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 28 of 49
- A. ns¹
- B. ns²
- C. ns²np⁵
- D. ns²np⁶
Explanation: The group with the electron configuration ns²np⁶ represents the noble gases.
Correct answer: ns²np⁶- A. N
- B. Cl
- C. O
- D. He
Explanation: Electron affinity is the energy change when an electron is added to a neutral atom.
Correct answer: He- A. High I.E of metal
- B. Low lattice energy
- C. Low E.A of nonmetal
- D. Low I.E of metal
Explanation: For an ionic bond to form, a metal atom must lose one or more electrons to become a cation.
Correct answer: Low I.E of metal- A. OH⁻
- B. BF₄⁻
- C. NH₄⁺
- D. H₃O⁺
Explanation: A dative (or coordinate covalent) bond involves one atom providing both electrons for the shared pair.
Correct answer: OH⁻- A. Nitride ion
- B. Chloronium ion
- C. Hydronium ion
- D. All of these
Explanation: The hydronium ion (H₃O⁺) is formed when a water molecule (H₂O) uses one of its lone pairs of electrons to form a bond with a hydrogen ion…
Correct answer: Hydronium ion- A. 25% and 33%
- B. 33% each
- C. 33% and 25%
- D. 25% each
Explanation: In both the tetrafluoroborate ion (BF₄⁻) and the ammonium ion (NH₄⁺), there are four total covalent bonds.
Correct answer: 25% each- A. Ionic
- B. Polar covalent
- C. Non-polar covalent
- D. Metallic
Explanation: When there is an unequal sharing of electrons due to a moderate difference in electronegativity between the bonded atoms, the bond is…
Correct answer: Polar covalent- A. H₂S
- B. SO₂
- C. O₃
- D. BeCl₂
Explanation: In Beryllium Chloride (BeCl₂), the central Beryllium atom has two bonding pairs and zero lone pairs of electrons.
Correct answer: BeCl₂- A. CH₄
- B. PCl₅
- C. NH₄⁺
- D. PCl₃
Explanation: In Phosphorus Trichloride (PCl₃), the central phosphorus atom forms three single bonds with the chlorine atoms and has one lone pair of…
Correct answer: PCl₃- A. Linear
- B. Angular
- C. Pyramidal
- D. Tetrahedral
Explanation: The amide ion (NH₂⁻) has a central nitrogen atom with two bonding pairs and two lone pairs of electrons.
Correct answer: Angular- A. CO₂
- B. PH₃
- C. NO₃⁻
- D. SO₃
Explanation: In Sulfur trioxide (SO₃), the central sulfur atom is bonded to three oxygen atoms with no lone pairs.
Correct answer: SO₃- A. It doesn't address the shapes of the molecules
- B. It doesn't involve the criteria of bond formation
- C. It doesn't explain the paramagnetic behavior of O₂
- D. None of the above
Explanation: Valence Bond Theory predicts that the O₂ molecule should be diamagnetic because it shows all electrons as paired.
Correct answer: It doesn't explain the paramagnetic behavior of O₂- A. Sigma bond
- B. Pi bond
- C. Metallic bond
- D. Coordinate covalent bond
Explanation: A sigma (σ) bond is a type of covalent bond formed by the direct, head-on overlap of atomic orbitals along the internuclear axis.
Correct answer: Sigma bond- A. Non-hybridized p-orbitals
- B. Hybrid orbitals
- C. Hybrid and non-hybrid orbitals
- D. Atomic orbital and hybrid orbital
Explanation: Pi (π) bonds are formed by the sideways or parallel overlap of unhybridized p-orbitals.
Correct answer: Non-hybridized p-orbitals555. The concept of hybridization was introduced to explain which of the following drawbacks of VBT?
- A. It does not explain paramagnetism of O₂
- B. It does not explain odd electron systems
- C. It could not explain the tetravalency of carbon
- D. All of the above
Explanation: The ground state electron configuration of carbon only has two unpaired electrons, suggesting it should form two bonds.
Correct answer: It could not explain the tetravalency of carbon- A. s-s orbitals
- B. p-p head-on overlapping of orbitals
- C. s-p orbitals
- D. p-p parallel overlapping of orbitals
Explanation: A chlorine atom has one unpaired electron in a 3p orbital. The covalent bond in a Cl₂ molecule is formed by the direct, head-on overlap of…
Correct answer: p-p head-on overlapping of orbitals- A. Dissolution
- B. Resonance
- C. Hybridization
- D. Ionization
Explanation: Hybridization is a theoretical concept where atomic orbitals of slightly different energies and shapes mix to form a new set of hybrid…
Correct answer: Hybridization- A. 1
- B. 3
- C. 2
- D. 4
Explanation: The ground state electron configuration of carbon is 1s² 2s² 2p². According to Hund's rule, the two electrons in the 2p subshell will…
Correct answer: 2- A. C
- B. O
- C. P
- D. F
Explanation: Phosphorus (P) is in the third period of the periodic table, which means it has access to empty 3d orbitals.
Correct answer: P- A. Benzene
- B. Boron trifluoride
- C. Ethene
- D. Phosphorus trichloride
Explanation: Phosphorus trichloride (PCl₃) has a trigonal pyramidal shape because the phosphorus atom has one lone pair.
Correct answer: Phosphorus trichloride