Examples Examples Na+1 + o-2 

Examples

• Examples

• Na+1 + O-2 

• Ca+2 + P-3 

• C+4 + O-2 

Chemical Nomenclature--> system used to name chemical substances.

• Chemical Nomenclature--> system used to name chemical substances.

• The Name of a compound indicates the composition of the substance.

• From the name one can

• deduce a chemical formula.

The first element is named as usual but only a stem of the second is used followed by the suffix “ide”

• The first element is named as usual but only a stem of the second is used followed by the suffix “ide”

• For example: MgCl2 is Magnesium chloride

• : Al2O3 is Aluminum Oxide

• The Chlorine and Oxygen must change their suffix from “ine” and “ygen” to “ide” !

Try these!

• Try these!

• NaCl

• Li3N

• MgI2

A compound that contains a transitional metal must be named so that the oxidation # of the metal is identified.

• A compound that contains a transitional metal must be named so that the oxidation # of the metal is identified.

• A Roman numeral is placed after the metal. It represents the oxidation # of the metal.

• Ex. FeCl3  Iron (III) Chloride

• CuCl2  Copper (II) Chloride

The total charge on any compound or molecule

• The total charge on any compound or molecule

• is always equal to zero.

• To determine unknown oxidation #s, add up the oxidation #s of the Cation and Anion and set them equal to zero. (Create an algebra formula and solve for X.)

• Example Cr2O3 total charge = 0

• Cr = x , O = -2

• Formula 2x + 3(-2)= 0  2x-6= 0 x= +3 Cr= +3

Name These,

• Name These,

• FeCl2

• CrO2

• NiP

If two non-metals are bonded covalently, the name can be shown using prefixes.

• If two non-metals are bonded covalently, the name can be shown using prefixes.

• The number of atoms for each element in a molecule is usually indicated by the prefix:

• mono - 1 atom - hexa - 6 atoms
• di - 2 atoms - hepta - 7 atoms
• tri - 3 atoms - octa - 8 atoms
• tetra - 4 atoms
• penta - 5 atoms

Examples:

• Examples:

• nitrogen dioxide is NO2

• dinitrogen pentoxide is N2O5

• phosphorus tribromide is PBr3

• The prefix represents the subscript.

•  If the subscript is one mono is not needed.

Name these :::

• Name these :::

• Use Old Naming system and Stock system

• PCl3

• PCl5

• SO2

Formulas of compounds containing polyatomic ions are written in a manner to stress the fact that the ions are independent units

• Formulas of compounds containing polyatomic ions are written in a manner to stress the fact that the ions are independent units

• An example is Sodium Nitrate which contains the nitrate ion (NO3)-1 is written NaNO3

When naming these compounds the name of the poly-ion is unchanged.

• When naming these compounds the name of the poly-ion is unchanged.

• Examples

• 1. Na2SO4  Sodium Sulfate

• 2. (NH4)2Se  Ammonium Selenide

• If Ammonium is the poly-atomic ion, the non-metal still maintains its “ide” suffix.

If a compound contains a polyatomic ion with a subscript of two or more the ion is enclosed in parenthesis:

• If a compound contains a polyatomic ion with a subscript of two or more the ion is enclosed in parenthesis:

• Example:

• calcium bicarbonate Ca(HCO3)2
• ammonium sulfide (NH4)2S

Name these ::: Go to page 226 or your packet for help.

• Name these ::: Go to page 226 or your packet for help.

• Ca(ClO3)2

• NH4OH

• Cr(SO4)2

• Memorize the 12 Common Poly-atomic Ions.

• There will be an Ion quiz very soon.

Polyatomic Ions containing Oxygen can be represented a number of different ways.

• Polyatomic Ions containing Oxygen can be represented a number of different ways.

• If one less Oxygen in the formula. The suffix is changed from “ate” to “ite”. The ion’s charge does not change.

• Ex. (NO3)-1  Nitrate vs. (NO2)-1  Nitrite

• If two less Oxygens the prefix “hypo-” is placed in front of the “ite” name.

• Ex. (ClO)-1  hypo- Chlorite

• If one more Oxygen the prefix “per-” is placed in front of the “ate” name.

• Ex. (ClO4)-1  Per Chlorate

Acids have their own naming system and they must be recognized when dealing with nomenclature.

• Acids have their own naming system and they must be recognized when dealing with nomenclature.
• The name acid comes from the Latin term for “sour”
• {Acids are sour to the taste}
• Acids are substances that donate protons (H+)
• {usually when dissolved in water}
• The Chemical formula almost always begins with Hydrogen
• Example: hydrochloric acid  HCl
• sulfuric acid  H2SO4

Lets separate acids into 2 types:

• Lets separate acids into 2 types:

• Acids that contain oxygen
• H3PO4 H2SO4
• HNO3 H2O
• Acids that do not contain oxygen
• HCl HBr
• HF H2S

Naming acids containing oxygen:

• Naming acids containing oxygen:

• For acids containing “-ate” anions:
• Use root of the anion (for sulfate, SO42-, use sulfur)
• Add “-ic” suffix then end with “acid”
• Example: H3PO4 is Phosphoric acid
• For acids with “-ite” anions:
• Use root of the anion (for sulfite, SO32-, use sulfur)
• Add “-ous” suffix then end with “acid”
• Example: H2SO3 is sulfurous acid

Naming acids not containing oxygen:

• Naming acids not containing oxygen:

• Add “hydro-” prefix to beginning
• Use root of the anion (i.e. Cl- use chlor)
• Add “-ic” suffix then end with “acid”
• Example: HCl is hydrochloric acid

• Name the following acids:

• HF
• HNO2
• HCN
• H3PO4

A hydrate molecule is a ionic compound that contains water molecules trapped inside the crystalline structure.

• A hydrate molecule is a ionic compound that contains water molecules trapped inside the crystalline structure.

• The Formula includes a dot followed by the number of water molecules

• Ex: Copper(II) Sulfate Pentahydrate

• CuSO4 · 5H2O

• The Name of a hydrate molecule would

• include two separate names.

• To name, use the name of the ionic compound followed by the term … hydrate. A Greek Prefix would be used to represent the number of water molecules that are trapped.

• CoCl2 · 2 H2O

• Colbalt(II) Chloride Dihydrate