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Chemical Bonding and Molecular Structure Practice Questions - DPP for NEET

Q: 2. What are the different types of chemical bonds?

Ans. There are three main types of chemical bonds:1. Ionic Bond: It is formed when there is a complete transfer of electrons from one atom to another, resulting in the formation of ions. These oppositely charged ions are held together by electrostatic forces.2. Covalent Bond: It is formed when atoms share electrons to complete their outermost electron shells. Covalent bonds can be further classified as polar or nonpolar, depending on the electronegativity difference between the atoms.3. Metallic Bond: It is formed between metal atoms and involves the delocalization of electrons throughout the lattice. This results in the formation of a sea of electrons that hold the metal atoms together.

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 Page 1


PART-I (Single Correct MCQs)
1. Which of the following has the highest dipole moment?
(a)
(b)
(c)
Page 2


PART-I (Single Correct MCQs)
1. Which of the following has the highest dipole moment?
(a)
(b)
(c)
(d)
2. In compounds of type ECl
3
, where E = B, P, As or Bi, the angles Cl - E-
Cl for different E are in the order.
(a) B > P = As = Bi
(b) B > P > As > Bi
(c) B < P = As = Bi
(d) B < P < As < Bi
3. The electronegativity difference between N and F is greater than that
between N and H yet the dipole moment ofNH
3
 (1.5 D) is larger than
that of NF
3
 (0.2D). This is because
(a) in NH
3
 the atomic dipole and bond dipole are in the same direction
whereas in NF
3
 these are  in opposite directions.
(b) in NH
3
 as well as NF
3
 the atomic dipole and bond dipole are in opposite
directions.
(c) in NH
3
 the atomic dipole and bond dipole are in the opposite directions
whereas in NF
3
 these are in the same direction.
(d) in NH
3
 as well as in NF
3
 the atomic dipole and bond dipole are in the
same direction.
4. On changing N
2
 to , the dissociation energy of N–N bond ..... and on
changing O
2 
to
 
O
+
? 2
 the dissociation energy of O–O bond....
(a) increases, decreases
(b) decreases, increases
(c) decreases in both cases
(d) increases in both cases
5. Which of the two ions from the list given below have the geometry that
Page 3


PART-I (Single Correct MCQs)
1. Which of the following has the highest dipole moment?
(a)
(b)
(c)
(d)
2. In compounds of type ECl
3
, where E = B, P, As or Bi, the angles Cl - E-
Cl for different E are in the order.
(a) B > P = As = Bi
(b) B > P > As > Bi
(c) B < P = As = Bi
(d) B < P < As < Bi
3. The electronegativity difference between N and F is greater than that
between N and H yet the dipole moment ofNH
3
 (1.5 D) is larger than
that of NF
3
 (0.2D). This is because
(a) in NH
3
 the atomic dipole and bond dipole are in the same direction
whereas in NF
3
 these are  in opposite directions.
(b) in NH
3
 as well as NF
3
 the atomic dipole and bond dipole are in opposite
directions.
(c) in NH
3
 the atomic dipole and bond dipole are in the opposite directions
whereas in NF
3
 these are in the same direction.
(d) in NH
3
 as well as in NF
3
 the atomic dipole and bond dipole are in the
same direction.
4. On changing N
2
 to , the dissociation energy of N–N bond ..... and on
changing O
2 
to
 
O
+
? 2
 the dissociation energy of O–O bond....
(a) increases, decreases
(b) decreases, increases
(c) decreases in both cases
(d) increases in both cases
5. Which of the two ions from the list given below have the geometry that
is explained by the same hybridization of orbitals, NO
2
? –
, NO
3
? –
, NH
2
? –
,
NH
4
? +
, SCN
– 
?
(a) and 
(b) and 
(c) SCN
–
 and 
(d) and 
6. Which of the following pairs of ions are isoelectronic and isostructural
?
(a)
(b)
(c)
(d)
7. Which of the following is correct increasing order of lone pair of
electrons   on the central atom?
(a) IF
7
 < IF
5
 < ClF
3
 < XeF
2
(b) IF
7
 < XeF
2
 < ClF
2 
< IF
5
(c) IF
7
 < ClF
3
 < XeF
2
 < IF
5
(d) IF
7
 < XeF
2
 < IF
5 
< ClF
3
8. Consider the molecules CH
4
, NH
3
 and H
2
O. Which of the given
statements is false?
(a) The H–C–H bond angle in CH
4
, the H–N–H bond angle in NH
3
, and the
H–O–H bond angle in H
2
O are all greater than 90°.
(b) The H–O–H bond angle in H
2
O is larger than the H–C–H bond angle in
CH
4
.
(c) The H–O–H bond angle in H
2
O is smaller than the H–N–H bond angle
in NH
3
.
Page 4


PART-I (Single Correct MCQs)
1. Which of the following has the highest dipole moment?
(a)
(b)
(c)
(d)
2. In compounds of type ECl
3
, where E = B, P, As or Bi, the angles Cl - E-
Cl for different E are in the order.
(a) B > P = As = Bi
(b) B > P > As > Bi
(c) B < P = As = Bi
(d) B < P < As < Bi
3. The electronegativity difference between N and F is greater than that
between N and H yet the dipole moment ofNH
3
 (1.5 D) is larger than
that of NF
3
 (0.2D). This is because
(a) in NH
3
 the atomic dipole and bond dipole are in the same direction
whereas in NF
3
 these are  in opposite directions.
(b) in NH
3
 as well as NF
3
 the atomic dipole and bond dipole are in opposite
directions.
(c) in NH
3
 the atomic dipole and bond dipole are in the opposite directions
whereas in NF
3
 these are in the same direction.
(d) in NH
3
 as well as in NF
3
 the atomic dipole and bond dipole are in the
same direction.
4. On changing N
2
 to , the dissociation energy of N–N bond ..... and on
changing O
2 
to
 
O
+
? 2
 the dissociation energy of O–O bond....
(a) increases, decreases
(b) decreases, increases
(c) decreases in both cases
(d) increases in both cases
5. Which of the two ions from the list given below have the geometry that
is explained by the same hybridization of orbitals, NO
2
? –
, NO
3
? –
, NH
2
? –
,
NH
4
? +
, SCN
– 
?
(a) and 
(b) and 
(c) SCN
–
 and 
(d) and 
6. Which of the following pairs of ions are isoelectronic and isostructural
?
(a)
(b)
(c)
(d)
7. Which of the following is correct increasing order of lone pair of
electrons   on the central atom?
(a) IF
7
 < IF
5
 < ClF
3
 < XeF
2
(b) IF
7
 < XeF
2
 < ClF
2 
< IF
5
(c) IF
7
 < ClF
3
 < XeF
2
 < IF
5
(d) IF
7
 < XeF
2
 < IF
5 
< ClF
3
8. Consider the molecules CH
4
, NH
3
 and H
2
O. Which of the given
statements is false?
(a) The H–C–H bond angle in CH
4
, the H–N–H bond angle in NH
3
, and the
H–O–H bond angle in H
2
O are all greater than 90°.
(b) The H–O–H bond angle in H
2
O is larger than the H–C–H bond angle in
CH
4
.
(c) The H–O–H bond angle in H
2
O is smaller than the H–N–H bond angle
in NH
3
.
(d) The H–C–H bond angle in CH
4
 is larger than the H–N–H bond angle
in NH
3
.
9. In which of the following species the interatomic bond angle is 109°
28’?
(a) NH
3
, 
(b) , BF
3
(c) NH
3
, BF
4
(d) , BF
3
.
10. Hybridisation of the underline atom changes in:
(a) changes to 
(b) changes to H
3
O
+
(c) changes to 
(d) in all cases
11. The states of hybridization of boron and oxygen atoms in boric acid
(H
3
BO
3
) are respectively
(a) sp
3
 and sp
2
(b) sp
2
 and sp
3
(c) sp
2
 and sp
2
(d) sp
3
 and sp
3
12. Among the following ions, the p – d overlap could be present in
(a)
(b)
(c)
(d)
13. Which one of the following pairs of species have the same bond order?
Page 5


PART-I (Single Correct MCQs)
1. Which of the following has the highest dipole moment?
(a)
(b)
(c)
(d)
2. In compounds of type ECl
3
, where E = B, P, As or Bi, the angles Cl - E-
Cl for different E are in the order.
(a) B > P = As = Bi
(b) B > P > As > Bi
(c) B < P = As = Bi
(d) B < P < As < Bi
3. The electronegativity difference between N and F is greater than that
between N and H yet the dipole moment ofNH
3
 (1.5 D) is larger than
that of NF
3
 (0.2D). This is because
(a) in NH
3
 the atomic dipole and bond dipole are in the same direction
whereas in NF
3
 these are  in opposite directions.
(b) in NH
3
 as well as NF
3
 the atomic dipole and bond dipole are in opposite
directions.
(c) in NH
3
 the atomic dipole and bond dipole are in the opposite directions
whereas in NF
3
 these are in the same direction.
(d) in NH
3
 as well as in NF
3
 the atomic dipole and bond dipole are in the
same direction.
4. On changing N
2
 to , the dissociation energy of N–N bond ..... and on
changing O
2 
to
 
O
+
? 2
 the dissociation energy of O–O bond....
(a) increases, decreases
(b) decreases, increases
(c) decreases in both cases
(d) increases in both cases
5. Which of the two ions from the list given below have the geometry that
is explained by the same hybridization of orbitals, NO
2
? –
, NO
3
? –
, NH
2
? –
,
NH
4
? +
, SCN
– 
?
(a) and 
(b) and 
(c) SCN
–
 and 
(d) and 
6. Which of the following pairs of ions are isoelectronic and isostructural
?
(a)
(b)
(c)
(d)
7. Which of the following is correct increasing order of lone pair of
electrons   on the central atom?
(a) IF
7
 < IF
5
 < ClF
3
 < XeF
2
(b) IF
7
 < XeF
2
 < ClF
2 
< IF
5
(c) IF
7
 < ClF
3
 < XeF
2
 < IF
5
(d) IF
7
 < XeF
2
 < IF
5 
< ClF
3
8. Consider the molecules CH
4
, NH
3
 and H
2
O. Which of the given
statements is false?
(a) The H–C–H bond angle in CH
4
, the H–N–H bond angle in NH
3
, and the
H–O–H bond angle in H
2
O are all greater than 90°.
(b) The H–O–H bond angle in H
2
O is larger than the H–C–H bond angle in
CH
4
.
(c) The H–O–H bond angle in H
2
O is smaller than the H–N–H bond angle
in NH
3
.
(d) The H–C–H bond angle in CH
4
 is larger than the H–N–H bond angle
in NH
3
.
9. In which of the following species the interatomic bond angle is 109°
28’?
(a) NH
3
, 
(b) , BF
3
(c) NH
3
, BF
4
(d) , BF
3
.
10. Hybridisation of the underline atom changes in:
(a) changes to 
(b) changes to H
3
O
+
(c) changes to 
(d) in all cases
11. The states of hybridization of boron and oxygen atoms in boric acid
(H
3
BO
3
) are respectively
(a) sp
3
 and sp
2
(b) sp
2
 and sp
3
(c) sp
2
 and sp
2
(d) sp
3
 and sp
3
12. Among the following ions, the p – d overlap could be present in
(a)
(b)
(c)
(d)
13. Which one of the following pairs of species have the same bond order?
(a) CN
–
 and NO
+
(b) CN
–
 and CN
+
(c) and CN
–
(d) NO
+
 and CN
+
14. N
2
 and O
2
 are converted into monocations,  and respectively.
Which of the following statements is wrong?
(a) In , N - N bond weakens
(b) In , the O - O bond order increases
(c) In , paramagnetism decreases
(d) becomes diamagnetic
15. The bond dissociation energy of B – F in BF
3
 is 646 kJ mol
–1
 whereas
that of  C – F in CF
4
 is 515 kJ mol
–1
. The correct reason  for higher B – F
bond dissociation energy as compared to that of C – F is
(a) stronger s bond between B and F in BF
3
 as compared to that between C
and F in CF
4
.
(b) significant pp – pp interaction between B and F in BF
3
 whereas there is
no possibility of such interaction between C and F in CF
4
.
(c) lower degree of pp – pp interaction between B and F in BF
3
 than that
between C and F in CF
4
.
(d) smaller size of B– atom as compared to that of C– atom.
16. ortho-Nitrophenol is less soluble in water than p- and m- Nitrophenols
because :
(a) o-Nitrophenol is more volatile steam than those of m- and p-isomers.
(b) o-Nitrophenol shows intramolecular H-bonding.
(c) o-Nitrophenol shows intermolecular H-bonding.
(d) Melting point of o-Nitrophenol is lower than those of m- and p-
isomers.
17. Amongst LiCl, RbCl, BeCl
2
 and MgCl
2
 the compounds with the

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FAQs on Chemical Bonding and Molecular Structure Practice Questions - DPP for NEET

1. What is chemical bonding and why is it important in molecular structure?

Ans. Chemical bonding refers to the process of combining atoms to form molecules or compounds. It is important in molecular structure because it determines the arrangement of atoms and the type of chemical bonds present in a molecule. The type of bonding influences various properties of molecules such as their shape, polarity, and reactivity.

2. What are the different types of chemical bonds?

Ans. There are three main types of chemical bonds: 1. Ionic Bond: It is formed when there is a complete transfer of electrons from one atom to another, resulting in the formation of ions. These oppositely charged ions are held together by electrostatic forces. 2. Covalent Bond: It is formed when atoms share electrons to complete their outermost electron shells. Covalent bonds can be further classified as polar or nonpolar, depending on the electronegativity difference between the atoms. 3. Metallic Bond: It is formed between metal atoms and involves the delocalization of electrons throughout the lattice. This results in the formation of a sea of electrons that hold the metal atoms together.

3. How can we determine the polarity of a chemical bond?

Ans. The polarity of a chemical bond depends on the electronegativity difference between the atoms involved. Electronegativity is the ability of an atom to attract shared electrons towards itself in a covalent bond. If the electronegativity difference is significant, the bond is polar. If the electronegativity difference is small or zero, the bond is nonpolar. To determine the polarity of a bond, you can compare the electronegativity values of the atoms using a periodic table. If the electronegativity difference is between 0.5 and 1.7, the bond is polar covalent. If the electronegativity difference is greater than 1.7, the bond is ionic.

4. How does the VSEPR theory help in predicting molecular geometry?

Ans. The VSEPR (Valence Shell Electron Pair Repulsion) theory is used to predict the molecular geometry of a molecule based on the repulsion between electron pairs. According to this theory, electron pairs in the valence shell of an atom repel each other and try to stay as far apart as possible to minimize repulsion. The VSEPR theory states that the shape of a molecule is determined by the number of electron pairs around the central atom. These electron pairs can be either bonding pairs or lone pairs. By considering the number of bonding and lone pairs, we can predict the molecular geometry using the VSEPR model.

5. How does molecular structure affect the physical and chemical properties of substances?

Ans. The molecular structure of a substance plays a crucial role in determining its physical and chemical properties. Here are a few examples: 1. Boiling and Melting Points: The strength and type of intermolecular forces present in a substance depend on its molecular structure. Substances with stronger intermolecular forces tend to have higher boiling and melting points. 2. Solubility: The polarity of a molecule affects its solubility in different solvents. Polar molecules dissolve in polar solvents, while nonpolar molecules dissolve in nonpolar solvents. 3. Reactivity: The arrangement of atoms in a molecule can influence its reactivity. For example, the presence of functional groups in organic molecules determines their reactivity in various chemical reactions. 4. Biological Activity: The three-dimensional structure of biomolecules, such as enzymes and receptors, determines their interactions with other molecules and their biological activity.

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