Naming Compounds Day 2 Working backwards name to

Naming Compounds Day 2

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. O • For covalent compounds, simply use the prefixes to tell you the number of each element: • What is the formula for dinitrogen trioxide? N 2 O 3 • Give formulae for: lithium sulfide, dinitrogen monoxide, lead(IV) sulfate

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

Assignment 1. Name each according to the rules: a) Zn. S, b) Fe. Cl 3, c) Ca. CO 3, d) P 2 O 5, e) Na. CN, f) N 2 F 2, g) Mg. HPO 4, h) Cu(Br. O 3)2, i) K 2 O, j) BF 3 2. Give the valence of a) Fe in Fe. O, b) Mn in Mn. O 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

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

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

Answers – 3 a) Na 2 O h) Cl 2 O b) KI i) Ag 2 S c) Pb. S 2 j) Mg 3 N 2 d) Hg 2 O k) Al(Cl. O)3 e) Fe. O l) f) m) Ca. Cr. O 4 Fe 3(PO 4)2 g) Cu. F 2 IF 5 n) P 2 S 5

Naming Acids: Binary acids • 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: 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) hydrogen HBr(s) bromide hydrosulfuric H S(aq) H S(g) 2 acid 2 hydr(o)iodic HI(aq) acid hydrogen sulfide

Naming Acids: Oxyacids • 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 1) sulphite, 2) sulphous, 3) sulphurous, 4) sulphurous acid HNO 2 hypochlorous acid H 3 PO 4(aq) carbonic acid

Naming Acids: Oxyacids • 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 1) sulphite, 2) sulphous, 3) sulphurous, 4) sulphurous acid HNO 2 hypochlorous acid - nitrous acid - HCl. O H 3 PO 4(aq) carbonic acid - phosphoric acid - H 2 CO 3

Assignment: give formula or name 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) HCl. O 2 k) HF(aq) a) HCl. O 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

Hydrates • Some compounds contain H 2 O in their structure. 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. Cu. SO 4 • 5 H 2 O is copper(II) sulfate pentahydrate. • A greek prefix indicates the # of H 2 O groups. Na 2 SO 4 • 10 H 2 O sodium sulfate decahydrate nickel(II) sulfate hexahydrate Ni. SO 4 • 6 H 2 O sodium carbonate monohydrate Na 2 CO 3 • H 2 O Ba. Cl 2 • 2 H 2 O barium chloride dihydrate