Free Chemical Bonding MCQs with Answers
964 Chemical Bonding MCQs from Chemistry, each with the correct answer and a written explanation of why it is correct. Free and unlimited, with no account needed.
Chemical bonding explains molecular shape through VSEPR theory and distinguishes sigma bonds from pi bonds. Questions involve hybridization, bond angles, dipole moment and bond energy, including how electron-pair repulsion determines geometry and how bond polarity differs from the overall polarity of a molecule.
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Read the Chemical Bonding notesFree MDCAT chapter notes with key terms964 questions · page 21 of 49
- A. Ionic bond
- B. Covalent bond
- C. Coordinate covalent bond
- D. Metallic bond
Explanation: Option C is correct. A coordinate covalent bond is also known as a dative bond.
Correct answer: Coordinate covalent bond- A. All iodine centres are either sp3d or sp3d2 hybridized
- B. The minimum angular separation between fluorine atoms is 60°
- C. The anionic species are both isoelectronic and isostructural to XeF2 and XeF4
- D. There is no species having a single lone pair of electrons
Explanation: Hybridisation and structure of IF-2 → sp3d & linear.Hybridisation and structure of XeF2 → sp3d & linear.So,Both XeF2 and IF-2 are…
Correct answer: The anionic species are both isoelectronic and isostructural to XeF2 and XeF4- A. smaller size Li+ impart significant covalent character in LiF
- B. the hydration energies of Li+ and F- are quite higher
- C. lattice energy of LiF is quite higher due to the smaller size of Li+ and F-
- D. LiF have strong polymeric network in solid
Explanation: The small size of both Li+ and F- ion leads to a very high value of lattice energy and thus the crystal of LiF is very difficult to break.
Correct answer: lattice energy of LiF is quite higher due to the smaller size of Li+ and F-- A. Option A
- B. Option B
- C. Option C
- D. Option D
- E. Option E
Explanation: From the above resonance diagrams, it is clear that (A) and (B) are the correct representations for N2 O.
Correct answer: Option E- A. large cation and small anion
- B. large cation and large anion
- C. small cation and small anion
- D. small cation and large anion
Explanation: Ionic bonds are mainly formed due to the transfer of atoms because of the higher degree of the electrostatic force between the two…
Correct answer: large cation and small anion- A. II > III > I > IV
- B. II > III = I > IV
- C. III > IV > I > II
- D. IV > III > IV > I
Explanation: As the s-character of the hybridized orbital of the C-atom increases, the bond length decreases.
Correct answer: II > III > I > IV- A. LiCl.2H2O
- B. NaCl.2H2O
- C. KCl.2H2O
- D. All of these
Explanation: Because of the greater φ value of Li ,Li + + most likely form hydrated salts.
Correct answer: LiCl.2H2O- A. O-H - - S
- B. S-H- - -O
- C. F-H- - -F
- D. O-H- - -O
Explanation: F, being the most electronegative, will yield the strongest H-bond.
Correct answer: F-H- - -F409. I4O9 is an:
- A. covalent compound
- B. coordinate compound
- C. ionic compound
- D. double salt
Explanation: I4O9 actually exists as I(IO3)3= I3++ 3IO-3
Correct answer: ionic compound410. N(SiH3)3 has:
- A. sp3 hybridisation, pyramidal shape
- B. sp2 hybridisation, planar shape
- C. sp3 hybridisation, tetrahedral shape
- D. dsp2 hybridisation, square planar shape
Explanation: Lone pair of e-s of nitrogen is donated to the vacant d-orbital of Si.
Correct answer: sp2 hybridisation, planar shape- A. SnF4
- B. SnCl4
- C. SnBr4
- D. SnI4
Explanation: Because of the charge transfer spectra, SnI4 is orange in colour. SnI4 absorbs light and re-emit the complementary colour of yellow- orange.
Correct answer: SnI4- A. He2+ is more stable than H2+.
- B. Bond dissociation energy of H2+ is more than bond dissociation energy of He2+.
- C. Since bond orders of He2+ and H2+ are equal hence both will have equal bond dissociation energy.
- D. Bond length of H2+ is less than bond length of H2.
Explanation: The more the negative energy, the more is the stability of the ion/molecule. H2+ is more stable than He2+.
Correct answer: Bond dissociation energy of H2+ is more than bond dissociation energy of He2+.- A. 43%
- B. 50%
- C. 55.3%
- D. 72.24%
Explanation: ∆ EN=4.0 - 1.2=2.8 % Ionic Character = 16∆EN + 3.5(∆EN)2= 16 x 2.8+3.5(2.8)2= 72.24 %
Correct answer: 72.24%- 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
Explanation: Ionic compounds have high M.P. and B.P. Ionic bond is primary bond and hence very strong bond.
Correct answer: high melting points and high boiling points- A. HCl
- B. NH3
- C. C2H2
- D. H2SO4
Explanation: This is the following solution:H2so4 has 2 coordinate covalent bonds.
Correct answer: H2SO4- A. Molten NaOH
- B. Molten KOH
- C. Solid NaCl
- D. Aqueous NaCl
Explanation: In solid state, ionic compounds are bad conductors of electricity. Ionic compounds conduct electricity only in molten or aqeous state .
Correct answer: Solid NaCl- A. Heptagonal
- B. Octahedral
- C. Trigonal bipyramidal
- D. Pentagonal bipyramidal
Explanation: b. p. = 7 ,l.p. = 0 sp3d3 pentagonal bipyramidal.
Correct answer: Pentagonal bipyramidal- A. H-F > H-O > H-N
- B. H-N > H-O > H-F
- C. H-O > H-N > H-F
- D. H-F > H-N > H-O
Explanation: [Strength of H-bond ∝ E.N. of Z atom] As electronegativity of fluorine is highest... So hf is the strongest bond.
Correct answer: H-F > H-O > H-N- A. Nitrogen bond pair electron cloud concentrates near the central atom because of its higher electronegativity, thus the bond pair - bond pair repulsion increases which in turn decreases the bond angle in NH3.
- B. Due to larger size of the lone pair electron cloud, there is larger lone pair - bond pair repulsion in PH3 compared to NH3.
- C. Due to quite high energy difference between 3s and 3p orbitals, the lone pair on phosphorous prefers to occupy unhybridized s-orbital rather than hybridized sp3 hybridized orbital which causes its s-orbital energy to increase.
- D. Phosphorous forms pπ - dπ bonds while nitrogen doesn't.
Explanation: The energy difference between 3s and 3p orbitals is quite high in group 15 and group 16 hydrides (except for NH3 and H2O).
Correct answer: Due to quite high energy difference between 3s and 3p orbitals, the lone pair on phosphorous prefers to occupy unhybridized s-orbital rather than hybridized sp3 hybridized orbital which causes its s-orbital energy to increase.- A. sp>sp2>sp3
- B. sp3>sp2>sp
- C. sp2>sp>sp3
- D. sp>sp3>sp2
Explanation: The order "sp³ > sp² > sp" represents the decreasing degree of p-character in hybrid orbitals.
Correct answer: sp3>sp2>sp