Unit 9 Chemical Compounds Chapter 6 P. Sci. Unit 9 Chemical Compounds Chapter 6

Compound Names and Formulas Part 2 Compound Names and Formulas

Binary Compounds Al(ClO3)3 P2O5 NaCl Most of the compounds that you will have to name will have only 2 elements (called binary – bi meaning 2) or an element and a polyatomic ion. NaCl CaCl2 P2O5 NaNO3 Al(ClO3)3 CaCl2 NaNO3

First you have to identify what type of compound it is : Naming Compounds First you have to identify what type of compound it is : Ionic – metal and non-metal. Covalent – two non-metals Polyatomic - both NaCl N2O4 CaCO3

Write the name of the metal (cations = + ion) Ionic Compounds Write the name of the metal (cations = + ion) Examples: Na = Sodium Ca = Calcium Al = Aluminum

Ionic compounds cont. Write the name of the non-metal (anion = - ion) but change the ending to “ide”. Examples: Chlorine – Chloride Fluorine – Fluoride Oxygen – Oxide Sulfur – Sulfide Phosphorus – Phosphide Iodine - Iodide

NaCl = Sodium chloride CaI2 = Calcium iodide CsBr = Cesium bromide Examples NaCl = Sodium chloride CaI2 = Calcium iodide CsBr = Cesium bromide Al2O3 = Aluminum Oxide For ionic compounds – pay no attention to the subscripts.

Now you try Name the following ionic compounds. LiF = MgO = SrCl = K2S = Ca3N2 =

Answers LiF = Lithium fluoride MgO = Magnesium oxide SrCl = Strontium chloride K2S = Potassium sulfide Ca3N2 = Calcium Nitride

Covalent Compounds First Name If there is only one atom of this element, just write the name of the element. Example: N = Nitrogen C = Carbon P = Phosphorus

Covalent compounds cont. First Name cont. If there is more than one atom of the element, write the name of the element with the pre-fix that tells how many atoms are there.

Pre-fixes 1 – mono 6 – hexa 2 – di 7 – hepta 3 – tri 8 – octa 4 – tetra 9 – nona 5 – penta 10 – deca

Examples: H2 – di-hydrogen C3 – tri-carbon Br4 – tetra-bromine

Covalent compounds cont. Second Name – Always has a prefix. Always starts with a prefix that tells how many atoms are there. (even if there is only one)

Covalent compounds cont. Second Name cont. ends in “ide” Examples : CO – carbon monoxide CO2 – carbon dioxide CO3 – carbon trioxide

Name the following covalent compounds. Now you try Name the following covalent compounds. NO2 = PBr3 = AsCl = H2O = H2O2 =

Answers NO2 = Nitrogen dioxide PBr3 = Phosphorus tribromide AsCl = Arsenic monochloride H2O = Di-hydrogen monoxide H2O2 = Di-hydrogen dioxide

Polyatomic Ions Compounds with both ionic and covalent bonds. Acts the same as any other ion.

Examples: Ammonium NH4+ Hydroxide OH- Sulfate SO4+2 Carbonate CO3-2 Polyatomic ions cont. Examples: Ammonium NH4+ Hydroxide OH- Sulfate SO4+2 Carbonate CO3-2

Follow step one for ionic compounds. (Write the name of the metal) Polyatomic compounds Follow step one for ionic compounds. (Write the name of the metal) Write the name of the polyatomic ion (do not change to “ide”) Examples: NaNO3 = Sodium nitrate Al(ClO3)3 = Aluminum chlorate

The End