The following graph is given, between total energy and distance between the two nuclei for species H2+, H2, He2+ & He2. Which of the following statements is correct:
Correct answer: B. Bond dissociation energy of H2+ is more than bond dissociation energy of He2+.
- 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+. The graph indicates that H2+ reaches a lower energy state, which means more energy is released during its formation, resulting in higher stability and bond dissociation energy. Option A is incorrect because He2+ is less stable due to its higher energy state. Option C is incorrect as it misunderstands the relationship between bond order and energy release; equal bond orders do not imply equal bond dissociation energies. Lastly, Option D is incorrect because the graph does not provide information on bond lengths.
Last updated
About Chemical Bonding
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.
Practise Chemical Bonding
964 free Chemical Bonding MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Exams that ask Chemistry questions like this
Chemistry is on 12 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
Related questions
50% inversion of configuration and 50% retention of configuration observed is characteristics of mechanism:
A bonding electron pair is attracted by of atoms?
A Cl₂ molecule is formed by the overlap of:
A co-ordinate covalent bond is present in:
A covalent bond formed by the parallel overlap of p-orbitals is a weaker bond called: