2. Chapter 5 Molecules and Compounds 2006, Prentice Hall Sucrose molecule (sugar), contains C, H, and O atoms. However, the properties of sucrose are very different from those of C, H, and O alone. The properties of a compound are, in general, different from the properties of the elements that compose it. molecular formula C 12 H 22 O 11

3. 2 CHAPTER OUTLINE  Definitions of Molecules and Compounds  Law of Constant Composition  Types of Compounds  Binary Ionic Compounds (Type I and Type II)  Polyatomic Ions  Binary Molecular Compounds  Naming Acids and Oxyacids  Formula Mass

4. molecule - consist of at least two different atoms in a definite arrangement held together by very strong chemical bonds. compound is a substance consisting of two or more elements in fixed and definite proportions Definition of Molecule and Compound

5. Molecules and Compounds Salt –Sodium – shiny, reactive, poisonous –Chlorine – pale yellow gas, reactive, poisonous –Sodium chloride – table salt Sugar –Carbon – pencil or diamonds –Hydrogen – flammable gas –Oxygen – a gas in air –Combine to form white crystalline sugar

6. Law of Constant Composition all pure substances have constant composition –all samples of a pure substance contain the same elements in the same percentages (ratios) –mixtures have variable composition H 2 O molecules always a 2 H to 1 O ratio H 2 & O 2 mixture; we could vary the amount of either element

7. 6 LAW OF DEFINITE COMPOSITION  In a pure compound, the elements are always present in the same definite proportion by mass. Mass of sample Mass of NMass of H Sample 11.840 g1.513 g0.327 g Sample 22.000 g1.644 g0.356 g % N in Sample 1 = % N in Sample 2 =  Based on this law, the mass of an element can be determined from its mass percent in a compound.

8. 7 Barium iodide, BaI 2, contains 35.1% barium by mass. How many grams of barium does an 8.50 g sample of barium iodide contain? Example 1: 35.1 100 2.98 3 significant figures

9. 8 When 12.66 g of calcium are heated in air, 17.73 g of calcium oxide is formed. What is the percent of oxygen in this compound? Example 2: 3 significant figures Mass of oxygen =17.73 g – 12.66 g = 5.07 g Percent oxygen =

10. Formulas Describe Compounds a compound is a distinct substance that is composed of atoms of two or more elements a compound can be described by the number and type of each atom in the simplest unit of the compound –molecules or ions each element is represented by its letter symbol the number of atoms of each element is written to the right of the element as a subscript

11. Formulas Describe Compounds water = H 2 O  two atoms of hydrogen and 1 atom of oxygen table sugar = C 12 H 22 O 11  12 atoms of C, 22 atoms of H and 11 atoms O

12. Tro's Introductory Chemistry, Chapter 5 11 Order of Elements in a Formula metals written first –NaCl nonmetals written in order from Table 5.1 –CO 2 –there are occasional exceptions for historical or informational reasons H 2 O fits rule, but does NaOH? Table 5.1 Order of Listing Nonmetals in Chemical Formulas CPNHSIBrClOF

13. Types of Chemical Formulas An empirical formula gives the relative number of atoms of each element in a compound. A molecular formula gives the actual number of atoms of each element in a molecule of the compound. For example, the molecular formula for hydrogen peroxide is H 2 O 2, and its empirical formula is HO. The molecular formula is always a whole number multiple of the empirical formula. For many compounds, such as H 2 O, the molecular formula is the same as the empirical formula. A structural formula uses lines to represent chemical bonds and shows how the atoms in a molecule are connected to each other.

14. Comparison of Formulas and Models for Methane, CH 4 The molecular formula of methane indicates that methane has 1 carbon atom and 4 hydrogen atoms. The structural formula shows how the atoms are connected: each hydrogen atom is bonded to the central carbon atom. The ball-and-stick model and the space-filling model illustrate the geometry of the molecule: how the atoms are arranged in three dimensions.

15. Tro's Introductory Chemistry, Chapter 5 Classifying Materials atomic elements = elements whose particles are single atoms molecular elements = elements whose particles are multi-atom molecules molecular compounds = compounds whose particles are molecules made of only nonmetals ionic compounds = compounds whose particles are cations and anions

16. 15 Molecular Elements Certain elements occur as 2 atom molecules Rule of 7’s –there are 7 common diatomic elements –find the element with atomic number 7, N –make a figure 7 by going over to Group 7A, then down –don’t forget to include H 2 H2H2 Cl 2 Br 2 I2I2 7 VIIA N 2 O 2 F 2

17. Molecular Compounds two or more nonmetals smallest unit is a molecule

18. Ionic Compounds metals + nonmetals no individual molecule, instead these have 3- dimensional array of cations and anions made of formula units (NaCl)

19. Classify each of the following as either an atomic element, molecular element, molecular compound or ionic compound aluminum, Al aluminum chloride, AlCl 3 chlorine, Cl 2 acetone, C 3 H 6 O carbon monoxide, CO cobalt, Co = atomic element = ionic compound = molecular element = molecular compound = atomic element

20. 19 TYPES OF COMPOUNDS  Compounds are pure substances that contain 2 or more elements combined in a definite proportion by mass.  Compounds can be classified as one of two types: Metals and non-metals Two non- metals

21. Nomenclature of Compounds Common Names – Are Exceptions (like nicknames) H 2 O = water, steam, ice NH 3 = ammonia CH 4 = methane NaCl = table salt C 12 H 22 O 11 = table sugar

22. Metal Cations Type I –metals whose ions can only have one possible charge IA, IIA, (Al, Ga, In) –determine charge by position on the Periodic Table IA = +1, IIA = +2, (Al, Ga, In = +3) Type II –metals whose ions can have more than one possible charge –determine charge by charge on anion How do you know a metal cation is Type II? its not Type I !!!

23. 22 BINARY IONIC COMPOUNDS (TYPE I)  Binary compounds contain only two elements.  Ionic compounds are formed by combination of a metal and a non-metal.  Type I ions are those cations that form only one ion.  In these compounds, charges of the cations must equal the charges of the anions since the net charge is zero.

24. 23 BINARY IONIC COMPOUNDS (TYPE I)  Subscripts are used to balance the charges between cations and anions. sodium bromide Na + Br  +1 -1 = 0 NaBr No subscripts needed potassium sulfide K+K+ S2S2 +1 -2  0 K2+K2+ +2 -2 = 0 K2SK2S

25. 24 Write formulas for the following ionic compounds: calcium chloride Ca 2+ Cl  +2 -1  0 CaCl 2 sodium sulfide Na + S2S2 +1 -2  0 +2 -2 = 0 Na 2 S Example 1: Cl 2  +2 -2 = 0 Na 2 +

26. 25 Type I Binary Ionic Compounds Contain Metal Cation + Nonmetal Anion Metal listed first in formula & name 1.name metal cation first, name nonmetal anion second 2.cation name is the metal name 3.nonmetal anion named by changing the ending on the nonmetal name to -ide

27. 26 BINARY IONIC COMPOUNDS (TYPE I) MgCl 2 magnesium chloride NaI sodium iodide AlF 3 aluminum fluoride

28. 27 Name the following ionic compounds: barium chloride Na 3 Psodium phosphide BaCl 2 Example 2:

29. 28 BINARY IONIC COMPOUNDS (TYPE II)  Type II ions are those cations that form more than one ion.  When naming compounds formed from these ions, include the ionic charge as Roman numeral, in parentheses, after the metal’s name.  This method of nomenclature is called the “stock” system.

30. 29 1.name metal cation first, name nonmetal anion second 2.metal cation name is the metal name followed by a Roman Numeral in parentheses to indicate its charge (only difference from type II!) –determine charge from anion charge 3.nonmetal anion named by changing the ending on the nonmetal name to -ide BINARY IONIC COMPOUNDS (TYPE II)

31. 30 BINARY IONIC COMPOUNDS (TYPE II) FeCl 2 ? -1 ? -2 = 0 +2 -1 iron (II) chloride FeCl 3 ? -1 ? -3 = 0 +3 -1 iron (III) chloride

32. 31 BINARY IONIC COMPOUNDS (TYPE II) Cu 2 O ? -2 2? -2 = 0 +1 -2 copper (I) oxide Roman numeral DOES NOT represent the subscript CuO ? -2 ? -2 = 0 +2 -2 copper (II) oxide

33. 32 BINARY IONIC COMPOUNDS (TYPE II)  Type II cations can also be named by an older method (classical).  In this system, cations with the higher charge end in –ic, while cations with the lower charge end in –ous.  In this system, some cations are named based on their Latin roots.

34. 33 CLASSICAL SYSTEM (DERIVED FROM LATIN) gold (aurum for Aurora the Roman goddess of the dawn ) silver (argentum for 'bright' ) copper (cuprum for 'Cyprus' where the Romans first obtained copper ) tin (stannum for alloys containing lead ) lead (plumbum for 'lead' ) mercury (hydrargyrum for 'liquid silver' or quick silver ) antimony (stibium for 'not alone' ) iron (ferrum for 'firmness‘ ) potassium (kalium via the Arabic qali for alkali ) sodium (natrium for soda )

35. 34 BINARY IONIC COMPOUNDS (TYPE II) FeCl 2 +2 -1 ferrous chloride FeCl 3 +3 -1 ferric chloride Lower charge Higher charge

36. 35 BINARY IONIC COMPOUNDS (TYPE II) Cu 2 O +1 -2 cuprous oxide CuO +2 -2 cupric oxide Lower charge Higher charge

37. 36 SnCl 2 ? -1 ? -2 = 0 +2 -1 tin (II) chloride Example 1: Name each of the following compounds using the stock and classical nomenclature system: Stock Classical Lower charge stannous chloride

38. 37 Cu 2 S ? -2 2? -2 = 0 +1 -2 copper (I) sulfide Example 1: Name each of the following compounds using the stock and classical nomenclature system: Stock Classical Lower charge cuprous sulfide

39. 38 Sn Example 2: Write formulas for each of the following compounds: Tin (II) bromideBr +2 -1 +2 -1  0 Br 2 SnBr 2 +2 -2 = 0

40. 39 Sn Example 2: Write formulas for each of the following compounds: Stannic oxideO +4 -2 +4 -2  0 SnO 2 +4 - 4 = 0 O2O2

41. Examples What, if anything, should go into the parenthesis LiCl = lithium ( ) chloride AlCl 3 = aluminum ( ) chloride PbO = lead ( ) oxide PbO 2 = lead ( ) oxide Mn 2 O 3 = manganese ( ) oxide X X II IV III

42. 41 POLYATOMIC IONS  Some ionic compounds contain polyatomic ions, an ion composed of several atoms bound together.

43. Patterns for Polyatomic Ions 1.elements in the same column form similar polyatomic ions –same number of O’s and same charge ClO 3 - = chlorate  BrO 3 - = bromate 2. if the polyatomic ion starts with H, the name adds hydrogen- prefix before name and add 1 to the charge CO 3 2- = carbonate  HCO 3 -1 = hydrogencarbonate

44. Periodic Pattern of Polyatomic Ions -ate groups BO 3 -3 NO 3 SiO 3 -2 PO 4 -3 SO 4 -2 ClO 3 AsO 4 -3 SeO 4 -2 BrO 3 TeO 4 -2 IO 3 CO 3 -2 IIIAIVA VA VIA VIIA

45. Patterns for Polyatomic Ions -ate ion –chlorate = ClO 3 -1 -ate ion + 1 O  same charge, per- prefix –perchlorate = ClO 4 -1 -ate ion – 1 O  same charge, -ite suffix –chlorite = ClO 2 -1 -ate ion – 2 O  same charge, hypo- prefix, -ite suffix –hypochlorite = ClO -1

46. © 2012 Pearson Education, Inc. Naming Ionic Compounds Containing a Polyatomic Ion Some examples of more than two ions in the series. ClO − hypochloriteBrO − hypobromiteIO − hypoiodite ClO 2 − chloriteBrO 2 − bromiteIO 2 − iodite ClO 3 − chlorateBrO 3 − bromateIO 3 − iodate ClO 4 − perchlorateBrO 4 − perbromateIO 4 − periodate When naming these ions in the homework, be sure to include the word ion in your answer, as in “perchlorate ion.”

47. 46 POLYATOMIC COMPOUNDS  When writing formulas for polyatomic compounds, treat the polyatomic ion as one group. potassium nitrate K+K+ NO 3 – +1 -1 = 0 KNO 3 calcium hydroxide Ca 2+ OH – +2 -1  0 (OH – ) 2 Ca(OH) 2 +2 -2 = 0

48. 47 POLYATOMIC COMPOUNDS ammonium acetate NH 4 + C2H3O2–C2H3O2– +1 -1 = 0 NH 4 C 2 H 3 O 2 sodium sulfate Na + SO 4 2– +1 -2  0 Na 2 + Na 2 SO 4 +2 -2 = 0

49. 48 POLYATOMIC COMPOUNDS copper (II) nitrate Cu 2+ NO 3 – +2 -1  0 Cu(NO 3 ) 2 (NO 3 – ) 2 +2 -2 = 0 Type II Roman numeral represents charge of ion Alternate name =cupric nitrate

50. 49 Mg(OH) 2 magnesium hydroxide NaCN Example 2: Name the following polyatomic compounds: Type I ion (Does not require roman numeral) sodium cyanide Fe 2 (SO 4 ) 3 Type II ion (Requires roman numeral) +3  2 iron (III) sulfate ferric sulfate

51. Subclasses Compounds containing a metal and a nonmetal = binary ionic –Type I and II Compounds containing a polyatomic ion = ionic with polyatomic ion

52. 51 BINARY MOLECULAR COMPOUNDS  Molecular compounds are formed by combination of 2 or more non-metals.  The smallest particles of molecular compounds are molecules.  These compounds are named similar to ionic compounds, with the second element named based on its root and suffix “-ide”.

53. 52 BINARY MOLECULAR COMPOUNDS  Greek prefixes are used to indicate the number of atoms in these compounds. NumberPrefixNumberPrefix 1mono-6hexa- 2di-7hepta- 3tri-8octa- 4tetra-9nona- 5penta-10deca-

54. 53 Examples: Name the following binary molecular compounds: CS 2 carbon disulfide First atom uses a prefix only when more than one atom is present Second atom always uses a prefix indicates 1 carbon atom indicates 2 sulfur atoms

55. 54 Examples: Name the following binary molecular compounds: IF 7 iodine heptafluoride indicates 1 iodine atom indicates 7 fluorine atoms

56. 55 SUMMARY OF BINARY NOMENCLATURE Ionic Molecular Type I Type II

57. Naming Acids Contain H + cation and anion –in aqueous solution Binary acids have H + cation and nonmetal anion Oxyacids have H + cation and polyatomic anion

58. Naming Acids Binary Acids = hydro prefix + stem of the name of the nonmetal + ic suffix Example: HCl  hydrochloric acid Oxyacids –if polyatomic ion ends in –ate = name of polyatomic ion with –ic suffix Example: HNO 3  nitric acid –if polyatomic ion ends in –ite = name of polyatomic ion with –ous suffix Example: H 2 SO 3  sulfurous acid base name of oxyanion + -icacid base name of oxyanion + -ous acid

59. 58 ACIDS  Acids are molecular compounds that form ions when dissolved in water. Binary Acids  Formulas are written similar to binary ionic compounds, assigning a +1 charge to hydrogen. HCl +1 -1 H2SH2S +1 -2

60. 59 NAMING BINARY ACIDS  When naming the acids, use hydro- prefix, followed by the name of the non-metal with an –ic ending, followed with the word acid. HCl H2SH2S acidhydrochloric hydrosulfuric acid HFhydrofluoric acid

61. 60 POLYATOMIC ACIDS  Several polyatomic acids are important in the study of chemistry, and their names must be learned.  These acids and the polyatomic ions that form from their ionization are as follows:  Most of these are oxyacids

62. 61 POLYATOMIC ACIDS sulfuric acidH 2 SO 4 SO 4 2  sulfate phosphoric acidH 3 PO 4 PO 4 3  phosphate nitric acidHNO 3 NO 3  nitrate

63. 62 POLYATOMIC ACIDS carbonic acidH 2 CO 3 CO 3 2  carbonate HCO 3  bicarbonate acetic acid HC 2 H 3 O 2 C 2 H 3 O 2  acetate

64. The names of acids containing oxyanions ending with -ite take this form: The names of acids containing oxyanions ending with -ate take this form: base name of oxyanion + ous base name of oxyanion + ic

65. Names of Some Common Oxyacids and Their Oxyanions

66. Formula Mass: The Mass of a Molecule or Formula Unit also known as molecular mass For any compound, the formula mass is the sum of the atomic masses of all the atoms in its chemical formula: Mass of 1 molecule of H 2 O = 2(1.01 amu H) + 16.00 amu O = 18.02 amu

67. 66 THE END