativity equal to or less than 1.7 generally indicates a covalent bond.

239 Medium

239 of 579

Application +4 | -1

Which of the following will be octahedral

View answer and explanation

Correct option: A

S F_6

Option A (

S F_6

) is correct because the sulfur atom in

SF_6

sp^3d^2

hybridized, resulting in an octahedral geometry with six bonding pairs and no lone pairs.

240 Medium

240 of 579

Understanding +4 | -1

Chlorine atom differs from chloride ion in the number of:

View answer and explanation

Correct option: C

Electrons

Option C (Electrons) is correct because a chloride ion is formed when a chlorine atom gains an electron.

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