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Peeb MCAT > Gen Chem Quicksheets > Flashcards

Gen Chem Quicksheets 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
Change in enthalpy of a reaction equation
/\Hrxn = /\Hproducts - /\Hreactants
26
Bond dissociation energy
Average energy required to break a particular type of bond b/w atoms in the gas phase
27
Bond beak is endo/exothermic? Bond forming is endo/exothermic?
Endo, exothermic
28
How to find the change in enthalpy of a reaction with bond breaking/forming?
/\Hrxn =/\H bonds broken - /\H bonds formed
29
Second law of thermodynamics
Energy will spread out from 1 point
30
Entropy
Spontaneous dispersal of energy at a specific temperature: how much or how widely energy is spread out
31
Equation for change in entropy
/\S = Qreversible/temp
32
How to calculate entropy of a reaction
/\Srxn = /\Sproducts - /\Sreactants
33
Equation for Gibbs free energy (mnemonic)
Get Higher Test Scores | /\G = /\H -T/\S
34
Standard Gibbs free energy from equilibrium constant
-RTlnKeq
35
Gibbs free energy from reaction quotient
/\Grxn + RTlnQ = RTln (K/Q)
36
precipitation reaction
formation of a solid from an aqueous solution
37
displacement reaction
displacement of shuffling of an atom or group from 1 molecule to another
38
redox reaction
changing the oxidation states of the elements
39
planck's quantum theory
energy emitted as electromagnetic radiation from matter exists in discrete bundles called quanta
40
balmer series
group of hydrogen emission lines corresponding to transitions from upper levels n>2 to n=2
41
lyman series
group of hydrogen emission lines corresponding to transitions b/w upper levels n>1 to n=1
42
heisenberg uncertainty principle
impossible to determine which perfect accuracy the momentum and position of an electron simultaneously
43
4 quantum numbers
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
max # electrons in an energy level
2n^2
45
max # elections in a subshell
4L+2
46
what is the only periodic trend that goes opposite of all the others? describe
atomic radius! decreases from L to R and B to T while everything else increases
47
hund's rule
fill up orbitals halfway with parallel spins first
48
octet rule
an atom will bond until it has a full outermost shell, an atom wants to have a configuration like a noble gas
49
steps to draw lewis structure
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
formal charge
charge an atom would have if all the electrons in bonds were shared equally
51
polar covalent bond
bonding electron pair NOT shared equally and pulled more to an electronegative atom
52
angle between e- pairs of: linear trig planar tetrahedral
180 120 109.5
53
chelation
central cation can bond to same ligand multiple times
54
dispersion forces
bonding electrons in covalent bonds not actually shared equally tho they appear that way, "DISPERSED" randomly and causes really short polarization, form dipoles
55
basic rate law equation
rate = k[A]^x[B]^y x and y and k determined experimentally
56
combustion rxn
fuel + oxidant makes oxide and water (CO2 and water)
57
combination rxn
2 or more rxns form 1 product
58
decomposition rxn
compound breaks down into 2 or more substances as a result of heat or electrolysis
59
single-displacement rxn
atom (ion) replaced by an atom or another element
60
Double-displacement rxn
metathesis - switch 2!
61
spectator ion
ion doesn't take part in the net rxn but remains in solution
62
neutralization rxn
specific double-displacement occurs when an acid reacts with a base to produce salt and water
63
what factors affect the rxn rate
reactant conc, temp, medium, catalysts
64
catalyst
not consumed, lower activation energy barrier
65
Kc
equilibrium constant - conc of products/reactants
66
what does not appear in equilibrium constant expressions?
solids or liquids
67
le chatelier's principle
direction of rxn at equilibrium when subjected to stress will change to relieve the applied stress
68
law of conservation of energy
energy neither created or destroyed, types of energy are interconvertible
69
hess's law
enthalpies of rxn's are additive, a reversed rxn has the same magnitude of enthalpy with the opposite sign
70
Ideal gas law
PV=nRT
71
deviations on ideal gas law due to pressure
as pressure of a gas increases -> particles pushed close together, gases volume less than predicted, by ideal gas law cuz intermolecular attractions!
72
deviations on ideal gas law due to temperature
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
1 mol gas at STP = ? L
22.4
74
molality
moles solute/kg solvent
75
raoult's law
partial vapor pressure of each liquid component in a mixture is based on its mol fraction
76
diffusion
gas molecules distribute thru a volume by random motion
77
effusion
flow of gas particles under pressure from 1 compartment to another thru small opening
78
normality
gram equivalents solute/L of solution
79
arrhenius acid or base
acid - produce excess H+ | base - produce excess OH-
80
bronsted-Lowry acid or base
acid - donates H+ | base - accepts H+
81
Lewis acid or base
acid - e-pair acceptor | base - e-pair donor
82
pH =
-log[H+] = log(1/[H+])
83
pOH =
-log[OH-] = log(1/[OH-])
84
Kw =
[H+][OH-]=10^-14
85
pOH +pH =
14
86
hydrolysis
reverse reaction of a neutralization - salt and water react to give acid and base
87
amphoteric
act as acid or base
88
oxidizing agent
reduced, causes another atom to be oxidized
89
reducing agent
oxidized, causes another atom to be reduced
90
reduction potential
tendency to acquire electrons and be reduced
91
emf
standard reduction potentials used to calculate electromotive force = Ered, cathode - Ered, anode
92
galvanic cell
spontaneous, supplies energy for work, energy harnessed by redox half-rxns
93
electrolytic cell
nonspontaneous, needs electrical energy to react

Peeb MCAT (7 decks)

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