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.

Ozone (O3) exhibits resonance due to the delocalization of electrons.

H2O has two bonding pairs and two lone pairs, leading to a bent molecular geometry.

H2O has two bonding pairs and two lone pairs, leading to a bent molecular geometry.

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.

CO2 has a linear shape due to the arrangement of its double bonds.

PCl5 has five bonding pairs and no lone pairs, leading to a trigonal bipyramidal geometry.

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.

Ammonia (NH3) is polar due to its trigonal pyramidal shape and the presence of a lone pair on nitrogen.

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.

N2 and CO both have a bond order of 3.

In SF4, the sulfur atom is sp3d hybridized, resulting in a seesaw molecular geometry.

F2 has a bond order of 1, calculated as (8 bonding electrons - 6 antibonding electrons)/2 = 1.

In CCl4, the central carbon atom is sp3 hybridized, forming a tetrahedral geometry.

CO2 has a linear geometry due to the sp hybridization of the carbon atom.

BeCl2 has two bonding pairs and no lone pairs, resulting in a linear molecular geometry.

BeCl2 has two bonding pairs and no lone pairs, resulting in a linear shape.

CH4 has a tetrahedral shape due to sp3 hybridization of the carbon atom.

PCl5 has five bonding pairs and no lone pairs, resulting in a trigonal bipyramidal geometry.