CHAPTER 9: MOLECULAR GEOMETRY AND BONDING THEORIES

electron density

electron density

Antibonding orbitals invariably have a plane in the region between the nuclei where the ________ is zero.

Lewis

In ________ theory, covalent bonding occurs when atoms share electrons because the sharing concentrates electron density between the nuclei.

VSEPR modelis

The ________ based on the idea that electron domains are negatively charged and therefore repel one another.

MO

The energy of the resulting ________ is lower in energy than the two atomic orbitals from which it was made.

Pauli

Each MO can accommodate, at most, two electrons, with their spins paired (________ exclusion principle)

octahedron

A(n) ________ is a polyhedron with six vertices and eight faces, each an equilateral triangle.

multiple bond

In general, each nonbonding pair, single bond, or ________ produces a single electron domain around the central atom in a molecule.

dipole moment

For a molecule consisting of more than two atoms, the ________ depends on both the polarities of the individual bonds and the geometry of the molecule.

atom

If the A(n) ________ lies in the same plane as the B ________, the shape is called trigonal planar.

Electrons

________ occupying a bonding molecular orbital are called bonding electrons.

overlap region

Because the electrons in the ________ are simultaneously attracted to both nuclei, they hold the atoms together, forming a covalent bond.

p bonds

Delocalization of the electrons in its ________ gives benzene a special stability.

Lewis

________ structures, however, do not indicate the shapes of molecules; they simply show the number and types of bonds.

VSEPR model

The ________ provides a simple means for predicting molecular geometries but does not explain why bonds exist between atoms.

Lewis

Draw the ________ structure of the molecule or ion, and count the number of electron domains around the central atom.