Honors Chemistry

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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
80
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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