-Chapter 1-

qualitive vs quantitative observations

qualitive - descriptions, element type

quantitative - facts, measurements, temperature

-Chapter 2-

Distinguish between elements, compounds, mixtures

compound - consist of 2 or more elements chemically combined

element - simplest form of matter

mixture - when each substance retains individual properties

physical - what is looks and feels like

chemical -how it reacts

distillation - uses pure water and gas to seperate

In distillation, water undergoes a physical change because no new substances are formed

electrolysis - uses electricity to seperate into a gas

In electrolysis, it represents a chemical change because substances formed have entirely different properties than the compund

-Chapter 3-

atomic number vs mass number

atomic number - equals the number of protons

gives you the order on the period table

mass number - equals number of protons + number of neutrons

protons - positively charged particales

neutrons - no charge; slightly massive than protons

electrons - far away and small

Atomic Structure theories and contributions:

Dalton, Thompson, Rutherford

Dalton - made a model, Law of Constant Composition (the elemental composition of a pure substance never varies)

Thompson - ''plum pudding'' model (pudding = positive charge spread over sphere, plums = negative electron)

Rutherford - gold foil

Alkali metals - first vertical row, not including hydrogen

alkaline earth metals - 2nd vertical row

transition metals - 3-12 vertical rows

halogens - 2nd to last vertical row

noble gases - last vertical row

cation - positive ion

anion - negative ion

molecular -

ionic - compound that forms between a metal and a nonmetal

-Chapter 4-

writing formulas

for

Ionic Compounds

Type 1 Metals

Type 2 Metals (Roman Numeral)

Binary

Molecular Compounds

basically....

the first 2 rows and the other misc. elements have the charges listed on the back

the big middle area is the roman numerals, which tell you the charge

and the group on the right side of the big black line is the prefixes

mono, di, tri, tetra, penta, hexa, hepta, octa

-Chapter 5-

Significant Figures

Conversions

Density

Significant Figures -

examples

0.0025 - don't count

208 or 3.05 - always count

100. vs 100 - depends....one with . is

(the number of significant figures in the answer is the same as the lowest number of significant figures in the original problem)

Conversions - mili before kili

mili is 1000 times smaller

killi is 1000 times bigger

Density - ??? dont see it anywhere

-Chapter 6-

Mole, Avogradro's Number

Molar Mass

% Composition

Empirical vs Molecular

(very important stuff...but very familiar)

Mole - 6.02 x 10^23

Molar Mass - best way to explain this is an example

CH4

1 C atom and 4 H atoms

1(12.01) + 4(1.01) = 16.05 amu

% Composition -

mass % element = mass element/mass compound x 100

kind of tricky...look back in packet

Empirical Formula vs Molecular -

this is the thing were you find the moles of the elements and then whichever is the smallest you divide them by

(sound familiar?)

thats empirical

Molecular is a bit different

it will give you the molar mass

and then you figure out the empirical formula, and then the mass of that formula

then divide them

-Chapter 7-

(smallest chapter ;)

Law of Conservation Mass

Reactants vs Products

Coefficients vs Subscripts

Law of Conservation Mass - mass is neither created or detroyed in chemical equations

(relates to why we bother balancing equations)

Reactants vs Products -

reactant is the first part of the chemical equation

product is the 2nd part

Coefficients vs Suscripts -

coefficient is the smallest integers in a balanced equation

subscript- ?? doesnt say anywhere

-Chapter 8-

(the big one)

Driving Forces for Chemical Reactions

Types of Chemical Reactions

Complete ionic reactions

Net Ionic Reactions

Spectator Ions

Strong Electrolytes

Properties of Acids and Bases

Salts

oh wow....ok

Driving Forces - formation of

a solid

water

electrons

a gas

Types of Chemical Reactions -

Synthesis - 2 elements together

Decomposition - breaking it down to 2 elements

Single Replacement - same as precipitation but there will be an odd element out

Double Displacement - broken down A LOT (look it up)

Combustion - add O2

Precipitation - switch the two beginings and ends

Acid-Base - water (l) and then what you did for precipitation

Redox - many of the ones above

 Properties of Acids and Bases -

Acids are sour, conduct an electric current, turn blue litimus paper red, low pH ( I think of a lemon

Bases are bitter and feel slippery, they conduct an electric current, turn red litimus paper blue, high pH (think of laundry detergent)

Salts - occur when a strong acid and a strong base mix

Chapter 9 and 10

(DONE!!!)

Limiting Reactant

Theoretical Yield

Actual Yield

% Yield

______________

Exothermic vs Endothermic

State Functions : Energy, Enthalpy, Entropy

Heat vs Work

Temperature

Kinetic vs Potential Energy

1st Law Thermodynamics

Hess's Law

Calorimetry

Limiting Reactant - pretty self explainitory

Theoretical Yield- the amount supposed to be produced

actual- the amount actually produced

% yield - actual/theoretical

Exothermic vs Endothermic -

exo bonds are being formed and so heat is released

endo are being broken so heat is taken

State Functions