The correct configuration for F2 is (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)⁴(π*2p)².

The correct configuration for O2 is (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)²(π*2p)¹.

The correct configuration for F2 is (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)⁴(π*2p)².

The correct configuration for O2 is (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)²(π*2p)¹.

π bonds are formed by the side-to-side overlap of p orbitals, resulting in a planar shape.

The HOMO of benzene is cyclic due to the delocalization of π electrons in the ring structure.

The highest energy molecular orbital in O2 is a π* orbital, which has a dumbbell shape.

The highest energy molecular orbital in O2 is a diatomic molecular orbital, specifically a π* orbital.

H2 has a bond order of 1, calculated as (2 bonding electrons - 0 antibonding electrons)/2 = 1.

N2 has the highest bond order of 3, while O2 has a bond order of 2 and F2 has a bond order of 1.

BF3 has a trigonal planar geometry with bond angles of approximately 120 degrees.

He2 has a bond order of 0, calculated as (2 bonding electrons - 2 antibonding electrons)/2 = 0.

H2 has a bond order of 1, calculated as (2 bonding electrons - 0 antibonding electrons)/2 = 1.

N2 has the highest bond order of 3 among the given options.

F2 has the lowest bond energy due to the repulsion between the lone pairs on the fluorine atoms.

He2 has a bond order of 0, calculated as (2 bonding electrons - 2 antibonding electrons)/2 = 0.

According to the Aufbau principle, the σ1s molecular orbital is filled first as it has the lowest energy.

σ2s is lower in energy than the 2p atomic orbitals.

Li2 has a bond order of 1, calculated as (2 bonding electrons - 0 antibonding electrons)/2 = 1.

N2 has a bond order of 2, calculated as (number of bonding electrons - number of antibonding electrons)/2 = (10-6)/2 = 2.

O2 has a bond order of 2, while N2 has a bond order of 3, so none have a higher bond order than N2.

N2 has a bond order of 3, while O2 has a bond order of 2, so N2 has a higher bond order.

N2 has a triple bond, consisting of one sigma bond and two pi bonds.

N2 has the highest bond order of 3, calculated as (10 bonding electrons - 2 antibonding electrons)/2 = 3.

F2 is diamagnetic as it has all electrons paired in its molecular orbitals.

C2 is isoelectronic with N2, both having 10 electrons.

N2 is isoelectronic with Ne, both having 10 electrons.

Li2 is stable with a bond order of 1, while He2 and Be2 are not stable.

C and N will form a bond with the highest bond order of 3, as seen in the molecule CN.

C and N will form a stable diatomic molecule as they have suitable bond orders and electron configurations.