Chapter 11 - Liquids and Intermolecular

Intermolecular means

forces between molecules

What breaks intermolecular forces

Boiling

Gases and Liquids

Fluids

Liquids and Solids

Condensed states

Dispersion forces or London forces

Only occurs in non-polar molecules. It is constantly shifting to a different set of temporary forces.

Polarizability

The tendency of an electron cloud to disort.

Tighter molecules

Lower surface area, lower boiling point

Dipole-dipole interactions

They form permanent dipoles. Occurs in polar molecules.

Bad interactions

2 positive or 2 negative banging into each other

Hydrogen bonding

Strongest force. It can only be formed with a hydrogen atom bonding with a nitrogen, oxygen, or fluorine atom.

Crystalatus

Smallest defined unit that repeats inside a molecule.

Only liquid that freezes from the top

Water

Ion-dipole interactions

* Found in solutions of ions.
* Can only occur with polar compounds.

2 molecules with comparable moral masses and shapes

Dispersion forces are equal.

2 molecules have very different molar masses and there's no H-bonding

Dispersion force determines the substance with stronger attractions.

Viscosity

Resistance of a liquid to flow.

Increases with strong forces, decreases with higher temperature.

Surface tension

Water acts as if it has a skin be of the extra forces on the surface allowing water to bead up when in contact with nonpolar surfaces.

Capillary action

The rise of liquid up narrow tubes.

Cohesive forces

Intermolecular forces that bind similar molecules to one another.

Adhesive forces

Intermolecular forces that bind a substance to a surface.

Phase change

Conversion from one state to matter to another.

Melting / Fusion

Solid to liquid, endothermic.

Freezing

Liquid to solid, exothermic.

Vaporization

Liquid to gas, endothermic.

Condensation

Gas to liquid, exothermic.

Sublimation

Solid to gas, endothermic.

Deposition

Gas to solid, exothermic.

Heating curve

Graph of temperature (y) and the heat added (x).

Vapor pressure formula

* **P = nRT/V**
* **P = MRT**
* M - molarity
* R - gas constant

Vapor pressure

How much of a liquid evaporates at a certain pressure.

Vapor pressure at any temperature

__Some__ liquid molecules have enough energy to escape the surface and become a gas.

Vapor pressure while temperature increases

__More__ molecules are able to have enough energy to become a gas.

Natural log of the vapor pressure

It’s inversely proportional to its temperature.

Clausius-Clayperon equation

Clausius-Clayperon equation uses

* We can find **ΔH of vaporization** if we know the vapor pressure and the temperature at one point.
* We can find the **pressure at point 1** when we know the ΔH of vaporization and the temperature at point 2.

Phase diagram

A graph that shows the states of matter under conditions of temperature and pressure.

Triple point

The point where all three states of matter coexist.

between what are triple points

between the liquid and gas or between two solids

Critical point

* The point at which no amount of pressure alone can liquify the gas.
* Here you can’t tell the difference between a gas and a liquid.

How many triple points does carbon has

2