Ionic bonds
When one atom gives up an electron to an atom that wants to receive an electron.
-Atoms want to gain/lose electrons in their valence shells to look more like the noble gases.
-Afterwards, the atoms have charges. Negative, if they gained an electron, and p
Covalent bonds
When the atoms share electrons to fulfill their valence shell preferences.
-Depending on the electronegativity of each atom, there may be partial charges (ex. H2O)
Electronegativity
How badly it wants to hog electrons in a bond; the power of an atom in a molecule to attract electrons o itself
Electron Affinity
How much it wants electrons
Balancing equations
Make sure molecules are the same on both sides.
Tip: put an initial 1 in front of the most complex compound
Extensive vs. intensive property
Extensive - a property that changes when the size of the sample changes
Intensive - a property that DOESN'T change when the size changes
metathesis rxn
A reaction in which compounds exchange ions
redox rxn
A reaction in when there's an oxidation/reaction, or losing/gaining of an electron
Reduction vs. oxidation half-rxn
You can write a redox reaction as two half-reactions, one showing the reduction process, and one showing the oxidation process.
In a reduction half-rxn, the one being REDUCED is gaining the electron while the other compound causing the reduction is the RE
s, p, d, f orbitals
1, 2, 3... denote the energy level
s, p, d, f... denote the shape of the orbital
-these orbital shapes are around the x, y, z axes
How much each orbital holds (within each orbital is two electrons max):
s: 2 (1 spot)
p: 6 (3 spots)
d: 10 (5 spots)
f: 14 (
VSEPR shapes
Electron Configuration Notation
Use the electron filling pattern and the number of valence electrons of an element to figure out the notation. Fill in the amount of valence electrons, writing the number of electrons in each orbital energy level in superscript until you run out.
Bronsted-Lowry bases & acids
BL BASE is a proton DONOR
BL ACID is a proton ACCEPTOR
equilibrium constant K
Keq = [products]^coefficient / [reactants]^coefficient
To get the Keq of the reverse reaction, flip the equation
If K is large, then the products are favored.
Kp formula
An equilibrium constant like Keq, but instead deals with partial pressures of the gaseous compounds
IUPAC rules
1) Identify the longest carbon chain, this will be the parent chain
2) Start number ing the carbons on the end that will give the substituents the lowest number
3) When there is only one type of substituent and number more 2+, use the prefixes (di, tri, t
IUPAC substituents
Arrhenius equation
k = Ae^(-Ea/RT)
k - rate constant
A - frequency factor
Ea - Activation energy
R - Gas constant
T - temperature in Kelvin
Henderson-Hasselbach equation
pH = pKa - log([conjugate base]/[acid])
Henry's law
At a given temperature, the solubility of a gas (S) in a liquid is directly proportional to the pressure (P) of the gas above the liquid.
So as pressure of a gas increases, so does its solubility
Nuclear reactions (alpha, beta, gamma particles)
Nuclear reactions involve changes in the nucleus whereas chemical reactions involve a transfer of electrons.
nuclide symbolism: A/Z X
A - mass number (number of neutrons and protons)
Z - atomic number
X - elemental symbol
- alpha emission: Helium particle
pH equation
pH = -log [H+]
Take the log of the concentration of the hydronium ion.
pOH equation
pOH = -log [OH-]
Take the log of the concentration of the hydroxide ion.
Periodic table trends
Electron Affinity: increases from left to right & bottom to top
Ionization Energy: increases from left to right & bottom to top
Electronegativity: increases from left to right & bottom to top
Atomic Radius: increases from right to left & top to bottom
Met
Rate law and order reactions
Zero-order rate law: rate = k
-independent of the concentration of the compound, the rate is the same (horizontal straight line)
First-order rate law: rate = k[A]
-reaction that depends linearly on only one reaction (negative straight line)
Second-order r
Half life equations
Zero-order half-life: t(1/2) = [Ao]/2k
First-order half-life: t(1/2) = 0.693/k
Second-order half-life: t(1/2) = 1/k[Ao]
Gas law
PV = nRT
P - pressure
V - volume
n - number of moles
R - Gas constant
T - temperature
Gas constant R
0.0821 L
atm/mol
K OR
8.314 J/mol*K
Combined gas law
P1V1/T1 = P2V2/T2
Avogadro's constant
6.022 x 10^23
moles to grams
moles x grams/1 mole = grams of molecule
To get moles: 1 mole/grams x grams of molecule = number of moles
How do you know if a rxn is spontaneous or not?
Delta G = Delta H - (T)(Delta S)
Delta G - measure of free energy in the system (Gibbs Free Energy)
Delta H - measure of heat that is given off (-) or absorbed (+) by the environment (Enthalpy)
Delta S - measure of entropy of the system
T - temperature in
Endothermic vs exothermic graphs
In endothermic reactions, the products will have a higher potential energy. And since heat is absorbed, delta H is positive
In exothermic reactions, the products will have a lower potential energy. And since heat is expelled, delta H is negative.
Nernst equation
Allows us to calculate the cell potential under non-standard state conditions
E = E^o - (RT)lnQ/(NF)
OR if you plug in the constants and temperature at 298.15K (25C):
E = E^o - (0.0257)lnQ/n
E - instantaneous cell potential
E^o - instantaneous cell potent
Galvanic cells
When Delta G is negative, the redox reaction is still going and there is a voltage.
Delta G = Delta G^o + RTlnQ
Delta G - free energy
Delta G^o - free energy under standard conditions (-212kJ/mol)
R - Gas constant
T - temperature in Kelvin
Q - [products]/
Functional Groups
Alcohol: -OH
Ketone: O=C-R^2
Aldehyde: O=C-H
Carboxylic acid: O=C-OH
Ether: R-O-R
Amine: N-H^2-R
Molarity
concentration based on mol/Liter
Normality
grams solute / (amt. of solute (L) * equivalent weight)
equivalent weight = molecular weight/valence capacity
ortho vs para
cis vs trans
cis - groups are on the same side
trans - groups are criss-crossed