Equations

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Equations
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Nomenclature
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Nomenclature

• Terminology of chemistry. Also known as the
  naming process of compounds.

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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)

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Chemical Bonds

• When elements join together, they form a chemical
  bond.

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Types of chemical bonds

• Ionic Bonds
• Covalent Bonds
• Metallic Bonds

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Ionic Bonds

• When one or more electrons move from one element
  to another to form a bond

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Ion

• When the charge of an atom is not neutral. It
  will have either more protons than electrons or
  more electron than protons.

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Covalent Bonds

• When one or more electrons are shared between two
  elements to form a bond.

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Molecule

• Two or more atoms joined together by covalent
  bonds

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Metallic Bonds

• A special case where three or more metals bond
  together. One or more electrons are shared among
  more than two elements.

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Forms of Matter

• Elemental Matter
• Compounds
• Mixtures

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Elemental Matter

• A substance that is made up of only one kind of
  element

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Compounds

• A substance that is made up of more than one kind
  of element.

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Superscript

• The numbers written in the upper right hand
  corner of the atomic symbol of an element

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Subscript

• The number written in the lower right hand corner
  of an element and tells the number of element
  found in the chemical.

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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

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Prefixes used in naming

• Mono- 1
• Di- 2
• Tri- 3
• Tetra- 4
• Penta- 5

• Hexa- 6
• Hepta- 7
• Octa- 8
• Nona- 9
• Deca- 10

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Example using prefixes

• H20
• Dihydrogen monoxide
• CO2
• Carbon dioxide

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-ide

• Suffix used to end the anion in naming a compound
• Ex Sodium Chloride (NaCl)

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-ide

• Is used for ions which only contain the atoms
  heard in the name.
• Ex Chloride (Cl-1)

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Hydro-, -ic

• Prefix and suffix used for acids that were
  derived from ion with no oxygen.
• Ex Hydrochloric Acid (HCl)

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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
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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
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Coefficient

• Is the number found in front of an ion or
  compound. It tells the number of that ion or
  compound you have

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Polymer

• Large molecule formed by bonding many smaller
  molecules together, most often in long chains

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Long Chain
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Hydrocarbons

• A compound composed carbon and hydrogen. They
  make good type of fuel.

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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

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Polar Molecules

• A compound with one end having a positive charge
  and the other end with a negative charge.

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Nonpolar Molecule

• A compound that is neutral.

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Binary Compounds

• A compound composed of two elements.

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Organic Matter

• Matter which contains Carbon

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Equations
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Chemical Reaction

• When a substance goes through a reaction and
  changes into another substance.

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Chemical Equations

• A formula which shows how elements or compounds
  react to form new compounds

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2H O-2 ? H2O
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Parts of a chemical equations

• Reactants
• Yield Sign
• Products

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Reactants

• The elements or compounds that are found on the
  left side of the yield sign

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Yield Sign

• An arrow found in the equation which works like
  an equal sign

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Products

• The elements or compounds that are found on the
  right side of the yield sign

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Electrolysis

• The process of using electricity to break the
  chemical bonds.

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Activation Energy

• The amount of energy it takes to start a reaction.

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Catalysts

• A substance that increases the rate of chemical
  reactions without themselves becoming chemically
  changed or part of the product

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Inhibitor

• A substance that decreases the rate of chemical
  reactions without themselves becoming chemically
  changed or part of the product

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Endothermic Reactions

• Reactions that release less energy than was used
  to start reaction

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Exothermic Reactions

• Reactions that release more energy than was used
  to start reaction

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Catalyst

• A substance that increases the rate of a chemical
  reaction by lowering activation energies but is
  not itself consumed in the reaction.

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Inhibitor

• A substance that slows down the reaction rate of
  a chemical reaction or prevents a reaction from
  happening.

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Law of Conservation of Mass

• States that in any reaction, the same amount of
  mass must be found on both sides of the equation.

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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

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All chemical equations must be balanced.
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To balance an equation, you can change the
coefficient. However, you can never, never,
never change the subscript.
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Chemical Equilibrium

• A time period where the reactants come together
  just as quickly as the products breakdown

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Purity of a substance determines the behavior of
the substances.
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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).

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Synthesis Reactions

• A reaction where the reactants combine to form a
  bigger compound (also known as combination)

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Synthesis Reactions

• 2H O-2 ? H2O

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Decomposition Reaction

• A reaction where the reactants break down
  (decompose)

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Decomposition Reaction

• H2O ? 2H O-2

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Single Displacement Reaction

• A reaction where one element replaces another
  element in a compound

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Single Displacement Reaction

• 2Al3 3Ag2S ? Al2S3 6Ag2

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Double Displacement Reactions

• A reaction where the positive ion of two
  compounds switch, which forms two new compounds

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Double Displacement Reactions

• HCl NaOH ? NaCl H2O

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Combustion

• A reaction in which a compound (often carbon)
  reacts with oxygen

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Combustion

• C O2 ? CO2
• CH4 2O2 ? CO2 2H2O
• C3H8 5O2 ? 3CO2 4H2O
• C6H12O6 6O2 ? 6CO2 6H2O

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Redox Reactions

• A reaction where one compound loses electrons and
  becomes a smaller compound, while another
  compound gains electrons and becomes a bigger
  compound.

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Redox Reactions

• C6H12O6 6O2 ? 6CO2 6H2O

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Oxidized Compound

• The compound that loses electrons and becomes a
  smaller compound

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Reduced Compound

• The compound that gains electrons and becomes a
  bigger compound

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Oxidation-Reduction Reaction

• Another name for the Redox Reaction