The central atom X uses $sp$ hybrid orbitals for bonding.

The molecule is linear.

The central atom X has no lone pairs of electrons.

The molecule must be polar if X and Y have different electronegativities.

${\rm{HF}}$

${\rm{N}}{{\rm{F}}_3}$

${\rm{B}}{{\rm{F}}_3}$

${\rm{Cl}}{{\rm{F}}_3}$

Difference in hybridization of axial and equatorial chlorine atoms.

Unequal sharing of electrons between phosphorus and axial vs. equatorial chlorine atoms.

Greater repulsion experienced by axial bond pairs due to 90° interactions with equatorial bond pairs.

The presence of d-orbitals in phosphorus preferentially influences axial bond lengths.

The formation of a covalent bond always results in a net decrease in potential energy, leading to greater stability compared to isolated atoms.

Overlapping of atomic orbitals leads to increased electron density between the nuclei, contributing to bond formation.

The strength of a covalent bond is inversely proportional to the extent of orbital overlap.

The stability of a covalent bond arises from the balance between attractive forces between nuclei and electrons, and repulsive forces between nuclei and between electrons.

CO₂

HC≡CH (Ethyne)

N₂

All of the above

${\rm{NO}}_3^ -$

${\rm{PO}}_4^{3 - }$

${\rm{CO}}_3^{2 - }$

${\rm{NO}}_2^ -$

Naphthalene

Diamond

$NaCl$

$Mn$

The central atom X uses $sp$ hybrid orbitals for bonding.

The molecule is linear.

The central atom X has no lone pairs of electrons.

The molecule must be polar if X and Y have different electronegativities.

Boiling of ${{\rm{H}}_2}{\rm{O}}$

Melting of $KCN$

Boiling of ${\rm{C}}{{\rm{F}}_4}$

Melting of ${\rm{Si}}{{\rm{O}}_2}$

Super oxide ion

Oxygen

Carbon molecule

Unipositive ion of ${{\rm{N}}_2}$ molecule

$8{\rm{ }}and{\rm{ }}2$

$6{\rm{ }}and{\rm{ }}2$

$12{\rm{ }}and{\rm{ }}Zero$

$12{\rm{ }}and{\rm{ }}2$