Chemical Bonding and Molecular Structure Questions and Answers pdf
Chemical Bonding and Molecular Structure Questions and Answers pdf
Multiple Choice Questions – 1
Que 1. The lattice energy of an ionic compound depends upon
(a) Charge on the ion only (b) Size of the ion only
(c) Packing of ions only (d) Charge on the ion and size of the ion
Que 2. In the given bonds which one is most ionic
(a) Cs -Cl (b) Al -Cl
(c) C -Cl (d) H -Cl
Que 3. Element x is strongly electropositive and y is strongly electronegative. Both elements are univalent, the compounds formed from their combination will be
(a) x+ y– (b) x– y+
(c) x – y (d) x ® y
Que 4. In the formation of NaCl from Na and Cl
(a) Sodium and chlorine both give electrons
(b) Sodium and chlorine both accept electrons
(c) Sodium loses an electron and chlorine accepts an electron
(d) Sodium accepts an electron and chlorine loses an electron
Que 5. Which of the following is an electrovalent linkage
(a) CH4 (b) MgCl2
(c) SiCl4 (d) BF3
Chemical Bonding and Molecular Structure Questions and Answers pdf
Que 6. Electrovalent compounds do not have
(a) High M.P. and Low B.P. (b) High dielectric constant
(c) High M.P. and High B.P. (d) High polarity
Que 7. Many ionic crystals dissolve in water because
(a) Water is an amphiprotic solvent
(b) Water is a high boiling liquid
(c) The process is accompanied by a positive heat of solution
(d) Water decreases the interionic attraction in the crystal lattice due to solvation
Que 8. The electronic structure of four elements A, B, C, D are
(A) 1s2 (B) 1s2, 2s2 2p2
(C) 1s2, 2s2 2p5 (D) 1s2, 2s2 2p6
The tendency to form an electrovalent bond is largest in
(a) A (b) B (c) C (d) D
Que 9. With which of the given pairs CO2 resembles
(a) HgCl2, C2H2 (b) HgCl2, SnCl4
(c) C2H2, NO2 (d) N2O and NO2
Que 10. The electron pair which forms a bond between two similar non-metallic atoms will be
(a) Dissimilar shared between the two
(b) By complete transfer from one atom to other
(c) In a similar spin condition
(d) Equally shared in between the two
Chemical Bonding and Molecular Structure Questions and Answers pdf
Que 11. For the formation of a covalent bond, the difference in the value of electronegativities should be
(a) Equal to or less than 1.7 (b) More than 1.7
(c) 1.7 or more (d) None of these
Que 12. Which type of bond is formed between similar atoms
(a) Ionic (b) Covalent
(c) Coordinate (d) Metallic
Que 13. Covalent compounds are generally …… in water
(a) Soluble (b) Insoluble
(c) Dissociated (d) Hydrolysed
Que 14. Which one is the electron deficient compound
(a) ICl (b) NH3
(c) BCl3 (d) PCl3
Que 15. Which among the following elements has the tendency to form covalent compounds
(a) Ba (b) Be
(c) Mg (d) Ca
Que 16. Silicon has 4 electrons in the outermost orbit. In forming the bonds
(a) It gains electrons (b) It loses electrons
(c) It shares electrons (d) None of these
Que 17. According to VSEPR theory, the geometry of a covalent molecule depends upon
(a) the number of bond pairs of electrons
(b) the number of lone pairs of electrons
(c) the number of electron pairs present in the outer shell of the central atom
(d) All the above
Que 18. The geometry of – ClO– ion according to Valence Shell Electron Pair Repulsion (VSEPR) theory will be
(a) planar triangular (b) pyramidal
(c) tetrahedral (d) square planar
Que 19. In BrF3 molecule, the lone pairs occupy equatorial positions to minimize
(a) lone pair-bond pair repulsion only
(b) bond pair-bond pair repulsion only
(c) lone pair – lone pair repulsion and lone pair-bond pair repulsion
(d) lone pair – lone pair repulsion only
Que 20. Which of the correct increasing order of lone pair of electrons on the central atom?
(a) IF7 < IF5 < CIF3 < XeF2
(b) IF7 < XeF2 < CIF2 < IF5
(c) IF7 < CIF3 < XeF2 < IF5
(d) IF7 < XeF2 < IF5 < CIF3
Chemical Bonding and Molecular Structure Questions and Answers pdf
Que 21. The number of lone pair and bond pair of electrons on the sulphur atom in sulphur dioxide molecule is respectively
(a) 1 and 3 (b) 4 and 1
(c) 3 and 1 (d) 1 and 4
Que 22. A molecule has two lone pairs and two bond pairs around the central atom. The molecule shape is expected to be
(a) V-shaped (b) triangular
(c) linear (d) tetrahedral
Que 23. Using VSEPR theory, predict the species which has a square pyramidal shape
(a) SnCl2 (b) CCl4
(c) SO3 (d) BrF5
Que 24. The ground state electronic configuration of valence shell electrons in nitrogen molecule (N2) is written as KK σ2s, σ*2s, л2px, л2py, σ2pz Bond order in nitrogen molecule is
(a) 0 (b) 1 (c) 2 (d) 3
Que 25. Bond order in benzene is
(a) 1 (b) 2 (c) 1.5 (d) None of these
Que 26. In O2– , O2 and O2– molecular species, the total number of antibonding electrons respectively are
(a) 7, 6, 8 (b) 1, 0, 2 (c) 6, 6, 6 (d) 8, 6, 8
Que 27. Hybridization and structure of I3– are
(a) sp2 and trigonal planar (b) sp3d2 and linear
(c) sp3d and linear (d) sp3 and T-shape
Que 28. In which of the following species, all the three types of hybrid carbons are present?
(a) CH2 = C = CH2
(b) CH3 – CH = CH – CH2+
(c) CH3 – C = C – CH2+
(d) CH3 – CH = CH – CH2–
Que 29. Which of the following molecules has trigonal planar geometry?
(a) BF3 (b) NH3 (c) PCl3 (d) IF3
Que 30. Which of the following molecules is planar?
(a) SF4 (b) XeF4 (c) NF3 (d) SiF4
Chemical Bonding and Molecular Structure Questions and Answers pdf
Que 30. Hybridization present in ClF3 is
(a) sp2 (b) sp3 (c) dsp2 (d) sp3d
Que 31. Match Column-I (molecule) with Column-II (type of hybridization) and choose the correct option from the codes given below.
Column-I Column-II
(Molecule) (Type of hybridisation)
(A) SF6 (p) sp3d
(B) PF5 (q) sp3
(C) BCl3 (r) sp3d2
(D) C2H6 (s) sp2
(a) A – (r), B – (p), C – (s), D – (q)
(b) A – (r), B – (p), C – (q), D – (s)
(c) A – (p), B – (r), C – (q), D – (s)
(d) A – (p), B – (r), C – (s), D – (q)
Que 32. Match Column-I with Column-II and Column-III and choose the correct option from the given codes.
Column-I Column-II Column-III
Molecule (No. of lone pairs and bond pairs) (Shape of molecule)
(A) NH3 (i) 1, 2 (p) Bent
(B) SO2 (ii) 1, 4 (q) Trigonal pyramidal
(C) SF4 (iii) 2, 3 (r) T-shape
(D) ClF3 (iv) 1, 3 (s) See-Saw
(a) A – (iv, q); B – (ii, p); C – (i, r); D – (iii, s)
(b) A – (iv, q); B – (i, p); C – (ii, s); D – (iii, r)
(c) A – (i, p); B – (iii, s); C – (iv, r); D – (ii, q)
(d) A – (iv, p); B – (i, r); C – (iii, q); D – (ii, s)
Que 33. Match the columns
Column-I Column-II
(A) HCl (p) Covalent compound with directional bond
(B) CO2 (q) Ionic compound with non-directional bonds
(C) NaCl (r) Polar molecule
(D) CCl4 (s) Non-polar molecule
(a) A – (p, q, r), B – (q, r), C – (p, q), D – (r)
(b) A – (q), B – (r), C – (p), D – (s)
(c) A – (p, r), B – (p, s), C – (q), D – (p, s)
(d) A – (q), B – (r), C – (p, q), D – (s)
Que 34. Assertion: The lesser the lattice enthalpy more stable is the ionic compound.
Reason: The lattice enthalpy is greater, for ions of the highest charge and smaller radii.
Que 35. Assertion: Sulphur compounds like SF6 and H2SO4 have 12 valence electrons around the S atom.
Reason: All sulphur compounds do not follow the octet rule
Que 36. Assertion: The shape of the NH3 molecule is tetrahedral.
Reason: In NH3 nitrogen is sp3 hybridized.
Que 37. Assertion: pi bonds are weaker than V bonds.
Reason: pi bonds are formed by the overlapping of p-p orbitals along their axes.
Que 38. Read the following statements and choose the correct sequence of T and F from the given codes. Here T represents true and F represents false statement.
(i) The number of dots in the Lewis symbol represents the number of valence electrons.
(ii) Number of valence electrons helps to calculate the group valence of elements.
(iii) Group valence is given as 8 minus the number of inner-shell electrons.
(a) T T T (b) T F F (c) T T F (d) F F F
Que 39. Read the following statements and choose the correct option. Here T stands for True and F stands for False statement.
(i) The smaller the size of the cation and the larger the size of the anion, the greater the covalent character of an ionic bond.
(ii) The smaller the charge on the cation, the greater the covalent character of the ionic bond.
(iii) For cations of the same size and charge, the one, with electronic configuration (n – 1)dn ns0, typical of transition metals, is more polarising than the one with a noble gas configuration, ns2 np6, typical of alkali and alkaline earth metal cations.
(a) T T T (b) T T F (c) T F T (d) F T T
Que 40. Which of the following statements is/are not correct for the combination of atomic orbitals?
(i) The combining atomic orbitals must have the same or nearly the same energy.
(ii) Greater the extent of overlap, the greater will be the electron density between the nuclei of a molecular orbital.
(iii) 2pz orbital of one atom can combine with either of 2px, 2py, or 2pz orbital of other atoms as these orbitals have the same energy.
(a) (i) and (ii) (b) (iii) only
(c) (i) only (d) (ii) and (iii)
Chemical Bonding and Molecular Structure Questions and Answers pdf
Que 41. Intramolecular hydrogen bond exists in
(a) ortho nitrophenol (b) ethyl alcohol
(c) water (d) diethyl ether
Que 42. The boiling point of p-nitrophenol is higher than that of o-nitrophenol because
(a) NO2 group at p-position behave in a different way from that at o-position.
(b) intramolecular hydrogen bonding exists in p-nitrophenol
(c) there is intermolecular hydrogen bonding in p-nitrophenol
(d) p-nitrophenol has a higher molecular weight than o-nitrophenol.
Que 43. Which one of the following is the correct order of interactions?
(a) Covalent < hydrogen bonding < vander Waals < dipole-dipole
(b) vander Waals < hydrogen bonding < dipole < covalent
(c) vander Waals < dipole-dipole < hydrogen bonding < covalent
(d) Dipole-dipole < vander Waals < hydrogen bonding < covalent.
Que 44. The strongest hydrogen bond is shown by
(a) water (b) ammonia
(c) hydrogen fluoride (d) hydrogen sulphide
Que 45. The low density of ice compared to water is due to
(a) induced dipole-induced dipole interactions
(b) dipole-induced dipole interactions
(c) hydrogen bonding interactions
(d) dipole-dipole interactions
Chemical Bonding and Molecular Structure Questions and Answers pdf
Que 46. 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
Que 47. 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
Que 48. The most polar bond is
(a) C – F (b) C – O (c) C – Br (d) C – S
Que 49. Which of the following is the electron-deficient molecule?
(a) C2H6 (b) B2H6
(c) SiH4 (d) PH3
Que 50. Which of the following compounds does not follow the octet rule for electron distribution?
(a) PCl5 (b) PCl3 (c) H2O (d) PH3
Chemical Bonding and Molecular Structure Questions and Answers pdf
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Chemical Bonding and Molecular Structure
For further studies click the links below:
MOLECULAR ORBITAL THEORY AND HYDROGEN BONDING
CONCEPT OF HYBRIDISATION WITH EXAMPLES
VALANCE ELECTRON THEORIES AND ORBITAL OVERLAP
RESONANCE DIPOLE MOMENT AND BOND PARAMETERS
PROPERTIES OF IONIC BOND AND OCTET RULE