The highest energy molecular orbital in O2 is a diatomic molecular orbital, specifically a π* orbital.

PCl5 has a trigonal bipyramidal shape due to five bonding pairs around the phosphorus atom.

SF6 has six bonding pairs and no lone pairs, leading to an octahedral shape.

AX2E2 indicates two bonding pairs and two lone pairs, resulting in a bent shape.

AX3E indicates three bonding pairs and one lone pair, resulting in a trigonal pyramidal shape.

AX4 indicates four bonding pairs and no lone pairs, resulting in a tetrahedral shape.

The water molecule has a bent shape due to the two lone pairs on the oxygen atom.

NaCl is formed by an ionic bond due to the transfer of electrons from sodium to chlorine.

Metallic bonds are formed between metal atoms, characterized by a 'sea of electrons' that are free to move.

Ethylene has sp2 hybridization due to the presence of a double bond between the carbon atoms.

The carbon atoms in ethylene undergo sp2 hybridization.

BF3 has sp2 hybridization as it has three bonding pairs and no lone pairs.

Ethylene has sp2 hybridization as each carbon atom forms three sigma bonds and one pi bond.

Methane has sp3 hybridization as it has four equivalent bonds formed by the mixing of one s and three p orbitals.

The carbon atoms in ethylene undergo sp2 hybridization, resulting in a planar structure.

H2O exhibits hydrogen bonding due to the presence of hydrogen atoms bonded to highly electronegative oxygen.

Water exhibits hydrogen bonding due to the presence of O-H bonds.

Water exhibits hydrogen bonding due to the presence of O-H bonds and the polarity of the molecule.

Water exhibits all three types of intermolecular forces, including hydrogen bonds, dipole-dipole interactions, and London dispersion forces.

sp3 hybridization corresponds to a tetrahedral molecular geometry, as seen in CH4.

In CO2, the carbon atom is sp hybridized as it forms two double bonds with oxygen.

O3 (ozone) has a bent shape due to the presence of a lone pair on the central oxygen atom.

PCl5 has phosphorus in the center, which is dsp3 hybridized, leading to a trigonal bipyramidal geometry.

In CO2, the carbon atom is sp hybridized, forming two double bonds with oxygen.

XeF4 has four bonding pairs and two lone pairs, leading to a square planar geometry.

Triple bonds are the strongest type of covalent bond due to the presence of three shared electron pairs.

NH3 exhibits hydrogen bonding due to the presence of a nitrogen atom bonded to hydrogen.

In SF4, the sulfur atom is sp3d hybridized, resulting in a seesaw molecular geometry.

C2H2 (ethyne) has a linear shape due to sp hybridization of carbon.

BF3 has a trigonal planar geometry due to the sp2 hybridization of boron.