Nitrogen (N2) exhibits a triple covalent bond.

Covalent bonds involve the sharing of electrons between nonmetals.

Electrons are transferred from a metal to a nonmetal in ionic bonds.

Atoms gain or lose electrons to achieve a full outer shell, following the octet rule.

Ionic bonds result from the attraction between oppositely charged ions.

Nonpolar covalent bonds involve equal sharing of electrons.

Electronegativity measures an atom's ability to attract electrons.

HCl has a polar covalent bond between hydrogen and chlorine.

The bond angle in a water molecule is approximately 104.5 degrees.

Sigma bonds result from the head-to-head overlap of atomic orbitals.

Fluorine has the highest electronegativity.

The bond in methane (CH4) is covalent, involving the sharing of electrons.

Hydrogen bonds form between hydrogen and highly electronegative atoms.

Polar covalent bonds have unequal electron sharing due to electronegativity differences.

A double covalent bond involves the sharing of two pairs of electrons.

A molecule with tetrahedral electron domain geometry has a tetrahedral shape.

Metallic bonds result from the attraction between positive metal ions and a sea of electrons.

Cl2 has a nonpolar covalent bond due to identical atoms.

Nitrogen (N2) is represented by a triple covalent bond in its Lewis structure.

Polar molecules have an unequal distribution of electron density.

Sodium chloride (NaCl) exhibits an ionic bond.

A molecule with linear electron domain geometry has a linear shape.

H2O has a bent shape due to the lone pairs on the central oxygen atom.

The bond angle in a trigonal planar molecule is approximately 120 degrees.

Nonpolar covalent bonds result from atoms with identical electronegativities.

The bond angle in a tetrahedral molecule is approximately 109.5 degrees.

Nonpolar covalent bonds involve equal sharing of electrons between identical atoms.

A molecule with trigonal bipyramidal electron domain geometry has a trigonal bipyramidal shape.

Polar covalent bonds result from a significant electronegativity difference in shared electrons.

Methane (CH4) is represented by four single covalent bonds in its Lewis structure.

Dipole-dipole bonds result from the attraction between polar molecules.

The bond angle in a bent molecule is typically less than 109.5 degrees.

Pi bonds involve the overlapping of p orbitals.

A molecule with trigonal pyramidal electron domain geometry has a trigonal pyramidal shape.

Nitrogen trifluoride (NF3) is represented by three single covalent bonds in its Lewis structure.

Metallic bonds result from the attraction between positive metal ions and delocalized electrons.

A linear molecule has a bond angle of 180 degrees.

London dispersion forces result from temporary dipoles in adjacent atoms.

A molecule with seesaw electron domain geometry has a seesaw shape.

VSEPR theory predicts molecular shapes based on electron domain geometry.

Ionic bonds involve the transfer of electrons between atoms.

The bond angle in a trigonal bipyramidal molecule is approximately 90 degrees.

Carbon dioxide (CO2) is represented by one double covalent bond in its Lewis structure.

Nonpolar covalent bonds involve identical atoms sharing electrons.

The bond angle in a tetrahedral molecule is approximately 109.5 degrees.

Carbon dioxide (CO2) has a linear shape without lone pairs on the central carbon atom.

A molecule with octahedral electron domain geometry has an octahedral shape.

Nonpolar covalent bonds involve no difference in electronegativity.

Water (H2O) is represented by two single covalent bonds in its Lewis structure.

Dipole-dipole bonds involve the attraction between polar molecule ends.

The bond angle in a trigonal pyramidal molecule is approximately 107 degrees.

Polar covalent bonds involve a slight difference in electronegativity.

A molecule with square pyramidal electron domain geometry has a square pyramidal shape.

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

The bond angle in a seesaw molecule is approximately 180 degrees.

Hydrogen bonds result from the attraction between positive and negative ends of molecules.

Nitrogen trifluoride (NF3) is represented by three single covalent bonds in its Lewis structure.

Polar covalent bonds involve a significant electronegativity difference.

The bond angle in a square planar molecule is approximately 90 degrees.

Sulfur trioxide (SO3) exhibits resonance structures due to delocalization of electrons.

A molecule with linear electron domain geometry has a linear shape.

Hydrogen bonds involve the attraction between hydrogen and a nearby lone pair of electrons.

The bond angle in a bent molecule is typically less than 109.5 degrees.

Ionic bonds occur between oppositely charged ions in a crystal lattice.

A molecule with square planar electron domain geometry has a square planar shape.