Bond strength determines reactivity of diatomic gases Steps:

• Identify bond types: N2 has a triple bond (945 kJ/mol), O2 a double bond (498 kJ/mol), Cl2 a single bond (243 kJ/mol).
• Compare bond energies: Higher energy in N2 requires more activation to break, reducing reactivity.
• Evaluate electron configurations: All molecules achieve octet rule via bonding, so stability isn't due to incomplete shells.
• Assess polarity: All homonuclear diatomic bonds are nonpolar, so polarity doesn't explain differences.

Why D is correct:

• D selects statements accurately explaining N2's high bond dissociation energy as the primary factor limiting reactivity, per bond energy principles.

Why the others are wrong:

• A: True but incomplete; doesn't address why O2/Cl2 react easier despite their bonds.
• B: False; O2 and Cl2 bonds are nonpolar like N2, as atoms are identical.
• C: False; all atoms in N2, O2, Cl2 achieve full octets through covalent bonding.

Final answer: D