Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chem 122 Final > Final > Flashcards

Final Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Reaction mechanism

A

sequence of steps that sum to give the overall reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

diffusion

A

the spread of one substance throughout a space or throughout a second substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

effusion

A

escape of gas molecules through a tiny hole into an evacuated space

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Dispersion forces

A
  • more electrons, bigger molecule, stronger attractions

- bigger surface area, more disperson forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

catalyst

A

speeds up reaction, lower activation energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Le Chatelier principle

A

states that when a stress is applied to a system at equilibrium, the system will respond by shifting in the direction that minimizes at equilibrium by any of the following means

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Molecules exhibiting hydrogen bonding

A

H - O: water, alcohols, -OH
H - N: amines
h - F

high boiling points

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Properties of liquids

A

vapor pressure: tendency of a molecule to have enough KE to escape into the gas phase
Pvap increases with temperature
Pvap increases until rate of evaporation equals the rate of condensation
weak IMFs, higher vapor pressure
Pvap increases until evaporation rate = condensation rate /with temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

surface tension

A

the amount of energy requires to stretch or increase the surface oif a liquid by a unit area
The stronger the IMF, the higher the surface tension

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

capillary action

A

the movement of a liquid up a narrow tube

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

cohesion

A

attraction between like molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

adhesion

A

is the attraction between unlike molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

dipole-dipole interactions

A

attractive forces that act between polar molecules

the larger the dipole, the larger the attractive force

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Hydrogen bonding

A

molecules that contain H bonded to a small, highly electronegative atom, such as N, O, or F

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Ion-dipole interactions

A

attractions between ions and polar molecules
magnitude of ion-dipole interactions depends on the charge and the size of the ion, and on the dipole moment and size of the polar molecule
-Cations generally interact more strongly with dipoles than anions (of the same magnitude charge) because they tend to be smaller

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

misicible

A

two liquids are said to be miscible if they are completely soluble in each other in all proportions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Coordination number

A

the number of atoms surrounding an atom in a crystal lattice
-indicates how tightly packed the atoms are
-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Unit cell

A

basic repeating structural unit of a crystalline solid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

simple cubic

A

8 corner atoms, CN=6

1 EQUIVALENT ATOM

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Body centered

A

8 corner atoms
CN=8
2 equivalent atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Face centered cubic

A

CN=12

4 equivalent atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

saturated solution

A

one that contains the maximum amount of a solute that will dissolve in a solvent at a specific temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

solubility

A

the amount of solute dissolved in a given volume of a saturated

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

unsaturated solution

A

one that contains less solute than it has the capacity to dissolve

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

supersaturated solution

A

contains more dissolved solute than is present in a saturated solution. Generally not stable, and eventually the dissolved solute will come out of solution.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Ion-dipole

A

the charge of an ion is attracted to the partial charge on a polar molecule ex. NaCl or KI in H2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Dipole-induced dipole

A

The partial charge on a polar molecule induces a temporary partial charge on a neighboring nonpolar molecule or atom Ex. He or CO2 in H2O

28
Q

Ion-induced dople

A

The charge of an ion induces a temporary partial charge on a neighboring nonpolar molecule or atom

29
Q

colligative properties

A

properties that depend on the number of solute particles in solution but do not depend on the nature of the solute particles.

30
Q

Raoult’s Law

A

relates the the vapor pressure of an solution is dependent on the mole fraction of a solute added to solution.

Psolution = ΧsolventP0solvent

where
Psolution is the vapor pressure of the solution
Χsolvent is mole fraction of the solvent
P0solvent is the vapor pressure of the pure solvent

If more than one solute is added to the solution, each individual solvent’s component is added to the total pressure.

31
Q

colloids

A

disperson of particles from one substance through another substance

32
Q

aerosol

A

liquid or solid dispersed into a gas

33
Q

emulsions

A

liquids dispersed in another liquid

34
Q

sols

A

solid dispersed in a liquid or in another solid

35
Q

gels

A

liquid dispersed in a solid

36
Q

Dispersion forces are greater in a _____ molecule?

A

The shape of the molecule affects the strength of dispersion forces: long, skinny
molecules (like n-pentane tend to have stronger dispersion forces than short, fat ones (like
neopentane).

37
Q

Ionic Crystals Cohesive forces are

A

Coulubic forces and dispersion forces. Example being NACL, LiF, MgO, CaCo3

38
Q

Covalent cohesive forces are

A

Covalent bonds being diamond and quartz

39
Q

Molecular cohesive forces are

A

Dispersion and dipole dipole forces and hydrogen bonds

40
Q

Metallic cohesive forces are

A

Metallic bonds being including all metallic elements, Na,Mg and Fe

41
Q

The higher the lattice energy the more stable the compound

A

Because the have stronger cohesive forces and therefor a high melting point

42
Q

What is fusion

A

Fusion is the the energy required in kj/mole to melt i mole of solid

43
Q

Henrys Law

A

(c) the molar concentrations of a dissolved gas. (p) is pressure, and K is the proportionate constant.
C=kp

44
Q

Henry’s Law States ___

A

That the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution.

45
Q

What is the universal solvent?

A

Water

46
Q

What is a solute?

A

Something that is dissolved in a solvent

47
Q

Volatile

A

They vapor pressure is measurable

48
Q

Boiling point

A

Is the temperature at which vapor pressure equals external atmospheric pressure.

49
Q

Statement The presences of a nonvolatile substance lowers the vapor pressure of the solution . Increases the boiling point and lowers the freezing point (freezing point depression).

A

:D

50
Q

Heterogeneous Catalyst

A

The reactants and the catalyst are in different phases. The catalyst is usually a solid. Reactants are either gases or liquids.

51
Q

Homogeneous Catalysis

A

The reactants and the catalyst are dispersed in a single phase, usually liquid.

52
Q

Le chateliers Principle

A

States that when stress is applied to a system, the system will shift to minimize the stress.

53
Q

What counts as stress?

A

addition or removal of reactant or product
change in volume
change in temperature

54
Q

The addition of a product or removal of a reactant will cause the equilibrium to shift to the ___.

A

Left

55
Q

The addiction of a reactant or removal of a product will cause the reaction to shift to the __.

A

right

56
Q

Entropy definition

A

How spread out a systems energy is

57
Q

Standard Reduction potential

A

E cell

58
Q

2nd law of thermodynamics

A

The entropy change for the universe is positive for spontaneous process and zero for a equilibrium process

59
Q

The 3rd lave of thermodynamics

A

The entropy change is perfectly crystalline at zero Kelvin.

60
Q

A spontaneous process

A

Occurs under a specific set of conditions.

61
Q

Buffer

A

Substance that contains a weak acid and its conjugate base is a buffer solution.

62
Q

Gamma Partical

A

Nuetron

63
Q

Alpha partical

A

Is positively charged particle, they are deflected away from the positively charged plate.

64
Q

Beta particle

A

electrons

65
Q

Buffer

A

A solution that contains a weak acid and its conjugate base (or a weak base and its conjugate acid)

  • resist changes in pH upon addition of small amounts of either an acid or a base
  • a buffer’s ability to convert a strong base to a weak base minimizes the effect of the addition on pH.

Chem 122 Final (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions