Nomenclature (Chemistry Terms)

Acetate

C₂H₃O₂⁻

Carbonate

CO₃²⁻

hydrogen carbonate (bicarbonate)

HCO₃⁻

Hydroxide

OH⁻

Nitrate

NO₃⁻

Nitrite

NO₂⁻

Chromate

CrO₄²⁻

Dichromate

Cr₂O₇²⁻

Phosphate

PO₄³⁻

Hydrogen Phosphate

HPO₄²⁻

Ammonium

NH₄⁺

Hypochlorite

ClO⁻

Chlorite

ClO₂⁻

Chlorate

ClO₃⁻

Perchlorate

ClO₄⁻

Permanganate

MnO₄⁻

Sulfate

SO₄²⁻

Sulfite

SO₃²⁻

hydrogen sulfite (bisulfite)

HSO₃⁻

hydrogen sulfate (bisulfate)

HSO₄⁻

Peroxide

O₂²⁻

Cyanide

CN⁻

Kilo

1000 - 10³ - thousand

centi

hundredth - 10^-2 - 0.01

milli

thousandth - 0.001 - 10^-3

deci

tenth - 0.1 - 10¹

How many inches in a foot

12 inches in 1 foot

What charge does Ag (Silver)

Plus 1 charge

What charge does Zn (Zinc) have

Plus 2 charge

Order of listing elements for molecular compounds

C, P, N, H, S, I, Br, Cl, O, F

Order of prefixes from 1 - 10

Mono, Di, Tri, Tetra, Penta, Hexa, Hepta, Octa, Nona, Deca

If an acid ends with “ite“ what should the ending be

-ous

if an acid ends with “ate“ what should the ending be

-ic

Ionic compounds are what with what

Metal and Nonmetal

Molecular compounds are what with what

Nonmetals only

Acids are what?

H and one or more nonmetals

Binary acids are what with what?

hydrogen and a nonmetal - HCL - Hydrochloric acid

Oxyacids are what with what

Oxygen with a hydrogen and a nonmetal

What is Cd (Cadmium) charge

+2

What is Ga (Galliums) charge

+3

What is In (Indium) charge

+3

How to calculate the formula mass for both an element or a compound

Formula Mass for water is in Amu or g/mol and is the mols of an element times the Amu’s + the same thing for the other elements

Avogadros Number

1 mol = 6.022 × 10²³

Single element Mols to atoms and atoms to mols

Multiply mols by avogadros number (make sure to include units) to get atoms. Divide atoms by avogadros number to get mols

Single element Grams to mols

Divide the grams of the element by its amu to get mols. (Since amu can be written as mols per gram or grams per mol you can cancel them)

Single element Grams to atoms

Divide grams by amu, then multiply by avogadro’s number

Compound Grams to mols

Get the formula mass (molar mass) of the whole compound. Then treat it like a regular single element equation.

Compound grams to atoms.

Get the formula mass of the compound, change it to mols then multiply by avogadros number.

Number of mols of an element in a compound

Find the ratio (In H20 there are 2 H mols per 1 mol of H20) then cancel by the mols of H20 you have

Finding the grams an element has in a compound

Change grams of the compound to mols of a compound, then find the ratio of mols of the element to mols of the compound, then convert the mols of the element to grams

Empirical formulas are what?

Compounds whos subscripts cannot be reduced (Such as H302C5, Unlike H202C2 which could be molecular)

When using mass percents what should the bottom number be and what should the grams be

If you have 39.9% Cu then it should be 39.9 grams of Cu over 100 g of Cu02

How to find mass percent for an element from grams of a compound

Divide the grams of the element you want to find by the grams of the compound you have, then multiply by 100% (move the decimal to the right)

How to find mass percent from a chemical formula

Divide the molar mass of the element by the molar mass of the compound (also multiply by the ration of the top to bottom)

If the empirical formula numbers are not whole number what should you multiply with

These numbers (any just try to get the decimal to a whole number)

How to get empirical formula from grams

Change the grams to mols then shove them together, divide the mols of the compound by the mols of the smallest element, then multiply by the table of decimals to get a whole number (here it would be 2 resulting in N205, also try rounding to get 2 or 3 decimal places when getting the mols)

Getting empirical formula from percents

Change percents to grams, then those to mols, then divide by the smallest mol element, then multiply by the decimal table

Percent formulas add to what and how to get grams of an unknown element in a compound

Percent formulas add to 100% and if you have the grams of the compound and the grams of an element in the compound, conservation of mass lets you subtract the elements mass from the compound to get the rest.

Getting molecular formulas from empirical formulas

You get the molar mass of the empirical formula and the molar mass of the molecular compound you want to find. You divide the molar mass of the unknown compound by the molar mass of the empirical formula to get a number. You multiply that number to the empirical formula to get a molecular formula.

Mega symbol, size is what?

M / 10⁶

Kilo Symbol, Size is what?

k / 10³ / 1000

Deci Symbol, Size is what?

d / 10^-1 / 0.1

Centi Symbol, Size is what?

c / 10^-2

Milli Symbol, Size is what?

m / 10^-3

Micro Symbol, Size is what?

µ / 10^-6

Nano Symbol, Size is what?

n / 10^-9

1 lb = ? grams

453.59 grams = 1 ?

1 mile = ? km

1.609 km = 1 ?

1 cal = ? Joule

4.184 Joule = 1 ?

1 inch = ? cm

2.54 cm = ? inch

1 L = ? qt

1.0567 qt = ? L

1 L = ? mL

1000 mL = ? L

1 mL = ? cm³

1 cm³ = ? mL

1 atm = ? torr

760.00 torr = ? atm

°F = ?

(°C × 1.8) + 32

K = ?

°C + 273.15

density = ?

mass / volume

Mass Number

# of protons + # of neutrons

Atomic Number

# of Protons

Percent Natural Abundance

(Percent Natural Abundance of iso-1 / 100 Iso-1 Mass) + (PNA of iso-2 /100 * Iso-2 mass)….etc

Bromate

BrO₃^-

Hydrogen Sulfide

H2S^-

Carbon, Nitrogen, Oxygen, Fluoride, Chlorine, Bromine, Iodine

When they have an O₁ = They turn to -hypo (Hypochlorite - ClO^-)

When they have an O₂ = They turn to -ite (Carbonite - CO₂^2-)

When they have an O₃ = They turn to -ate

(Carbonate - CO₃^2-)

When they have an O₄ = They turn to -per

(Perbromate - BO₄^-)

Note: The charges also do not change

Phosphorous, Sulfur, Selenide, Arsenic

When they have an O₂ = they turn into hypo-

(Hyposulfite - SO₂^2-)

When they have an O₃ = They turn to -ite

(Phosphite - PO₃^3-)

When they have an O₄ = They turn to -ate

(Selenate - SeO₄^2-)

Note: The charges also do not change

Perflorate

FO₄^-

Perbromate

BrO₄^-

Periodate

IO₄^-

Selenate

SeO₄^2-

Arsenate

AsO₄^3-

Multiplying significant figures

The final answer will have the least number of significant figures.

3.95 × 0.2010 = 0.7935 is wrong (4 sig figs instead of 3)

0.794 is correct

Adding or subtracting significant figures

The final answer will have the least digits after the decimal

495+15.659+14.0 = 524.65 is wrong (2 decimal places instead of 0)

525 is right

How many sig figs are in 55.000

5 sig figs (any zero after a decimal is a sig fig)

How many sig figs are in 0.00600

3 sig figs (any zero before a nonzero is not a sig fig, but any number after is)

Hydronium

H₃O⁺

When finding molar mass or moles, the sig figs to use are the ones from the first number

46.68 g N * 1 mol/14.007 = 3.333 (the starting number had 4 sig figs)

Diatomic Elements

H₂, O₂, N₂, F₂, Br₂, I₂

Strong Acids

HCl, HBr, HI

HNO3

HClO4

H2SO4

Strong Bases

LiOH, NaOH, KOH

Ca(OH)2 (slightly soluble)

Ba(OH)2

Sr(OH)2

When you have strong bases or acids

separate bases and acids (H⁺ (aq) + Cl^- (aq) )
Keep weak acids together (NH₃)

Soluble Compounds (With Exceptions)

All sodium (Na⁺), potassium (K⁺), and ammonium (NH₄⁺) salts are SOLUBLE

All nitrate (NO₃^-), acetate (CH₃CO₂^-), chlorate (ClO₃^-), and perchlorate (ClO₄^-) salts are SOLUBLE

All chloride (and that means ANYTHING WITH Cl) (Cl^-), bromide (Br^-), and iodide (I^-) salts are SOLUBLE — EXCEPT those containing: lead, silver, or mercury (I) (Pb²⁺, Ag⁺, Hg₂²⁺) which are NOT soluble.

All sulfate (SO₄^2-) salts are SOLUBLE — EXCEPT those containing: calcium, silver, mercury (I), strontium, barium, or lead (Ca²⁺, Ag⁺, Hg₂²⁺, Sr²⁺, Ba²⁺, Pb²⁺) which are NOT soluble.