AP Chemistry Unit 3: Gases, IMF, and Bonding

Network Solid

Large single molecules in which all of the atoms are covalently bonded to each other.

Bucky Ball

C₆₀ fullerenes shaped like a soccer ball.

Crystaline Solids

Particles are in a highly ordered arrangement of particles.

Amorphous Solids

No particular ordering the arrangement of particles.

Metallic Bonds

Formed by the attraction between positively charged metal ions and delocalized electrons, allowing for conductivity and malleability.

Alloy

Behaves like a metal, but is a mixture.

Doping

Adding an impurity to the host.

2/3 Cu, and 1/3 Zn

What is brass?

Fe interstitial with C

What is steel?

Subsitutional Alloys

Similar sized atoms.

Intersitional Alloys

Different sized atoms.

Strong Intramolecular Forces

The attraction forces within the compounds (between atoms).

Weak Intermolecular Forces (IMF’s)

The attraction between compounds (molecules).

LDF

2 nonpolar molecules.

Dipole-Dipole

1 polar molecules.

H-Bonding

Molecules containing F, O, or N, that are attracted to each other.

Dipole- Induced Dipole

1 polar and 1 nonpolar molecule.

Ion-Dipole

Ion and polar covalent compound.

Ion- Ion

This is a BOND, not an attraction.

Cohesive Forces

The attraction between atoms/elements of the same substance.

Adhesive Forces

The attraction between atoms/elements of different substances.

Surface Tension

Results for the net inward force experienced by the molecules on the surface of a liquid.

Viscosity

Resistance of a liquid to flow.

Vapor Pressure

Results from molecules that have enough energy to escape into the gas phase.

Vapor

Substance that more commonly is a liquid.

Boiling Point

Vapor pressure of a liquid equals atmospheric pressure.

H_F

Energy required to change a solid at its melting point to a liquid.

H_V

Energy required to change a liquid.

Diffusion

Mixing of gases.

Effusion

Moving of gases from high to low pressure through a small hole.

0^oC is the same as…

273.15 Kelvin.

R (The constant)

0.08257L blahblahblah

To make a gas more ideal:

Decrease IMF’s, and decrease size.

Solutions

Homogeneous mixtures of 2 or more pure substances.

Solvent

Dissolves the solute.

Solute

What gets dissolved.

Solubility-Related to Attraction Forces

1. Solute-solute attractions.

2. Solvent-solvent molecule attractions.

3. Solvent must be attracted to solvent.

Lattice Energy

Breaking ionic bonds.

S_g=kP_g

• S_g: Solubility of the gas.

• k: Henny’s law constant.

• P_g: The partial pressure of the gas.

Saturated

Solvent holds as much solute as is possible at that temperature.

Unsaturated

Less than the maximum amount of solute for that temperature is dissolved in the solvent.

Supersaturated

Solvent holds more solute than is normally possible at that temperature.