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Peeb MCAT > Gen Chem Quicksheets > Flashcards

Gen Chem Quicksheets Flashcards

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MCAT flashcards
1
Q

System

A

Matter being observed

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2
Q

Surroundings

A

Everything outside of system

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3
Q

Isolated system

A

System can’t exchange energy (heat and work) or matter with surroundings

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4
Q

Closed system

A

System can exchange energy (heat and work) but not matter with surroundings

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5
Q

Open system

A

System can exchange energy and matter with surroundings

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6
Q

First law of thermodynamics

A

/\U=Q-W

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7
Q

Constant temp implies what about the energy of the system?

A

Constant internal energy

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8
Q

Adiabatic process

A

No heat exchanged b/w system and environment /\U=-W (work done on the system). Hyperbolic graph on P vs V graph

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9
Q

Isothermal process

A

Constant temp /\U=0 so Q=W. Hyperbolic curve on P vs V graph

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10
Q

Isobaric process

A

Same pressure. Flat line on p vs v graph

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11
Q

Isovolumetric process

A

Isochoric, constant volume, no work is performed /\U=Q. Vertical line on p vs V graph

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12
Q

State functions (mnemonic)

A

When I’m under Pressure and feeling dense, all I want to do is watch TV and get HUGS

Pressure, density, temperature, volume, enthalpy, internal energy, Gibbs free energy, entropy

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13
Q

Standard conditions

A

25 Celsius (298 K), 1 atm, 1 M

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14
Q

STP

A

Standard temperature and pressure - 0 celsius (273 K), 1 atm

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15
Q

Is evaporation endo or exothermic?

A

Endothermic

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16
Q

Sublimation

A

solid - gas phase

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17
Q

Temperature

A

Average kinetic energy of particles of a substance

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18
Q

Heat

A

Transfer of energy from 1 substance to another

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19
Q

Zeroth law of thermodynamics

A

Objects are in thermal equilibrium only when their temperatures are equal

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20
Q

Equation for heat transfer

A

Q=MCAT

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21
Q

Specific heat of water

A

1 cal/gK

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22
Q

Calorimetry

A

Process of measuring transferred heat

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23
Q

Equation for heat during phase changes

A

Q=mL (latent heat: enthalpy of an isothermal process cal/g)

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24
Q

Enthalpy

A

Heat changes at constant temperature

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25
Q

Change in enthalpy of a reaction equation

A

/\Hrxn = /\Hproducts - /\Hreactants

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26
Q

Bond dissociation energy

A

Average energy required to break a particular type of bond b/w atoms in the gas phase

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27
Q

Bond beak is endo/exothermic? Bond forming is endo/exothermic?

A

Endo, exothermic

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28
Q

How to find the change in enthalpy of a reaction with bond breaking/forming?

A

/\Hrxn =/\H bonds broken - /\H bonds formed

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29
Q

Second law of thermodynamics

A

Energy will spread out from 1 point

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30
Q

Entropy

A

Spontaneous dispersal of energy at a specific temperature: how much or how widely energy is spread out

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31
Q

Equation for change in entropy

A

/\S = Qreversible/temp

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32
Q

How to calculate entropy of a reaction

A

/\Srxn = /\Sproducts - /\Sreactants

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33
Q

Equation for Gibbs free energy (mnemonic)

A

Get Higher Test Scores

/\G = /\H -T/\S

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34
Q

Standard Gibbs free energy from equilibrium constant

A

-RTlnKeq

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35
Q

Gibbs free energy from reaction quotient

A

/\Grxn + RTlnQ = RTln (K/Q)

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36
Q

precipitation reaction

A

formation of a solid from an aqueous solution

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37
Q

displacement reaction

A

displacement of shuffling of an atom or group from 1 molecule to another

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38
Q

redox reaction

A

changing the oxidation states of the elements

39
Q

planck’s quantum theory

A

energy emitted as electromagnetic radiation from matter exists in discrete bundles called quanta

40
Q

balmer series

A

group of hydrogen emission lines corresponding to transitions from upper levels n>2 to n=2

41
Q

lyman series

A

group of hydrogen emission lines corresponding to transitions b/w upper levels n>1 to n=1

42
Q

heisenberg uncertainty principle

A

impossible to determine which perfect accuracy the momentum and position of an electron simultaneously

43
Q

4 quantum numbers

A

n - shell
l - subshell (from 0 to n-1 or 0=s, 1=p, 2=d,3=f)
ml - orbital between -l and l
ms - +1/2 or -1/2

44
Q

max # electrons in an energy level

A

2n^2

45
Q

max # elections in a subshell

A

4L+2

46
Q

what is the only periodic trend that goes opposite of all the others? describe

A

atomic radius! decreases from L to R and B to T while everything else increases

47
Q

hund’s rule

A

fill up orbitals halfway with parallel spins first

48
Q

octet rule

A

an atom will bond until it has a full outermost shell, an atom wants to have a configuration like a noble gas

49
Q

steps to draw lewis structure

A
  1. write skeletal structure
  2. count all valence e-
  3. draw single bonds
  4. complete octets of all atoms
  5. extra e- on the central atom
50
Q

formal charge

A

charge an atom would have if all the electrons in bonds were shared equally

51
Q

polar covalent bond

A

bonding electron pair NOT shared equally and pulled more to an electronegative atom

52
Q

angle between e- pairs of:
linear
trig planar
tetrahedral

A

180
120
109.5

53
Q

chelation

A

central cation can bond to same ligand multiple times

54
Q

dispersion forces

A

bonding electrons in covalent bonds not actually shared equally tho they appear that way, “DISPERSED” randomly and causes really short polarization, form dipoles

55
Q

basic rate law equation

A

rate = k[A]^x[B]^y

x and y and k determined experimentally

56
Q

combustion rxn

A

fuel + oxidant makes oxide and water (CO2 and water)

57
Q

combination rxn

A

2 or more rxns form 1 product

58
Q

decomposition rxn

A

compound breaks down into 2 or more substances as a result of heat or electrolysis

59
Q

single-displacement rxn

A

atom (ion) replaced by an atom or another element

60
Q

Double-displacement rxn

A

metathesis - switch 2!

61
Q

spectator ion

A

ion doesn’t take part in the net rxn but remains in solution

62
Q

neutralization rxn

A

specific double-displacement occurs when an acid reacts with a base to produce salt and water

63
Q

what factors affect the rxn rate

A

reactant conc, temp, medium, catalysts

64
Q

catalyst

A

not consumed, lower activation energy barrier

65
Q

Kc

A

equilibrium constant - conc of products/reactants

66
Q

what does not appear in equilibrium constant expressions?

A

solids or liquids

67
Q

le chatelier’s principle

A

direction of rxn at equilibrium when subjected to stress will change to relieve the applied stress

68
Q

law of conservation of energy

A

energy neither created or destroyed, types of energy are interconvertible

69
Q

hess’s law

A

enthalpies of rxn’s are additive, a reversed rxn has the same magnitude of enthalpy with the opposite sign

70
Q

Ideal gas law

A

PV=nRT

71
Q

deviations on ideal gas law due to pressure

A

as pressure of a gas increases -> particles pushed close together, gases volume less than predicted, by ideal gas law cuz intermolecular attractions!

72
Q

deviations on ideal gas law due to temperature

A

as temp decreases -> velocity of gas decreases, intermolecular forces increase! so smaller volume than predicted by ideal gas law
as temp extremely low -> larger volume of gas particles than expected

73
Q

1 mol gas at STP = ? L

A

22.4

74
Q

molality

A

moles solute/kg solvent

75
Q

raoult’s law

A

partial vapor pressure of each liquid component in a mixture is based on its mol fraction

76
Q

diffusion

A

gas molecules distribute thru a volume by random motion

77
Q

effusion

A

flow of gas particles under pressure from 1 compartment to another thru small opening

78
Q

normality

A

gram equivalents solute/L of solution

79
Q

arrhenius acid or base

A

acid - produce excess H+

base - produce excess OH-

80
Q

bronsted-Lowry acid or base

A

acid - donates H+

base - accepts H+

81
Q

Lewis acid or base

A

acid - e-pair acceptor

base - e-pair donor

82
Q

pH =

A

-log[H+] = log(1/[H+])

83
Q

pOH =

A

-log[OH-] = log(1/[OH-])

84
Q

Kw =

A

[H+][OH-]=10^-14

85
Q

pOH +pH =

A

14

86
Q

hydrolysis

A

reverse reaction of a neutralization - salt and water react to give acid and base

87
Q

amphoteric

A

act as acid or base

88
Q

oxidizing agent

A

reduced, causes another atom to be oxidized

89
Q

reducing agent

A

oxidized, causes another atom to be reduced

90
Q

reduction potential

A

tendency to acquire electrons and be reduced

91
Q

emf

A

standard reduction potentials used to calculate electromotive force = Ered, cathode - Ered, anode

92
Q

galvanic cell

A

spontaneous, supplies energy for work, energy harnessed by redox half-rxns

93
Q

electrolytic cell

A

nonspontaneous, needs electrical energy to react

Peeb MCAT (7 decks)

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