Honors Chemistry

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element

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

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compound

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

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191 Terms

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element

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

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compound

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

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molecule

a group of atoms bonded together

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homogenous mixture

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

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heterogenous

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

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decantation

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

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filtration

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

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distillation

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

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intensive property

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

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extensive property

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

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physical property

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

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chemical property

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

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solid

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

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liquid

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

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gas

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

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plasma

particles ionize

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Law of Conservation of Energy

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

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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)

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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

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tera-

T, 10^12

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giga-

G, 10^9

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mega-

M, 10^6

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kilo-

k, 10^3

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hecto-

h, 10^2

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deka-

da, 10^1

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deci-

d, 10^-1

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centi-

c, 10^-2

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milli-

m, 10^-3

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micro-

μ, 10^-6

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nano-

n, 10^-9

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pico-

p, 10^-12

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C to F equation

F = 1.8C + 32

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K to C equation

C = K - 273

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precision

how close a group of measurements are to each other

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accuracy

how close a measurement is to the true value

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percent error equation

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

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sig figs

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

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John Dalton

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

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JJ Thomson

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

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Ernest Rutherford

discovered the nucleus through Gold-Foil experiment

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Neils Bohr

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

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James Chadwick

discovered the neutron

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average atomic mass=

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

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

transition metals

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isotope notation

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

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ion

charged atom

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ionic compound

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

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cations (metals)

positively charged ions

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anions (nonmetals)

negatively charged ions

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naming ionic compounds

metal anion(ide)

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silver (Ag) is always ____ charge

+1

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zinc (Zn) is always ____ charge

+2

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hydronium

H3O+

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cyanide

CN-

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oxalate

C2O4 2-

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nitrite

NO2-

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sulfite

SO3 2-

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phosphite

PO3 3-

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hypochlorite

ClO-

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chlorate

ClO3-

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permanganate

MnO4-

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chromate

CrO4 2-

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dichromate

Cr2O7 2-

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ammonium

NH4+

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hydroxide

OH-

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carbonate

CO3 2-

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nitrate

NO3-

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sulfate

SO4 2-

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phosphate

PO4 3-

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chlorite

ClO2-

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perchlorate

ClO4-

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acetate

C2H3O2-, CH3COO-, CH3CO2-

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Avogradro's number

6.02x10^23

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covalent compound

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

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tetra

4

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penta

5

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hexa

6

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octa

8

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nona

9

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deca

10

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naming covalent compounds

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

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percent composition

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

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molecular formula (finding the "magic number)

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

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synthesis reaction

A+B-->AB

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decomposition reaction

AB --> A + B

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single replacement reaction

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

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double replacement reaction

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

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combustion reaction

hydrocarbon + O2 --> CO2 + H2O

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diatomic elements

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

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stoichiometry

using coefficients to convert between different types of elements

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percent yield

(actual yield*100)/(theoretical yield)

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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)

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molarity equation

(moles of solute)/(liters of solution)

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concentration

how much "stuff"" is in the solution

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solution

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

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solute

the substance being dissolved (usually smaller)

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solvent

the dissolving medium (usually larger)

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dissociation

separation of ions in a solution for ionic compounds

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ionization

separation of ions in a solution for covalent compounds

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electrolytes

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