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Chemistry > Final Review CHGN 122 > Flashcards

Final Review CHGN 122 Flashcards

1
Q

deltaG<0

A

Spontaneous process

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2
Q

deltaG>0

A

Nonspontaneous process

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3
Q

deltaG=0

A

reversible/ system at equilibrium

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4
Q

solid->liquid

A

fusion, deltaS>0

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5
Q

liquid->solid

A

freezing, deltaS<0

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6
Q

liquid->gas

A

vaporization, deltaS>0

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7
Q

gas->liquid

A

condensation, deltaS<0

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8
Q

solid->gas

A

sublimation, deltaS>0

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9
Q

gas->solid

A

deposition, deltaS<0

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10
Q

favorable energy

A

favorable for energy in system to decrease, deltaH<0 is favorable

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11
Q

favorable entropy

A

favorable for entropy of a system to increase, deltaS>0 is favorable

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12
Q

diffusion

A

spread of one substance throughout another by unhindered random trajectories

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13
Q

effusion

A

one-way leakage of a gas thru a pinhole

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14
Q

IMF in decreasing strength

A

Hydrogen bonding, ion-dipole forces, dipole-dipole forces, London dispersion forces

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15
Q

Hydrogen bonding

A

Hydrogen bonded to O, N, or F

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16
Q

electronegativety trend

A

up and to the right more EN on Periodic table, F most EN

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17
Q

EN bonds

A

A-A, C-H bonds are nonpolar A-B bonds polar, unless deltaEN>2 (then ionic)

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18
Q

London Dispersion Forces (strongest to weakest)

A

ion induced dipole dipole induced dipole induced dipole induced dipole

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19
Q

As strength of IMF increases:

A

BP increases MP increases viscosity increases (resistance to flow) Surface tension increases Vapor pressure decreases (less volatile)

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20
Q

evaporation vs. vaporization

A

vaporization= liquid->gas, at BP evaporation= vaporization below BP at the surface of the liquid

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21
Q

Vapor Pressure

A

equilibrium partial pressure of a substance

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22
Q

Solid categories:

A

crystalline solids- regular, repeating lattice, most common Amorphous solids- lack long-range order on atomic scale

23
Q

Solid classifications:

A

ionic- ionic bonds (holds lattices together) metallic- metallic bonds covalent- covalent bonds and possibly IMF’s

24
Q

Carbon structures

A

Diamond- 3-D covalent network Graphite- 2-D covalent network Graphene- single sheet of graphite Fullerenes- ‘buckyballs’ soccer ball shaped molecules Carbon Nanotubes- tubes of a single rolled sheet of graphite

25
Mixture
homogeneous- uniform mixtures heterogeneous- Colloids- non-uniform, don't separate over time, smallish molecules Suspensions- non-uniform, separate over time, larger molecules than Colloids
26
Colligative Properties
properties of solvents that change when a solute is dissolved in it, dependent on concentration: VP lowering MP depression BP elevation Osmosis
27
Intermediate
a species produced in an early step of a multi step reaction and consumed in a later step, valley in a multi-step reaction profile
28
Catalyst
a species consumed in an early stage and then regenerated in a later step; speeds up reaction by lowering energy of the rate determining step. homogeneous- same phase as reactants heterogeneous- different phase than reactants, usually a solid
29
molecularity
number of molecule colliding during an element step
30
elementary reaction
single-step reaction
31
equilbrium
static dynamic- all chem rxn homogeneous- single phase heterogeneous- more than one phase \*omit pure substance (l) & (s) b/c same concentrations throughout
32
LeChatelier's Principle
when a system at equilibrium is stressed, there will be a net rxn to form a new equilibrium in the direction that reduces the stress Types of stress: changing temp adding or removing reactants/ products changing V at constant T of a gas
33
Arrhenius Acid/ Base
Acid- produces an H+ Base- contains an OH-
34
Bronsted-Lowry Acid/ Base
Acid- proton donor Base- proton aceptor
35
Lewis Acid/ Base
Acid- electron pair accepter Base- electron pair donor
36
Strong Acids
HClO4 (Perchloric Acid), HNO3 (Nitric Acid), HCl & HBr & HI, H2SO4 (Sulfuric Acid), H3O+ (Hydronium)
37
Strong Bases
OH- (any soluble hydroxide; NaOH, KOH, Br(OH)2), NH2-,O2- (Oxide), H- (Hydride)
38
Weak Acids
HF (Hydrofluoric Acid), NH4+ (Ammonium), and all others unless otherwise noted
39
Weak Bases
NH3 (Ammonia)
40
Conjugate Acid
add H+ to formula
41
Conjugate Base
remove H+ from formula
42
Buffer
an aqueous solution that contains significant amounts of both a WA and its conjugate WB, that resists pH change due to the common ion effect
43
Oxidation
loss of electrons
44
Reduction
gain of electrons
45
LEOGER
Lose Electrons Oxidation, Gain Electrons Reduction
46
Galvanic/ Voltaic Cell
operate in spontaneous direction, chemical energy to electrical energy... Batteries
47
Electrolytic Cell
electrical energy to chemical energy; non-spontaneous, recharging battery, production of metals
48
Standard Electrochemical Cell
25 degrees C, all aq. solns 1.0 M, all gasses 1 atm
49
Ecell\>0
spontaneous cell- Galvanic/ voltaic
50
Ecell\<0
non-spontaneous cell- Electrolytic Cell
51
Anode
where oxidation occurs, electrons produced, anions migrate to anode, + (galvanic), - (electrolytic)
52
Cathode
where reduction occurs, electrons consumed, cations migrate to cathode, - (galvanic), + (electrolytic)
53
Rate Determining Step (RDS)
the slowest step in a multi-step mechanism that will decide the overall rate of the entire mechanism

Chemistry (4 decks)

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