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Chapter 1

Elements and Symbols

Name	Symbol	Name	Symbol
Antimony	Sb	Iron	Fe
Aluminum	Al	Lead	Pb
Argon	Ar	Lithium	Li
Arsenic	As	Magnesium	Mg
Barium	Ba	Manganese	Mn
Beryllium	Be	Mercury	Hg
Bismuth	Bi	Neon	Ne
Boron	B	Nickel	Ni
Bromine	Br	Nitrogen	N
Cadmium	Cd	Oxygen	O
Calcium	Ca	Phosphorous	P
Carbon	C	Platinum	Pt
Cesium	Cs	Potassium	K
Chlorine	Cl	Radium	Ra
Chromium	Cr	Rubidium	Rb
Cobalt	Co	Silicon	Si
Copper	Cu	Silver	Ag
Fluorine	F	Sodium	Na
Gallium	Ga	Strontium	Sr
Germanium	Ge	Sulfer	S
Gold	Au	Tin	Sn
Helium	He	Titanium	Ti
Hydrogen	H	Uranium	U
Iodine	I	Zinc	Zn

Metric Prefixes

Prefix	Symbol	Numerical Value
Giga	G	10⁹
Mega	M	10⁶
kilo	k	10³
centi	c	10^-2
milli	m	10^-3
micro	u	10^-6
nano	n	10^-9

1 mL = 1 cm³

Equations

Converting Celsius to Kelvin: K = C + 273.15

Equation for work:

w=F\times d
w = work
F = force
d = distance

Chapter 2

The following widely used metals have several common oxidation states:
- Vanadium V
- Chromium Cr
- Manganese Mn
- Iron Fe
- Cobalt Co
- Nickel Ni
- Copper Cu
- Gold Au
- Mercury Hg
- Antimony Sb
- Tin Sn
- Lead Pb
- Uranium U

Metalloids

B, Si, Ge, As, Sb, Te

Average Mass

The formula for calculating the average mass of isotopes is:
Average mass = (mass₁ × % abundance₁) + (mass₂ × %abundance₂) + ... + (massₙ × %abundanceₙ)
Where:
- mass₁, mass₂, ..., massₙ are the masses of the isotopes
- abundance₁, abundance₂, ..., abundanceₙ are the relative abundances of the isotopes

Groups of the periodic table

Alkali metals (1A)
Alkaline-earth metals(2A)
Transition metals (3-12)
Halogens (7A)
Noble gases (8A)

Polyatomic Ions

Name	Equation	Name	Equation
Hydroxide	OH^{-}	Bicarbonate	HCO_{3}^{-}
Hydronium	H_{3}O^{+}	Cyanide	CN^{-}
Ammonium	NH_{4}^{+}	Sulfate	SO_{4}^{2-}
Nitrate	NO_{3}^{-}	Sulfite	SO_{3}^{2-}
Nitrite	NO_{2}^{-}	Phosphate	PO_{4}^{3-}
Perchlorate	ClO_{4}^{-}	Hydrogen Phosphate	HPO_{4}^{2-}
Chlorate	ClO_{3}^{-}	Dihydrogen Phosphate	H_{2}PO_{4}^{-}
Chlorite	ClO_{2}^{-}	Phosphite	PO_{3}^{3-}
Hypochlorite	ClO^{-}	Acetate	C_{2}H_{3}O_{2}^{-}
Carbonate	CO_{3}^{2-}	Permanganate	MnO_{4}^{-}

Important Molecules

Water: (H₂O)

Ammonia: (NH₃)

Hydrogen Sulfide: (H₂S)

Acids

Strong:

Hydrofluoric acid (HF)

Hydrochloric acid (HCl)

Hydrobromic acid (HBr)

Hydroiodic acid (HI)

Chloric acid (HClO₃)

Perchloric acid (HClO₄)

Nitric acid (HNO₃)

Sulfuric acid (H₂SO₄)

Weak:

Acetic acid (C₂H₄O₂)

Organic/Base Molecules

Methane (CH₄)

Ethane (CH₃-CH₃)

Propane (CH₃-CH₂-CH₂) as base molecules

Change ending to –ol for alcohols

Strong Bases

Group 1A metal hydroxides

Heavy group 2A metal hydroxides ( Ca(OH)2 ) and down.

Chapter 3

Symbols for Chemical Reactions

(g) = gas
(l) = liquid
(s) = solid
(aq) = dissolve in aqueous (water) solution
(Δ) = heat needed for reaction.

Reactions

Be able to recognize/name Combination, Decomposition, and Combustion reactions.

Formula for Percent Composition

Avogadro’s Number:

6.022×10²³ particles/mols

Formula for Percent Yield

What To Memorize: Chapters 1-3