2.  Type III  two nonmetals but no polyatomic ions  Name the elements as you see them in the formula  The last element has –ide for an ending  Each element has a prefix referring to the number of ATOMS (not electrons) 1 = mono6 = hexa 2 = di7 = hepta 3 = tri8 = octa 4 = tetra9 = nona 5 = penta10 = deca O N Y OUR P ERIODIC T ABLE

3.  Type III  If the first element is mono, drop it from the name (all other monos are kept) Monocarbon monoxide  Carbon monoxide  When “ao” or “oo” are created when combining a prefix with element name, drop the first vowel Monooxide  Monoxide Decaoxide  Decoxide Trioxide  Trioxide

4.  Examples  CCl 4 Carbon tetrachloride P2O3P2O3 Diphosporus trioxide  IF 7 Iodine heptafluoride

5.  Now try going from the name to the chemical formula  Dinitrogen trioxide N2O3N2O3  Dichlorine octoxide Cl 2 O 8  Carbon tetrabromide CBr 4  Dihydrogen monoxide H2OH2O

7.  Acid  A compound that produces hydrogen ions (H + ) when dissolved in water  An ionic compound Cation = H + Anion = monatomic or polyatomic ions Only ionic compounds with two nonmetals

8.  Naming Acids  Monatomic (single atoms) anions Acid name begins with hydro- Add –ic to the name of the element Add acid to the end HCl  Hydrochloric acid H 2 S  Hydrosulfuric acid

9.  Naming Acids  Polyatomic anions If it ends in –ite Change end to –ous Add acid to the end  H 2 SO 3  Sulfurous acid If it ends in –ate Change end to –ic Add acid to the end  HNO 3  Nitric acid

10.  Examples  HF Hydrofluoric acid  H 2 SO 4 Sulfuric acid  HClO 2 Chlorous acid

11.  Now try going from the name to the chemical formula  Phosphorous acid H 3 PO 3  Hydrobromic acid HBr  Chloric acid HClO 3