Chemistry EOC Review Semester 1

Chlorate

Chlorate

ClO3 -1

Phosphate

PO4 -3

Nitrate

NO3 -1

Carbonate

CO3 -1

Matter

anything that has mass and takes up space

Liquid

the state of matter that has a definite volume but not a definite shape

Solid

the state of matter in which the volume and shape of a substance are fixed

Gas

a form of matter that doesn't have a definite volume or shape

Compound

a compound made up of atoms of two or more different elements joined by chemical bonds

Symbol

Abbreviations used in chemistry for chemical, functional groups and chemical compounds

Formula

the way of presenting information about the chemical proportions of atoms that constitutions a particular chemical compound or molecule using chemical element symbols, numbers, and sometimes other symbols

Mixture

two or more liquids mixed together physically not chemically- not solid or a gas

Proton

positively charged ion

Electron

negatively charged ion

Neutron

an ion that has no charge

Law of Conservation of Mass

the law that states that mass cannot be created or destroyed in ordinary chemical and physical changes

Mono

1

Di

2

Tri

3

Tetra

4

Penta

5

Hexa

6

Hepta

7

Octa

8

Nona

9

Deca

10

Non acid that looses one oxygen (remember ates)

-ite

Non acid that looses two oxygen (remember ates)

hypo- -ite

Non acid that gains one oxygen

per- -ate

Basic Acid

hydro- -ic

Ending with ate acid

-ic

Acid that lost oxygen (ite in basic)

-ous

Acid that lost two oxygens (hypo- -ite in basic)

hypo- -ous

Acid that gains an oxygen (per- -ate in basic)

per- -ic

Ammonium

NH4 +1

Acetate

C2H3O2 -1

Chromate

CrO4 -2

Dichromate

c2O7 -2

Hydroxide

OH -1

Hydride

H -1

Mole

6.02 X 10^23

Salts containing Group 1 elements

Soluble

Salts containing the ammonium ion NH4 +1

Soluble

Salts containing nitrate ion NO3 -3 or chlorate ion ClO3 -1

Soluble

Salts containing Cl- Br- I- Exclusions to rule: Ag+ Pb+2 Hg+2

Soluble

Salts containing acetate

Soluble

Silver salts

Insoluble

Sulfate salts Exceptions: BaSO4 PbSO4 Ag2SO4 CaSO4 SrSO4

Soluble

Sulfides Exceptions: Barium, Calcium, Strontium, and column 1 metals

Insoluble

Carbonates Exceptions: Column one metals

Insoluble

Chromates Exceptions: Column one metals

Insoluble

Phosphates Exceptions: Column one metals

Insoluble

Fluorides Exceptions: Column one metals

Insoluble

Silicates Exceptions: Column one metals

Insoluble

Strong Acids

HNO3, HCl, HClO4, HI, HBr, H2SO4

Strong Bases

NaOH, KOH, Ca(OH)2, Ba(OH)2, Sr(OH)2

Organic Compounds (soluble or insoluble)

Almost always insoluble

Water (soluble or insoluble)

Not soluble

Percent Composition

Find the weight of each element and divide that by the total weight of the compound

Empirical Formula

A. If given percents - make the mythical 100 gram sample and then turn it into moles. Divide the lowest number to get a ratio, if the ratio is a whole number (or close by .1 or .9) then you can round. If it is not a whole number you can multiply them ALL by 2,3,4,5,etc... to get them to whole numbers. B. Given a compound weight - find the weight of the empirical formula and divide the given weight by the weight of the empirical formula. However many times the empirical weight goes into the compound weight must multiply the empirical formula by that number.

Net Ionic Equations

1. Balance the equation

2. Decide if the compounds are soluble or not

3. Break apart the soluble ones with charges

4. Cross out ions same on both sides of equation

5. Remaining ions (with charges)/compounds = net ionic equation

Stoichiometry

1. Write/balance the equation

2. Convert what was given into moles

3. Converts moles of what is given to moles of what is asked for (this means the ratio from the balanced equation)

4. Convert moles of what is wanted to grams

If given amounts of two reactants then must get moles of both then compare the amounts to the ratio from the equation, if the number is too big that means the one on the bottom is the limiting reagent and if the number is too big the one on the top is the limiting reagent. Then use the mole of the limiting reagent to move forward starting at number 3 above.

Li

Lithium (+1)

Na

Sodium (+1)

K

Potassium (+1)

Rb

Rubidium (+1)

Cesium (+1)

Cs

Fr

Francium (+1)

Beryillum

Be (+2)

Mg

Magnesium (+2)

Ca

Calcium (+2)

Strontium (+2)

Sr

Ba

Barium (+2)

Radium (+2)

Ra

Al

Aluminum (+3)

Fe

Iron (+2)

W

Tungsten

Au

Gold

Ag

Silver (+1)

Zinc

Zn (+2)

Cd

Cadmium (+2)

Pb

Lead

Boron

B (+3)

Carbon

C (-4)

Phosphorous

P (-3)

Oxygen

O (-2)

Ionic Compound

A metal and non metal

Converting moles to grams

moles x molar mass/1 mol

• Start with moles (2.792 mole H2O), multiply by grams (18 grams in H2O) and divide by 1 mole (6.02) = 50.0 gr H20

Converting grams to moles

grams x 1 mol/ molar mass of element

• 116 gr O2, multiply by 1 mole (6.02) and divide by molar mass (32 gr total in O2)

Helium

He (neutral)

Fluorine

F (neutral or -1)

Neon

Ne

Silicone

Si

Argon

Ar

Scandium

Sc (+3)

Titanium

Ti

Vanadium

V

Chromium

Cr

Manganese

Mn

Cobalt

Co