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 22 of 49
- A. 106°51', sp3
- B. 104°31', sp3
- C. 110°, sp3
- D. None of these
Explanation: The bond angle in CH3OCH3 is 110° in spite of sp3 hybridization of O and two lone pair due to steric hindrance.
Correct answer: 110°, sp3- A. Fumaric acid shows intermolecular H-bonding
- B. Fumaric acid shows intramolecular H-bonding
- C. Maleic acid is dibasic acid
- D. Maleic acid shows chelation or intramolecular H-bonding
Explanation: Maleic acid shows intramolecular H-bonding (chelation) and thus-COOH is stabilized.
Correct answer: Maleic acid shows chelation or intramolecular H-bonding- A. AsH3> BiH3> SbH3> NH3> PH3
- B. BiH3> SbH3> AsH3> PH3> NH3
- C. NH3> PH3> AsH3> SbH3> BiH3
- D. PH3> NH3> AsH3> SbH3> BiH3
Explanation: Dipole moment of MH3 decreases down the group as the electronegativity of the central atom M decreases.
Correct answer: NH3> PH3> AsH3> SbH3> BiH3- A. dsp2 , square planar
- B. sp3 , tetrahedral
- C. sp3d, trigonal bipyramidal
- D. d2sp3,octahedral
Explanation: In Wilkinson's catalyst (a homogeneous catalyst), (Ph3P)3 RhCl, Rh is dsp2 hybridized giving a square planar shape to the compound.
Correct answer: dsp2 , square planar- A. dsp2 , dsp3 , sp2 and sp3
- B. sp3, dsp2, dsp3, sp2
- C. dsp2, sp2, sp3, dsp3
- D. dsp2, sp3, sp2, dsp3
Explanation: There is only one option with sp3 hybridization of NH3 and sp2 hybridization of BCl3.
Correct answer: sp3, dsp2, dsp3, sp2- A. the molecular plane
- B. a plane parallel to the molecular plane
- C. a plane perpendicular to the molecular plane which bisects the carbon−carbon σ−bond at right angle
- D. a plane perpendicular to the molecular plane which contains the carbon−carbon σ−bond.
Explanation: Nodal plane is a plane where the probability of finding an electron is almost zero.
Correct answer: a plane parallel to the molecular plane- A. LiCl> BeCl2> BCl3> CCl4
- B. LiCl< BeCl3< BCl3< CCl4
- C. LiCl> BeCl2> CCl4> BCl3
- D. LiCl< BeCl3< BCl3> CCl4
Explanation: Smaller cation causes more polarization of anion. The covalent character of ionic compound can be determined by Fajans rules,the cation…
Correct answer: LiCl< BeCl3< BCl3< CCl4- A. nitrogen has no vacant 2 d-orbitals
- B. NCl5 is unstable
- C. nitrogen atom is much smaller than P
- D. nitrogen is highly inert
Explanation: Excitation of 2s electron in N is not possible. PCl5 forms five bonds by using the d-orbitals to "expand the octet" and have more "places"…
Correct answer: nitrogen has no vacant 2 d-orbitals- A. inCl4-
- B. S inSO3
- C. N inNO-3
- D. S in SO2-3
Explanation: P in PO3-4 has sp3 hybridization like S in SO2-3 .
Correct answer: S in SO2-3- A. BeF2
- B. BCl3
- C. NH3
- D. CIF3
Explanation: ClF3 has sp3d hybridization with two lone pairs of electron on the central Cl atom.
Correct answer: CIF3- A. Mg2+
- B. Al3+
- C. Ca2+
- D. Na+
Explanation: A small cation has more polarizing power. Polarising power depends upon size of cation and charge of cation so higher the charge of cation…
Correct answer: Al3+- A. He2+
- B. H2
- C. H2+
- D. H2-
Explanation: Molecular orbital configuration for H2 is s1s2 in which all the electrons are paired. As diamagnetism is shown by paired electrons only.
Correct answer: H2- A. One sigma, one pi
- B. One sigma, two pi
- C. Two sigma, one pi
- D. Two sigma, two pi
Explanation: Calcium carbide is an ionic carbide having [:C ≡ C :] 2+. In the C ≡ C bond, there are one sigma and two pi bonds.
Correct answer: One sigma, two pi- A. The number of unpaired p-electrons
- B. The number of paired d-electrons
- C. The number of unpaired s-and p-electrons
- D. The actual number of s-and p-electrons in the outermost shell.
Explanation: In chemical bonding, atoms can share electrons to form covalent bonds. The number of covalent bonds an atom can form, known as its…
Correct answer: The actual number of s-and p-electrons in the outermost shell.- A. To decrease number of electrons in the outermost orbit.
- B. To attain an inert gas configuration.
- C. To increase number of electrons in the outermost orbit.
- D. To attain 18 electrons in the outermost orbit.
Explanation: The combination of atoms occurs because they want to attain an inert gas configuration.
Correct answer: To attain an inert gas configuration.- A. Around one atom of the molecule
- B. Between the two nuclei of the molecule
- C. At the region away from the nuclei of the molecule
- D. at no place
Explanation: In an antibonding molecular orbital, electron density is minimum between the two nuclei of the molecule.
Correct answer: Between the two nuclei of the molecule- A. F-
- B. O2-
- C. N3-
- D. Na+
Explanation: Ionic size decreases along the period form left to right. More over anions are of larger size as compare to cations.
Correct answer: N3-- A. Increases
- B. Decreases
- C. Remains same
- D. First decreases, then increases
Explanation: Atomic radius decreases along the period due to Increasing effective nuclear charge.
Correct answer: Decreases- A. A->A>A+
- B. A>A+>A-
- C. A+>A>A-
- D. A->A+>A
Explanation: A2->A->A>A+>A2+On the periodic table, atomic radius generally decreases as you move from left to right across a period (due to increasing…
Correct answer: A->A>A+- A. V A
- B. VI A
- C. VII A
- D. VIII A
Explanation: Electron affinity is the amount of energy released when an electron is added to the valence shell of an isolated gaseous atom and its…
Correct answer: VII A