Given below are two statements:
Statement I: A hypothetical diatomic molecule with bond order zero is quite stable.
Statement II: As bond order increases, the bond length increases.
In the light of the above statements, choose the most appropriate answer from the options given below:

CONCEPT:

Bond Order and Bond Stability

• Bond Order is defined as the number of chemical bonds between a pair of atoms. It can be determined using Molecular Orbital Theory (MOT).
• A bond order of zero means that there are equal numbers of bonding and antibonding electrons, resulting in no net bond formation.
• A molecule with a bond order of zero is considered unstable and cannot exist under normal conditions.

Bond Order and Bond Length

• Bond order is inversely related to bond length. As bond order increases, the bond strength increases, and the bond length decreases.
• Higher bond order indicates stronger bonds, which are shorter in length.

EXPLANATION:

• Statement I: "A hypothetical diatomic molecule with bond order zero is quite stable." This statement is false. A bond order of zero implies no bond formation, and the molecule would not exist as a stable entity.
• Statement II: "As bond order increases, the bond length increases." This statement is also false. As bond order increases, bond strength increases, and bond length decreases.

Therefore, the correct answer is: Option 2: Both Statement I and Statement II are false.