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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
Q

Mixture

A

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
Q

Colligative Properties

A

properties of solvents that change when a solute is dissolved in it, dependent on concentration: VP lowering MP depression BP elevation Osmosis

27
Q

Intermediate

A

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
Q

Catalyst

A

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
Q

molecularity

A

number of molecule colliding during an element step

30
Q

elementary reaction

A

single-step reaction

31
Q

equilbrium

A

static dynamic- all chem rxn homogeneous- single phase heterogeneous- more than one phase *omit pure substance (l) & (s) b/c same concentrations throughout

32
Q

LeChatelier’s Principle

A

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
Q

Arrhenius Acid/ Base

A

Acid- produces an H+ Base- contains an OH-

34
Q

Bronsted-Lowry Acid/ Base

A

Acid- proton donor Base- proton aceptor

35
Q

Lewis Acid/ Base

A

Acid- electron pair accepter Base- electron pair donor

36
Q

Strong Acids

A

HClO4 (Perchloric Acid), HNO3 (Nitric Acid), HCl & HBr & HI, H2SO4 (Sulfuric Acid), H3O+ (Hydronium)

37
Q

Strong Bases

A

OH- (any soluble hydroxide; NaOH, KOH, Br(OH)2), NH2-,O2- (Oxide), H- (Hydride)

38
Q

Weak Acids

A

HF (Hydrofluoric Acid), NH4+ (Ammonium), and all others unless otherwise noted

39
Q

Weak Bases

A

NH3 (Ammonia)

40
Q

Conjugate Acid

A

add H+ to formula

41
Q

Conjugate Base

A

remove H+ from formula

42
Q

Buffer

A

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
Q

Oxidation

A

loss of electrons

44
Q

Reduction

A

gain of electrons

45
Q

LEOGER

A

Lose Electrons Oxidation, Gain Electrons Reduction

46
Q

Galvanic/ Voltaic Cell

A

operate in spontaneous direction, chemical energy to electrical energy… Batteries

47
Q

Electrolytic Cell

A

electrical energy to chemical energy; non-spontaneous, recharging battery, production of metals

48
Q

Standard Electrochemical Cell

A

25 degrees C, all aq. solns 1.0 M, all gasses 1 atm

49
Q

Ecell>0

A

spontaneous cell- Galvanic/ voltaic

50
Q

Ecell<0

A

non-spontaneous cell- Electrolytic Cell

51
Q

Anode

A

where oxidation occurs, electrons produced, anions migrate to anode, + (galvanic), - (electrolytic)

52
Q

Cathode

A

where reduction occurs, electrons consumed, cations migrate to cathode, - (galvanic), + (electrolytic)

53
Q

Rate Determining Step (RDS)

A

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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