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Chapter 2
Elements are made up of small particles called atoms. All atoms of the same
elements are identical.
Compounds are made up of atoms of more than just one element.
Chemical reactions are the separation, combination or rearrangement of atoms, it
doesn’t result in their creation or destruction.
Atoms are composed of electrons (negatively charged), neutrons (neutrally charge),
and protons (positively charged).
Z is the Atomic Number is the
number of protons in the nucleus of
each atom.
A is the Mass number is the total
number of neutrons and protons
present in the nucleus of an atom of an element.
The periodic table is a chart where elements are organized depending on how
similar they are. The horizontal rows are called periods and the vertical columns
are called groups or families.
The periodic table can be classified into metals, nonmetals, and metalloids.
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A molecule is two or more atoms in an arrangement created by chemical forces.
An ion is an atom or a group of atoms that has either a positive or negative charge.
Chemical formulas shows the exact number of atoms of each element in the smallest
unit of a substance.
Nomenclature
To name Ionic Compounds (compounds made of of cations and anions):
Add the suffix -ide to the anions.
For example, O2- is named Oxide
Al2O3 therefore is Aluminum Oxide
To name Transition Metals, you say the
name of the metal and the number of
ions.
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For example, F2+ is named Iron (II)
FeCl2 therefore is Iron (II) Chloride.
Naming other molecular compounds can consist of
Adding prefix
1 Mono2 Di3 Tri4 Tetra5 Penta-
6 Hexa7 Hepta8 Octa9 Nona10 Deca-
Naming Acids and Bases
Acids start with a hydro- prefix and an –ic ending, for example HCl is named
hydrocloric acid.
Chapter 3
Atomic mass is the mass of the atomic in amu (atomic mass units). Moles are the
amount of a substance that contains as many elementary entities as there are atoms
in exactly 12 g of the carbon-12 isotope.
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Grams = number of atoms divided by Avogadro’s
number.
Number of atoms = grams divided by
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Avogradro’s number
Avogadro's number = 6.0221415 × 1023
Percent composition of an element = n x molar mass of element divided by molar
mass of compound
For example to get the percent composition for iron(III) oxide you would write
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Chemical Equations uses chemical symbols to describe a chemical reaction.
Reactants are starting materials and products are
the finishing results.
Balancing chemical equations
Great tutorial on balancing chemical equations
Amounts of Reactants and Products
to find the number of moles in 2.00 g of NaCl, one would do the following:
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For example to completely react with 85.0 grams of iron (III) oxide, 28.7
grams of aluminum are needed.
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Chapter 4
General Properties of Aqueous Solutions
Solute is the substance present in a smaller amount and a solvent is the substance
present in a larger amount.
An electrolyte is a substance that results in a product that can conduct electricity,
when dissolved with water.
Acids

Have sour taste

Cause color changes in
plant dyes

React with metals to
produce hydrogen gas.

React with carbonates
and bicarbonates to
produce carbon
dioxide gas.

Aqueous acid
solutions conduct
electricity.
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Bases

Have bitter taste

Feel slippery

Cause color changes in
plant dyes

Aqueous base solutions conduct electricity.
Oxidation Reduction Reactions are electron-transfer reactions.
For example,
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Reduction reaction is a half=reaction that involves the gain of electrons. The
reducing agent donates electrons, whereas the oxidizing agent accepts electrons.
There is 3 types of Redox reactions:
Combination reaction is when two or more substances combine to form a single
product.
Decomposition reaction where is the opposite, in where there’s breakdown of a
compound into two or more components.
Displacement Reactions occur when an ion in a compound is replaced by an ion of
another element.

Hydrogen displacement

Metal displacement

Halogen displacement
Molarity is calculated as following:
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Titration is when a solution of accurately known concentration is added gradually
to another solution of unknown concentration, until the chemical reaction between
the two solutions is complete.