Equations

Nomenclature

Nomenclature

Terminology of chemistry. Also known as the naming process of

compounds.

Oxidation NumberThe 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 BondsWhen one or more

electrons are shared between two elements

to form a bond.

Molecule

Two or more atoms joined together by

covalent bonds

Metallic BondsA 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• Di- 2• Tri- 3• Tetra- 4• Penta- 5

• Hexa- 6• Hepta- 7• Octa- 8• Nona- 9• Deca- 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.

Ex: Chloride (Cl-1)

Hydro-, -icPrefix 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

CoefficientIs 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 e-

Strongest of the bonds• Double Bond: contains 4 e-

• Triple Bond: contains 6 e-

Weakest of the bonds

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 ReactionWhen a substance goes through a reaction and changes into another

substance.

Chemical EquationsA formula which

shows how elements or compounds react to form new compounds

2H+ + O-2 H2O

Parts of a chemical equations

• Reactants

• Yield Sign

• Products

ReactantsThe elements or

compounds that are found on the left side

of the yield sign

Yield SignAn arrow found in the equation which works

like an equal sign

ProductsThe 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.

CatalystsA substance that increases

the rate of chemical reactions without themselves becoming chemically changed or part of

the product

InhibitorA 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 EquationFor 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+ + O-2 H2O

Decomposition Reaction

A reaction where the reactants break down

(decompose)

Decomposition Reaction

H2O 2H+ + O-2

Single Displacement Reaction

A reaction where one element replaces

another element in a compound

Single Displacement Reaction

2Al3+ + 3Ag2S Al2S3 + 6Ag2+

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

CombustionA reaction in which a

compound (often carbon) reacts with

oxygen

CombustionC + O2 CO2

CH4 + 2O2 CO2 + 2H2O

C3H8 + 5O2 3CO2 + 4H2O

C6H12O6 + 6O2 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 ReactionsC6H12O6 + 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

Oxidation-Reduction Reaction

Another name for the Redox Reaction