Linear molecule and sp-hybridized

Tetrahedral molecule and $s{p^3}$-hybridized

The species ${{\rm{C}}_2}$

Has one $\sigma $ bond and one $\pi $ bond

Solid ${\rm{NaCl}}$ is a bad conductor of electricity because:

In solid ${\rm{NaCl}}$ there is no velocity of ions

In solid ${\rm{NaCl}}$there are no ions

In solid ${\rm{NaCl}}$there are no electrons

${\rm{N}}{{\rm{H}}_3}$ has a net dipole moment, but boron trifluoride $\left( {{\rm{B}}{{\rm{F}}_3}} \right)$ has zero dipole moment, because:

${\rm{N}}{{\rm{H}}_3}$ is pyramidal while ${\rm{B}}{{\rm{F}}_3}$ is trigonal planar

$B$ is less electronegative than $N$

$F$ is more electronegative than $H$

${\rm{B}}{{\rm{F}}_3}$ is pyramidal while ${\rm{N}}{{\rm{H}}_3}$ is planar

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NEET • CHEMISTRY • CHEMICAL BONDING & MOLECULAR STRUCTURE

Chemical bonding & molecular structure practice · Mixed difficulty

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Showing 1-30 of 579 questions

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1 Easy

1 of 579

Understanding +4 | -1

The example of the

p - p

-orbital overlapping is the formation of:

View answer and explanation

Correct option: B

\mathrm{C}{\mathrm{l}_2}

molecule

Option B (

\mathrm{C}{\mathrm{l}_2}

molecule) is correct because chlorine has the electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁵, and the bond is formed by the overlap of p orbitals.

2 Medium

2 of 579

Understanding +4 | -1

Which is expected to conduct electricity?

View answer and explanation

Correct option: C

Molten KCl

Option C (Molten KCl) is correct because molten ionic compounds conduct electricity due to the mobility of ions.

3 Medium

3 of 579

Remembering +4 | -1

Hybridization involves:

View answer and explanation

Correct option: B

Mixing of atomic orbitals

Option B (Mixing of atomic orbitals) is correct because hybridization is the process of mixing atomic orbitals to form new hybrid orbitals.

4 Easy

4 of 579

Understanding +4 | -1

Which of the following is correct?

View answer and explanation

Correct option: A

Decreases in bond length means increase in bond strength

Option A (Decreases in bond length means increase in bond strength) is correct because shorter bond lengths generally indicate stronger bonds due to increased electron density between the atoms.

5 Easy

5 of 579

Analyzing +4 | -1

Which has the lowest anion to cation size ratio?

View answer and explanation

Correct option: D

\mathrm{CsF}

Option D (CsF) is correct because Cs has the largest cation size and F has the smallest anion size among the given options, leading to the lowest ratio.

6 Hard

6 of 579

Analyzing +4 | -1

Which species has the highest bond order?

View answer and explanation

Correct option: C

{\mathrm{N}_2}

Option C (

{\mathrm{N}_2}

) is correct because it has a bond order of 3, which is higher than the bond orders of

{\mathrm{O}_2}

(2) and

{\mathrm{O}_2^{2 - }}

(1).

7 Easy

7 of 579

Analyzing +4 | -1

Which of the following has been arranged in order of decreasing dipole moment

View answer and explanation

Correct option: A

C{H_3}Cl > C{H_3}F > C{H_3}Br > C{H_3}I

Option A (

C{H_3}Cl > C{H_3}F > C{H_3}Br > C{H_3}I

) is correct because the dipole moment depends on both electronegativity difference and bond length, and the product of these factors is largest for

CH_3Cl

8 Medium

8 of 579

Remembering +4 | -1

Molecular orbital theory was given by

View answer and explanation

Correct option: C

Mulliken

Option C (Mulliken) is correct because Robert S. Mulliken is credited with the development of the Molecular Orbital Theory.

9 Medium

9 of 579

Application +4 | -1

The pair of species that has the same bond order in the following is

View answer and explanation

Correct option: A

{CO}, {NO}^{+}

Option A (

{CO}, {NO}^{+}

) is correct because both species have 14 electrons, resulting in a bond order of 3.

10 Medium

10 of 579

Application +4 | -1

A binary compound formed between the elements with the atomic number 19 and 17 is expected to be

View answer and explanation

Correct option: D

A water-soluble compound forming a conducting solution in water

Option D is correct because elements with atomic numbers 19 (Potassium) and 17 (Chlorine) form an ionic compound (KCl) that dissolves in water to form a conducting solution.

11 Easy

11 of 579

Remembering +4 | -1

Valence bond theory of metallic bond was given by

View answer and explanation

Correct option: D

Pauling

Option D (Pauling) is correct because Linus Pauling is credited with developing the valence bond theory to explain metallic bonding.

12 Easy

12 of 579

Analyzing +4 | -1

Species having same bond order are

View answer and explanation

Correct option: C

F_2^ + ,\,\,\,O_2^{ - 1}

Option C (

F_2^+ , O_2^{-1}

) is correct because both species have a bond order of 1.5 based on their molecular orbital configurations.

13 Easy

13 of 579

Application +4 | -1

Molecule having non-zero value of dipole moment is

View answer and explanation

Correct option: B

{CHCl}_3

Option B (

{CHCl}_3

) is correct because chloroform has polar C-Cl bonds and an asymmetrical tetrahedral structure, resulting in a non-zero dipole moment, while the other molecules are symmetrical and non-polar.

14 Medium

14 of 579

Application +4 | -1

Chlorine atom, in its third excited state, reacts with fluorine to form a compound X. The formula and shape of X are

View answer and explanation

Correct option: D

\mathrm{Cl}{\mathrm{F}_7}

pentagonal bipyramidal

Option D (

\mathrm{Cl}{\mathrm{F}_7}

pentagonal bipyramidal) is correct because chlorine in its third excited state can form 7 bonds with fluorine atoms, resulting in

ClF_7

with a pentagonal bipyramidal shape.

15 Easy

15 of 579

Analyzing +4 | -1

Which has the least bond angle

View answer and explanation

Correct option: C

{H}_2 {O}

Option C (

{H}_2 {O}

) is correct because its bent geometry and two lone pairs on the oxygen atom result in the smallest bond angle (approximately 104.5 degrees) compared to the other options.

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16 Easy

16 of 579

Remembering +4 | -1

Co-ordinate covalent bond is formed by

View answer and explanation

Correct option: C

donation of electrons

Option C (donation of electrons) is correct because a coordinate covalent bond is formed when one atom donates a pair of electrons to another atom.

17 Easy

17 of 579

Remembering +4 | -1

The carbon atoms of graphite are

View answer and explanation

Correct option: A

sp^2

hybridised

Option A (

sp^2

hybridised) is correct because each carbon atom in graphite is bonded to three other carbon atoms, resulting in

sp^2

hybridization.

18 Medium

18 of 579

Application +4 | -1

Bond angle between two hybrid orbitals is

105^\circ .

Hybrid character orbital is:

View answer and explanation

Correct option: D

Between

22 - 23\%

Option D (Between

22 - 23\%

) is correct because the relationship between bond angle and s-character allows us to determine the s-character percentage based on the given bond angle.

19 Medium

19 of 579

Understanding +4 | -1

O{F_2}

is:

View answer and explanation

Correct option: C

Bent molecule and

s{p^3}

-hybridized

Option C (Bent molecule and

s{p^3}

-hybridized) is correct because

OF_2

has a bent shape due to the two lone pairs on the oxygen atom, and the oxygen atom is

s{p^3}

hybridized.

20 Medium

20 of 579

Remembering +4 | -1

What is the

I – I – I

bond angle in the

I_3^-

ion?

View answer and explanation

Correct option: A

180^\circ

Option A (

180^\circ

) is correct because the

I_3^-

ion has a linear structure due to the three lone pairs on the central iodine atom, resulting in a linear arrangement of the other two iodine atoms.

21 Easy

21 of 579

Analyzing +4 | -1

Which among the following can have largest

C - O

bond length?

View answer and explanation

Correct option: D

{\left[ {Cr{{\left( {CO} \right)}_5}} \right]^{2 - }}

Option D (

{\left[ {Cr{{\left( {CO} \right)}_5}} \right]^{2 - }}

) is correct because the negative charge on the metal increases back-bonding to CO, weakening the C-O bond and thus increasing its length.

22 Medium

22 of 579

Application +4 | -1

Which of the following has regular tetrahedral shape?

View answer and explanation

Correct option: C

{\left[ {\mathrm{B}{\mathrm{F}_4}} \right]^ - }

Option C (

{\left[ {\mathrm{B}{\mathrm{F}_4}} \right]^ - }

) is correct because Boron has 4 bond pairs and no lone pairs, resulting in a tetrahedral shape.

23 Easy

23 of 579

Understanding +4 | -1

Which bond has the highest bond energy?

View answer and explanation

Correct option: C

Multiple bond

Option C (Multiple bond) is correct because multiple bonds (double or triple bonds) have higher bond energy than single bonds (sigma bonds) or coordinate bonds.

24 Hard

24 of 579

Understanding +4 | -1

The species

{\mathrm{C}_2}

View answer and explanation

Correct option: B

Has both

\pi

bonds

Option B (Has both

\pi

bonds) is correct because, according to molecular orbital theory, the electronic configuration of

C_2

results in both bonds being pi bonds.

25 Medium

25 of 579

Application +4 | -1

If a molecule

M{X_3}

has zero dipole moment the sigma bonding orbitals used by

M

(at. No. < 21) is:

View answer and explanation

Correct option: C

s{p^2}

-hybrid

Option C (

s{p^2}

-hybrid) is correct because a molecule

MX_3

with zero dipole moment implies a symmetrical trigonal planar geometry, which corresponds to

sp^2

hybridization.

26 Easy

26 of 579

Remembering +4 | -1

s p^3

hybridization leads to which shape of the molecule

View answer and explanation

Correct option: A

Tetrahedron

Option A (Tetrahedron) is correct because

sp^3

hybridization results in four hybrid orbitals arranged in a tetrahedral geometry.

27 Hard

27 of 579

Remembering +4 | -1

The single, double and triple bond lengths of carbon in carbon dioxide are respectively

View answer and explanation

Correct option: B

1.22,1.15

and

1.10 \mathop {\text{A}}\limits^ \circ

Option B (

1.22,1.15

and

1.10 \mathop {\text{A}}\limits^ \circ

) is incorrect. The question asks for single, double, and triple bond lengths of carbon IN CARBON DIOXIDE. Carbon dioxide has two double bonds (O=C=O), so the question is flawed. However, if we interpret the question as asking for typical single, double, and triple carbon bond lengths, then the closest answer is B where 1.22 is a typical C=O double bond length, 1.15 is not a standard bond length, and 1.10 is a typical C≡C triple bond length. This question is poorly worded and has no correct answer. The question should be removed or reworded.

28 Medium

28 of 579

Analyzing +4 | -1

Which of the following two are isostructural?

View answer and explanation

Correct option: A

\mathrm{Xe}{\mathrm{F}_2},\mathrm{IF}_2^ -

Option A (

\mathrm{Xe}{\mathrm{F}_2},\mathrm{IF}_2^ -

) is correct because both have a linear shape with 3 lone pairs and 2 bond pairs around the central atom.

29 Medium

29 of 579

Understanding +4 | -1

Solid

\mathrm{NaCl}

is a bad conductor of electricity because:

View answer and explanation

Correct option: C

In solid

\mathrm{NaCl}

there is no velocity of ions

The correct answer is that in solid NaCl there is no velocity of ions because in the solid state, ions are held in fixed positions within the crystal lattice and cannot move freely to conduct electricity.

30 Medium

30 of 579

Understanding +4 | -1

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

has a net dipole moment, but boron trifluoride

\left( {\mathrm{B}{\mathrm{F}_3}} \right)

has zero dipole moment, because:

View answer and explanation

Correct option: D

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

is pyramidal while

\mathrm{B}{\mathrm{F}_3}

is trigonal planar

Option D (

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

is pyramidal while

\mathrm{B}{\mathrm{F}_3}

is trigonal planar) is correct because the geometry of the molecules determines whether the individual bond dipoles cancel out or add up to a net dipole moment.

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