1. Naming Polyatomics, Acids, and Bases

2. Naming Polyatomics The most common form of a polyatomic ion containing oxygen ends in –ate. Changing the number of oxygen atoms will be reflected with prefixes and suffixes.

3. CO 3 -2 No change Carbonate CO 4 -2 Add “per” as a prefix Percarbonate CO 2 -2 Change the ending to `-ite` Carbonite CO -2 Change the ending to `-ite`and add `hypo`as a prefix Hypocarbonite Gain 1 O atom Lose 1 O atom Lose 2 O atoms * Note: The charge never changes!!

4. Name the following polyatomics 1.SO 4 -2 2.SO 3 -2 3.SO 2 -2 4.SO 5 -2 5.NO 2 - 6.NO 4 - 7.IO 3 -

5. Write the formula for the following polyatomics 1.Phosphate 2.Hypophosphite 3.Bromate 4.Bromite 5.Hypoiodite 6.Carbonite

6. Naming Acids Binary Acids: Contain “H” and one other element Depends on the state of the acid To Name aqueous: (prefix) hydro- “nonmetal name” (suffix) –ic acid HCl (aq) hydrochloric acid H 2 S (aq) hydrosulfuric acid To Name non-aqueous (solid or gas): Hydrogen “nonmetal” – change the ending to -ide HCl (g) hydrogen chloride H 2 S (g) hydrogen sulfide

7. HBr(s) HI(aq) H 2 S(aq) H 2 S(g) hydrogen bromide hydr(o)iodic acid hydrogen sulfide hydrosulfuric acid

8. Naming Oxyacids Contain “H”, “O” and one more element Naming does not depend on the state (aq) Steps 1) name the polyatomic ion 2) replace -ate with ic, -ite with ous 3) change non-metal root for easier pronunciation 4) add “acid” to the name E.g. H 2 SO 3 1) sulphite, 2) sulphous, 3) sulphurous, 4) sulphurous acid

9. HNO 3 HNO 2 H 3 PO 4 H 3 PO 3 H 2 SO 4 H 2 SO 3 HClO 4 HClO 3 HClO 2 HClO nitric acid nitrous acid phosphoric acid phosphorous acid sulfuric acid sulfurous acid perchloric acid chloric acid chlorous acid hypochlorous acid

10. Bases Recall: All bases contain a hydroxide ion (OH - ). Bases are made of OH - bonded to a metal

11. How to name bases. Metal name + hydroxide Examples: 1.Ca(OH) 2 – calcium hydroxide 2.NaOH – sodium hydroxide 3.Fe(OH) 3 – iron (III) hydroxide

12. Practicing Naming Acids FormulaBinary or Oxyacid Name HCl (aq) HI (aq) HNO 3 H 2 SO 4 H 3 PO 4 H 2 CO 3

13. Practicing Naming Acids & Bases FormulaBinary or Oxyacid Name HClBHydrochloric Acid HIBHydroiodic Acid HNO 3 ONitric Acid H 2 SO 4 OSulfuric Acid H 3 PO 4 OPhosphoric Acid H 2 CO 3 OCarbonic Acid

14. Some compounds contain H 2 O in their struc-ture. These compounds are called hydrates. This is different from (aq) because the H 2 O is part of the molecule (not just surrounding it). The H 2 O can usually be removed if heated. A dot separates water: e.g. CuSO 4 5H 2 O is copper(II) sulfate pentahydrate. A greek prefix indicates the # of H 2 O groups. Hydrates sodium sulfate decahydrate nickel(II) sulfate hexahydrate Na 2 CO 3 H 2 O BaCl 2 2H 2 O Na 2 SO 4 10H 2 O NiSO 4 6H 2 O sodium carbonate monohydrate barium chloride dihydrate

15. Naming Gases Noble Gases (monoatomic) Example: He – helium gas Argon gas - Ar Diatomic gases (two atoms) I 2 – iodine gas Br 2 – bromine gas Cl 2 – chlorine gas F 2 - – fluorine gas O 2 – oxygen gas N 2 – nitrogen gas H 2 – hydrogen gas I Bring Clay For Our New House