Chemical Bonding MCQs with Answer

Chemical Bonding MCQs
Multiple Choice Questions for NEET IIT-JEE and CUET

1. An electrovalent compound is made up of:

• (a) electrically charged molecules
• (b) neutral molecules
• (c) neutral atoms
• (d) electrically charged atoms or group of atoms

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Correct Answer: (d) electrically charged atoms or group of atoms

An electrovalent compound (ionic compound) is formed when electrons are transferred from one atom to another, producing cations and anions. These charged species are held together by strong electrostatic forces.

2. Electrovalent bond-formation depends on:

• (a) ionization energy
• (b) lattice energy
• (c) electron affinity
• (d) all of these

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Correct Answer: (d) all of these

The formation of ionic bonds is influenced by ionization energy (ease of losing electrons), electron affinity (ease of gaining electrons), and lattice energy (stability of the ionic lattice).

3. An atom of sodium loses one electron and chlorine atom accepts one electron. This results in the formation of sodium chloride molecule. This type of molecule will be:

• (a) electrovalent
• (b) covalent
• (c) coordinate
• (d) metallic bond

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Correct Answer: (a) electrovalent

Sodium chloride is an ionic compound formed by complete transfer of electrons, resulting in Na⁺ and Cl^- ions.

4. Which of the following is an electrovalent linkage?

• (a) CH₄
• (b) SiCl₄
• (c) MgCl₂
• (d) BF₃

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Correct Answer: (c) MgCl₂

Magnesium chloride is ionic in nature, formed by Mg²⁺ and Cl^- ions. The others are covalent compounds.

5. The electronic structure of four elements A, B, C, D are:
(A) 1s²
(B) 1s², 2s²2p²
(C) 1s², 2s², 2p⁵
(D) 1s², 2s², 2p⁶
The tendency to form electrovalent bond is largest in:

• (a) A
• (b) B
• (c) C
• (d) D

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Correct Answer: (c) C

Element C (configuration ending with 2p⁵) resembles halogens, which readily gain electrons to form stable ionic bonds.

6. Sodium chloride easily dissolves in water. This is because:

• (a) salt reacts with water
• (b) it is a white substance
• (c) it is a covalent compound
• (d) its ions are easily solvated

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Correct Answer: (d) its ions are easily solvated

NaCl dissolves because water molecules stabilize Na⁺ and Cl^- ions through solvation, reducing lattice energy.

7. What is the nature of chemical bonding between Cs and F?

• (a) Ionic
• (b) Covalent
• (c) Coordinate
• (d) Metallic

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Correct Answer: (a) Ionic

Cesium (Cs) readily loses one electron to form Cs⁺, while fluorine (F) gains one electron to form F^-, resulting in ionic bonding.

8. Metals combine with non-metals, the metal atom tends to:

• (a) lose electron
• (b) gain electron
• (c) remain electrically neutral
• (d) none of the above

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Correct Answer: (a) lose electron

Metals have low ionization energies and readily lose electrons to form cations when bonding with non-metals.

9. Which of the following halides has maximum melting point?

• (a) NaF
• (b) NaCl
• (c) NaBr
• (d) NaI

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Correct Answer: (a) NaF

NaF has the strongest ionic bond due to the smallest anion (F^-), leading to the highest lattice energy and melting point.

10. Atoms or group of atoms which are electrically charged are known as:

• (a) Atoms
• (b) Ions
• (c) Cations
• (d) Anions

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Correct Answer: (b) Ions

Ions are atoms or groups of atoms carrying a net charge, either positive (cations) or negative (anions).

11. Which of the following compounds is ionic?

• (a) H₂
• (b) CH₄
• (c) KI
• (d) Diamond

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Correct Answer: (c) KI

Potassium iodide (KI) is ionic, formed by K⁺ and I^- ions. The others are covalent or network covalent structures.

12. Which of the following pairs of species has the same electronic configuration?

• (a) Ti⁴⁺ and V³⁺
• (b) Co²⁺ and Ni²⁺
• (c) Zn²⁺ and Ni²⁺
• (d) Co³⁺ and Ni⁴⁺

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Correct Answer: (a) Ti⁴⁺ and V³⁺

Both Ti⁴⁺ and V³⁺ have the same number of electrons (18), giving them identical electronic configurations.

13. The number of electrons involved in the bond formation of N₂ molecule:

• (a) 2
• (b) 4
• (c) 6
• (d) 10

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Correct Answer: (c) 6

N₂ has a triple bond (one sigma and two pi bonds), involving 6 shared electrons.

14. Which compound is highest covalent?

• (a) LiF
• (b) LiCl
• (c) LiBr
• (d) LiI

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Correct Answer: (d) LiI

LiI is most covalent due to the large size and high polarizability of I^-, which enhances covalent character.

15. Which one is an electron-deficient compound?

• (a) NH₃
• (b) BCl₃
• (c) PCl₃
• (d) ICl

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Correct Answer: (b) BCl₃

BCl₃ is electron-deficient because boron has only six electrons in its valence shell after bonding, not achieving an octet.

16. Which of the following compounds is covalent?

• (a) H₂
• (b) KCl
• (c) Na₂S
• (d) CaO

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Correct Answer: (a) H₂

Hydrogen molecule is covalent, formed by sharing of electrons. The others are ionic compounds.

17. Which is the most covalent?

• (a) C–F
• (b) C–O
• (c) C–S
• (d) C–Br

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Correct Answer: (d) C–Br

C–Br bond is most covalent due to lower electronegativity difference compared to C–F or C–O bonds.

18. As compared to covalent compounds, electrovalent compounds generally have:

• (a) low melting points and low boiling points
• (b) high melting points and high boiling points
• (c) low melting points and high boiling points
• (d) high melting points and low boiling points

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Correct Answer: (b) high melting points and high boiling points

Ionic compounds have strong electrostatic forces, requiring large amounts of energy to break, hence high melting and boiling points.

19. Which of the following statements regarding covalent bond is not true?

• (a) The electrons are shared between atoms
• (b) The bond formed may or may not be polar
• (c) The strength of the bond depends upon the extent of overlapping
• (d) The bond is non-directional

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Correct Answer: (d) The bond is non-directional

Covalent bonds are directional in nature, depending on orbital overlap. Ionic bonds are non-directional.

20. Which of the following compounds does not follow the octet rule for electron distribution?

• (a) H₂O
• (b) PH₃
• (c) PCl₃
• (d) PCl₅

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Correct Answer: (d) PCl₅

PCl₅ expands its octet, having 10 electrons around phosphorus, violating the octet rule.

21. Boron forms covalent compounds due to:

• (a) small size
• (b) lower ionization energy
• (c) both (a) and (b)
• (d) small size and higher ionization energy

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Correct Answer: (c) both (a) and (b)

Boron’s small size and relatively low ionization energy favor covalent bonding rather than ionic bonding.

22. A simple example of a coordinate covalent bond is exhibited by:

• (a) HCl
• (b) NH₃
• (c) C₂H₂
• (d) H₂SO₄

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Correct Answer: (b) NH₃

NH₃ can donate a lone pair to form a coordinate bond, e.g., with BF₃.

23. The bond that exists between NH₃ and BF₃ is called:

• (a) electrovalent
• (b) covalent
• (c) coordinate
• (d) hydrogen bond

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Correct Answer: (c) coordinate

NH₃ donates its lone pair to BF₃, forming a coordinate covalent bond.

24. Which of the following does not have a coordinate bond?

• (a) SO₂
• (b) H₂SO₃
• (c) HNO₂
• (d) HNO₃

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Correct Answer: (d) HNO₃

Nitric acid does not exhibit coordinate bonding in its structure, unlike the others.

25. Sulphuric acid provides an example of:

• (a) non-covalent compound
• (b) non-covalent ion
• (c) coordinate bond
• (d) covalent and coordinate bond

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Correct Answer: (d) covalent and coordinate bond

H₂SO₄ contains covalent bonds within SO₄^2- and coordinate bonds in its protonated forms.

26. Which molecule has zero dipole moment?

• (a) HF
• (b) HBr
• (c) H₂O
• (d) CO₂

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Correct Answer: (d) CO₂

CO₂ is linear and symmetrical, so individual bond dipoles cancel, resulting in zero dipole moment.

27. Which molecule has the largest dipole moment?

• (a) HF
• (b) HCl
• (c) HBr
• (d) HI

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Correct Answer: (a) HF

HF has the greatest electronegativity difference between H and F, giving it the largest dipole moment.

28. Which of the following will show least dipole moment?

• (a) Ethane
• (b) Ether
• (c) Ethanol
• (d) Water

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Correct Answer: (a) Ethane

Ethane is a non-polar hydrocarbon with negligible dipole moment compared to polar molecules like water and ethanol.

29. Which shows the least dipole moment?

• (a) CHCl₃
• (b) CH₃CH₂OH
• (c) CH₃COCH₃
• (d) CCl₄

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Correct Answer: (d) CCl₄

CCl₄ is symmetrical, so dipoles cancel, resulting in zero dipole moment.

30. Which molecule has zero dipole moment?

• (a) HBr
• (b) AgI
• (c) PbSO₄
• (d) H₂O

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Correct Answer: (b) AgI

AgI is largely ionic but in solid crystalline form exhibits negligible dipole moment compared to polar molecules like H₂O.

31. N₂ is less reactive than CN due to:

• (a) difference in spin quantum number
• (b) presence of more electrons in orbitals
• (c) absence of dipole moment
• (d) none of the above

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Correct Answer: (c) absence of dipole moment

N₂ is non-polar and highly stable due to its triple bond, making it less reactive compared to polar CN.

32. Identify the non-polar molecule in the set HCl, HF, H₂, HBr:

• (a) H₂
• (b) HCl
• (c) HBr
• (d) HF, HBr

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Correct Answer: (a) H₂

H₂ is non-polar because both atoms have identical electronegativity, resulting in no dipole moment.

33. Which one is a polar molecule among the following?

• (a) CH₄
• (b) CCl₄
• (c) CO₂
• (d) H₂O

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Correct Answer: (d) H₂O

Water is polar due to its bent geometry and electronegativity difference between H and O.

34. If the electron pair forming a bond between two atoms A and B is not in the centre, then the bond is:

• (a) Single bond
• (b) Pi-bond
• (c) Polar bond
• (d) Non-polar bond

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Correct Answer: (c) Polar bond

Unequal sharing of electrons leads to a polar bond, with partial charges on atoms.

35. Which of the following liquids is not deflected by a non-uniform electrostatic field?

• (a) H₂O
• (b) CHCl₃
• (c) C₆H₁₄
• (d) C₆H₅NO₂

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Correct Answer: (c) C₆H₁₄

Hexane (C₆H₁₄) is non-polar, so it is not deflected by an electrostatic field. Polar liquids like water are deflected.

36. Amongst ClF, BF₃, and NH₃ molecules, the one with non-polar geometry is:

• (a) NH₃
• (b) BF₃
• (c) ClF₃
• (d) none of these

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Correct Answer: (b) BF₃

BF₃ is trigonal planar and symmetrical, so dipoles cancel, making it non-polar.

37. Which of the following has a high polarising power?

• (a) Na⁺
• (b) Ca²⁺
• (c) Al³⁺
• (d) Mg²⁺

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Correct Answer: (c) Al³⁺

Al³⁺ has the highest charge density, giving it strong polarising power.

38. Polarisability of halide ions increases in the order:

• (a) F^-, Cl^-, Br^-, I^-
• (b) I^-, Br^-, Cl^-, F^-
• (c) Cl^-, Br^-, F^-, I^-
• (d) F^-, I^-, Br^-, Cl^-

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Correct Answer: (a) F^-, Cl^-, Br^-, I^-

Polarisability increases with ionic size, so I^- is most polarisable, F^- least.

39. Pauling's electronegativity values for elements are useful in predicting:

• (a) polarity of bonds in molecules
• (b) co-ordination number
• (c) dipole moments of various molecules
• (d) position of elements in electrochemical series

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Correct Answer: (a) polarity of bonds in molecules

Electronegativity differences predict bond polarity and ionic/covalent character.

40. Amongst LiCl, RbCl, BeCl₂, and MgCl₂, the compounds with the greatest and least ionic character respectively are:

• (a) LiCl and RbCl
• (b) RbCl and MgCl₂
• (c) RbCl and BeCl₂
• (d) MgCl₂ and BeCl₂

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Correct Answer: (c) RbCl and BeCl₂

RbCl is highly ionic due to large cation size, while BeCl₂ is covalent due to high polarising power of Be²⁺.

41. Bond polarity of a diatomic molecule is because of:

• (a) difference in electron affinity
• (b) difference in electronegativities
• (c) difference in ionisation potential
• (d) all of the above

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Correct Answer: (b) difference in electronegativities

Bond polarity arises mainly due to electronegativity differences between atoms.

42. The bond in the formation of fluorine molecule will be:

• (a) due to s–s overlapping
• (b) due to s–p overlapping
• (c) due to p–p overlapping
• (d) due to hybridisation

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Correct Answer: (c) due to p–p overlapping

F₂ bond is formed by overlap of p orbitals, giving a sigma bond.

43. Which type of overlapping results in the formation of a σ-bond?

• (a) Axial overlapping of s–s orbitals
• (b) Axial overlapping of p–p orbitals
• (c) Axial overlapping of s–p orbitals
• (d) Lateral overlapping of p–p orbitals

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Correct Answer: (a), (b), (c)

σ-bonds are formed by axial overlap of orbitals (s–s, s–p, or p–p). Lateral overlap gives π-bonds.

44. The number and type of bonds between two carbon atoms in calcium carbide are:

• (a) 1σ, 1π
• (b) 1σ, 2π
• (c) 2σ, 2π
• (d) 2σ, 1π

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Correct Answer: (b) 1σ, 2π

CaC₂ contains C≡C units with one sigma and two pi bonds.

45. The bond angle in ethylene is:

• (a) 90°
• (b) 109°
• (c) 120°
• (d) 180°

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Correct Answer: (c) 120°

Ethylene (C₂H₄) has sp² hybridization, giving bond angles of approximately 120°.

46. Compound formed by sp³d hybridization will have structure:

• (a) planar
• (b) pyramidal
• (c) angular
• (d) trigonal bipyramidal

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Correct Answer: (d) trigonal bipyramidal

sp³d hybridization leads to trigonal bipyramidal geometry, as in PCl₅.

47. In which of the following species is the interatomic bond angle 109°28′?

• (a) NH₃, BF₄^-
• (b) NH₄⁺, BF₃
• (c) NH₃, BF₃
• (d) NH₂^-, BF₃

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Correct Answer: (a) NH₃, BF₄^-

Both NH₃ and BF₄^- exhibit tetrahedral geometry with bond angles close to 109°28′.

48. Which of the following statements is not correct?

• (a) Hybridisation is the mixing of atomic orbitals prior to their combining into molecular orbitals
• (b) sp² hybrid orbitals are formed from two p-orbitals and one s-orbital
• (c) d²sp³ hybrid orbitals are directed towards the corners of a regular octahedron
• (d) dsp³ hybrid orbitals are all at 90° to one another

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Correct Answer: (d) dsp³ hybrid orbitals are all at 90° to one another

dsp³ hybridization gives trigonal bipyramidal geometry, not all orbitals at 90°.

49. The C–H bond distance is the longest in:

• (a) C₂H₂
• (b) C₂H₄
• (c) C₂H₆
• (d) C₂H₄Br₂

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Correct Answer: (c) C₂H₆

In ethane, sp³ hybridization leads to longer C–H bond distances compared to sp² or sp hybridized carbons.

50. In ethene, the bond angle(s) is/are:

• (a) 120°
• (b) 180°
• (c) 109°
• (d) different

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Correct Answer: (a) 120°

Ethene has sp² hybridization, giving bond angles of approximately 120°.

51. A square planar complex is formed by hybridization of which atomic orbitals?

• (a) s, p_x, p_y, d_yz
• (b) s, p_x, p_y, d_z2
• (c) s, p_x, p_y, d_x2-y2
• (d) s, p_x, p_y, d_xy

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Correct Answer: (c) s, p_x, p_y, d_x2-y2

Square planar complexes arise from dsp² hybridization involving s, p_x, p_y, and d_x2-y2 orbitals.

52. Which of the following bonds requires the largest amount of bond energy to dissociate?

• (a) H–H bond in H₂
• (b) O=O bond in O₂
• (c) N≡N bond in N₂
• (d) C–C bond in C₂H₆

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Correct Answer: (c) N≡N bond in N₂

The triple bond in N₂ is extremely strong, requiring the highest bond dissociation energy.

53. The bond angle between H–O–H in ice is closest to:

• (a) 60°
• (b) 90°
• (c) 105°
• (d) 120°28′

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Correct Answer: (c) 105°

In ice, hydrogen bonding slightly distorts the H–O–H angle from the ideal 104.5° of water, making it close to 105°.

54. BCl₃ is a planar molecule while NCl₃ is pyramidal, because:

• (a) BCl₃ has no lone pair of electrons but NCl₃ has a lone pair
• (b) B–Cl bond is more polar than N–Cl bond
• (c) nitrogen atom is smaller than boron atom
• (d) N–Cl bond is more covalent than B–Cl bond

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Correct Answer: (a) BCl₃ has no lone pair of electrons but NCl₃ has a lone pair

BCl₃ is trigonal planar due to sp² hybridization, while NCl₃ is pyramidal because of the lone pair on nitrogen.

55. The isoelectronic pair is:

• (a) IF₂⁺, I₃^-
• (b) ICl₂^-, ClO₂
• (c) ClO₂^-, ClF₂^-
• (d) Cl₂O, ICl₂^-

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Correct Answer: (b) ICl₂^-, ClO₂

Isoelectronic species have the same number of electrons. ICl₂^- and ClO₂ both have 36 electrons.

56. According to VSEPR theory, the most probable shape of the molecule having 4 electron pairs in the outermost shell of the central atom is:

• (a) linear
• (b) tetrahedral
• (c) hexagonal
• (d) octahedral

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Correct Answer: (b) tetrahedral

Four electron pairs around a central atom arrange themselves tetrahedrally to minimize repulsion.

57. The bond order of NO molecule is:

• (a) 1
• (b) 2
• (c) 2.5
• (d) 3

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Correct Answer: (c) 2.5

Molecular orbital theory shows NO has a bond order of 2.5, indicating intermediate strength between a double and triple bond.

58. Molecular orbital theory was developed mainly by:

• (a) Pauling
• (b) Mulliken
• (c) Thomson
• (d) Pauling and Slater

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Correct Answer: (b) Mulliken

Robert S. Mulliken, and Friedrich Hund, developed the Molecular Orbital (MO) Theory in the late 1920s and early 1930s, which explains bonding in terms of molecular orbitals.

59. Which of the following is paramagnetic?

• (a) O₂^-
• (b) CN^-
• (c) NO
• (d) Both O₂^- and NO

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Correct Answer: (d) Both O₂^- and NO

O₂^- and NO both have unpaired electrons, making them paramagnetic.

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