Colavent bonding

Polar covalent compounds are poor conductors of electricity in the solid state, as they lack free-moving ions or electrons.

Polar covalent compounds like HCl ionize in water (HCl → H⁺ + Cl⁻), allowing the solution to conduct electricity.

Covalent compounds do not contain ions, and their electrons are localized within bonds, preventing electrical conductivity.

CO₂ is a small, non-polar covalent molecule with weak intermolecular forces, so it exists as a gas at room temperature.

Covalent compounds typically have weaker intermolecular forces (such as van der Waals forces or dipole interactions) compared to the strong ionic bonds in ionic compounds.

H₂O has strong hydrogen bonding between molecules, which results in higher melting and boiling points compared to other covalent compounds listed.

A polar covalent bond forms when there is a significant difference in electronegativity between the atoms, causing unequal sharing of electrons.

In polar covalent compounds, electrons are unequally shared, leading to partial charges on the atoms (e.g., H₂O, where oxygen is partially negative, and hydrogen is partially positive).

In CH₄, carbon shares its four valence electrons with four hydrogen atoms, forming single covalent bonds (represented by shared electron pairs).

H₂O is a covalent compound where oxygen and hydrogen share electrons, forming polar covalent bonds.