Warm UP - 10/24/2016 Write the compound formula or name the following formula for the following: 1) Sodium Acetate 2) Calcium Nitride 3) Ca3(PO4)2 4) Rb3P

Practice 1. Magnesium Sulfate 2. Ammonium Chloride 3. Iron (III) Carbonate 4. Ammonium Phosphate 5. Aluminum Cyanide

Practice Name or write the following compounds Ca(MnO4)2 Cobalt (III) Nitrate CsC2H3O2 Calcium Sulfate

Practice Name the following: 6. Ba3(PO4)2 7. ZnCO3 8. (NH4)Cl 9. KMnO4 Write formulas for: 1. Sodium Dichromate 2. Iron (II) sulfate 3. Silver hydroxide 4. Ammonium Phosphate 5. Copper (II) Sulfite Name the following: 6. Ba3(PO4)2 7. ZnCO3 8. (NH4)Cl 9. KMnO4 10. Cu(NO3)2

Practice Naming or writing Compounds Mn(ClO2)7 PbS NH4HSO3 KCN Cd(NO3)2 Lead (IV) perchlorate Beryllium Acetate Copper (II) Bisulfate

Practice Name the following: 1. (NH4)3P 2. Na2CO3 3. Fe(OH)3 4. CuSO4 5. AlCl3

Naming/Writing Hydrates Hydrates are substances that include water in their formula. The water is not actually part of the chemical substance and this is reflected in the way the formula is written. Example: CuSO4 ⋅ 5H2O

Rules 1) The ionic compound (WITHOUT the waters of hydration) is named first by using the rules for naming ionic compounds (e.x., Ba(OH)2•8H2O = "barium hydroxide” 2) Greek Prefixes are attached to the word "hydrate" to indicate the number of water molecules per formula unit for the compound (e.g., Ba(OH)2•8H2O; 8 water molecules = "octahydrate") 3) When the chemical formula for a hydrated ionic compound is written, the formula for the ionic compound is separated from the waters of hydration by a centered "dot".

Practice 2) MgSO4 • 7 H2O 3) CrBr3• 6H2O 4) Pb(ClO3)2 • 3H2O 1) MnBr2• 4 H2O 2) MgSO4 • 7 H2O 3) CrBr3• 6H2O 4) Pb(ClO3)2 • 3H2O

2) Cobalt(II) chloride hexahydrate 3) Mercury(II) nitrate monohydrate Practice 1) Beryllium hydroxide octahydrate 2) Cobalt(II) chloride hexahydrate 3) Mercury(II) nitrate monohydrate 4) Tin(IV) chloride pentahydrate

Naming & Identifying Acids All acids contain hydrogen When acids are dissolved in water, H+ ions are generated Acids that generate a lot of H+ are strong acids Acids that generate only a small amount of H+ are weak acids

Strong Acids HCl is a strong acid because no HCl molecules are in a water solution of HCl. Because of the strong attraction between the water molecules and HCl molecules, every HCl molecule ionizes.

Naming & Identifying Acids Cont. The formula for an acid is: HX Where X = an anion

Naming Binary Acids Naming Acids: 1. Begin with the regular name Example HCl is Hydrogen Chloride 2. If the anion ends is “-ide,” add “hydro” as a prefix 3. Replace “-ide” with “-ic”and add acid Example: HCl Hydrogen chloride becomes hydrochloric acid NOTE: It is only an acid with the ending ends in aqueous. If the compound is either gas, liquid, or solid it is not an acid, it is the normal compound.

Name the following binary acids Answers: 1. Hydrofluoric Acid 2. Hydrobromic Acid 3. Hydroiodic Acid 1. HF 2. HBr 3. HI

Naming Ternary Acids Ternary acids contain polyatomic ions To name acids (with 3 or more different elements): 1. Determine regular name of the compound 2. If the anion end in “-ite,” add “-ous” in place of “-ite” and add acid to the end 3. If the anion ends in “-ate,” add “-ic” in place of “-ate” and add acid to the end

Examples of Naming Ternary Acids 1. H2SO3 Name: Hydrogen Sulfite Name of Acid: Sulfurous Acid 2. HNO3 Name: Hydrogen Nitrate Name of Acid: Nitric Acid Begin 3rd 4-28

Name the following ternary acids 1. H3PO4 2. H2CO3 3. H3PO3

Write formulas for the following acids: 1. Chlorous Acid 2. Acetic Acid