BL Ch 9 Molecular Shape and Bonding

The number of protons in the nucleus

The repulsion between electron pairs

The mass of the atoms involved

The temperature of the environment

Linear

Tetrahedral

Trigonal bipyramidal

Octahedral

Trigonal planar

Bent

Tetrahedral

Trigonal bipyramidal

They increase the bond angles.

They have no effect on bond angles.

They compress the bond angles.

They make bond angles equal to 90°.

Only elements with four or fewer electron domains can exist.

Some elements can have more than four electron domains, resulting in trigonal bipyramidal or octahedral geometries.

All elements must follow the octet rule strictly.

Expanding beyond the octet rule leads to linear geometries only.

There are two distinct positions: axial and equatorial.

Lone pairs occupy axial positions.

Three equatorial positions form an equilateral triangle.

Lone pairs occupy equatorial positions.

Trigonal bipyramidal

Seesaw

Square planar

T-shaped

A nonpolar molecule has equal and oppositely directed bond dipoles, resulting in no overall dipole moment.

A polar molecule has equal and oppositely directed bond dipoles, resulting in no overall dipole moment.

A nonpolar molecule has bond dipoles that do not cancel, resulting in an overall dipole moment.

A polar molecule has no bond dipoles.

Electrons of two atoms begin to occupy the same space.

This is called 'overlap' of orbitals.

The sharing of space between two electrons of opposite spin results in a covalent bond.

Electrons of two atoms never share the same space.

The atoms move infinitely close together

The potential energy increases without limit

A balance is reached between repulsion and attraction

Electrons are lost from the atoms

sp hybridization involves the mixing of one s and one p orbital

Beryllium forms two bonds due to sp hybridization

sp hybrid orbitals are always unpaired

sp hybridization results in three hybrid orbitals