introductory chemistry a foundation fourth edition by ：介绍化学基础，第四版

1,NomenclatureChapter 5,2,Common Names - Exceptions,H2O = water, steam, iceNH3 = ammoniaCH4 = methaneNaCl = table saltC12H22O11 = table sugar,3,Naming Starts with Classifying Compounds,Binary Compounds = only 2 elementsCompounds containing polyatomic ionsAcids = formula often starts with H,4,Classifying Binary Compounds,Compounds containing a metal and a nonmetal are binary ionicType I and IICompounds containing two nonmetalsType IIICompounds containing H and a nonmetal = Acids,5,Binary Ionic,Made of metal cation and nonmetal anionName by naming the ions,6,Metal Cations,Type I Metals that can only have one possible chargeDetermine charge by position on the Periodic TableType IIMetals that can have more than one possible chargeDetermine metal cations charge from the charge on anion,7,Type I Binary Ionic Compounds,Contain Metal Cation + Nonmetal AnionMetal listed first in formula & nameName metal cation first, name nonmetal anion secondSimple metal cation name is the metal namesimple metals are Groups 1A, 2A and Al, Ga & In Nonmetal anion named by changing the ending on the nonmetal name to -ide,8,9,Type II Binary Ionic Compounds,Contain Metal Cation + Nonmetal AnionMetal listed first in formula & nameName metal cation first, name nonmetal anion secondMetal cation name is the metal name followed by a Roman Numeral in parentheses to indicate its chargeDetermine charge from anion chargeCommon Type II cations in Table 5.2Nonmetal anion named by changing the ending on the nonmetal name to -ide,10,11,Determining the Charge on a Cation Au2S3,Determine the charge on the anionAu2S3 - the anion is S, since it is in Group 6A, its charge is -2Determine the total negative chargesince there are 3 S in the formula, the total negative charge is -6Determine the total positive chargesince the total negative charge is -6, the total positive charge is +6Divide by the number of cationssince there are 2 Au in the formula & the total positive charge is +6, each Au has a +3 charge,12,Type III - Binary Compounds of 2 Nonmetals,Name first element in formula first, use the full name of the elementName the second element in the formula as if it were an anionHowever, remember these compounds do not contain ions!Use a prefix in front of each name to indicate the number of atomsNever use the prefix mono- on the first element,13,Prefixes,Drop last “a” in the prefix if the name begins with vowel,14,Compounds Containing Polyatomic Ions,Polyatomic ions are charged entities that contain more than one atomMust memorize name, formula and chargeLook for Patterns!Polyatomic compounds contain one or more polyatomic ionsName polyatomic compounds by naming cation and anionNon-polyatomic ions named like Type I and IIPolyatomic Acids contain H+ and a polyatomic anion,15,Patterns for Polyatomic Ions,Elements in the same column on the Periodic Table form similar polyatomic ionssame number of Os and same chargeClO3- = chlorate BrO3- = bromateIf the polyatomic ion starts with H, add hydrogen- before the ions name and add 1 to the chargeCO32- = carbonate HCO3- = hydrogen carbonate,16,Patterns for Polyatomic Ions,-ate ionchlorate = ClO3-ate ion plus 1 O same charge, per- prefixperchlorate = ClO4-ate ion minus 1 O same charge, -ite suffixchlorite = ClO2-ate ion minus 2 O same charge, hypo- prefix, -ite suffixhypochlorite = ClO-,17,18,Acids,Contain H+ cation and anionBinary acids have H+ cation and a nonmetal anionOxyacids have H+ cation and a polyatomic anion,19,20,21,Writing the Formulas from the Names,For Type III compounds, use the prefixes to de