Chemistry Objective Questions and Answers: Chapter 04 Chemical Bonding and Molecular Structure
Review structured MCQ sets for Class 11 Chemistry Chapter 04 Chemical Bonding and Molecular Structure. Built according to official CBSE guidelines, these downloadable questions support daily revision and core concept reinforcement.
Download Chapter 04 Chemical Bonding and Molecular Structure MCQs with Answers
Access the complete set of multiple-choice questions for Chapter 04 Chemical Bonding and Molecular Structure below. This focused format allows students to isolate specific topics for thorough review and uninterrupted practice alongside official CBSE textbooks.
Question: The attractive force which holds various constituents (atoms, ions etc.) together in different chemical species is called a
a) chemical bond
b) ionic bond
c) chemical compound
d) covalent bond
Answer: chemical bond
Question: 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) All of the above
b) periodic table
c) electronic configuration of elements
d) structure of atom
Answer: All of the above
Question: In the formation of a molecule which of the following take part in chemical combination?
a) valence electron
b) cation
c) anion
d) inner shell electron
Answer: valence electron
Question: The bond formed as a result of the electrostatic attraction between the positive and negative ions is termed as ...
a) Electrovalent bond
b) Covalent bond
c) Chemical bond
d) Co-ordinate bond
Answer: Electrovalent bond
Question: Cation and anion combines in a crystal to form following type of compound
a) ionic
b) covalent
c) metallic
d) dipole-dipole
Answer: ionic
Question: Electrovalence of calcium and chlorine respectively is
a) + 2, – 1
b) 1, – 2
c) + 1, – 1
d) + 2, – 2
Answer: + 2, – 1
Question: When a metal atom combines with non-metal atom, the non-metal atom will
a) gain electrons and increase in size
b) gain electrons and increase in size
c) lose electrons and increase in size
d) lose electrons and decrease in size
Answer: gain electrons and increase in size
Question: In N2 molecule, the number of electrons shared by each nitrogen atom is
a) 3
b) 2
c) 5
d) None of these
Answer: 3
Question: The lowest energy structure is the one with the ______ formal charges on the atoms.
a) smallest
b) highest
c) zero
d) negative
Answer: smallest
Question: In the cyanide ion, the formal negative charge is on
a) N
b) C
c) Both C and N
d) Resonate between C and N
Answer: N
Question: What are the exceptions of the octet rule ?
a) All of these
b) Expanded octet of the central atom
c) An odd number of electrons on central atom
d) The incomplete octet of central atom
Answer: All of these
Question: In which of the following molecules octet rule is not followed?
a) NO
b) CH4
c) NH3
d) CO2
Answer: NO
Question: Among the following the electron deficient compound is
a) BCl3
b) PCl5
c) CCl4
d) BeCl2
Answer: BCl3
Question: Which of the following is the electron deficient molecule?
a) B2H6
b) PH3
c) SiH4
d) None of these
Answer: B2H6
Question: Which of the following compounds does not follow the octet rule for electron distribution?
a) PCl5
b) H2O
c) PH3
d) PCl3
Answer: PCl5
Question: Which of the following pairs will form the most stable ionic bond ?
a) Mg and F
b) Na and F
c) Na and Cl
d) Li and F
Answer: Mg and F
Question: Which of the following methods is used for measuring bond length ?
a) All of these
b) Spectroscopic techniques
c) Electron-diffraction
d) X-ray diffraction
Answer: All of these
Question: _______ 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) Covalent radius
b) Ionic radius
c) Bond length
d) van der Waal’s radius
Answer: Covalent radius
Question: All the bond lengths of sulphur – oxygen in sulphate ion, are equal because of:
a) resonance
b) symmetry
c) high electronegativity of oxygen
d) None of these
Answer: resonance
I. MCQ - Choose Appropriate Alternative
1. The energy required to break a chemical bond to form neutral atoms is called __________. (Ionization Potential, Electron Affinity, Bond Energy)
2. The chemical bond present in H-Cl is __________. (Non Polar, Polar Covalent, Electrovalent)
3. A polar covalent bond is formed between two atoms when the difference between their E.N values is __________. (Equal to 1.7, less than 1.7, More than 1.7)
4. The most polar covalent bond out of the following is __________. (H-Cl, H-F, H-I)
5. __________ bond is one in which an electron has been completely transferred from one atom to another. (Ionic, Covalent, co-ordinate)
6. __________ bond is one in which an electron pair is shared equally between the two atoms. (Ionic, Covalent, Co-ordinate)
7. Bond angle in the molecule of CH4 is of __________. (120°, 109.5°, 180°)
8. A molecule of CO2 has __________ structure.
9. The sigma bond is __________ than pi bond. (Weaker, Stronger, Unstable)
10. The sp3 orbitals are __________ in shape. (Tetrahedral, Trigonal, Diagonal)
11. The shape of CH4 molecule is __________. (Tetrahedral, Trigonal, Diagonal)
12. The bond in Cl2 is __________. (Non polar, Polar, Electrovalent)
13. Water is __________ molecule. (None polar, Polar, Electrovalent)
14. Covalent bonds in which electron pair are shared equally between the two atoms is called __________ covalent bond. (Non polar, Polar, Co-ordinate)
15. Each carbon atom in CH4 is __________ hybridized. (sp3, sp2, sp)
16. Each carbon atom in C2H4 is __________ hybridized. (sp3, sp2, sp)
17. Each carbon atom in C2H2 is __________ hybridized. (sp3, sp2, sp)
18. Oxygen atom in H2O has __________ unshared electron pair. (One, two , three)
19. Nitrogen atom in NH3 has __________ unshared electron pair. (One, two, three)
20. The cloud of charge that surrounds two or more nuclei is called __________ orbital. (Atomic, Molecular, Hybrid)
21. A substance, which is highly attracted by a magnetic field, is called __________. (Electromagnetic, Paramagnetic, Diamagnetic)
22. HF exists in liquid due to __________. (Vander Waal Forces, Hydrogen bond, covalent Bond)
23. Best hydrogen bonding is found in __________ (HF, HCl, HI)
24. Shape of CCl4 molecule is __________. (tetrahedral, Trigonal, Diagonal)
25. __________ bond is formed due to linear overlap.(Sigma bond, Pi bond, Hydrogen bond)
26. __________ is defined as the quantity of energy required to break one mole of covalent in gaseous state.(Bond energy, Ionization energy, Energy of Activation)
27. Repulsive force between electron pair in a molecule is maximum when it has an angle of __________.(120°, 109.5°, 180°)
28. Repulsive force between electron pair in a molecule is maximum when it has an angle of __________.(120°, 109.5°, 180°)
29. The sum of total number of electrons pairs (bonding and lone pairs) is called __________.(Atomic Number, Avogadro’s Number, Steric Number)
30. Shape of __________ molecule is tetrahedral.(BaCl2, BF3, NH3)
II. Fill in the Blank
1. A bond formed due to transference of electron is called __________.
2. A bond formed due to sharing of electron is called __________.
3. Sigma bond is __________ than pi bond.
4. The shape of methane molecule is __________.
5. One s and 3p orbitals overlap to produce four __________ hybrid orbitals.
6. Ethene, C2H4 is an example of __________ hybridization.
7. Water molecule has __________ structure.
8. Water molecules are inter-linked with one another due to __________.
9. Polarity of the molecule is due to the difference of __________ between the two bonded atoms.
10. A chemical bond formed between to different atoms by mutual sharing of electron is termed as __________.
11. A chemical bond formed between two similar atoms by mutual sharing of electrons is known as __________.
12. The difference between the Electronegativity values of the two atoms forming covalent bond must be __________ than 1.7.
13. When two orbitals of different atoms by hybridize with each other having their axes in the same straight lines, the bond formed is termed as __________.
14. __________ bond is formed when p-orbitals of the two atoms with their axes parallel to each other overlap with each other.
15. Melting and boiling point of ionic compounds are usually __________ than that of covalent compounds.
16. Non polar compounds are usually __________ in non polar solvent.
17. The nitrogen in NH3 is __________ hybridized.
18. A hybrid orbital is called __________ orbital.
19. Since dipole moment of CS2 is zero, it is a __________ molecule.
20. A bond formed due to the electrostatic forces of attraction between the oppositely charged ions is called __________ bond.
21. The ionic bond is formed between the atoms with low ionization potential and high __________.
22. A bond formed by the sharing of an electron pair contributed by one atom only is called a __________ bond.
23. A co-ordinate covalent bond is also known as __________ bond.
24. Polar covalent bond is __________ than a non polar covalent bond.
25. H-F bond is __________ than H-Br bond.
26. The SI unit of dipole moment is __________.
27. Commonly used unit of dipole moment is __________.
28. Dipole moment of non-polar compound is __________ D.
29. The reactions of ionic compounds are usually very __________.
30. Covalent compounds are generally __________ in nature.
31. Ionic compounds are generally __________ in nature.
32. A covalent bond is represented by a __________.
33. A co-ordinate covalent bond is represented by an __________.
34. The covalent bond between H-F is called __________ covalent bond.
35. The power of an atom to attract a shared pair of electron itself is called __________ of that atom.
36. m = d x e represents __________.
37. CO2 and SO2 molecules have __________ polar bonds.
38. NH3 molecule has __________ polar bonds.
39. A double bond has __________ bond energy than a single bond.
40. An orbital which surrounds a single nucleus is called __________ orbital.
41. An orbital which surrounds two or more atomic nuclei is called __________ orbital.
42. A molecular orbital, which is of lower energy than the atomic orbitals from which it is derived, is known as __________ orbital.
43. A molecular orbital, which has higher energy than the atomic orbitals from which it is derived, is known as __________ orbital.
44. Orbitals formed after hybridization are called __________ orbitals.
45. Bond angle in sp3 hybridization is of __________.
46. Bond angle in sp2 hybridization is of __________.
47. Bond angle in sp hybridization is of __________.
48. sp3 hybridization is also known as __________.
49. sp2 hybridization is also known as __________.
50. Sp hybridization is also known as __________.
51. A pair of electrons residing on the central atom and which is not used in bonding is called a __________.
52. The sum of total number of electron pairs (bonding and lone pairs) is called __________ number.
53. __________ bond is usually expressed by dotted line.
54. Water molecule has dipole moment because of its __________ structure.
55. CO2 is non polar because of its __________ structure.
56. Overlapping in __________ bond is perfect.
57. Overlapping in __________ bond is not perfect.
58. H-H bond is __________ than H-Cl bond.
59. __________ hybrid orbitals are not co-planar.
60. Covalent bond in Cl2 molecule is __________.
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Download Chapter MCQs: Class 11 Chemistry Chapter 04 Chemical Bonding and Molecular Structure
About Chapter 04 Chemical Bonding and Molecular Structure MCQs for Class 11 Chemistry
Review structured objective questions for Class 11 Chemistry Chapter 04 Chemical Bonding and Molecular Structure. Built according to official CBSE guidelines, these MCQ sets support daily revision and core concept reinforcement.
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FAQs
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