Chemistry Ii Chapter 11/12

Front 1

Properties of Liquids

Back 1

1. High density compared to gases
2. Indefinite shape and assume shape of container
3. Definite volume; not easily compressed

Front 2

Properties of solids

Back 2

1. High density in comparison to gases
2. Definite shape
3. Definite volume
4. Crystalline (ordered) or amorphous (disordered)

Front 3

Properties of gas

Back 3

1. Low density
2. Indefinite shape
3. Indefinite volume

Front 4

Which has strong molecular forces? weak?

Back 4

1. Strong - solids
2. Weak - gases

Front 5

Crystalline solid versus amorphous solid?

Back 5

1. Crystalline - atoms/molecules arranged in an order
2. Amorphous - disordered

Front 6

Intermolecular forces are _____________ than bonding forces.

Back 6

1. much weaker

Front 7

Dispersion force (London force)

Back 7

1. Intermolecular force exhibited by all atoms/molecules that results from fluctuations in the electron distribution.

Front 8

An instantaneous dipole on any one helium atom induces _____________________________, which then attract one another.

Back 8

1. Instantaneous dipoles on neighboring atoms

Front 9

Dispersion force increases with __________ molar mass because _________________________________.

Back 9

1. Increasing
2. higher molar mass = more electrons dispersed over greater volume.

Front 10

Boiling points ________ with increasing _______________.

Back 10

1. Rise
2. Molar Mass

Front 11

Miscibility - of liquids

Back 11

1. Ability to mix without separating into two phases

Front 12

Dipole-Dipole force exists______________________.

Back 12

1. In all molecules that are polar

Front 13

Dipole-Dipole force

Back 13

1. Intermolecular force exhibited by polar molecules that results in an uneven charge distribution.

Front 14

Permanent Dipole

Back 14

1. Permanent separation of charge
2. Molecule always has one end slightly negative and the other slightly positive.

Front 15

Boiling points ______________ with decreasing dipole moment.

Back 15

1. Decreases
2. It increases with increasing dipole moment.

Front 16

Hydrogen bond

Back 16

1. Strong dipole-dipole attraction force between a hydrogen bonded to O, N or F and one of these electronegative atoms on a neighboring molecule.

Front 17

Ion-Dipole forces are present in mixtures between ______________________ and are ___________.

Back 17

1. Ionic Compounds and Polar Compounds
2. VERY STRONG
3. Important in aqueous solutions.

Front 18

Four types of Intermolecular forces going from weakest to strongest...

Back 18

1. Dispersion
2. Dipole-Dipole
3. Hydrogen Bonding
4. Ion-Dipole

Front 19

Surface Tension

Back 19

1. Tendency of liquids to minimize their surface area.
2. Energy required to increase the surface area by a unit amount.
3. Decreases with decreasing intermolecular forces.

Front 20

Viscosity

Back 20

1. Resistance of a liquid to flow
2. Greater in substances with strong intermolecular forces because molecules strongly attracted to eachother and don't flow around eachother as easily.

Front 21

Capillary Action

Back 21

1. Ability of a liquid to flow against gravity up a narrow tube.

Front 22

Vaporization

Back 22

1. Phase transition from liquid to gas

Front 23

Condensation

Back 23

1. Phase transition from gas to liquid

Front 24

Volatile vs Non-volatile

Back 24

1. Volatile - vaporize easily
2. Nonvolatile - do not vaporize easily

Front 25

Rate of vaporization in comparison to temp, surface, strength of intermolecular forces

Back 25

1. RofVap increases with increasing TEMP
2. RofVap increases with increasing SURFACE AREA
3. RofVap increases with decreasing strength of intermolecular forces.

Front 26

Heat of Vaporization

Back 26

1. Amount of heat required to vaporize one mole of a liquid to gas

Front 27

Dynamic Equilibrium...

Back 27

1. Rate of evaporation = Rate of Condensation

Front 28

Strong Intermolecular Forces result in _______________ substances and ___________ vapor pressures.

Back 28

1. Nonvolatile
2. Low

Front 29

Boiling point of a liquid

Back 29

1. Temperature at which vapor pressure equals external pressure.

Front 30

Critical Pressure/Temperature

Back 30

1. Point at which liquid cannot exist

Front 31

Sublimation vs deposition

Back 31

1. Phase transition from solid to gas - Sublimation
2. Phase transition from gas to solid - deposition

Front 32

Melting/Fusion vs freezing

Back 32

1. Phase transition from solid to liquid - melting/fusion
2. Phase transition from liquid to solid - freezing

Front 33

How large is the band gap in a conductor, semiconductor and insulator?

Back 33

1. Conductor - no energy gap
2. Semiconductor - small energy gap
3. Insulator - large energy gap

Front 34

n-type semiconductor vs p-type semiconductor?

Back 34

1. N-type: charge carries are negatively charged
2. P-type: hole acts as a positive charge

Front 35

Diodes

Back 35

1. Elements that allow the flow of electrical current in one direction.

Front 36

Solute vs Solvent

Back 36

1. Solvent - majority
2. Solute - minority

Front 37

Entropy

Back 37

1. Energy randomization or energy dispersal in a system.