The bond angle in methane (CH4) is approximately 109.5 degrees due to its tetrahedral geometry.

The geometry is linear when there are two bonding pairs and no lone pairs on the central atom.

NaCl is formed by the transfer of an electron from sodium to chlorine, resulting in an ionic bond.

A covalent bond is formed when two atoms share electrons to achieve stability.

A covalent bond is formed when two atoms share electrons to achieve stability.

O2 has a double bond, as two pairs of electrons are shared between the two oxygen atoms.

Liquid water exhibits hydrogen bonding due to the attraction between the hydrogen atoms of one water molecule and the oxygen atom of another.

NaCl has the highest electronegativity difference between sodium and chlorine, leading to a strong ionic bond.

HCl has a dipole moment because it is a polar molecule with a significant difference in electronegativity between hydrogen and chlorine.

H2O is a covalent compound formed by the sharing of electrons between hydrogen and oxygen atoms.

Nitrogen can form a triple bond, as seen in N2, where three pairs of electrons are shared between the two nitrogen atoms.

Sodium is most likely to form an ionic bond as it readily loses an electron to form Na+.

Sodium is most likely to form an ionic bond as it readily loses an electron to form Na+.

C≡C (triple bond) has the highest bond energy due to the strong attraction between the two carbon atoms.

CH4 (methane) has the lowest boiling point due to weak London dispersion forces compared to the other molecules.

All of the ions Na+, Cl-, and Mg2+ have achieved a stable octet configuration.

Water (H2O) has a polar covalent bond due to the difference in electronegativity between hydrogen and oxygen.

Water (H2O) has a polar covalent bond due to the difference in electronegativity between hydrogen and oxygen.