Chem 108 Exam 1

Front 1

At constant pressure, state of matter depends on _____________ and _______________.

Back 1

thermal energy; strength of intermolecular forces

Front 2

In the gaseous state, ___________ has overcome _____________, giving molecules total freedom of motion.

Back 2

thermal energy; attractive forces between

molecules

Front 3

In the solid state, molecules don't have enough _____________ to overcome _____________.

Back 3

thermal energy; attractive forces between

molecules

Front 4

In the liquid state, molecules have enough ____________ to overcome only some ________________.

Back 4

thermal energy; attractive forces

Front 5

Coulomb's Law

Back 5

Energy of ion interaction is proportional to the charges of the two particles over the distance between them.

Front 6

Ion-Dipole

Back 6

Interaction between an ion and the partial charge of a molecule with a permanent dipole.

Front 7

Sphere of Hydration

Back 7

cluster of water molecules around an ion as it dissolves in an aqueous solution.

Front 8

Dipole-Dipole

Back 8

Interaction of two molecules with dipole

moments

Front 9

Hydrogen Bonding

Back 9

Special class of dipole-dipole interactions;

requires an H atom bonded to strongly eneg. atom (F, O, or N)

Front 10

London/Dispersion Forces

Back 10

Temporary intermolecular forces caused by the constant movement of electrons; occurs

between non-polar molecules. Can also occur between polar molecules but with little effect.

Front 11

Ion-Induced and Dipole-Induced Dipoles

Back 11

Ion or dipole induces a dipole on an otherwise non-polar molecule

Front 12

van der Waals Forces

Back 12

collection of attractive forces that hold

molecules together

Front 13

Ion and polar molecule = _____________

Back 13

Ion-Dipole IMF

Front 14

Ion and non-polar molecule = ________________

Back 14

ion-induced dipole IMF

Front 15

O-H, F-H, N-H

Back 15

Hydrogen bonding

Front 16

Polar molecule and polar molecule = _________

Back 16

dipole-dipole IMF

Front 17

Polar and non-polar molecule = ______________

Back 17

dipole-induced dipole IMF

Front 18

True or False: dispersion forces are always present regardless of the polarity of the two

molecules.

Back 18

TRUE

Front 19

Increase IMF = (increase/decrease) BP

Back 19

Increase

Front 20

Increase IMF = (increase/decrease) vapor

pressure

Back 20

decrease

Front 21

Increase IMF = (increase/decrease) melting point

Back 21

increase

Front 22

Increase IMF = (increase/decrease) surface

tension

Back 22

increase

Front 23

Increase IMF = (increase/decrease) viscosity

Back 23

increase

Front 24

Define boiling point

Back 24

temperature at which vapor pressure is equal to pressure on liquid, which is usually atmospheric pressure.

Front 25

When pressure on a liquid increases, the boiling point (increases/decreases).

Back 25

increases

Front 26

When pressure on a liquid decreases, the boiling point (increases/decreases).

Back 26

decreases

Front 27

Induced Dipole

Back 27

separation of charge in an atom/molecule due to a momentary unequal distribution of electrons

Front 28

Polarizability

Back 28

tendency of electron density to be distorted by a charged particle; related to strength of the

nucleus's pull on its electrons.

Front 29

A larger molecule/atom will have (stronger/weaker) dispersion forces than a

smaller molecule/atom.

Back 29

stronger

Front 30

A molecule with higher surface area will have (stronger/weaker) dispersion forces than a

molecule with lower surface area.

Back 30

stronger

Front 31

True or False: linear molecules exhibit stronger dispersion forces than branched molecules.

Back 31

TRUE

Front 32

Increase in Polarity of substance =

(increase/decrease) in Solubility of Polar

Substance

Back 32

Increase

Front 33

Solubility depends on......

Back 33

relative strength of solute-solvent interactions compared to solute-solute and solvent-solvent interactions.

Front 34

Substances with similar IMF (will/will not) form a solution.

Back 34

will

Front 35

Henry's Law

Back 35

C = KP

Where C = concentration of the gas

K = Henry's Law constant

P= partial pressure of gas

Front 36

True or False: pressure has little to no effect on the solubility of solids or liquids in water.

Back 36

TRUE

Front 37

Solubility of gas (increases/decreases) as

pressure increases.

Back 37

increases

Front 38

Factors that affect physical state

Back 38

temperature, IMF, pressure

Front 39

Triple Point

Back 39

spot on a phase diagram where all three phases exist

Front 40

Critical Point

Back 40

specific temperature and pressure at which the liquid and gas phases have the same density

Front 41

Supercritical Fluid

Back 41

a substance above its critical temperature and pressure