1. CHEM 1405: Introductory Chemistry Houston Community College Dr. Laura Jakubowski Chapter 6 – Language of Chemistry Textbook “Introductory Chemistry: Concepts and Critical Thinking” Seventh Edition by Charles H. Corwin © 2014 Pearson Education, Inc.

2. Language of Chemistry By the 1700s, more than 10,000 compounds were discovered How should they be named? In 1787, Antoine Lavoisier developed a systematic method of naming substances, based on what they were composed of 5 compounds shown all contain Mn but have different properties Lavoisier’s method became the basis for our current system of naming 2 © 2014 Pearson Education, Inc.

3. Classification of Compounds In 1940, the International Union of Pure and Applied Chemistry (IUPAC) released a set of comprehensive rules on the nomenclature of inorganic compounds – referred to as IUPAC nomenclature An inorganic compound does not contain carbon (with the exception of CO 2, CS 2, and compounds containing CO 3 2- and HCO 3 - ) Inorganic compounds can be placed into 5 common categories: binary ionic compound, ternary ionic compound, binary molecular compound, binary acid, and ternary oxyacid An aqueous solution is produced when a compound dissolved in water – typically indicated by the symbol (aq) 3 © 2014 Pearson Education, Inc.

4. Classification of Inorganic Compounds 4 © 2014 Pearson Education, Inc. 2 elements: metal, nonmetal 3 elements: metal, nonmetal, other 2 elements: both nonmetals 2 elements (aq): hydrogen, nonmetal 3 elements (aq): hydrogen, nonmetal, oxygen

5. Classifying Compounds and Acids Classify each of the following as a binary ionic compound, ternary ionic compound, binary molecular compound, binary acid, or ternary oxyacid: calcium oxide, CaO silver chromate, Ag 2 CrO 4 carbonic acid, H 2 CO 3 (aq) sulfur dioxide, SO 2 hydrofluoric acid, HF(aq) carbon disulfide, CS 2 magnesium iodide, MgI 2 hydrochloric acid, HCl(aq) lithium dichromate, Li 2 Cr 2 O 7 nitric acid, HNO 3 (aq) 5 © 2014 Pearson Education, Inc.

6. Classifying Compounds and Acids Classify each of the following as a binary ionic compound, ternary ionic compound, binary molecular compound, binary acid, or ternary oxyacid: calcium oxide, CaO binary ionic compound silver chromate, Ag 2 CrO 4 ternary ionic compound carbonic acid, H 2 CO 3 (aq) ternary oxyacid sulfur dioxide, SO 2 binary molecular compound hydrofluoric acid, HF(aq) binary acid carbon disulfide, CS 2 binary molecular compound magnesium iodide, MgI 2 binary ionic compound hydrochloric acid, HCl(aq) binary acid lithium dichromate, Li 2 Cr 2 O 7 ternary ionic compound nitric acid, HNO 3 (aq) ternary oxyacid 6 © 2014 Pearson Education, Inc.

7. Classifying Ions Ions are also named systematically, according to IUPAC nomenclature A positive ion is a cation and a negative ion is an anion A single, charged atom is a monoatomic ion A group of atoms, having an overall charge is called a polyatomic ion 7 © 2014 Pearson Education, Inc.

8. Classifying Cations and Anions Classify each of the following as a monoatomic cation, monoatomic anion, polyatomic cation or polyatomic anion barium ion, Ba 2+ chloride ion, Cl - ammonium ion, NH 4 + carbonate ion, CO 3 2- hydronium ion, H 3 O + sulfide ion, S 2- permanganate ion, MnO 4 - stannous ion, Sn 2+ 8 © 2014 Pearson Education, Inc.

9. Classifying Cations and Anions Classify each of the following as a monoatomic cation, monoatomic anion, polyatomic cation or polyatomic anion barium ion, Ba 2+ monoatomic cation chloride ion, Cl - monoatomic anion ammonium ion, NH 4 + polyatomic cation carbonate ion, CO 3 2- polyatomic anion hydronium ion, H 3 O + polyatomic cation sulfide ion, S 2- monoatomic anion permanganate ion, MnO 4 - polyatomic anion stannous ion, Sn 2+ monoatomic cation 9 © 2014 Pearson Education, Inc.

10. Naming Metal Ions Metal atoms can lose valence electrons and become cations Metal cations are named for the parent metal followed by the word ion Na + is sodium ion; Mg 2+ is magnesium ion; Al 3+ is aluminum ion Main-group metals usually form one type of cation, except Sn and Pb Transition metals often form more than one type of cation Iron can form both Fe 2+ and Fe 3+ To name cations of metals which can have more than one charge, it is necessary to specify the charge IUPAC recommends to name the parent metal, followed by its charge (in Roman numerals), followed by the word ion Fe 2+ is named iron(II) ion and Fe 3+ is named iron(III) ion 10 © 2014 Pearson Education, Inc.

11. Naming Metal Ions This system for naming is also called the Stock system IUPAC also allows, but discourages, the Latin system, where the suffix -ous (for lower charge) or -ic (for higher charge) is added on to the Latin name of the metal 11 © 2014 Pearson Education, Inc. CATION STOCK SYSTEM LATIN SYSTEM Cd + cadmium ion Cu + copper(I) ion cuprous ion Cu 2+ copper(II) ion cupric ion Fe 2+ iron(II) ion ferrous ion Fe 3+ iron(III) ion ferric ion Hg 2 2+ mercury(I) ion* mercurous ion Hg 2+ mercury(II) ion mercuric ion Ag + silver ion Zn 2+ zinc ion

12. Naming Nonmetal Ions Nonmetal atoms can gain valence electrons and become anions In the IUPAC method, nonmetal ions are named by using the nonmetal stem plus the suffix -ide and the word ion Cl - is chloride ion; S 2- is sulfide ion; P 3- is phosphide ion 12 © 2014 Pearson Education, Inc.

13. Predicting Formulas of Monoatomic Ions As discussed in Chapter 5, the charge of an ion can be predicted based on the group number of the element Transition metals are an exception – most lose their two s electrons, but others have additional charges which are unpredictable 13 © 2014 Pearson Education, Inc.

14. Names and Formulas of Monoatomic Ions Provide a formula for the following monoatomic ions barium ion cobalt(II) ion fluoride ion oxide ion iron(III) ion Provide a systematic name for the following monoatomic ions Al 3+ Co 3+ Br - N 3- H + 14 © 2014 Pearson Education, Inc.

15. Names and Formulas of Monoatomic Ions Provide a formula for the following monoatomic ions barium ion Ba 2+ cobalt(II) ion Co 2+ fluoride ion F - oxide ion O 2- iron(III) ion Fe 3+ Provide a systematic name for the following monoatomic ions Al 3+ aluminum ion Co 3+ cobalt(III) ion (or cobaltic ion) Br - bromide ion N 3- nitride ion H + hydrogen ion 15 © 2014 Pearson Education, Inc.

16. Polyatomic Ions Polyatomic anions usually contain one or more elements combined with oxygen – termed an oxyanion Most end in -ate or -ite, depending on O Some end in -ide A common polyatomic cation is NH 4 +, called ammonium ion Flash cards are useful for memorization 16 © 2014 Pearson Education, Inc.

17. Names and Formulas of Polyatomic Ions Provide a systematic name for each of the following: CO 3 2- CrO 4 2- ClO 2 - HSO 4 - OH - Provide the formula for each of the following: acetate ion perchlorate ion dichromate ion hydrogen carbonate ion ammonium ion 17 © 2014 Pearson Education, Inc.

18. Names and Formulas of Polyatomic Ions Provide a systematic name for each of the following: CO 3 2- carbonate ion CrO 4 2- chromate ion ClO 2 - chlorite ion HSO 4 - hydrogen sulfate ion OH - hydroxide ion Provide the formula for each of the following: acetate ion C 2 H 3 O 2 - perchlorate ion ClO 4 - dichromate ion Cr 2 O 7 2- hydrogen carbonate ion HCO 3 - ammonium ion NH 4 + 18 © 2014 Pearson Education, Inc.

19. Writing Chemical Formulas An ionic compound is composed of both positive and negative ions A formula unit is the simplest representative particle of an ionic compound, it is neutral – total + charge must equal total - charge Sodium chloride contains Na + and Cl -, formula is NaCl Calcium chloride contains Ca 2+ and Cl -, formula is CaCl 2 Aluminum chloride contains Al 3+ and Cl -, formula is AlCl 3 The same applies for polyatomic ions Compound with K + and SO 4 2-, formula is K 2 SO 4 Compound with Mg 2+ and SO 4 2-, formula is MgSO 4 Parentheses are needed to indicate multiple number of polyatomic ions Compound with NH 4 + and SO 4 2-, formula is (NH 4 ) 2 SO 4 19 © 2014 Pearson Education, Inc.

20. Writing Chemical Formulas Write the chemical formula for each of the following compounds: copper(I) oxide, Cu + and O 2- cobalt(III) oxide, Co 3+ and O 2- iron(II) sulfide, Fe 2+ and S 2- mercury(I) fluoride, Hg 2 2+ and F - lead(IV) oxide, Pb 4+ and O 2- calcium carbonate, Ca 2+ and CO 3 2- calcium hydroxide, Ca 2+ and OH - calcium phosphate, Ca 2+ and PO 4 3- copper(II) permanganate, Cu 2+ and MnO 4 - iron(III) carbonate, Fe 3+ and CO 3 2- potassium dichromate, K + and Cr 2 O 7 2- 20 © 2014 Pearson Education, Inc.

21. Writing Chemical Formulas Write the chemical formula for each of the following compounds: copper(I) oxide, Cu + and O 2- Cu 2 O cobalt(III) oxide, Co 3+ and O 2- Co 2 O 3 iron(II) sulfide, Fe 2+ and S 2- FeS mercury(I) fluoride, Hg 2 2+ and F - Hg 2 F 2 lead(IV) oxide, Pb 4+ and O 2- PbO 2 calcium carbonate, Ca 2+ and CO 3 2- CaCO 3 calcium hydroxide, Ca 2+ and OH - Ca(OH) 2 calcium phosphate, Ca 2+ and PO 4 3- Ca 3 (PO 4 ) 2 copper(II) permanganate, Cu 2+ and MnO 4 - Cu(MnO 4 ) 2 iron(III) carbonate, Fe 3+ and CO 3 2- Fe 2 (CO 3 ) 3 potassium dichromate, K + and Cr 2 O 7 2- K 2 Cr 2 O 7 21 © 2014 Pearson Education, Inc.

22. Binary Ionic Compounds Overall, an ionic compound has a charge of zero, even though it contains charged ions To name ionic compounds correctly, the charge must first be determined For example, what is charge of Fe in Fe 2 O 3 ? Oxide ion is always O 2- : therefore, 3 × (-2) = -6 Total charge from Fe should be +6: 2 × (c) = +6  c = +3 (Fe 3+ ) Metal cation is named first, and then monoatomic anion with -ide suffix Fe 2 O 3 is named iron(III) oxide Remember that formulas of compounds can be predicted based on the formula of a similar compound in the same periodic group (LiCl, NaCl, KCl); (BaCl 2, MgCl 2, CaCl 2, SrCl 2 ) 22 © 2014 Pearson Education, Inc.

23. Binary Ionic Compounds Determine the charge for each transition metal: Cu 3 P CoN Name the following compounds: ZnO SnF 2 Mn 3 P 2 Fe 2 S 3 Provide the formula for the following: lithium fluoride mercury(II) oxide Given that aluminum oxide is Al 2 O 3, write formulas for: gallium oxide aluminum sulfide 23 © 2014 Pearson Education, Inc. Fe 2 S pyrite or “fool’s gold”

24. Binary Ionic Compounds Determine the charge for each transition metal: Cu 3 P Cu + CoN Co 3+ Name the following compounds: ZnO zinc oxide SnF 2 tin(II) fluoride Mn 3 P 2 manganese(II) phosphide Fe 2 S 3 iron(III) sulfide Provide the formula for the following: lithium fluoride LiF mercury(II) oxide HgO Given that aluminum oxide is Al 2 O 3, write formulas for: gallium oxide Ga 2 O 3 aluminum sulfide Al 2 S 3 24 © 2014 Pearson Education, Inc. Fe 2 S pyrite or “fool’s gold”

25. Ternary Ionic Compounds Name ternary ionic compounds similarly to binary ionic compounds, but suffix on anion usually ends with -ate or -ite First, determine the charge of each ion For example, what is charge of Fe in Fe 3 (PO 4 ) 2 ? Phosphate ion is PO 4 3- : 2 × (-3) = -6 Total charge from Fe should be +6: 3 × (c) = +6  c = +2 (Fe 2+ ) Metal cation is named first, followed by name of anion (memorize) Fe 3 (PO 4 ) 2 is named iron(II) phosphate Remember that formulas of compounds can be predicted based on the formula of a similar compound in the same periodic group (LiNO 3, NaNO 3, KNO 3 ); (Ba 3 (PO 4 ) 2, Mg 3 (PO 4 ) 2, Ca 3 (PO 4 ) 2, Sr 3 (PO 4 ) 2 ) 25 © 2014 Pearson Education, Inc.

26. Ternary Ionic Compounds 26 © 2014 Pearson Education, Inc. Determine the charge for each transition metal: Hg(OH) 2 Co(ClO 3 ) 3 Name the following compounds: KMnO 4 Hg(NO 3 ) 2 BaCrO 4 Cu(NO 2 ) 2 Provide the formula for the following: nickel(II) acetate mercury(I) nitrite Calcium carbonate is CaCO 3, write formulas for: radium carbonate calcium silicate KMnO 4 multiple uses

27. Ternary Ionic Compounds 27 © 2014 Pearson Education, Inc. Determine the charge for each transition metal: Hg(OH) 2 Hg 2+ Co(ClO 3 ) 3 Co 3+ Name the following compounds: KMnO 4 potassium permanganate Hg(NO 3 ) 2 mercury(II) nitrate BaCrO 4 barium chromate Cu(NO 2 ) 2 copper(II) nitrite Provide the formula for the following: nickel(II) acetate Ni(C 2 H 3 O 2 ) 2 mercury(I) nitrite Hg 2 (NO 2 ) 2 Calcium carbonate is CaCO 3, write formulas for: radium carbonate Ra 2 CO 3 calcium silicate Ca 2 SiO 3 KMnO 4 multiple uses

28. Binary Molecular Compounds The simplest representative particle in a binary molecular compound is a molecule – generally, the more metallic element is written second in the chemical formula: C, P, N, H, S, I, Br, Cl, O, F (CH 4, NH 3, HBr) Name the first element, followed by the second with -ide suffix The number of atoms of each element should be indicated using the following Greek prefixes, mono- used only when necessary, CO carbon monoxide 28 © 2014 Pearson Education, Inc.

29. Binary Molecular Compounds Name the following compounds: IF 6 Br 3 O 8 Cl 2 O 5 P 4 S 10 PH 3 Provide a formula for each of the following: tetraphosphorus trisulfide tetraiodine nonaoxide diphosphorus tetraiodide sulfur hexafluoride dihydrogen oxide 29 © 2014 Pearson Education, Inc. www.redorbit.com SO 2 used as preservative

30. Binary Molecular Compounds Name the following compounds: IF 6 iodine hexafluoride Br 3 O 8 tribromine octaoxide Cl 2 O 5 dichlorine pentaoxide P 4 S 10 tetraphosphorus decasulfide PH 3 phosphorus trihydride Provide a formula for each of the following: tetraphosphorus trisulfide P 4 S 3 tetraiodine nonaoxide I 4 O 9 diphosphorus tetraiodide P 2 I 4 sulfur hexafluoride SF 6 dihydrogen oxide H 2 O 30 © 2014 Pearson Education, Inc. www.redorbit.com SO 2 used as preservative

31. Binary Acids A binary acid is always an aqueous solution of a compound containing hydrogen and a nonmetal Chemical formula always begins with H, followed by the nonmetal, and the symbol (aq) For naming, the prefix hydro- is used before the nonmetal stem and the suffix -ic acid For example, HCl (aq) is hydrochloric acid NOTE – HCl in gas form, HCl (g) is named hydrogen chloride Name or give the formula for the following: hydrofluoric acid H 2 S (aq) 31 © 2014 Pearson Education, Inc.

32. Binary Acids A binary acid is always an aqueous solution of a compound containing hydrogen and a nonmetal Chemical formula always begins with H, followed by the nonmetal, and the symbol (aq) For naming, the prefix hydro- is used before the nonmetal stem and the suffix -ic acid For example, HCl (aq) is hydrochloric acid NOTE – HCl in gas form, HCl (g) is named hydrogen chloride Name or give the formula for the following: hydrofluoric acid HF H 2 S (aq) hydrosulfuric acid 32 © 2014 Pearson Education, Inc.

33. Ternary Oxyacids A ternary oxyacid is an aqueous solution of a compound containing hydrogen and an oxyanion Most ternary oxyacids are named by attaching the suffix -ic acid to the nonmetal stem of the oxyanion – HNO 3 (aq) is nitric acid Some ternary oxyacids are named by attaching the suffix -ous acid to the nonmetal stem of the oxyanion – HNO 2 (aq) is nitrous acid -ic acid corresponds to anion ending in -ate; and -ous acid to -ite 33 © 2014 Pearson Education, Inc. HClO 4 Perchloric acid NaClO 4 sodium perchlorate TERNARY OXYACID TERNARY COMPOUND HClO Hypochlorous acid NaClO sodium hypochlorite HClO 2 Chlorous acid NaClO 2 sodium chlorite HClO 3 Chloric acid NaClO 3 sodium chlorate

34. Ternary Oxyacids Name the following compounds: H 3 PO 4 (aq) HClO (aq) HMnO 4 (aq) H 2 SO 3 (aq) H 2 CO 3 (aq) Provide a formula for each of the following: phosphorous acid chromic acid sulfuric acid acetic acid perchloric acid 34 © 2014 Pearson Education, Inc. en.wikipedia.org HClO 4 used to make rocket fuel

35. Ternary Oxyacids Name the following compounds: H 3 PO 4 (aq) phosphoric acid HClO (aq) hypochlorous acid HMnO 4 (aq) permanganic acid H 2 SO 3 (aq) sulfurous acid H 2 CO 3 (aq) carbonic acid Provide a formula for each of the following: phosphorous acid H 3 PO 3 (aq) chromic acid H 2 CrO 4 (aq) sulfuric acid H 2 SO 4 (aq) acetic acid HC 2 H 3 O 2 (aq) perchloric acid HClO 4 (aq) 35 © 2014 Pearson Education, Inc. en.wikipedia.org HClO 4 used to make rocket fuel

36. Summary 36 © 2014 Pearson Education, Inc. Generally, inorganic compounds do not contain carbon and are named according to IUPAC nomenclature, five subcategories are binary ionic, ternary ionic, binary molecular, binary acid, ternary oxyacid; a substance dissolved in water is called an aqueous solution; ionic compounds are composed of positive cations and negative anions; a monoatomic ion is a single atom having a charge, and a polyatomic ion is a group of atoms bearing a charge The ionic charge on a metal is typically named using the Stock system, but the Latin system is still used as well; nonmetal monoatomic anions end in -ide Oxyanions contain one or more elements combined with oxygen; most end with -ate, some end with -ite

37. Summary 37 © 2014 Pearson Education, Inc. The simplest representative particle in an ionic compound is called a formula unit, the net charge for a formula unit is zero Binary ionic compounds have names ending in -ide Ternary ionic compounds generally end in -ate or -ite, with some exceptions The simplest representative particle in a binary molecular compound is called a molecule; they are named using appropriate Greek prefix before each elelement and the suffix -ide on last element A binary acid is an aqueous solution of a hydrogen containing compound, they are named as hydro + nonmetal stem + -ic acid

38. Summary 38 © 2014 Pearson Education, Inc. Ternary oxyacids are usually named nonmetal stem + -ic acid, but a few ternary oxyacids are named nonmetal stem + -ous acid, there are other exceptions as well Key terms: inorganic compound, IUPAC nomenclature, binary ionic compound, ternary ionic compound, binary molecular compound, binary acid, ternary oxyacid, aqueous solution, cation, anion, monoatomic ion, polyatomic ion, Stock system, Latin system, oxyanion, formula unit, molecule