It show bonding and lone pairs, but do not denote shape. It wlso help us to determine shape.

In this model, we can assume that the electron pairs are placed as far as possible from each other, we can predict the shape of the molecule

This is true whether there is one or more electron pairs pointing in that direction.

To determine the electron-domain geometry, count the total number of lone pairs, single, double, and triple bonds on the central atom.

Once you have determined the electron-domain geometry, use the arrangement of the bonded atoms to determine the molecular geometry.

In the linear domain, there is two molecular geometry

If there are only two atoms in the molecule, the molecule will be linear no matter what the electron domain is.

In two molecular geometries, _______ if all electron domains are bonding

In two molecular geometries, ________ if one of the domains is a nonbonding pair.

In three molecular geometries, _______ if all are bonding pairs

In three molecular geometries, ______ if one is a nonbonding pair

In three molecular geometries, _____ if there are two nonbonding pairs.

Nonbonding pairs are physically larger than bonding pairs.

In Nonbonding Pairs, their repulsions are lesser; this tends to compress bond angles.

Double and triple bonds have larger electron domains than single bonds.They exert a greater repulsive force than single bonds, making their bond angles greater.

Five electron domains

Six electron domains

There are two distinct positions in Trigonal Bipyramidal Electron Domain

There are four distinct molecular geometries in Trigonal Bipyramidal Electron Domain

Octathedral Electron Domain Three Molecular Geometries

Equal and oppositely directed bond dipoles

Bond Dipoles

electrons of two atoms begin to occupy the same space and the sharing of space between two electrons of opposite spin results in a covalent bond.

Increased overlap brings the electrons and nuclei closer together until a balance is reached between the like charge repulsions and the electron-nucleus attraction.

form by “mixing” of atomic orbitals to create new orbitals of equal energy, called degenerate orbitals.

When two orbitals “mix” they create two orbitals; when three orbitals mix, they create three orbitals; etc.

The elements which have more than an octet

Two types of Bonds

- head-to-head overlap. – cylindrical symmetry of electron density about the internuclear axis.

– side-to-side overlap. – electron density above and below the internuclear axis.

Single bonds are always σ-bonds. Multiple bonds have one σ-bond, all other bonds are π-bonds.

Bonding electrons (σ or π) that are specifically shared between two atoms are called ?

the other electrons (shared by multiple atoms) are called ?

This theory contains the wave properties are used to describe the energy of the electrons in a molecule.

are constructive combinations of atomic orbitals.

are destructive combinations of atomic orbitals.

occurs where electron density equals zero.

Whenever there is direct overlap of orbitals, forming a bonding and an antibonding orbital, they are called

is the result of all electrons in every orbital being spin paired. These substances are weakly repelled by a magnetic field.

is the result of the presence of one or more unpaired electrons in an orbital.

The more electronegative atom has orbitals higher in energy, so the bonding orbitals will more resemble them in energy.