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NOMENCLATURE

NOMENCLATURE. Chapter 5. Charges on Common Ions. -4. -3. -2. -1. +1. +2. +3. Table 5.1: Common Simple Cations and Anions. Chemical Bonds. - the forces that hold two or more atoms together to form a compound. - the two types of chemical bonds are: 1. Ionic bonds. NaCl KI

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NOMENCLATURE

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  1. NOMENCLATURE Chapter 5

  2. Charges on Common Ions -4 -3 -2 -1 +1 +2 +3

  3. Table 5.1: Common Simple Cations and Anions

  4. Chemical Bonds • - the forces that hold two or more atoms together to form a compound. • - the two types of chemical bonds are: • 1. Ionic bonds. • NaCl KI • 2. Covalent bonds. • H2O CH4 metal & nonmetal two nonmetals

  5. Chemical Bonds(continued) • Ionic Bonding: Force of attraction between oppositely charged ions. • - Chemical compounds must have a net charge of zero. • 1. Both cations and anions must be present. • 2. The number of cations and anions must be such that the net charge is zero.

  6. Writing Formulas for Ionic Compounds Charge must equal zero for each compound. 1+ & 1- = 0 2+ & 2- = 0 6+ & 6- = 0

  7. COMPOUNDS FORMED FROM IONS • CATION + ANION ---> • COMPOUND • Na+ + Cl- --> NaCl • A neutral compound requires equal number of (+) and (-) charges.

  8. Chemical Bonds(continued) • Covalent bonding:results from atoms sharing electrons. • Molecule: a collection of covalently-bonded atoms. • H2O C12H22O11

  9. Common Names • sugar of lead • blue vitriol • quicklime • Epsom salts • milk of magnesia • gypsum • laughing gas lead(II) acetate copper(II) sulfate calcium oxide magnesium sulfate magnesium hydroxide calcium sulfate dinitrogen monoxide

  10. Common Names - Exceptions • H2O = water, steam, ice • NH3 = ammonia • CH4 = methane • NaCl = table salt • C12H22O11 = table sugar

  11. Type I Cations: only one charge Group I ions Group II ions Aluminum Cadmium Silver Zinc Memorize Table 5.1, page 129 Type II Cations: more than one charge transition elements elements under the stairstep Memorize Table 5.2, page 133 Types of Cations

  12. Metal Cations • Type I • Metals that can only have one possible charge • Determine charge by position on the Periodic Table • Type II • Metals that can have more than one possible charge • Determine metal cation’s charge from the charge on anion

  13. Naming Compounds Binary Ionic Compounds: • 1. Cation first, then anion • 2. Monatomic cation = name of the element • Ca2+ = calciumion • 3. Monatomic anion = root + -ide • Cl = chloride • CaCl2 = calcium chloride

  14. Naming Compounds(continued) • - metal forms more than one cation • - use Roman numeral in name • CuCl2 Cu2+is cation • CuCl2 = Copper (II) chloride • Cupric chloride Binary Ionic Compounds (Type II):

  15. Naming Compounds(continued) • - Compounds between two nonmetals • -First element in the formula is named first. • -Second element is named as if it were an anion. • - Use prefixes (Table 5.3 on page 137). • - Never use mono- for the first element. • P2O5 = diphosphorus pentoxide Binary compounds (Type III):

  16. Subscript Prefix 1 mono- (not used on first nonmetal) 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- Prefixes • Drop last “a” in the prefix if the name begins with vowel

  17. Figure 5.1: A flow chart for naming binary compounds.

  18. Compounds: SO3 --Sulfur trioxide NO2 -- Nitrogen dioxide NO3 -- Nitrogen trioxide NH3 -- Ammonia Polyatomic ions: SO32- -- Sulfite ion NO21- -- Nitrite ion NO31- -- Nitrate ion NH41+ --Ammonium ion Common Nomenclature Mistakes

  19. MOLECULAR FORMULAS • Formula for glycine is C2H5NO2 • In one molecule there are • 2 C atoms • 5 H atoms • 1 N atom • 2 O atoms

  20. Molecular Modeling Drawing of glycine Ball & stick Space-filling

  21. POLYATOMIC IONS • Groups of atoms with a charge. • MEMORIZEthe names and formulas in Table 5.4, page 142.

  22. Table 5.4: Names of Common Polyatomic Ions

  23. Patterns for Polyatomic Ions • -ate ion • chlorate = ClO3- • -ate ion plus 1 O  same charge, per- prefix • perchlorate = ClO4- • -ate ion minus 1 O  same charge, -ite suffix • chlorite = ClO2- • -ate ion minus 2 O  same charge, hypo- prefix, -ite suffix • hypochlorite = ClO-

  24. Some Common Polyatomic Ions • NH4+ ammonium ion One of the few common polyatomic cations

  25. Some Common Polyatomic Ions • CO32- carbonate ion • HCO3- bicarbonate ion • - hydrogen carbonate ion

  26. Some Common Polyatomic Ions • SO42- sulfate ion • SO32- sulfite ion

  27. Some Common Polyatomic Ions • NO3- nitrate ion • NO2- nitrite ion

  28. Figure 5.2: Overall strategy for naming chemical compounds

  29. NOMENCLATURE OF COMPOUNDS Binary -- 2 elements Ternary -- (3 elements) - Ionic (metal ion + polyatomic ion) Type I - Ionic (Type I metal + nonmetal) Group I, II, Al+3, Ag1+, Cd2+, & Zn2+ NaCl -- Sodium Chloride Ca3(PO4)2 -- calcium phosphate FeSO4 -- iron (II) sulfate -- ferrous sulfate Type II - Ionic (Type II metal + nonmetal) All other metals Fe2S3 -- iron (III) sulfide -- ferric sulfide Type III - covalent (2 nonmetals) CO2 -- carbon dioxide

  30. Binary Acids • made up of two elements -- hydrogen and a nonmetal • named by using: • prefix hydro + root of nonmetal + ic + acid • HCl -- hydrochloric acid • H2Se -- hydroselenic acid

  31. Table 5.5: Names of Acids that Do Not Contain Oxygen

  32. Ternary Acids (oxyacids) • contain three elements -- hydrogen, nonmetal, and oxygen. • most oxygen per + root of nonmetal + ic + acid • less oxygen root of nonmetal + ic + acid • less oxygen root of nonmetal + ous + acid • least oxygen hypo + root of nonmetal + ous + acid

  33. Ternary Acids(continued) • HBrO4 perbromic acid • HBrO3 bromic acid • HBrO2 bromous acid • HBrOhypobromous acid • H3PO4 phosphoric acid • H3PO3 phosphorous acid • H3PO2 hypophosphorus acid

  34. Figure 5.3: A flow chart for naming acids

  35. Salt Nomenclature (continued) • Ternary salts ( metal and polyatomic ion) • name of positive ion + root of nonmetal + ate or ite • If the salt comes from anic acid, changeic toate. • H2CO3carbonicacid Na2CO3 sodiumcarbonate • H3PO4phosphoricacid K3PO4potassiumphosphate • If the salt comes from anousacid, changeoustoite. • H2SO3sulfurousacid Li2SO3 lithiumsulfite • HClOhypochlorousacid NaClO sodiumhypochlorite

  36. Chemical Nomenclature • Name each of the following: • CuCl • HgO • Fe2O3 • MnO2 • PbCl2 • CrCl3 copper(I) chloride cuprous chloride mercury(II) oxide mercuric oxide iron(III) oxide ferric oxide manganese(IV) oxide manganic oxide lead(II) chloride plumbous chloride chromium(III) chloride chromic chloride

  37. Chemical Nomenclature • Name each of the following: • P4O10 • N2O5 • Li2O2 • Ti(NO3)4 • SO3 • SF6 • O2F2 tetraphosphorus decoxide dinitrogen pentoxide lithium peroxide titanium(IV) nitrate sulfur trioxide sulfur hexafluoride dioxygen difluoride

  38. Writing the Formulas from the Names • For Type III compounds, use the prefixes to determine the subscripts • For Type I, Type II, polyatomic Compounds and Acids • Determine the ions present • Determine the charges on the cation and anion • Balance the charges to get the subscripts

  39. Determining the Charge on a Cation – Au2S3 Determine the charge on the anion Au2S3 - the anion is S, since it is in Group 6A, its charge is -2 Determine the total negative charge since there are 3 S in the formula, the total negative charge is -6 Determine the total positive charge since the total negative charge is -6, the total positive charge is +6 Divide by the number of cations since there are 2 Au in the formula & the total positive charge is +6, each Au has a +3 charge

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