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NEET Chemistry: Bond energy Practice Questions

15 free multiple-choice questions on Bond energy (Chemical Bonding and Molecular Structure) for NEET Chemistry, each with the correct answer and a step-by-step explanation. Attempt a question, then reveal the solution to check your reasoning.

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  1. Q1. If the bond order of a bond increases, what is the expected change in the bond energy?

    • AIt decreases because the bond becomes weaker.
    • BIt increases because there are more shared electron pairs holding the nuclei together.
    • CIt decreases due to increased repulsion between electrons.
    • DIt remains the same as the orbital overlap is the same.
    Show answer & explanation

    Correct answer: B — It increases because there are more shared electron pairs holding the nuclei together.

    Increased bond order (e.g., from single to double) means more shared electron pairs are present, leading to a stronger net attraction between the nuclei, thus increasing the bond energy.

  2. Q2. The bond energy of a molecule is primarily determined by:

    • AThe number of valence electrons only.
    • BThe total volume occupied by the atoms.
    • CThe bond length only.
    • DThe nature and strength of the individual bonds within the molecule.
    Show answer & explanation

    Correct answer: D — The nature and strength of the individual bonds within the molecule.

    Molecular bond energy is the sum of the energies required to break all the individual bonds within the molecule, which depends on the nature and strength of those individual bonds.

  3. Q3. Which bond generally has the highest bond dissociation energy among the following?

    • AO=O bond
    • BC≡C bond
    • CC-H bond
    • DC-C bond
    Show answer & explanation

    Correct answer: B — C≡C bond

    Triple bonds (like C≡C) generally have higher bond dissociation energies than single or double bonds because the bonds are shorter and stronger.

  4. Q4. Which statement correctly describes the trend in bond energy for the following series: C-H, C≡C, and C=C?

    • AC-H > C≡C > C=C
    • BC≡C > C=C > C-H
    • CC=C > C≡C > C-H
    • DC-H > C=C > C≡C
    Show answer & explanation

    Correct answer: B — C≡C > C=C > C-H

    In general, bond order dictates bond strength. Triple bonds (C≡C) are stronger than double bonds (C=C), which are stronger than single bonds (C-H).

  5. Q5. Which of the following statements best describes bond energy?

    • AThe energy required to break a specific bond in a molecule.
    • BThe potential energy stored in the electron cloud of an isolated atom.
    • CThe total kinetic energy of the atoms in a bond.
    • DThe energy released when two atoms combine to form a molecule.
    Show answer & explanation

    Correct answer: A — The energy required to break a specific bond in a molecule.

    Bond energy (or bond dissociation energy) is the energy required to break a specific bond in a molecule into its constituent atoms.

  6. Q6. If the bond dissociation energy of H₂ is 436 kJ/mol and O₂ is 498 kJ/mol, which bond is stronger?

    • AH-H bond
    • BBoth bonds have equal strength
    • CNeither bond is stronger
    • DO-O bond
    Show answer & explanation

    Correct answer: D — O-O bond

    The O-O bond dissociation energy (498 kJ/mol) is greater than the H-H bond dissociation energy (436 kJ/mol), meaning the O-O bond is stronger.

  7. Q7. What is the definition of bond dissociation energy (BDE)?

    • AThe energy released during the formation of ionic bonds.
    • BThe energy released when two atoms form a bond.
    • CThe energy required to break one mole of a specific bond.
    • DThe total energy stored in a molecule.
    Show answer & explanation

    Correct answer: C — The energy required to break one mole of a specific bond.

    Bond dissociation energy (BDE) is the amount of energy required to break one mole of a specific type of bond in the gaseous state.

  8. Q8. The energy released when bonds are formed is typically measured as:

    • AKinetic Energy
    • BInternal Energy
    • CPotential Energy
    • DBond Energy (Enthalpy of Bond Formation)
    Show answer & explanation

    Correct answer: D — Bond Energy (Enthalpy of Bond Formation)

    The energy released when bonds are formed is known as bond energy or the enthalpy of bond formation, which is related to the stability gained upon bonding.

  9. Q9. The bond dissociation energy (BDE) of a bond is defined as:

    • AThe energy required to form the bond.
    • BThe potential energy stored in a molecular structure.
    • CThe energy required to break one mole of bonds in the gaseous state.
    • DThe energy released when two atoms combine.
    Show answer & explanation

    Correct answer: C — The energy required to break one mole of bonds in the gaseous state.

    Bond dissociation energy is the energy required to break one mole of bonds in the gaseous state.

  10. Q10. Which type of bond generally has the highest bond dissociation energy?

    • ADouble bond
    • BTriple bond
    • CSingle bond
    • DCoordinate bond
    Show answer & explanation

    Correct answer: D — Coordinate bond

    Bond dissociation energy increases with the number of shared electron pairs, hence triple bonds (which involve three shared pairs) have the highest bond energy.

  11. Q11. When a bond is converted from a single bond to a double bond between the same two atoms, what happens to the bond energy?

    • AThe bond energy remains unchanged.
    • BThe bond energy increases.
    • CThe bond energy decreases.
    • DThe bond energy is halved.
    Show answer & explanation

    Correct answer: B — The bond energy increases.

    Converting a single bond to a double bond involves adding an additional shared electron pair, increasing the overall stability and strength of the bond, thus increasing the bond energy.

  12. Q12. The bond dissociation energy of a covalent bond is generally related to the bond length. What is the general trend observed?

    • AAs bond length increases, bond energy increases.
    • BAs bond length decreases, bond energy increases.
    • CBond energy is independent of bond length.
    • DBond energy decreases as bond length increases.
    Show answer & explanation

    Correct answer: B — As bond length decreases, bond energy increases.

    Shorter bonds (smaller internuclear distance) generally have higher bond energy because the attractive forces between the nuclei are stronger.

  13. Q13. Which type of bond generally requires the highest energy input to break?

    • AIonic bond
    • BSingle covalent bond
    • CDouble covalent bond
    • DTriple covalent bond
    Show answer & explanation

    Correct answer: D — Triple covalent bond

    Triple bonds (like in N₂ or O₂) involve stronger, shorter bonds, requiring more energy to break compared to single or double bonds of similar elements.

  14. Q14. The energy required to break a bond is related to the potential energy difference between the bonded state and the separated state. This energy is often referred to as:

    • ABond potential.
    • BInternal energy.
    • CBond energy.
    • DDissociation potential.
    Show answer & explanation

    Correct answer: C — Bond energy.

    The energy required to separate the atoms from their bonded state is the definition of bond energy (or dissociation energy).

  15. Q15. When comparing the bond dissociation energies of C-C single bond versus C=C double bond in ethene, which bond is stronger?

    • AThe C=C double bond
    • BThey have equal strength
    • CThe C-C single bond
    • DThe stability is determined by the surrounding environment
    Show answer & explanation

    Correct answer: A — The C=C double bond

    In general, the double bond (C=C) is stronger than the single bond (C-C) because it involves the sharing of two pairs of electrons, resulting in increased electron density and stronger attraction between the nuclei.

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