Equations
Nomenclature
Nomenclature
Terminology of chemistry.
Also known as the
naming process of
compounds.
Oxidation Number
The superscript which tells the
charge of the element and the
number of electrons it needs or
can give up in order to be stable
(happy)
Chemical Bonds
When elements join
together, they form a
chemical bond.
Types of chemical
bonds
• Ionic Bonds
• Covalent Bonds
• Metallic Bonds
Ionic Bonds
When one or more
electrons move from
one element to
another to form a bond
Ion
When the charge of an atom
is not neutral. It will have
either more protons than
electrons or more electron
than protons.
Covalent Bonds
When one or more
electrons are shared
between two elements
to form a bond.
Molecule
Two or more atoms
joined together by
covalent bonds
Metallic Bonds
A special case where
three or more metals
bond together. One or
more electrons are
shared among more
than two elements.
Forms of Matter
• Elemental Matter
• Compounds
• Mixtures
Elemental Matter
A substance that is
made up of only one
kind of element
Compounds
A substance that is
made up of more than
one kind of element.
Superscript
The numbers written in
the upper right hand
corner of the atomic
symbol of an element
Subscript
The number written in the
lower right hand corner of
an element and tells the
number of element found
in the chemical.
Naming Binary
Compounds
• Write down the Name of the
positive element
• Write down the root of the
negative element
• Add the suffix –ide to the root
Prefixes used in naming
• Mono- 1
• Di2
• Tri3
• Tetra4
• Penta- 5
• Hexa• Hepta• Octa- 8
• Nona• Deca-
6
7
9
10
Example using prefixes
• H20
• Dihydrogen monoxide
• CO2
• Carbon dioxide
-ide
Suffix used to end the
anion in naming a
compound
Ex: Sodium Chloride
(NaCl)
-ide
Is used for ions which
only contain the atoms
heard in the name.
-1
Ex: Chloride (Cl )
Hydro-, -ic
Prefix and suffix used for
acids that were derived
from ion with no oxygen.
Ex: Hydrochloric Acid (HCl)
When naming a hydrogen
atom and a halogen,
change hydrogen to hydro-.
To the halogen add –ic
suffix. This is also an acid.
Ex: HCl
Hydrochloric Acid
For metals with more than
one oxidation number, then
write its oxidation number in
the formula. Use a Roman
Numeral for this.
Ex: FeCl2
Iron(II) Chloride
Coefficient
Is the number found in front
of an ion or compound. It
tells the number of that ion
or compound you have
Polymer
Large molecule formed
by bonding many
smaller molecules
together, most often in
long chains
Long Chain
Hydrocarbons
A compound
composed carbon and
hydrogen. They make
good type of fuel.
Types of Electron Bonds
• Single Bond: contains 2
Strongest of the bonds
• Double Bond: contains 4 e• Triple Bond: contains 6 eWeakest of the bonds
e
Polar Molecules
A compound with one
end having a positive
charge and the other
end with a negative
charge.
Nonpolar Molecule
A compound that is
neutral.
Binary Compounds
A compound
composed of two
elements.
Organic Matter
Matter which contains
Carbon
Equations
Chemical Reaction
When a substance goes
through a reaction and
changes into another
substance.
Chemical
Equations
A formula which
shows how elements
or compounds react to
form new compounds
+
2H
+
-2
O
 H2O
Parts of a chemical
equations
• Reactants
• Yield Sign
• Products
Reactants
The elements or
compounds that are
found on the left side
of the yield sign
Yield Sign
An arrow found in the
equation which works
like an equal sign
Products
The elements or
compounds that are
found on the right side
of the yield sign
Electrolysis
The process of using
electricity to break the
chemical bonds.
Activation Energy
The amount of energy
it takes to start a
reaction.
Catalysts
A substance that increases
the rate of chemical reactions
without themselves becoming
chemically changed or part of
the product
Inhibitor
A substance that decreases
the rate of chemical reactions
without themselves becoming
chemically changed or part of
the product
Endothermic
Reactions
Reactions that release
less energy than was
used to start reaction
Exothermic
Reactions
Reactions that release
more energy than was
used to start reaction
Catalyst
A substance that increases
the rate of a chemical
reaction by lowering
activation energies but is not
itself consumed in the
reaction.
Inhibitor
A substance that
slows down the
reaction rate of a
chemical reaction or
prevents a reaction
from happening.
Law of Conservation of
Mass
States that in any reaction,
the same amount of mass
must be found on both sides
of the equation.
Balanced Equation
For each element in a
chemical equation, the same
number of each element must
be found on the left side of the
arrow as on the right side
All chemical equations
must be balanced.
To balance an
equation, you can
change the coefficient.
However, you can
never, never, never
change the subscript.
Chemical
Equilibrium
A time period where the
reactants come together just
as quickly as the products
breakdown
Purity of a substance
determines the behavior
of the substances.
Symbols used in Chemical
Equations
(l) The chemical is a liquid.
(s) The chemical is a solid.
(g) The chemical is a gas.
(aq) The chemical is aqueous
(dissolved in water).
Synthesis
Reactions
A reaction where the
reactants combine to form a
bigger compound (also
known as combination)
Synthesis
Reactions
+
2H
+
-2
O
 H2O
Decomposition
Reaction
A reaction where the
reactants break down
(decompose)
Decomposition
Reaction
H2O 
+
2H
+
-2
O
Single Displacement
Reaction
A reaction where one
element replaces
another element in a
compound
Single Displacement
Reaction
3+
2Al
+ 3Ag2S  Al2S3 +
2+
6Ag
Double Displacement
Reactions
A reaction where the
positive ion of two
compounds switch, which
forms two new
compounds
Double Displacement
Reactions
HCl + NaOH  NaCl + H2O
Combustion
A reaction in which a
compound (often
carbon) reacts with
oxygen
Combustion
C + O2
 CO2
 CO2 +
CH4 + 2O2
C3H8 + 5O2

C6H12O6 + 6O2
2H2O
3CO2 + 4H2O
 6CO2 + 6H2O
Redox Reactions
A reaction where one
compound loses electrons
and becomes a smaller
compound, while another
compound gains electrons
and becomes a bigger
compound.
Redox Reactions
C6H12O6 + 6O2  6CO2 + 6H2O
Oxidized
Compound
The compound that
loses electrons and
becomes a smaller
compound
Reduced
Compound
The compound that
gains electrons and
becomes a bigger
compound
OxidationReduction Reaction
Another name for the
Redox Reaction