Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure MCQ Questions with Answer

Class 11 Chemical Bonding and Molecular Structure MCQ is one of the best strategies to prepare for the CBSE Class 11 Board exam. If you want to complete a grasp concept or work on one’s score, there is no method except constant practice. Students can improve their speed and accuracy by doing more MCQs on Chemical Bonding and Molecular Structure Class 11, which will help them all through their board tests.

Class 11 Chemical Bonding and Molecular Structure MCQ

Class 11 Chemistry MCQ with answers are given here to Chapter 4 Chemical Bonding and Molecular Structure. These MCQs are based on the latest CBSE board syllabus and relate to the latest Class 11 Chemistry syllabus. By Solving these Class 11 MCQs, you will be able to analyze all of the concepts quickly in the chapter and get ready for the Class 11 Annual exam.

Learn Class 11 Chemical Bonding and Molecular Structure MCQs with answers pdf free download according to the latest CBSE and NCERT syllabus. Students should prepare for the examination by solving CBSE Class 11 Chemistry Chemical Bonding and Molecular Structure MCQ with answers given below

Question 1. The bond formed as a result of the electrostatic attraction between the positive and negative ions is termed as …
(a) Chemical bond
(b) Electrovalent bond
(c) Co-ordinate bond
(d) Covalent bond

Question 2. Which of the following is/are not the condition(s) for Lewis dot structure?
(i) Each bond is formed as a result of sharing of an electron pair between the atoms.
(ii) From the two combining atoms only one atom contribute electron(s) to the shared pair.
(iii) The combining atoms attain the outer shell noble gas configurations as a result of the sharing of electrons.
(a) (i) and (iii)
(b) (ii) and (iii)
(c) (ii) only
(d) (iii) only

Question 3. Who provide explanation of valence based on intertness of noble gases ?
(a) Lewis
(b) Kossel-Lewis
(c) Langmuir
(d) Sidgwick & Powell

Question 4. In the formation of a molecule which of the following take part in chemical combination?
(a) cation
(b) anion
(c) valence electron
(d) inner shell electron

Question 5. Who introduced the term covalent bond ?
(a) Lewis
(b) Langmuir
(c) Nyholm and Gillespie
(d) Heitler and London

Question 6. When a metal atom combines with non-metal atom, the non-metal atom will
(a) lose electrons and decrease in size
(b) lose electrons and increase in size
(c) gain electrons and decrease in size
(d) gain electrons and increase in size

Question 7. The attractive force which holds various constituents (atoms, ions etc.) together in different chemical species is called a
(a) chemical bond
(b) chemical compound
(c) ionic bond
(d) covalent bond

Question 8. Cation and anion combines in a crystal to form following type of compound
(a) ionic
(b) metallic
(c) covalent
(d) dipole-dipole

Question 9. Electrovalence of calcium and chlorine respectively is
(a) + 2, – 1
(b) + 1, – 1
(c) + 1, – 2
(d) + 2, – 2

Question 10. Which of the following compounds does not follow the octet rule for electron distribution?
(a) PCl₅
(b) PCl₃
(c) H₂O
(d) PH₃

Question 11. In N₂molecule, the number of electrons shared by each nitrogen atom is
(a) 1
(b) 2
(c) 3
(d) 5

Question 12. The evolution of various theories of valence and the interpretation of the nature of chemical bonds have closely been related to the developments in the understanding of
(a) structure of atom
(b) electronic configuration of elements
(c) periodic table
(d) All of the above

Question 13. The lowest energy structure is the one with the ………. formal charges on the atoms.
(a) smallest
(b) highest
(c) zero
(d) negative

Question 14. Which of the following is the electron deficient molecule?
(a) C₂H₆
(b) B₂H₆
(c) SiH₄
(d) PH₃

Question 15. In PO₄^3– ion, the formal charge on each oxygen atom and P—O bond order respectively are
(a) –0.75, 0.6
(b) – 0.75, 1.0
(c) – 0.75, 1.25
(d) –3, 1.25

Question 16. In the cyanide ion, the formal negative charge is on
(a) C
(b) N
(c) Both C and N
(d) Resonate between C and N

Question 17. Which of the following statements is incorrect ?
(a) The formation of ionic compounds depend upon the ease of formation of the positive and negative ions from the respective neutral atoms.
(b) Formation of ionic compounds depend upon arrangement of the positive and negative ions in the solid.
(c) Formation of positive ion involves addition of electron(s) while that of negative ion involves removal of electron(s).
(d) None of these

Question 18. A pair of compound which have odd electrons in the group NO, CO, ClO₂, N₂O₅, SO₂ and O₃ are
(a) NO and ClO₂
(b) CO and SO₂
(c) ClO₂ and CO
(d) SO₂ and O₃

Question 19. In which of the following molecules octet rule is not followed?
(a) NH₃
(b) CH₄
(c) CO₂
(d) NO

Question 20. The effect of more electronegative atom on the strength of ionic bond
(a) increases
(b) decreases
(c) remains the same
(d) decreases slowly

Question 21. Which of the following combination will form an electrovalent bond ?
(a) P and Cl
(b) NH₃ and BF₃
(c) H and Ca
(d) H and S

Question 22. What are the exceptions of the octet rule ?
(a) The incomplete octet of central atom
(b) An odd number of electrons on central atom.
(c) Expanded octet of the central atom
(d) All of these

Question 23. Among the following the electron deficient compound is
(a) BCl₃
(b) CCl₄
(c) PCl₅
(d) BeCl₂

Question 24. Which of the following bond will have highest ionic character?
(a) H–I
(b) H–F
(c) H–Cl
(d) H–Br

Question 25. In ionic solids how crystal structure get stabilized
(a) By the energy released in the formation of crystal lattice.
(b) By achieving octet of electrons around the ionicspecies in gaseous state. 
(c) By electron gain enthalpy and the ionization enthalpy.
(d) None of these

Question 26. Energy required to completely separate one mole of a solid ionic compound into gaseous constituent ions is called ………. .
(a) Ionisation enthalpy
(b) Electron gain enthalpy
(c) Bond dissociation enthalpy
(d) Lattice enthalpy

Question 27. Among the following which compound will show the highest lattice energy ?
(a) KF
(b) NaF
(c) CsF
(d) RbF

Question 28. The number of possible resonance structures for 2 CO₃²⁻ is
(a) 2
(b) 3
(c) 6
(d) 9

Question 29. All the bond lengths of sulphur – oxygen in sulphate ion, are equal because of:
(a) symmetry
(b) resonance
(c) high electronegativity of oxygen
(d) None of these

Question 30. Which one of the following is not the resonance structure of CO₂?
(a) O = C = O
(b) ^– O – C ≡ O⁺
(c) ⁺ O ≡ C – O^–
(d) O ≡ C = O

Question 31. Which of the following methods is used for measuringbond length ?
(a) X-ray diffraction
(b) Electron-diffraction
(c) Spectroscopic techniques
(d) All of these

Question 32. Which of the following pairs will form the most stable ionic bond ?
(a) Na and Cl
(b) Mg and F
(c) Li and F
(d) Na and F

Question 33. Which one of the following pairs of molecules will have permanent dipole moments for both members ?
(a) NO₂ and CO₂
(b) NO₂ and O₃
(c) SiF₄ and CO₂
(d) SiF₄ and NO₂

Question 34. The molecule which has zero dipole moment is
(a) CH₃Cl
(b) NF₃
(c) BF₃
(d) ClO₂

Question 35. Which of the following statement is correct?
(a) Amount of energy required to break one mole of bonds of a particular type between two atoms in a gaseous state is called bond enthalpy.
(b) The unit of bond enthalpy is kJ mol^–1
(c) Larger the bond dissociation enthalpy, stronger will be the bond in the molecule
(d) All of these

Question 36. ………. is measured as the radius of an atom’s core which is in contact with the core of an adjacent atom in a bonded situation.
(a) van der Waal’s radius
(b) Bond length
(c) Covalent radius
(d) Ionic radius

Question 37. Resonance is due to
(a) delocalization of sigma electrons
(b) delocalization of pi electrons
(c) migration of protons
(d) Both (a) and (b)

Question 38. Which one of the following molecules is expected to have zero dipole moment?
(a) H₂O
(b) CO₂
(c) SO₂
(d) CaF₂

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Question 39. The correct order of dipole moments of HF, H₂S and H₂O is
(a) HF < H₂S < H₂O
(b) HF < H₂S < H₂O
(c) HF < H₂S < H₂O
(d) HF < H₂O < H₂S

Question 40. Complete the following statements. With A in bond order, B increases and C decreases.
(a) A = increase, B = bond length, C = bond enthalpy
(b) A = decrease, B = bond enthalpy, C = bond length
(c) A = increase, B = bond enthalpy, C = bond length
(d) A = increase, B = bond angle, C = bond enthalpy

Question 41. Which of the following has dipole moment?
(a) CO₂
(b) p-dichlorobenzene
(c) NH₃
(d) CH₄

Question 42. Identify the non polar molecule in the following compounds
(a) H₂
(b) HCl
(c) HF and HBr
(d) HBr

Question 43. A neutral molecule XF₃ has a zero dipole moment. The element X is most likely
(a) chlorine
(b) boron
(c) nitrogen
(d) carbon

Question 44. Among the following, the molecule of high dipole moment is
(a) CCl₄
(b) NH₃
(c) H₂O
(d) CHCl₃

Question 45. The most polar bond is
(a) C – F
(b) C – O
(c) C – Br
(d) C – S

Question 46. According to Fajan’s rule, covalent bond is favoured by
(a) Large cation and small anion
(b) Large cation and large anion
(c) Small cation and large anion
(d) Small cation and small anion

Question 47. The correct sequence of increasing covalent character is represented by
(a) LiCl < NaCl < BeCl₂
(b) BeCl₂ < LiCl < NaCl
(c) NaCl < LiCl < BeCl₂
(d) BeCl₂ < NaCl < LiCl

Question 48. CO₂ is isostructural with
(a) C₂H₂
(b) SnCl₂
(d) MgCl₂
(c) NO₂         

Question 49. Which species has the maximum number of lone pair of electrons on the central atom ? 
(a) [CIO^–₃]
(b) XeF₄
(c) SF₄
(d) [I^–₃]         

Question 50. Which of the following salt shows maximum covalent character?
(a) AlCl₃
(b) MgCl₂
(c) CsCl
(d) LaCl₃

Question 51. Polarisibility of halide ions increases in the order
(a) F ^–, I ^–, Br^–, Cl^–
(b) Cl ^–, Br –, I^–, F^–
(c) I ^–, Br ^–, Cl^–, F^–
(d) F ^–, Cl ^–, Br^–, l^–

Question 52. Sodium chloride is an ionic compound whereas hydrogen chloride is mainly covalent because
(a) sodium is less reactive
(b) hydrogen is non-metal
(c) hydrogen chloride is a gas
(d) electronegativity difference in the case of hydrogen and chlorine is less than 2.1.

Question 53. A square planar complex is formed by hybridisation of the following atomic orbitals 
(a) s, p_x, P_y , Pz
(b) s, px, Py, Pz, d
(c) d, S, P_x, P_y       
(d) s, P_x, Py, p_z, d, d   

Question 54. Which of the following is a linear molecule? 
(a) BeCl₂
(b) H₂O
(c) SO₂
(d) CH₄         

Question 55. InP₄O₁₀ the
(a) second bond in P = O is formed by pn-dn back bonding
(b) P = 0 bond is formed by pn-pn bonding
(c) P = 0 bond is fo1med dn-dn bonding
(d) P = 0 bond is formed by dn-dn- 30′ back bonrung     

Question 56 . Which of the following molecules bas pyramidal shape?
(a) PCI₃
(b) SO₃
(c) CO₃^2-
(d) NO^–₃         

Question 57. How manycr and n-bonds are present in toluene?
(a) 3n + 8σ
(c) 3n + 15σ
(e) 6n+ 6σ
(b) 3n + l0σ
(d) 6n + 3σ     

Question 58. Pair of species having identical shapes for molecules is
(a) CF₄, SF₄
(b) BF₃, PCI₃ 
(c) XeF₂, CO₂ 
(d) PF₅, IF₇     

Question 59. The number of lone pairs of Xe in XeF₂ , XeF₄ and XeF₆ respectively are 
(a) 3,2, l
(b) 2,4, 6
(c) 1,2,3
(d) 6,4,2         

Question 60. Unusually high boiling point of water is result of
(a) intermolecular hydrogen bonding 
(b) intramolecular hydrogen bonding
(c) both intra and inter molecular hydrogen bonding
(d) high specific heat     

Question 61. Amongst the following, the molecule that is linear is
(a) SO₂
(b) BeH₂
(c) ClO₂
(d) NO₂     

Question 62. Which of the following hydrogen bonds are strongest in vapour phase? 
(a) HF …… HF
(b) HF ….. . HCI
(c) HCI. ….. HCI
(d) HF …… Hl       

Question 63. Which of the following compounds would have the highest boiling point ? 
(a) CH₃CH₂CH₂CH₃
(b) CH₃NH₂
(c) CH₃OH
(d) CH₂F₂       

Question 64. Number of P—0 bonds in P₄O₁₀ is 
(a) 17
(b) 16
(c) 15
(d) 6       

Question 65. Hydrogen bonding plays a central role in the following phenomena 
(a) ice floats in water
(b) higher Lewis basicity of primary amines than tertiary amines in aqueous solutions
(c) formic acid is more acidic than acetic acid
(d) dimerisation of acetic acid in benzene     

Question 66. Malleability and ductility of metals can be accounted due to
(a) the presence of electrostatic force
(b) the crystalline stmcture in metal
(c) the capacity of layers of metal ions to slide over the other
(d) the interaction of electrons with metal ions in the lattice     

Question 67. Which of the following has strongest hydrogen bonding?
(a) Ethylamine
(b) Ammonia 
(c) Ethyl alcohol
(d) Diethyl ether           

Question 68. The maximum number of hydrogen bonds that a molecule of water can have is 
(a) 1
(c) 3
(b) 2
(d) 4       

Question 69. NH₃ has much higher boiling point than PH₃ because
(a) NH₃ has larger molecular weight 
(b) NH₃ undergoes umbrella inversion
(c) NH₃ forms hydrogen bond
(d) NH₃ contains ionic bonds whereas PH₃ contains covalent bonds       

Question 70. Which compound is soluble in water? 
(a) CS₂
(b) C₂H₅OH
(c) CCI₄
(d) CHCI₃     

Question 71. Which molecule has hydrogen bonding?
(a) CH₄
(b) CH₃COOH
(c) GeH₄
(d) H₂Te       

Question 72. Glycerol is more viscous than ethanol due to 
(a) high molecular weight
(b) high boiling point
(c) many hydrogen bonds per molecule
(d) Fajan’s rule     

Question 73. Oxygen and sulphur both are the member of same group in Periodic Table but H₂O is liquid while H₂ Sis gas because
(a) molecular weight of water is more
(b) electronegativity of sulphur is more
(c) H₂S is weak acid
(d) water molecules are having strong hydrogen bonds between them     

Question 74. I. 1, 2-dihydroxy benzene
II. 1, 3-dihydroxy benzene
III. I, 4-dihydroxy benzene
IV. Hydroxy benzene
The increasing order of boiling points of above mentioned alcohols is
(a) I < II < ill< IV
(b) I< II < IV<ill
(c) IV < I < II < Ill
(d) IV < II < I < ill     

Question 75. H-bond is not present in
(a) water
(b) glycerol
(c) hydrogen fluoride
(d) hydrogen sulphide       

Question 76. Metallic lusture is explained by
(a) diffusion of metal ions
(b) osci Ila ti on of loose electrons
(c) excitation of free protons
(d) existence of bee lattice     

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