Question

The ions H₂⁺ have been observed in gas discharges. H₂⁺ has been reported to have a bond distance of 106 pm and a bond dissociation enthalpy of 255 kJ mol⁻¹. Comparable values for the neutral molecule are 74.2 pm and 436 kJ mol⁻¹. Explain.

A) The presence of an extra proton in H₂⁺ increases the bond distance and weakens the bond.
B) The extra proton in H₂⁺ strengthens the bond, leading to a longer bond distance.
C) The bond dissociation enthalpy of H₂⁺ is higher due to the additional proton, resulting in increased bond strength.
D) The neutral molecule H₂ has a stronger bond due to the absence of an extra proton, resulting in a shorter bond distance.

Answer 1

The presence of an extra proton in H₂⁺ strengthens the bond and shortens the bond distance.

Step-by-step explanation:

The presence of an extra proton in H₂⁺ actually strengthens the bond and shortens the bond distance.

When an extra proton is added, the positive charge increases, resulting in a stronger electrostatic attraction between the protons and the electron. This increased bond strength leads to a shorter bond distance compared to the neutral molecule.

Therefore, option B) The extra proton in H₂⁺ strengthens the bond, leading to a shorter bond distance is the correct explanation.