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Chem 122 Final > Final > Flashcards

Final Flashcards

1
Q

Reaction mechanism

A

sequence of steps that sum to give the overall reaction

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2
Q

diffusion

A

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

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3
Q

effusion

A

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

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4
Q

Dispersion forces

A
  • more electrons, bigger molecule, stronger attractions

- bigger surface area, more disperson forces

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5
Q

catalyst

A

speeds up reaction, lower activation energy

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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

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7
Q

Molecules exhibiting hydrogen bonding

A

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

high boiling points

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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

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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

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10
Q

capillary action

A

the movement of a liquid up a narrow tube

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11
Q

cohesion

A

attraction between like molecules

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12
Q

adhesion

A

is the attraction between unlike molecules

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13
Q

dipole-dipole interactions

A

attractive forces that act between polar molecules

the larger the dipole, the larger the attractive force

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14
Q

Hydrogen bonding

A

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

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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

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16
Q

misicible

A

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

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17
Q

Coordination number

A

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

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18
Q

Unit cell

A

basic repeating structural unit of a crystalline solid

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19
Q

simple cubic

A

8 corner atoms, CN=6

1 EQUIVALENT ATOM

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20
Q

Body centered

A

8 corner atoms
CN=8
2 equivalent atoms

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21
Q

Face centered cubic

A

CN=12

4 equivalent atoms

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22
Q

saturated solution

A

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

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23
Q

solubility

A

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

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24
Q

unsaturated solution

A

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

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25
supersaturated solution
contains more dissolved solute than is present in a saturated solution. Generally not stable, and eventually the dissolved solute will come out of solution.
26
Ion-dipole
the charge of an ion is attracted to the partial charge on a polar molecule ex. NaCl or KI in H2O
27
Dipole-induced dipole
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
Ion-induced dople
The charge of an ion induces a temporary partial charge on a neighboring nonpolar molecule or atom
29
colligative properties
properties that depend on the number of solute particles in solution but do not depend on the nature of the solute particles.
30
Raoult's Law
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
colloids
disperson of particles from one substance through another substance
32
aerosol
liquid or solid dispersed into a gas
33
emulsions
liquids dispersed in another liquid
34
sols
solid dispersed in a liquid or in another solid
35
gels
liquid dispersed in a solid
36
Dispersion forces are greater in a _____ molecule?
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
Ionic Crystals Cohesive forces are
Coulubic forces and dispersion forces. Example being NACL, LiF, MgO, CaCo3
38
Covalent cohesive forces are
Covalent bonds being diamond and quartz
39
Molecular cohesive forces are
Dispersion and dipole dipole forces and hydrogen bonds
40
Metallic cohesive forces are
Metallic bonds being including all metallic elements, Na,Mg and Fe
41
The higher the lattice energy the more stable the compound
Because the have stronger cohesive forces and therefor a high melting point
42
What is fusion
Fusion is the the energy required in kj/mole to melt i mole of solid
43
Henrys Law
(c) the molar concentrations of a dissolved gas. (p) is pressure, and K is the proportionate constant. C=kp
44
Henry's Law States ___
That the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution.
45
What is the universal solvent?
Water
46
What is a solute?
Something that is dissolved in a solvent
47
Volatile
They vapor pressure is measurable
48
Boiling point
Is the temperature at which vapor pressure equals external atmospheric pressure.
49
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).
:D
50
Heterogeneous Catalyst
The reactants and the catalyst are in different phases. The catalyst is usually a solid. Reactants are either gases or liquids.
51
Homogeneous Catalysis
The reactants and the catalyst are dispersed in a single phase, usually liquid.
52
Le chateliers Principle
States that when stress is applied to a system, the system will shift to minimize the stress.
53
What counts as stress?
addition or removal of reactant or product change in volume change in temperature
54
The addition of a product or removal of a reactant will cause the equilibrium to shift to the ___.
Left
55
The addiction of a reactant or removal of a product will cause the reaction to shift to the __.
right
56
Entropy definition
How spread out a systems energy is
57
Standard Reduction potential
E cell
58
2nd law of thermodynamics
The entropy change for the universe is positive for spontaneous process and zero for a equilibrium process
59
The 3rd lave of thermodynamics
The entropy change is perfectly crystalline at zero Kelvin.
60
A spontaneous process
Occurs under a specific set of conditions.
61
Buffer
Substance that contains a weak acid and its conjugate base is a buffer solution.
62
Gamma Partical
Nuetron
63
Alpha partical
Is positively charged particle, they are deflected away from the positively charged plate.
64
Beta particle
electrons
65
Buffer
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)

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