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 43 of 49
- A. SO3
- B. NH3
- C. CO2
- D. NO
Explanation: The reason why SO3 has a perfect triangular structure is because the sulfur atom has 6 valence electrons, and it shares 2 electrons with…
Correct answer: SO3- A. IA and IIA
- B. IB and VIIB
- C. IA, llA and VII A
- D. IA and IB
Explanation: In ionic compounds, one element donates electrons (typically a metal or an element with low electronegativity), becoming a positively…
Correct answer: IA, llA and VII A- A. 0
- B. 1
- C. 3
- D. 4
Explanation: Ammonia (NH3) has one unpaired electron. Each hydrogen (H) atom contributes one electron to form a covalent bond with the central nitrogen…
Correct answer: 1- 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, both will have equal bond dissociation energy.
- D. Bond length of H2+ is less than bond length of H2.
Explanation: The correct answer is that the bond dissociation energy of H2+ is more than that of He2+.
Correct answer: Bond dissociation energy of H2+ is more than bond dissociation energy of He2+.- 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 the significant energy difference between 3s and 3p orbitals, the lone pair on phosphorous prefers to occupy an unhybridized s-orbital rather than a hybridized sp3 orbital.
- D. Phosphorous forms pπ - dπ bonds while nitrogen doesn't.
Explanation: The correct explanation for the difference in bond angles between PH3 and NH3 lies in the high energy difference between the 3s and 3p…
Correct answer: Due to the significant energy difference between 3s and 3p orbitals, the lone pair on phosphorous prefers to occupy an unhybridized s-orbital rather than a hybridized sp3 orbital.- A. dsp2, dsp3, sp2, sp3
- B. sp3, dsp2, dsp3, sp2
- C. dsp2, sp2, sp3, dsp3
- D. dsp2, sp3, sp2, dsp3
Explanation: The hybridization of the central atoms can be determined based on the number of electron pairs and geometry:NH3: The nitrogen atom forms…
Correct answer: sp3, dsp2, dsp3, sp2- A. Lies in the plane of molecules
- 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: In ethene (C2H4), the π-bond is formed by the overlap of p-orbitals from each carbon atom.
Correct answer: Lies in the plane of molecules- A. LiCl> BeCl2> BCl3> CCl4
- B. LiCl< BeCl2< BCl3< CCl4
- C. LiCl> BeCl2> CCl4> BCl3
- D. LiCl< BeCl3< BCl3> CCl4
Explanation: The correct order of covalent character among these compounds is LiCl < BeCl2 < BCl3 < CCl4.
Correct answer: LiCl< BeCl2< BCl3< CCl4- A. CFl4, SF4
- B. PCl3, BF3
- C. XeF2, CO2
- D. PF5, IF5
Explanation: The correct answer is XeF2 and CO2. Both of these molecules are linear, with bond angles of 180 degrees.
Correct answer: XeF2, CO2- A. These are generally in solid state at room temperature.
- B. The force of attraction between ions is non-directional.
- C. Ionic compounds are not always soluble in any polar solvent. It depends on the solvent.
- D. They conduct electricity in molten and solution state.
Explanation: Ionic compounds are not always soluble in any polar solvent. It depends on the solvent.
Correct answer: Ionic compounds are not always soluble in any polar solvent. It depends on the solvent.- A. HI
- B. HF
- C. HCl
- D. HBr
Explanation: The ionic character of a bond is directly related to the difference in electronegativity between the bonded atoms.
Correct answer: HF- A. Benzene
- B. Boron trifluoride
- C. Ethene
- D. Phosphorus trichloride
Explanation: Phosphorus trichloride does not have a planar geometry. It has a trigonal pyramidal molecular geometry.
Correct answer: Phosphorus trichloride- A. Al2O3 and Al2Cl6
- B. P4O10 and PCl3
- C. SiO2 and SiCl4
- D. HF and PbCl4
Explanation: Al2O3 (aluminum oxide) is a giant ionic compound. It consists of a three-dimensional lattice of aluminum ions (Al+3) and oxygen ions…
Correct answer: Al2O3 and Al2Cl6- A. NF3
- B. C3H8
- C. C2Cl4
- D. C3H6
Explanation: The molecule C3H8, which is propane, has only non-coplanar tetrahedral geometry.Propane (C3H8) consists of three carbon atoms bonded…
Correct answer: C3H8- A. Option A: The bond angle between CH3 and C is 1200.
- B. Option B: The bond angle between C and O is 1800.
- C. Option C: The bond angle between CH3 and C is 109.50 and between C and O is 1050.
- D. Option D: The bond angle between CH3 and C is 900.
Explanation: The angle P(between CH3 and C)is 109.50.The carbon atom in the methyl group forms tetrahedral angles due to its four single bonds…
Correct answer: Option C: The bond angle between CH3 and C is 109.50 and between C and O is 1050.- A. C2H4
- B. H2S
- C. CO2
- D. NCl3
Explanation: In the nitrogen trichloride molecule (NCl3), there are three single bonds between the nitrogen and chlorine atoms.
Correct answer: NCl3- A. Ammonia (NH3)
- B. Sulfur trioxide (SO3)
- C. Sulfate ion (SO42-)
- D. Sulfur dioxide (SO2)
Explanation: The sulfate ion (SO4-2) has a tetrahedral geometry. It consists of four oxygen atoms bonded to the central sulfur atom, forming a…
Correct answer: Sulfate ion (SO42-)- A. Option A: C2H2 has two sigma (σ) bonds and two pi (π) bonds.
- B. Option B: C2H2 has two sigma (σ) bonds and one pi (π) bond.
- C. Option C: C2H2 has three sigma (σ) bonds and two pi (π) bonds.
- D. Option D: C2H2 has four sigma (σ) bonds and two pi (π) bonds.
Explanation: C2H2(acetylene) has a triple bond between the two carbon atoms, consisting of one sigma (σ) bond and two pi (π) bonds.
Correct answer: Option C: C2H2 has three sigma (σ) bonds and two pi (π) bonds.- A. Electronegativity difference
- B. Bond order
- C. S-character
- D. Number of lone pairs
Explanation: Lone pairs are non-bonding electron pairs present on an atom. They can exert repulsive forces on the electrons involved in neighboring…
Correct answer: Number of lone pairs- A. SO2
- B. CCl4
- C. SO3
- D. H2O
Explanation: Sulfur trioxide has a trigonal planar molecular geometry. It consists of three oxygen atoms bonded to a central sulfur atom, with no lone…
Correct answer: SO3