Mcat General Chemistry

Front 1

EQ - Max number of electrons that can fill a subshell

Back 1

4l + 2

Front 2

EQ - Max number of electrons allowed in single energy level in terms of n

Back 2

2n^2

Front 3

Diamagnetic vs Paramagnetic

Back 3

Diamagnetic - All electrons are spin-paired; unaffected by magnetic fields

Paramagnetic - Has unpaired electrons - affected by magnetic fields

Front 4

Heisenberg Uncertainty Principle:
Cannot know ________ + _______

Back 4

momentum and position

Front 5

Hund's Rule vs Pauli Exclusion Principle

Back 5

Hund - electrons fill empty orbitals first

Pauli - Each orbital contains two electrons of opposite spin

Front 6

Malleability vs ductility

Back 6

Malleable - mold into shapes
Ductile - drawn into wire

Front 7

Type of bond formed between Lewis Acid and Base

Back 7

Coordinate Covalent Bond

Ex - Ammonia has 3 polar covalent bonds
Ammonium has 1 more, which is coordinate covalent.

Front 8

Disperion Forces

Back 8

Types of van der Waals force that occurs among all bonded atoms due to unequal sharing of electrons

(Dipole-dipole is another type of vdW. Noble gases only have dispersion forces)

Front 9

Molarity Molality Normality

Back 9

Molarity - Moles/L
Molality - mol solute/ KILOGRAM solvent
Normality - Equivalents / L

Front 10

Molecule vs Compound

Back 10

All compounds are molecules but not all molecules are compounds

Molecules are discrete , isolateable units.

Ex - Ionic compounds are bonded interweavingly. No discrete units. So graphite consists of a bunch of carbons bonded in a random pattern.

Front 11

Ionic compounds are not molecules

Back 11

THEY ARE NOT FREAKING MOLECULES OKAY YOU IDIOT???
THEY ARE COMPOUNDS!
They don't have a molecular weight or are made from molecules.

Front 12

D - Gram Equivalent Weight

Back 12

Weight that would release one acid equivalent

So H2SO4 has a gram equivalent weight that's half of its molecular weight. Moron.

Front 13

Exponents of rate law vs equilibrium expression

Back 13

Equilibrium - exponents are the coefficients of each component

Rate law - exponents are the freaking rate law, idiot.

Front 14

EQ - Concentration of radioactive decay

Back 14

Radioactive decay is FIRST ORDER
[A] = [Ao]e^(-kt)

Front 15

Energy relationship of reactants, products, and transition sate

Back 15

Transition state ALWAYS has the highest.
Endothermic - reactants have lower
Exothermic - reactants have higher. Since you know, energy is being lost. Duhhhhh

Front 16

Relationship - Law of Mass Action and Reaction Quotient

Back 16

Law of Mass Action = Rate Law = reactants/products

Reaction quotient is a relative measure of how far a reaction is toward equilibrium:
Q < K - heading there
Q > K - exceeded
Q = K - reached it!

Front 17

Gibbs - Conditions for an endothermic, spontaneous reaction

Back 17

H is positive - because it's endothermic, duh
G is negative - because it's spontaneous

G = H - T(S)
In order to make G negative, T(S) has to be positive. T is always positive unless we violate the Third Law of Thermodynamics trollolololololol.

So S has to be positive.

Front 18

EQ - Solubility Product Constant

Back 18

PRODUCTS ONLY
RAISED BY THEIR STUPID COEFFICIENTS AS EXPONENTS
SONOFABEACH

Front 19

L - Systems (3)

Back 19

Isolated - doesn't exchange energy or matter,

Closed - Exchanges energy but not matter, like a radiator

Open - Exchanges energy and matte

Front 20

L - Processes (3)

Back 20

Isothermal - constant temperature, no duh
Adiabatic - no heat exchange
Isobaric - constant pressure

Front 21

L/D - State Functions

Back 21

Mneumonic - VG PHEST
Volume
Gibbs

Pressure
Enthalpy
Internal ENERGY
Entropy
Temperature

***** ALSO DENSITY

State Functions - independent of path taken
*not necessarily independent of each other

Front 22

Heat vs Temperature

Back 22

Heat is the transfer of energy

Temperature is a measure of particle average kinetic energy

Front 23

EQ - standard free energy using equilibrium constant

Back 23

G = -RTln(Keq) THIS IS AT EQUILIBRIUM

Afterwards, ya gotta use:

G = Go + RTlnQ
Which turns into:
G = RTln(Q/Keq)

Front 24

EQ - energy in relation to heat and work

Back 24

U = Q - W
Energy is heat minus work

HEAT MINUS WORK
DAMMIT HEAT MINUS WORK

Front 25

EQ - work in relation to volume and pressure

Back 25

W = -P(delta)V

Front 26

Adiabatic in terms of pressure and volume

Back 26

Volume changes that occur without a significant loss of heat (through manipulation of pressure for example)

Think PV curve in hot->cool transitions

Front 27

Different variables that influence BP and MP

Back 27

Branching decreases BP
Symmetry increases MP, decreases BP

linear compounds have higher BP and MP
Super branched compounds will have higher MP but lower BP

Front 28

Effect of branching on heat of reaction

Back 28

Branching DECREASES
Makes it harder to do, so more heat input is needed.

Front 29

e

Back 29

2.7

Front 30

Radical 3 and 2

Back 30

1.7 and 1.4

Front 31

R (gas constant)

Back 31

8.314 J/mol K
.082 Latm/molK

Front 32

density of water

Back 32

1000kg/m^3
1g/cm^3

Front 33

Difference between adiabatic and isothermal

Back 33

THEY ARE MUTUALLY EXCLUSIVE IF YOU EVER SAY THAT THEY CAN BOTH HAPPEN IN ONE PROCESS YOU'RE A DUMBHEAD

Adiabatic - no heat transfer
Isothermal - constant temperature (requires transfer of heat around)

Front 34

Endergonic/Exergonic vs Endothermic/Exothermic

Back 34

Exo/Endothermic are relative to enthalpy only
Ender/exergonic are relative to spontaneity. Endergonic is nonspontaneous storage of energy.
Exergonic is spontaneous release of energy

Front 35

Spontaneity
Q < Keq

Back 35

Spontaneous
Think G = RTln(Q/Keq), we want a fraction

Front 36

Spontaneity
Q > Keq

Back 36

Nonspontaneous
Think G = RTln(Q/Keq) we want a fraction

Front 37

To measure heat capacity/specific heat you use

Back 37

A calorimeter
Heat capacity - amount of energy/temp
Specific heat - energy to raise temperature of 1g by 1 Celsius

Front 38

Laws of thermodynamics expressed as equations

Back 38

1. E(system) + E(surroundings) = E(universe)
2. S(system + S(surroundings) = S(universe)
3. S(universe) = o at T = 0K
0th - thermal equilibrium

Front 39

EQ - average kinetic energy of a gas particle

Back 39

KE = .5mv^2 = 3/2kT

Front 40

Root-mean-square speed of gas

Back 40

u(rms) = radical(3RT/M)

Front 41

When do you have to consider van't Hoff Factors?

Back 41

In calculations involving colligative properties:
FBD - miK
BPE - miK
OP - iMRT

Front 42

Alloy vs Pure Metal MP/FP

Back 42

LOWER - pure metals have much stronger metallic bonding

Front 43

Solubility Rules

Back 43

SODIUM AND NITRATE SALTS ARE ALL SOLUBLE
1. Salts of Alkali Metals - soluble
2. Salts of Ammonium - soluble
3. Salts of Cl, Br, I soluble (EXCEPT Ag+, Pb2+, Hg2(2+))
4. Salts of Sulfate are soluble, except Pb2+, Ba2+, Sr2+, and Ca2+
5. All metal oxides except ones with alkali metals (and CaO, SrO, BaO) are INSOLUBLE
6. All hydroxides are INSOLUBLE except Ca2+, Sr2+ and Ba2+
7. Carboantes, phosphates, sulfides, and sulfites are all INSOLUBLE except alkali and ammonium

Front 44

L - UNITS OF CONCENTRATION

Back 44

Mole Fraction - moles of compound divided by total number of moles of all species within a system
- VPD and partial pressures

Molarity - Moles/liter(solution)

Molality - moles/kg(solvent)

Normality - Equivalents/Liter(solution)

Front 45

L - General Ksp values for salts

**************************************************************THIS WAS ON A PRACTICE TEST YOU HO

Back 45

MX3 - 27x^4
MX2 - 4x^3
MX - X^2

X = molar solubility, mols/L dissolved

Front 46

What the Aych Eee Double Hockey Sticks is I.P.??

Back 46

Ion Product. The same as Q for equilibrium constant. In relation to Ksp

If IP If IP=Ksp it's saturated
If IP>Ksp, solution is unsaturated, precipitation

REMEMBER:
Q < K - heading there
Q > K - exceeded
Q = K - reached it!

Front 47

Most dissolutions are _____________- EXCEPT

Back 47

Most dissolutions are endothermic
EXCEPT dissolution of gas into liquid (exothermic)

Front 48

D - solution

Back 48

homogenous mixtures of two or more substances that combine to form a single phase

* Solutions are mixture,s but not all mixtures are solutions

Front 49

Raoult's Law

Back 49

Ideal solution behavior is observed when solute-solute, solvent-solvent, and solute-solvent interactions are very similar

Front 50

How to determine charge density

Back 50

1.Calculate charge of ions (highest total charge, highest charge density)
2. Smallest size, highest charge density

Front 51

Mixtures that have higher vapor pressure than predicted by Raoult's Law

Back 51

Have stronger solvent-solvent/solute-solute interactions than solvent-solute

Front 52

Relationship between solubility and atmospheric pressure

Back 52

THEY IS DIRECTLY PROPORTIONAL POOBUTT

Front 53

Important Properties of logarithms

Back 53

log x^n = n log x
log10^x = x

Front 54

Strong Acids

Back 54

HCl
HBr
HI
H2SO4
HNO3
HClO4

Front 55

Strong Bases

Back 55

NaOH, KOH
other crap

Front 56

Gram Equivalent Weight

Back 56

Grams of substance divided equivalents

Front 57

Threshold for Ka acidity

Back 57

if Ka > 10^-7
ACID

Front 58

Characteristics of Concentration Cells

Back 58

Spontaneous redox reactions
Generate Current
Supply energy

*** current is dependent on ion concentration gradient, not difference in reduction potential.

Go and Eo are both 0, because current ceases when concentrations of ion are equal

Front 59

Compare Galvanic, Concentration, and Electrolytic Cells

Back 59

Galvanic - Spontaneous, current, energy, G-, E+
Concentration - Spontaneous, current, energy, G = 0, E = 0. Current is dependent on ion concentration gradient
Electrolytic - Nonspontaneous, requires external voltage, consumes energy. G+, E-

Front 60

EQ - Relationship between emf and equilibrium constant

Back 60

G = -nFE = -RTlnK

Holy crap that's confusing

Front 61

Characteristics of Concentration Cells

Back 61

Spontaneous redox reactions
Generate Current
Supply energy

*** current is dependent on ion concentration gradient, not difference in reduction potential.

Go and Eo are both 0, because current ceases when concentrations of ion are equal

Front 62

Compare Galvanic, Concentration, and Electrolytic Cells

Back 62

Galvanic - Spontaneous, current, energy, G-, E+
Concentration - Spontaneous, current, energy, G = 0, E = 0. Current is dependent on ion concentration gradient
Electrolytic - Nonspontaneous, requires external voltage, consumes energy. G+, E-

Front 63

Overall potential of a spontenous system

Back 63

POSITIVE

Front 64

What is E^o

Back 64

REDUCTION POTENTIAL. WHICH IS USED TO CALCULATE STANDARD ELECTROMOTIVE FORCE (EMF)

Metals have a very negative one, because they like to be oxidized

Front 65

A species with higher reduction potential...

Back 65

Is more likely to BE REDUCED, and DO THE OXIDIZING

Front 66

Redox of metal with oxygen

Back 66

METAL IS OXIDIZED (donates electrons)

Front 67

Is it possible for halogens to have a positive oxidation number?

Back 67

Yes apparently. Crap... example is Bleach, NaClO

Front 68

*** High Yield ***
When you have intermediates in your rate law (slow step) what do you do?

Back 68

Use prior steps to solve for concentrations, and substitute

Front 69

ite-ous

ate-ic

Back 69

duh.