The orbital electronic configuration of fluorine (Z = 9)
\(={ 1s }^{ 2 }{ 2s }^{ 2 }{ 2p }_{ x }^{ 2 }{ 2p }_{ y }^{ 2 }{ 2p }_{ z }^{ 1 }\)
M.O.E.C. of fluorine =[σ2s]² [σ*2s]² [σ2p_z]² [\(\pi\)2p_x]² [\(\pi\)2p_y]² [\(\pi\)*2p_x]² [\(\pi\)*2p_y]²
Due to presence of all filled orbitals, F2 is diamagnetic

Bond order is defined as half of the difference between the number of.electrons present in bonding and antibonding molecular orbitals.
Bond order (B.O.)\(\frac { 1 }{ 2 } \)[N_b - N_a]
If the bond order is positive (N_b > N_a), the molecule or ion will be stable. If it is negative (N_b < N_a) the molecule or ion will be unstable.

The product of magnitude of charges (+ve, or -ve) and distance between them is called dipole moment. It is usually denoted by \(\mu \) .
\(\mu =Q\times d\)
Its 51 unit is Debye.

The molecular orbital electronic configuration of both B₂ and C₂ are
B₂: [σ1s]² [σ*1s]² [σ2s]² [σ*2s]² [\(\pi\)2px]¹[\(\pi\)*2py]¹
C₂:  [σ1s]² [σ*1s]² [σ2s]² [σ*2s]² [\(\pi\)2px]²[\(\pi\)*2py]²
Since B₂ has two unpaired electrons, B₂ is paramagnetic. C₂ has no unpaired electron. Thus, C2 is diamagnetic.

CH₄ = sp³
CH = sp²
C₂H₂ = sp

Higher the bond order, greater is the stability.

2p_y and 2p_y orbitals will not a form a sigma bond. Taking x-axis as the internuclear axis, 2p_y and 2p_y orbitals will undergo lateral overlapping, thereby forming a pi (π) bond.

A Lewis Structure is a very simplified representation of the valence shell electrons in a molecule. It is used to show how the electrons are arranged around individual atoms in a molecule.
Electrons are shown as "dots" or for bonding electrons as a line between the two atoms. The goal is to obtain the "best" electron configuration, i.e., the octet rule and formal charges need to be satisfied.

Hence, given Lewis structure is not the correct

According to Kossel and Lewis, atoms combine together in order to complete their respective octets so as to acquire the stable inert gas configuration. This can occur in two ways; by transfer of one or more electrons from one atom to other or by sharing of electrons between two or more atoms.

Formic acid exists as dimer because of hydrogen bonding

Because of hydrogen bonding, it pretends larger size as well as molecular mass.

The central atom Br has seven electrons in the valence shell. Five of these will form bonds with five fluorine atoms and the remaining two electrons are present as one lone pair. Hence, total pairs of electrons are six (5 bond pairs and 1 lone pair).
To minimize repulsion between lone pairs and bond pairs, the shape becomes square pyramidal.

\(NO_{ 2 }^{ + }\)>NO₂ >\(NO_{ 2 }^{ - }\) This is because \(NO_{ 2 }^{ + }\) has no lone pair of electrons (i.e. has only bond pairs on two sides) and hence it is linear.
NO₂ has one unshared electron while \(NO_{ 2 }^{ - }\) has one unshared electron pair.
There are greater repulsion on N-O bonds in case of \(NO_{ 2 }^{ - }\) than in case of NO₂

Greater is the electronegativity difference between the two bonded atoms, greater is the ionic character.

Therefore, increasing order of ionic character of the given bonds is as follows.
C-H.

Ionic character \(\propto \)  lattice energy
\(\propto \frac { 1 }{ size \ of \ ion } \propto charge \ on \ ion,\)
A non-polar molecule like N₂ has almost negligible ionic character.
\(\therefore \)The order of ionic character is
\( ({ N }_{ 2 }<{ SO }_{ 2 }<{ CIF }_{ 3 }<{ K }_{ 2 }O\)