2. Naming Compounds Day 2

3. Working backwards: name to formula It’s possible to determine a formula from a name E.g. What is the formula of sodium oxide? To get the answer, first write the valences: Na 1 O 2  Na 2 O What is the formula of copper(II) oxide? Cu 2 O 2  Cu 2 O 2  CuO For covalent compounds, simply use the prefixes to tell you the number of each element: What is the formula for dinitrogen trioxide? N2O3N2O3 Give formulae for: lithium sulfide, dinitrogen monoxide, lead(IV) sulfate

4. Write and name the following covalent compounds Li 1 S 2  Li 2 S N2ON2O Pb 4 (SO 4 ) 2  Pb 2 (SO 4 ) 4  Pb(SO 4 ) 2 lithium sulfide dinitrogen monoxide lead(IV) sulfate

5. 1.Name each according to the rules: a) ZnS, b) FeCl 3, c) CaCO 3, d) P 2 O 5, e) NaCN, f) N 2 F 2, g) MgHPO 4, h) Cu(BrO 3 ) 2, i) K 2 O, j) BF 3 2.Give the valence of a) Fe in FeO, b) Mn in MnO 2 3. Write formulas for: a) sodium oxide, b) potassium iodide, c) plumbic sulfide, d) mercury(I) oxide, e) ferrous oxide, f) iron(II) phosphate, g) copper(II) fluoride, h) dichlorine monoxide, i) silver sulfide, j) magnesium nitride, k) aluminum hypochlorite, l) iodine pentafluoride, m) calcium chromate, n) diphosphorus pentasulfide Assignment

6. Complete exercises on handout Steps: 1.Determine if its ionic or covalent 2.If ionic, determine if its metal has one or more valence 3.Name according to appropriate rules

7. Answers – 1, 2 a)zinc sulfide b)iron(III) chloride c)calcium carbonate d)diphosporus pentoxide e)sodium cyanide f)dinitrogen difluoride g)magnesium hydrogen phosphate h)copper(II) bromate i)potassium oxide j)boron trifluoride 2 a) 2b) 4

8. Answers – 3 a)Na 2 O b)KI c)PbS 2 d)Hg 2 O e)FeO f)Fe 3 (PO 4 ) 2 g)CuF 2 h)Cl 2 O i)Ag 2 S j)Mg 3 N 2 k)Al(ClO) 3 l)IF 5 m)CaCrO 4 n)P 2 S 5

9. All acids start with H (e.g. HCl, H 2 SO 4 ) 2 acids types exist: binary acids and oxyacids Binary: H + non-metal. E.g. HCl Oxy: H + polyatomic ion. E.g. H 2 SO 4 Each have different naming rules. Naming Acids: Binary acids

10. Binary acids: naming depends on state of acid If it’s not aqueous: hydrogen + non-metal HCl(g) = hydrogen chloride If it is aqueous: hydro + non-metal + ic acid HCl(aq) = hydrochloric acid (aqueous hydrogen chloride) Naming Acids: Binary acids HBr(s) HI(aq) H 2 S(aq) H 2 S(g) hydrogen bromide hydr(o)iodic acid hydrogen sulfide hydrosulfuric acid

11. Naming does not depend on the state (aq) 1) name the polyatomic ion 2) replace ate with ic, ite with ous 3) change non-metal root for pronunciation 4) add “acid” to the name E.g. H 2 SO 3 Naming Acids: Oxyacids HNO 2 hypochlorous acid H 3 PO 4 (aq) carbonic acid 1) sulphite,2) sulphous, 3) sulphurous,4) sulphurous acid

12. Naming does not depend on the state (aq) 1) name the polyatomic ion 2) replace ate with ic, ite with ous 3) change non-metal root for pronunciation 4) add “acid” to the name E.g. H 2 SO 3 Naming Acids: Oxyacids HNO 2 hypochlorous acid H 3 PO 4 (aq) carbonic acid 1) sulphite,2) sulphous, 3) sulphurous,4) sulphurous acid - nitrous acid- HClO - phosphoric acid- H 2 CO 3

13. a) chloric acid b) hydrosulfuric acid c) hydrobromic acid d) phosphorous acid e) iodic acid f) HCl(g) g) HCl(aq) h) H 2 SO 4 (s) i) H 2 SO 4 (aq) j) HClO 2 k) HF(aq) Assignment: give formula or name a) HClO 3 b) H 2 S(aq) c) HBr(aq) d) H 3 PO 3 e) HIO 3 f) hydrogen chloride g) hydrochloric acid h) sulfuric acid i) sulfuric acid j) chlorous acid k) hydrofluoric 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