chem

balanced chemical equation

a chemical equation with the same amount of atoms on each side

precipitation reaction

another type of double displacement where one of the products is a solid

single replacement

A + BC --\> B +AC

double displacement

AB + CD --\> AD + CB

synthesis reaction

A + B --\> AB

acid-base reactions

acid + base --\> water + salt

decomposition reaction

AB --\> A + B

combustion reaction

CH + O2 --\> CO2 + H2O

reduction-oxidation reactions

A + B --\> A(+) + B(-)

stoichometry

study of reactants and products in a chemical reaction

moles to moles conversion

mole ratio

moles to grams conversion

molar mass

moles A to grams B

mole ratio --\> molar of B

grams A to grams B

molar mass A --\> mole ratio --\> molar mass B

Boyle's Law

P1V1 \= P2V2

Charles' Law

V1/T1 \= V2/T2

Avogadro's Law

V1/n1 \= V2/n2

Gay-Lussac's Law

P1/T1 \= P2/T2

Combine Gas Law

P1V1/T1 \= P2V2/T2

Ideal Gas Law

PV \= nRT (R \= 0.08206 L(atm)/mol(K))

molarity

moles of solute/liters of solution

dilution equation

M1V1 \= M2V2

strong electrolyte

a solution in which a large portion of the solute exists as ions

weak electrolyte

a compound that dissociates only to a small extent in aqueous solution

acid properties

sour taste, red litmus paper result, electrolytes, reacts with metals and carbonates

base properties

bitter taste, slippery feel, blue litmus paper result, dissolve proteins and lipids

conjugate acid

an acid that forms when a base gains a proton

conjugate base

the particle that remains when an acid has donated a hydrogen ion

pH

hydrogen ion concentration

pH below 7

acidic

pH that is 7

neutral

pH above 7

basic

\[H+]

hydrogen ion

\[OH-]

hydroxide ion

\[H+][OH-]

1.0 x 10^-14

pH (finding H+)

-log[H+]

pOH (finding OH-)

-log[OH-]

10^-pH

\[H+]

10^-pOH

\[OH-]

pH + pOH

neutral (14)

delta E

change in internal energy (q + w)

kinetic energy

the energy an object has due to its motion

potential energy

stored energy

exothermic reaction

a chemical reaction in which heat is released to the surroundings

endothermic reaction

a reaction in which energy is absorbed

if a system does work

w is negative

if the system gets work done on it

w is positive

if heat is added

q is positive

if heat leaves the system

q is negative

heat capacity equation

Q \= smΔT

enthalpy

total energy of a system

entropy

a measure of the disorder of a system

delta H is positive

endothermic

delta H is negative

exothermic

concentration

M1V1 \= M2V2

wavelength

the distance between two corresponding parts of a wave

frequency

the number of complete wavelengths that pass a point in a given time

amplitude

the height of a wave's crest

photon

a particle of light

orbitals

regions around the nucleus in which given electron or electron pair is likely to be found

sublevel

an atomic orbital, or collection of atomic orbitals, that occupy a principal energy level and are called s, p, d, and f.

energy level

the specific amount of energy an electron has

red wavelengths

longest and have lowest energy

violet wavelengths

shortest with the most energy

white light

combination of all colors

ROYGBIV

colors of the visible spectrum in order of wavelength and frequency (red being longest and lowest and violet being shortest and highest)

s sublevel

2 electrons (sphere)

p sublevel

6 electrons (dumbbell shape)

d sublevel

10 electrons (clover)

f sublevel

14 electrons

electron configuration

the arrangement of electrons in an atom

hydrogen electron configuration

1s^1

arsenic electron configuration

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3 / [Ar] 4s2 3d10 4p3

antimony electron configuration (Sb)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p3 / [Kr] 4d10 5s2 5p3

periodic table atom sizes

atom increases as period increase / more protons pulls in electrons making it smaller (more to left it gets smaller-more to the bottom it gets bigger)

Lewis Structure

a structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.

polar covalent bond

a covalent bond in which electrons are not shared equally