Honors Chemistry

element

a pure substance made of only one kind of atom, cannot be broken down

compound

a pure substance made of 2 or more kinds of atoms, cannot be broken down

element

a pure substance made of only one kind of atom, cannot be broken down

compound

a pure substance made of 2 or more kinds of atoms, cannot be broken down

molecule

a group of atoms bonded together

homogenous mixture

a mixture in which the composition is uniform throughout, can be separated

heterogenous

a mixture in which the composition is non-uniform throughout, can be separated

decantation

less dense liquid is poured off from the more dense liquid, therefore separating the liquid and solid

filtration

solids separated from liquids by using filter paper to trap solid component

distillation

using different boiling points of substances to separate homogenous mixtures into their components

intensive property

properties that do NOT depend on the amount of matter present (ex: melting point, conductivity, color)

extensive property

properties that depend on the amount of matter present (ex: volume, mass)

physical property

property used to describe matter without changing the composition of the matter (ex: color, boiling point)

chemical property

substance's ability to change into something new (ex: rusting, cooking, combustion reactions)

solid

definite volume + shape, packed particles, held by strong attractive forces, less energy

liquid

definite volume, indefinite shape, moves faster + slightly higher energy

gas

indefinite volume + shape, weak attraction, moves fastest + high energy

plasma

particles ionize

Law of Conservation of Energy

energy is neither created nor destroyed; only converted into a different form

physical change

change in substance that does not involve a change in composition of substance/change in matter where you don't create anything new (phase changes are all physical changes, physical changes could be reversed)

chemical change

a change in which one or more substances are converted into different substances - chemical changes cannot be reversed (any reaction) - signs: bubbles, production of new odor or vapor

tera-

T, 10^12

giga-

G, 10^9

mega-

M, 10^6

kilo-

k, 10^3

hecto-

h, 10^2

deka-

da, 10^1

deci-

d, 10^-1

centi-

c, 10^-2

milli-

m, 10^-3

micro-

μ, 10^-6

nano-

n, 10^-9

pico-

p, 10^-12

C to F equation

F = 1.8C + 32

K to C equation

C = K - 273

precision

how close a group of measurements are to each other

accuracy

how close a measurement is to the true value

percent error equation

(100)(experimental value-theoretical value)/theoretical value

sig figs

go from the right for decimals, go from the left for non-decimals

John Dalton

atomic theory, discovered initial model of the atom (knew nothing about subatomic particles)

JJ Thomson

discovery of negative subatomic particles, cathode ray experiment (discovered electrons), Plum Pudding Model

Ernest Rutherford

discovered the nucleus through Gold-Foil experiment

Neils Bohr

created Bohr Model (model that organized electrons in energy clouds around the nucleus)

James Chadwick

discovered the neutron

average atomic mass=

(mass isotope 1)(relative abundance) + (mass isotope 2)(relative abundance)

you have to add the charge for ____ when writing them out

transition metals

isotope notation

atomic mass on top, atomic number on bottom, the element to the right

ion

charged atom

ionic compound

nonmetal + metal, lose/gain electrons, strong conductors, high melting + boiling points, forms crystal lattice structure

cations (metals)

positively charged ions

anions (nonmetals)

negatively charged ions

naming ionic compounds

metal anion(ide)

silver (Ag) is always ____ charge

+1

zinc (Zn) is always ____ charge

+2

hydronium

H3O+

cyanide

CN-

oxalate

C2O4 2-

nitrite

NO2-

sulfite

SO3 2-

phosphite

PO3 3-

hypochlorite

ClO-

chlorate

ClO3-

permanganate

MnO4-

chromate

CrO4 2-

dichromate

Cr2O7 2-

ammonium

NH4+

hydroxide

OH-

carbonate

CO3 2-

nitrate

NO3-

sulfate

SO4 2-

phosphate

PO4 3-

chlorite

ClO2-

perchlorate

ClO4-

acetate

C2H3O2-, CH3COO-, CH3CO2-

Avogradro's number

6.02x10^23

covalent compound

nonmetal + nonmetal, shared electrons, strong insulators, do NOT conduct electricity, low melting + boiling point)

tetra

4

penta

5

hexa

6

octa

8

nona

9

deca

10

naming covalent compounds

add prefixes to element 1 (except if it is 1), add prefixes to element 2 (even if it is 1)

percent composition

(100*mass of element)/(total mass of compound)

molecular formula (finding the "magic number)

(molar mass of the compound)/(molar mass of the empirical formula)

synthesis reaction

A+B-->AB

decomposition reaction

AB --> A + B

single replacement reaction

AB + C --> AC + B (metals only switch w/ metals)

double replacement reaction

AB + CD --> AD + CB (metals only switch w/ metals)

combustion reaction

hydrocarbon + O2 --> CO2 + H2O

diatomic elements

H2, N2, O2, F2, Cl2, Br2, I2 (7)

stoichiometry

using coefficients to convert between different types of elements

percent yield

(actual yield*100)/(theoretical yield)

limiting reactant (reagent)

the reactant that is completely consumed when a reaction is run to completion (smallest when you test the reactants on one product)

molarity equation

(moles of solute)/(liters of solution)

concentration

how much "stuff"" is in the solution

solution

homogenous mixture of 2 or more substances in a single phase (aq)

solute

the substance being dissolved (usually smaller)

solvent

the dissolving medium (usually larger)

dissociation

separation of ions in a solution for ionic compounds

ionization

separation of ions in a solution for covalent compounds

electrolytes

a substance that dissolves in water to give a solution that conducts electric current