Questions on Bond Energy
Multiple-Choice Questions: Bond Energy
1. What does bond energy represent?
A) The energy stored in the nucleus
B) The energy required to break one mole of bonds in gaseous molecules
C) The energy released during bond formation
D) The energy of ionic attraction
E) The energy needed to form an atom
2. The greater the bond energy, the:
A) Easier it is to break the bond
B) Stronger the bond
C) Lower the reactivity
D) More polar the bond
E) Greater the bond angle
3. Which bond generally has the highest bond energy?
A) Single bond
B) Double bond
C) Triple bond
D) Ionic bond
E) Hydrogen bond
4. What is the typical unit of bond energy?
A) Grams
B) Joules
C) Newtons
D) kJ/mol
E) Volts
5. Which of the following has the weakest bond energy?
A) C–H
B) H–H
C) O=O
D) F–F
E) N≡N
6. Breaking chemical bonds is a(n):
A) Endothermic process
B) Exothermic process
C) Neutral process
D) Spontaneous process
E) Radioactive process
7. Bond energy is directly related to:
A) Atomic number
B) Bond polarity
C) Bond strength
D) Electronegativity
E) Isotopic mass
8. Which bond has the highest bond energy among the following?
A) H–H
B) C–C
C) N≡N
D) O=O
E) Cl–Cl
9. Why does a triple bond have higher bond energy than a single bond?
A) It has more atoms
B) It has more shared electrons
C) It is more polar
D) It has fewer lone pairs
E) It occurs in nonmetals only
10. Which of the following would likely have the lowest bond energy?
A) Short and strong bonds
B) Bonds between small atoms
C) Long and weak bonds
D) Bonds with high electron density
E) Bonds with multiple bonds
11. What happens to energy when a bond forms?
A) Energy is released
B) Energy is absorbed
C) Energy remains unchanged
D) Neutrons are emitted
E) Light is always produced
12. Which statement is true about bond energy and bond length?
A) Longer bonds have higher energy
B) Bond energy is independent of bond length
C) Stronger bonds are longer
D) Shorter bonds usually have higher bond energy
E) Triple bonds are always longer
13. If a molecule has high bond energy, it is likely to be:
A) Very reactive
B) Radioactive
C) More stable
D) Ionic
E) Polar
14. Which of these involves the greatest bond dissociation energy?
A) C–C
B) C=C
C) C≡C
D) C–H
E) H–H
15. Bond energies are typically determined through:
A) Electrolysis
B) Radioactive decay
C) Calorimetry and thermochemical calculations
D) Spectroscopy
E) Evaporation
16. The bond energy of a C–H bond is approximately:
A) 100 kJ/mol
B) 200 kJ/mol
C) 350 kJ/mol
D) 600 kJ/mol
E) 800 kJ/mol
17. Which statement best defines average bond energy?
A) Energy to break any bond
B) Energy of one specific bond in a single molecule
C) Mean energy to break a specific type of bond in different molecules
D) Energy stored in atomic nuclei
E) Total energy released in a reaction
18. A reaction is endothermic if the:
A) Energy released is greater than energy required
B) Products have lower energy than reactants
C) Total bond energy of products is higher than reactants
D) Activation energy is zero
E) Reaction happens spontaneously
19. Which of the following best explains why O=O has lower bond energy than N≡N?
A) Oxygen is larger than nitrogen
B) Oxygen has more lone pairs
C) Double bonds are weaker than triple bonds
D) Oxygen is more electronegative
E) N≡N is more polar
20. Which molecule contains bonds with delocalized bond energies due to resonance?
A) CH₄
B) CO₂
C) H₂O
D) NO₃⁻
E) HCl
- Questions on Lewis Electron-Dot Structures
- Questions on Covalent Bonding in Polyatomic Ions
- Questions: Resonance (Chemical)
Answers with Explanations
1. B) Bond energy is the energy required to break one mole of a bond in gaseous molecules.
2. B) A higher bond energy means a stronger bond.
3. C) Triple bonds have the highest bond energy due to more shared electrons.
4. D) Bond energy is measured in kilojoules per mole (kJ/mol).
5. D) The F–F bond is weak due to electron repulsion between lone pairs.
6. A) Breaking a bond requires energy, so it is endothermic.
7. C) Bond energy is a direct measure of bond strength.
8. C) N≡N (triple bond) has the highest bond energy.
9. B) Triple bonds have more shared electrons, increasing bond strength.
10. C) Long and weak bonds have the lowest bond energy.
11. A) Bond formation releases energy—exothermic.
12. D) Shorter bonds are typically stronger and have higher bond energies.
13. C) Molecules with high bond energy are more stable.
14. C) C≡C (triple bond) requires the most energy to break.
15. C) Calorimetry and thermochemical data are used to determine bond energies.
16. C) Approximate bond energy of C–H is 350 kJ/mol.
17. C) Average bond energy is the mean value for a bond type across molecules.
18. C) In endothermic reactions, products have higher bond energy.
19. C) A double bond (O=O) is weaker than a triple bond (N≡N).
20. D) NO₃⁻ exhibits resonance, distributing bond energy across the molecule.
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