Chem Polarity Vsepr and IMFs

Nonpolar electron negativity difference

0-0.5

Polar electron negativity difference

0.5-2

Most times a linear lewis structure means

nonpolar

most times a bent lewis structure means

polar

Where does the pole start

Partial Positive end

Intermolecular forces

Forces that bind atoms together to form compounds

Covelent bonds

chemical bonds between atoms where electrons are shared

Imf Influences

phase changes and surface tension

Phase changes

Melting point, evaporation, and freezing point

Surface tension

The property of a surface of a liquid that allows it to resist an external force

Ion-Ion

Forces between ionic compounds (opposites attract)

Ion-Dipole

The dissolving of compounds

Dipole-Dipole

An attraction between oppositely charges regions of a polar molecule

Hydrogen Bond

The dipole–dipole interactions experienced when H is bonded to N, O, or F are unusually strong.

London Dispersion Force

are attractions between an instantaneous dipole and an induced dipole.

The Larger Molecule the BLANK LDF’s

stronger

In dipole-dipole interactions, the more polar the molecule

the higher the boiling point

If two molecules are of comparable size

and shape, BLANK interactions

will likely be the dominating force.

dipole–dipole

If one molecule is much larger than

another, BLANK will likely

determine its physical properties.

dispersion forces

In the AXE formula X represents

number of single line pair

In the AXE formula E represnt

number of lone pairs

The atom with the higher electronegativity has a

partial negative charge

The atom with lower electronegativity has a

partial positive charge