chemistry from scratch

exothermic (E to e)

• releases heat into surroundings (more common)

• burn, condense, freeze, dissolve ionics

• graph: mid - high - low

• b/c total energy/heat made when bonds formed btwn solute/solvent is greater/stronger than total energy/heat absorbed when old bonds break, making it favorable/spontaneous as molecules move a ton since more extropy, less enthalpy

endothermic (e to E)

• gains heat from surroundings

• melt, evaporate, boil

• graph: low - high - mid

• positive enthalpy change

spontaneous, exergonic

• alone, disorded

• exergonic

non-spontaneous, endergonic

• needs input, ordered

• endergonic

Synthesis

+2 chemical compounds → more complex compound

Decomposition

More complex compound → +2 chemical compounds

Single Displacement

1 pure element displaces another element from a compound → new compound and the displaced element

Double Displacement

Parts of two ionic compounds exchange places → two new compounds

Combustion

Element, molecule, compound reacts with O2

Neutralization

Acid (H) reacts with base (OH) to form ionic compound and water

Law of Conservation of Mass

Energy cannot be made/destroyed

Law of Conservation of Atoms

# of atom types Before = After

percent yield

(actual yield / theoretical calculated yield)(100)

transitional KE

colliding objects

transfer of KE

conduction

2 qsmat formulas

• q=smAt

• sm(Tf-Ti) + sm(Tf-Ti) = 0

1st ThermoDynamics Law

energy cant be made/destroyed

2nd ThermoDynamics Law

entropy always increases (heat goes hot to cold, not cold to heat)

1 Calorie = 1000 calorie = 1 kilocalorie | 1 calorie = 4.184 Joule

1 Calorie = 1000 calorie = 1 kilocalorie | 1 calorie = 4.184 Joule

enthalpy

• E Measurement in a system

• ∆H = heat absorbed/released during process

Entropy

Disorder Measurement in molecules

Solids = ___ PE/entropy

LOWEST

Barometer

measures pressure of atmosphere by pushing

INVERSE BOYLE’S LAW

P₁V₁ = P₂V₂

DIRECT CHARLES’ LAW

V₁/T₁ = V₂/T₂

DIRECT GAY-LUSSAC

P₁/T₁ = P₂/T₂

DIRECT AVOGADROS LAW

Avogadro’s Law – V₁/n₁ = V₂/n₂

COMBINED GAS LAW

1 PV/T = 2 PV/T

IGL pervert PV = nRT

pressure x volume = mol x idg constant x time

Dalton’s Law of Partial Pressures

P_Total = P₁ + P₂ + P₃ + … + P_n

effusion

gas mcs confined+randomly passing thru container’s tiny hole

diffusion

2 gases gradual mixing

Standard T&P = IDG MOL V

1mol/22.4L

melt, freeze, evaporate, condense, sublime, depose

solid to gas, liquid to solid, liquid to gas, gas to liquid, solid to gas, gas to solid

normal b/f points

temp where it b/f at 1atm

intramolecular

in 1 mc

intermoleculare

multiple mcs

ion-dipole bond

STRONGESt

H-bond

Hydrogen bond w F/O/N

LDFs

from charge btwn instantaneous dipoles, in all molecules, direct relationship w contact surface area

dipole-dipole

only POLAR, from permanent dipole

substitutional vs intersitial alloy

similar size dupe = resist corrosion vs small-big dupe = stronger