Organic Chemistry namings
Alkanes: ane (methane)
Alkenes: ene (propene)
Alkynes: yne (butyne)
Cyclic hydrocarbon: cyclo (prefix)
Aromatic hydrocarbon: yl (end)
Alcohol: ol (end)
Haloalkanes: ane (end)
Aldehydes: al (end)
Ketones: one (end)
Carboxylic acid: oic acid (end)
Esters: oate (end)
Ethers: doesn’t have
Amines: amine (end)
Amides: amide (end)
s=1 orbit, p= 3 orbit, d= 5 orbit, f=7 orbit
Rate of reaction: r = k(A)(B)
Products
-----------Reactants
Hund’s law: says that when placing electrons
in orbitals of equal energy, place one in each
orbital before doubling up in order to arrive at
the lowest energy configuration.
Use ice chart to solve for esp from initial
concentration to equilibrium
Endothermic reactions have positive ΔH
and gain heat (for example, ice melting)
Aufbau’s law: states that energy levels must
be filled from the lowest to the highest and
you may not move on to the next level unless
the previous level is full. Use the periodic
table as a guide (read left to right):
Exothermic reaction have negative ΔH and
release heat
Pauli law: when electrons do share an
orbital, they must be of different “spin.”
Q=MCT
(m=mass) (c= specific heat capacity in J/mol)
(t=temperature)
Q can also = ΔH
AROC: slope of secant = to average rate
IROC: slope of tangent = instantaneous rate
Keq>1: at equilibrium there is more product
than reactant. Reaction is product favoured
Keq=1: at equilibrium there is equal amount
of product and reactants
Keq<1: at equilibrium there are more
reactants than products. Reaction is reactant
favoured
pH + pOH = 14
Arrhenius acid: produces hydronium ion in
water
Arrhenius base: produces hydroxide ion in
water
Bronsted-Lowry acid: Donates proton (H+)
Bronsted-Lowry base: accepts proton
Lewis acid: accepts electrons
Lewis base: donates electrons
Strong acids: HCl, Hbr, HI, HNO3, HClO3
Strong base: NaOh,KOH, Ca(OH)2,Ba(OH)2