Chapter 10 - Chemical Bonding II

VB theory

________ uses hypothetical hybrid orbitals to explain methane bonding.

electron density

The ________ in a sigma molecular orbital is focused symmetrically along a line connecting the two nuclei of the bonding atoms.

dipole moments

Because they lack ________, nonpolar molecules are nonpolar.

Polar molecules

________ are diatomic compounds with dipole moments that comprise atoms of various elements (for example, HCl, CO, and NO)

covalent link

A pi bond is a(n) ________ produced by sideways overlapping orbitals with electron density concentrated above and below the plane of the connecting atoms 'nucleus.

total number of atomic orbitals

The ________ formed is always equal to the total number of molecular orbitals formed.

number of electrons

The ________ in bonding molecular orbitals is always greater than that in antibonding molecular orbitals in a stable molecule.

covalent bonds

The molecular orbital theory defines ________ in terms of molecular orbitals, which are associated with the entire molecule and result from the interaction of the atomic orbitals of the bonding atoms.

electron density

The ________ is concentrated above and below a line connecting the two nuclei of the bonding atoms in a pi molecular orbital.

dipole moment

The ________, which is the product of the charge Q and the distance r between the charges, is a quantitative measure of a bond's polarity: µ= Q × r.