2. Ch. 7 (Con’t.) Formula Writing & Naming of Compunds

3. Predicting Charges on Monatomic Ions KNOW THESE !!!! +1 +2 -3 -2 -1 0 Cd +2

4. Chemical Formulas Chemical formula- –Consists of element symbols and subscripts C 6 H 12 O 6 –Formula Units – simplest whole # ratios of ions present in a compound (for ionic compounds) –Molecular Formulas- used for covalently bonded compounds. (show EVERY atom present in a molecule) Ex. H 2 O Water has 2 hydrogen atoms and 1 oxygen atom

5. Example: Aluminum Chloride Step 1: Step 2: 1 3 Step 3: Al Cl 3+ 1- write symbols & charge of elements criss-cross charges as subscripts combine as formula unit (“1” is never shown) (use smallest whole # ratio) Make sure you remove charges!! Aluminum Chloride AlCl 3 Cation (metal) always written 1 st ! Writing Balanced Chemical Formulas Criss-Cross Rule for Ionic Compounds

6. InBr 3 BaS charge on cation “becomes” subscript of anion charge on anion “becomes” subscript of cation ** Warning: Reduce subscripts to lowest terms. Al 2 O 3 Al 3+ and O 2– Al 2 O 3 Ba 2+ and S 2– Ba 2 S 2 In 3+ and Br 1– In 1 Br 3 aluminum oxidebarium sulfideindium bromide Ones are not included in formulas!!

7. Example: Magnesium Oxide Step 1: Magnesium Oxide Step 2: Mg 2+ O 2- Step 3: Mg O 22 Step 4: Mg 2 O 2 Step 5: MgO Criss-Cross Rule

8. Putting Ions Together Na + + Cl - = NaCl Ca +2 + O -2 = CaONa + + O -2 = Na 2 O Al +3 + S -2 = Al 2 S 3 Ca +2 + N -3 = Ca 3 N 2 Ca +2 + Cl - = CaCl 2 You try these! Mg +2 + F - = K + + Cl - = Al +3 + I - = Sr +2 + P -3 = Li + + Br - = Sr 3 P 2 AlI 3 MgF 2 KCl LiBr

9. Crisscross Switch the numerical value of the charges Ba 2+ N 3- 2 3 Ba 3 N2N2 Reduce ratio if possible

10. Learning Check Write the correct formula for the compounds containing the following ions: 1. Na +, S 2- a) NaS b) Na 2 Sc) NaS 2 2. Al 3+, Cl - a) AlCl 3 b) AlCl c) Al 3 Cl 3. Mg 2+, N 3- a) MgN b) Mg 2 N 3 c) Mg 3 N 2

11. Solution 1. Na +, S 2- b) Na 2 S 2. Al 3+, Cl - a) AlCl 3 3. Mg 2+, N 3- c) Mg 3 N 2

12. Polyatomic Ions There are some ions that are made up of more than one type of atom, these are called Polyatomic ions – groups of covalently bonded atoms with a charge For example, the polyatomic ion known as ammonium NH 4 + has 4 atoms of hydrogen and one atom of nitrogen, HOWEVER, the whole “group” has an overall charge of +1 ** you need to memorize the formulas & the charges of many polyatomic ions!

14. NO 3 - nitrate ion NO 2 - nitrite ion Polyatomic Ions

15. Naming Ternary Ionic Compounds contain at least 3 elements & the 1 st is a metal: there MUST be at least one polyatomic ion (it helps to circle the ions) Examples: NaNO 3 Sodium nitrate K 2 SO 4 Potassium sulfate Al(HCO 3 ) 3 Aluminum bicarbonate or Aluminum hydrogen carbonate

16. What About... What if I have to put multiple polyatomic ions in a compound, for example, magnesium nitrate? Magnesium has a charge of +2 Nitrate is polyatomic ion and has a charge of -1 Therefore, we need 2 nitrate ions for each magnesium In this case, we put the entire polyatomic ion in parenthesis and put the subscript outside the parenthesis Our answer would be Mg(NO 3 ) 2

17. IONIC COMPOUNDS remember: they have oppositely-charged ions in a rigid 3-D pattern NH 4 + Cl - ammonium chloride, NH 4 Cl

18. Ternary Ionic Nomenclature Sodium Sulfate Na + and SO 4 -2 Na 2 SO 4 Iron (III) hydroxide Fe +3 and OH - Fe(OH) 3 Ammonium carbonate NH 4 + and CO 3 –2 (NH 4 ) 2 CO 3

19. (NH 4 ) 3 N Fe 2 (Cr 2 O 7 ) 3 Sn(SO 4 ) 2 NH 4 ClO 3 Mg(NO 2 ) 2 BaSO 4 Writing Formulas w /Polyatomic Ions Reminder! Parentheses are required only when you need more than one “bunch” of a particular polyatomic ion. Ba 2 and SO 4 2– Mg 2+ and NO 2 1– NH 4 1+ and ClO 3 1– Sn 4+ and SO 4 2– Fe 3+ andCr 2 O 7 2– NH 4 1+ andN 3– barium sulfate magnesium nitrite ammonium chlorate tin (IV) sulfate iron (III) dichromate ammonium nitride

20. Learning Check 1. aluminum nitrate a) AlNO 3 b) Al(NO) 3 c) Al(NO 3 ) 3 2. copper(II) nitrate a) CuNO 3 b) Cu(NO 3 ) 2 c) Cu 2 (NO 3 ) 3. Iron (III) hydroxide a) FeOHb) Fe 3 OHc) Fe(OH) 3 4. Tin(IV) hydroxide a) Sn(OH) 4 b) Sn(OH) 2 c) Sn 4 (OH)

21. Many polyatomic ions with the same endings on their names have a different number of oxygen atoms attached to the central atom. For example chlorateClO 3 -1 sulfateSO 4 -2 phosphate PO 4 -3 acetateC 2 H 3 O 2 -1

22. Polyatomic Ion: a group of atoms that stay together and have a single, overall charge. BrO 4 1- Perbromate ion BrO 3 1- Bromate ion BrO 2 1- Bromite ion BrO 1- Hypobromite ion CO 4 2- CO 3 2- Carbonate ion CO 2 2- CO 2- ClO 4 1- ClO 3 1- Chlorate ion ClO 2 1- ClO 1- IO 4 1- IO 3 1- Iodate ion IO 2 1- IO 1- NO 4 1- NO 3 1- Nitrate ion NO 2 1- NO 1- PO 5 3- PO 4 3- Phosphate ion PO 3 3- PO 2 3- SO 5 2- SO 4 2- Sulfate ion SO 3 2- SO 2 2- 1 more oxygen“normal”1 less oxygen2 less oxygen

23. Salt metal polyatomic ion # Oxygen atoms ________ per_____ate 1 more O ________ _____ate common ________ _____ite 1 less O ________ hypo_____ite 2 less O’s ________ _____ide0 O’s The table below shows the prefixes and suffixes that tell the number of oxygen atoms present in the negative ion.

24. The oxy-ions of chlorine & bromine all have these trends in common. Look for them below…… perchlorate Cl O 4 -1 chlorate Cl O 3 -1 chlorite Cl O 2 -1 Hypochlorite Cl O -1 Perbromate BrO 4 -1 Bromate BrO 3 -1 Bromite BrO 2 -1 Hypobromite BrO -1 The most productive method of committing these ions to memory is first memorize the ones that have the -ate ending. This is the most common ending.

25. Practice Problem #2 sodium chlorite Choose the correct formula for the compound 1. NaCl 2. NaClO 3. NaClO 2 4. Na(ClO) 2 5. none of the above next problem Prefixes Periodic Chart

26. Naming Compounds What's in a name? That which we call a rose by any other name would smell as sweet." - William Shakespeare, Romeo and Juliet (II, ii)

27. Naming Compounds 1. Cation first, then anion 2. Monatomic cation = name of the element Ca 2+ = calcium ion 3. Monatomic anion = root + -ide Cl  = chloride CaCl 2 = calcium chloride Binary Ionic Compounds (metal & nonmetal):

28. Name these ions l Cl 1- Chloride ion l N 3- Nitride ion l Br 1- Bromide ion l O 2- Oxide ion l Ga 3+ Gallium ion

29. Naming Binary Ionic Compounds Examples: NaCl ZnI 2 Al 2 O 3 sodium chloride zinc iodide aluminum oxide

30. Formulas to Names: Ternary Compounds KMnO 4 potassium I’m a polyatomic ion 1.Write the names of the ions Final Name permanganate If the positive ion has a fixed charge, you are finished.

31. Formulas to Names: Ternary Compounds NH 4 NO 3 ammonium I’m a polyatomic ion 1.Write the names of the ions Final Name nitrate If the positive ion has a fixed charge, you are finished.

32. Learning Check Match each set with the correct name: 1. Na 2 CO 3 a) magnesium sulfite MgSO 3 b) magnesium sulfate MgSO 4 c) sodium carbonate 2.Ca(HCO 3 ) 2 a) calcium carbonate CaCO 3 b) calcium phosphate Ca 3 (PO 4 ) 2 c) calcium bicarbonate

33. Practice Naming Ionic Compounds Na 2 CO 3 -- CaSO 4 -- KBr -- MgS -- BeCl 2 -- NH 4 F --

34. Multiple Oxidation Numbers When the metal in an ionic compound is multi-valent (has more than 1 charge) there are 2 naming methods: –Latin & Stock Systems Latin is older (not useful for some compounds) The metal is named with it’s Latin or English root and ends in -ic or –ous to denote charge. E.g. Cu +1 is cuprous, E.g. Cu +2 is cupric Lower = ous, Higher = ic

35. Cu +2 + Cl -1 = CuCl 2 = cupric chloride Cu +1 + Cl -1 = CuCl = cuprous chloride For Latin naming: know rules, possible charges, Latin names, & suffixes Write the balanced formula for copper chloride & name it:

36. Examples of Older Names of Cations formed from Transition Metals

37. The oxidation number (charge) of the metal is indicated in parentheses using Roman numerals E.g. Cu 1+ is copper(I), Cu 2+ is copper(II) Numbers refer to charges not to #s of atoms Try: Cu 2+ +Cl -1 & Cu 1+ +Cl -1, Cu +2+ +Cl -1 = CuCl 2 = copper (II) chloride Co +1 + Cl -1 = CuCl = copper (I) chloride Multiple valence: Stock System

38. Formula to Name: How do I figure out the Roman Numeral?? Hint: We’ve already learned this! 1) Assign the element with the unknown charge a charge of x 2) Multiply the charge of each element by the number of atoms of that element to get the total charge. 3) Add the products from step 2 and set them equal to zero because compounds are neutral- zero charge 4) Solve for the unknown charge.

39. Binary Compounds Containing a Metal of Variable Oxidation Number To name these compounds, give the name of the metal (Type II cations) followed by Roman numerals in parentheses to indicate the oxidation number of the metal, followed by the name of the nonmetal, with its ending replaced by the suffix –ide. ExamplesStock System FeCl 2 (“ic” ending = higher oxidation state; “ous” is lower oxidation state) SnOTin oxide SnO 2 Tin oxide (II) (III) (II) (IV) Traditional (OLD) System Ferrous chloride Ferric chloride Stannous oxide Stannic oxide Iron chloride FeCl 3

40. Ternary Ionic Nomenclature Writing Formulas Write each ion, cation first. Don’t show charges in the final formula. Overall charge must equal zero. –If charges cancel, just write symbols. –If not, use subscripts to balance charges. Use parentheses to show more than one of a particular polyatomic ion. Use Roman numerals indicate the ion’s charge when needed (Stock System)

41. How do I figure out the Roman Numeral?

42. Solving for the roman numeral (charge) of Fe 2 O 3 (2x) + (3)(-2) = 0 –# of Fe atoms times charge of Fe + number of O atoms times charge of O = zero because compounds are neutral, no charge 2x + (-6) = 0 2x – 6 = 0 2x = 6 x= 3 Answer for the name: Iron (III) oxide

43. Examples #6- Formulas to Names Cu 2 S copper I’m not a polyatomic ion 2.Determine the charge of the positive ion 1.Write the names of the ions Final Name sulfide (I) 2Cu x (S) -2 = 0 2X + (-2) = 0 X = +1

44. Examples #1- Formulas to Names CuSO 3 copper I’m a polyatomic ion 1.Write the names of the ions Final Name sulfite (II) x X + (- 2) = 0 X = +2 Cu SO 3 = 0 You must know the charge on the sulfite ion is -2 The sum of the positive and negative charges must equal zero 2. Determine the charge of the positive ion -2 +2 Next +2

45. Examples #4- Formulas to Names SnF 2 tin 2.Determine the charge of the positive ion 1.Write the names of the ions Final Name fluoride (II) Sn x (F -1 ) 2 = 0 X + 2(-1) = 0 X = +2

46. Example #3-Names to Formulas nickel(III) acetate Ni C2H3O2C2H3O2 2. Determine number of ions 1. Write symbols of elements Final Formula (Ni +3 ) x (C 2 H 3 O 2 -1 ) y = 0 3X = 1y X(+3) + y(-1) = 0 X 1 Y 3 = 1 Choose the lowest set of integers that satisfies the equation (C 2 H 3 O 2 ) 3 If there is only one atom the “1” is not shown Next

47. Practice Problem #1 Fe(NO 3 ) 3 Choose the correct name for the compound 1. Iron trinitrate 2. iron(I) nitrate 3. iron(III) nitrite 4. iron(III) nitrate 5. none of the above next problem Polyatomic IonsPeriodic Chart

48. Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr 2 iron (_____) bromide CuClcopper (_____) chloride SnO 2 ___(_____ ) ______________ Fe 2 O 3 ________________________ Hg 2 S________________________

49. Nomenclature for molecular (Covalent) binary compounds (two nonmetals) Uses a Prefix System 1.Less electronegative atom comes first. (towards left side of P.T.) 2.Add numerical prefixes to indicate # of atoms of each element. 3.Change the ending of the second element to –ide (since it’s binary)

50. mono- 1 hepta- 7 di- 2 octa- 8 tri- 3 nona- 9 tetra- 4 deca- 10 penta- 5 hexa- 6 In order to be effective in using prefixes to name compounds containing two non- metals, these prefixes must be committed to memory:

51. Naming covalent compounds 1mono 2di 3tri 4tetra 5penta 6hexa 7hepta 8octa 9nona 10deca prefix refers to # of atoms - not charge N 2 O 4 = dinitrogen tetroxide Exception: don’t use mono for first element CO 2 = carbon dioxide The first vowel is often dropped to avoid the combination of “ao” or “oo”. CO = carbon monoxide (monooxide) P 4 O 10 = tetraphosphorus decoxide (decaoxide)

52. Covalent Compounds: Name to Formula You’ll like this! For covalent compounds, simply use the numerical prefixes to tell you the number (subscript) of each element (No charges, No criss-cross, No balancing needed!): What is the formula for dinitrogen trioxide? N2O3N2O3 dinitrogen monoxide? N 2 O

53. Example #1- Names to Formulas Sulfur trioxide S O 1 3 I’m a Binary Compound 2. Write number of atoms 1. Write symbols of elements Final Formula If no prefix, then 1 is implied and not written Two Non metals:

54. Example #2- Names to Formulas dichlorine heptaoxide Cl O 2 7 I’m a Binary Compound 2. Write number of atoms 1. Write symbols of elements Final Formula

55. Example #3- Names to Formulas oxygen difluoride O F 1 2 I’m a Binary Compound 2. Write number of atoms 1. Write symbols of elements Final Formula If no prefix, then 1 is implied and not written

56. Example #4- Names to Formulas dinitrogen tetraoxide N O 2 4 I’m a Binary Compound 2. Write number of atoms 1. Write symbols of elements Final Formula

57. Example #5- Names to Formulas phosphorus pentachloride P Cl 1 5 I’m a Binary Compound 2. Write number of atoms 1. Write symbols of elements Final Formula If no prefix, then 1 is implied and not written

58. Examples #2- Formulas to Names XeF 3 xenonmono tri I’m a Binary Compound 2. Write prefix for number of atoms 1. Write names of elements – last element ends in -ide Final Name fluor ide If first prefix is mono, it is implied and not written

59. Example - Formulas to Names AsI 3 arsenicmono tri I’m a Binary Compound 2. Write number of atoms 1.Write names of elements (-ide on last) Final Name iod ide If first prefix is mono, it is implied and not written

60. Examples #1- Formulas to Names CCl 4 carbonmonotetra I’m a Binary Compound 2. Write number of atoms 1. Write names of elements Final Name chlor ide If first prefix is mono, it is implied and not written Two Non metals:

61. Write and name the following covalent compounds (IUPAC) carbon tetrachloride diphosporus trioxide iodine heptafluoride CCl 4 P 2 O 3 IF 7 For more lessons, visit www.chalkbored.com www.chalkbored.com

62. CF 4 N 2 O SBr 6 –carbon tetrafluoride –dinitrogen monoxide –sulfur hexabromide Molecular Nomenclature: Examples

63. arsenic trichloride dinitrogen pentoxide tetraphosphorus decoxide –AsCl 3 –N2O5–N2O5 –P 4 O 10 More Molecular Examples

64. Learning Check Fill in the blanks to complete the following names of covalent compounds. CO carbon ______oxide CO 2 carbon _______________ PCl 3 phosphorus _______chloride CCl 4 carbon ________chloride N 2 O_____nitrogen _____oxide

65. Learning Check 1.P 2 O 5 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2.Cl 2 O 7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl 2 a) chlorine b) dichlorine c) dichloride

66. Practice Problem #1 ClF 3 Choose the correct name for the compound 1. carbon iodine trifluoride 2. chlorine trifluorine 3. chlorine trifluoride 4. chlorine tetrafluoride 5. none of the above

67. Practice Problem #2 arsenic pentabromide Choose the correct formula for the compound 1. AsBr 5 2. ArBr 5 3. AsBr 7 4. As 5 Br 5. none of the above next problem PrefixesElement List

68. Practice Problem #3 N2O3N2O3 Choose the correct name for the compound 1. nitrogen trioxide 2. dinitride trioxide 3. dinitrogen trioxygen 4. dinitrogen trioxide 5. none of the above next problem Prefixes

69. Practice Problem #6 dichlorine monoxide Choose the correct formula for the compound 1. ClO 2. Cl 2 O 3. ClO 2 4. Cl 2 O 2 5. none of the above next problem Prefixes

70. Acid Nomenclature AcidsAcids –Compounds that form H + in water. –Formulas usually begin with ‘H’. –In order to be considered an acid, they must be aqueous (dissolved in water – formulas end in aq) Examples:Examples: –HCl (aq) – hydrochloric acid –HNO 3 (aq) – nitric acid –H 2 SO 4 (aq) – sulfuric acid We will look at binary & ternary acids!

71. Naming Binary Acids H + 1 other element HX (aq) If the anion attached to hydrogen ends in -ide, add the prefix hydro- and change -ide to -ic acid HCl - hydrogen chloride becomes hydrochloric acid H 2 S - hydrogen sulfide becomes hydrosulfuric acid

72. Naming Ternary Acids H + a polyatomic ion – HXO (aq) change the suffix -ate to -ic acid HNO 3(aq) not hydrogen nitrate, but –nitric acid change the suffix -ite to -ous acid HNO 2(aq) not hydrogen nitrite, but –nitrous acid Ternary Acid names DO NOT begin with “hydro-”!

73. Acid Nomenclature Binary  Ternary To remember which goes with which… “In the cafeteria, you ATE something ICky”

74. Salt Hydrogen + polyatomic ion hydrogen per_____ate hydrogen _____ate hydrogen _____ite hydrogen hypo_____ite hydrogen _____ide Aqueous Acid hydrogen polyatomic ion per_____ic acid _____ic acid _____ous acid hypo______ous acid hydro______ic acid To transform the hydrogen _____ide salt into its corresponding aqueous acid name: 1) The name hydrogen is replaced with the prefix hydro- 2) The -ide ending is replaced with ____ic 3) The word acid is added to the name For example: hydrogen bromide > hydrobromic acid HBr (s) > HBr (aq)

75. To transform the hydrogen _____ate salt into its corresponding aqueous acid name: 1) The name hydrogen is dropped 2) The -ate ending is replaced with –ic 3) The word acid is added to the name For example: hydrogen acetate > acetic acid HC 2 H 3 O 2(s) > HC 2 H 3 O 2(aq) Salt Hydrogen + polyatomic ion hydrogen per_____ate hydrogen _____ate hydrogen _____ite hydrogen hypo_____ite hydrogen _____ide Aqueous Acid hydrogen + polyatomic ion per_____ic acid _____ic acid _____ous acid hypo______ous acid hydro______ic acid

76. To transform the hydrogen per____ate salt into its corresponding aqueous acid name: 1) The name hydrogen is dropped 2) The -ate ending is replaced with –ic 3) The word acid is added to the name For example: hydrogen perchlorate > perchloric acid HClO 4(s) > HClO 4 (aq) Aqueous Acid hydrogen polyatomic ion per_____ic acid _____ic acid _____ous acid hypo______ous acid hydro______ic acid Salt Hydrogen + polyatomic ion hydrogen per_____ate hydrogen _____ate hydrogen _____ite hydrogen hypo_____ite hydrogen _____ide

77. Salt Hydrogen + polyatomic ion hydrogen per_____ate hydrogen _____ate hydrogen _____ite hydrogen hypo_____ite hydrogen _____ide Aqueous Acid hydrogen polyatomic ion per_____ic acid _____ic acid _____ous acid hypo______ous acid hydro______ic acid To transform the hydrogen _____ite salt into its corresponding aqueous acid name: 1) The name hydrogen is dropped 2) The -ite ending is replaced with –ous 3) The word acid is added to the name For example:hydrogen nitrite > nitrous acid HNO 2(s) > HNO 2(aq)

78. Salt Hydrogen + polyatomic ion hydrogen per_____ate hydrogen _____ate hydrogen _____ite hydrogen hypo_____ite hydrogen _____ide Aqueous Acid hydrogen polyatomic ion per_____ic acid _____ic acid _____ous acid hypo______ous acid hydro______ic acid To transform the hydrogen hypo_____ite salt into its corresponding aqueous acid name: 1) The name hydrogen is dropped 2) The -ite ending is replaced with –ous 3) The word acid is added to the name For example: hydrogen hypoiodite > hypoiodous acid HIO (s) > HIO (aq)

79. Examples #1- Formulas to Names 2. Determine the ion and it’s acid ending. 1. The hydrogen out front & the (aq) subscript indicates an acid Final Name HBrO 2(aq) bromous acid bromite ____________ acid

80. Practice Problem #1 HIO 4(aq) Choose the correct name for the compound 1. iodoic acid 2. iodous acid 3. periodoic acid 4. hydrogen periodate 5. none of the above next problem Ion list

81. Writing Acid Formulas Hydrogen will always be first The name will tell you the anion If it starts with hydro- it’s binary - H + a non-metal, If it doesn’t start with hydro-, it’s ternary – H + a polyatomic ion. Remember: -ate comes from -ic, -ite comes from –ous Balance charges.

82. Example #1- Names to Formulas H ClO 3 2. Add hydrogen ions 1.Determine the formula & charge of the polyatomic ion Final Formula chloric acid (aq) chlorate +1 3. Balance charge with ions 4. Add the subscript: (aq) =0

83. hydrofluoric acidhydrofluoric acid sulfuric acidsulfuric acid nitrous acidnitrous acid –2 elements –3 elements, -ic –3 elements, -ous  HF (aq)  H 2 SO 4  HNO 2 Acid Nomenclature  H + F-  H + SO 4 2-  H + NO 2 -

84. HBr (aq)HBr (aq) H 2 CO 3H 2 CO 3 H 2 SO 3H 2 SO 3 –2 elements, -ide –3 elements, -ate –3 elements, -ite  hydrobromic acid  carbonic acid  sulfurous acid Acid Nomenclature

85. Practice Problem hydrobromic acid Choose the correct formula for the compound 1. HBrO (aq) 2. HBr (aq) 3. HBrO 3(aq) 4. HBrO 2(aq) 5. none of the above next problem Ion list

86. Acid Nomenclature Flowchart

87. A flow chart for naming binary compounds.

88. Mixed Review Name the following compounds: 1. CaO a) calcium oxideb) calcium(I) oxide c) calcium (II) oxide 2. SnCl 4 a) tin tetrachlorideb) tin(II) chloride c) tin(IV) chloride 3. N 2 O 3 a) nitrogen oxide b) dinitrogen trioxide c) nitrogen trioxide

89. Solution Name the following compounds: 1. CaO 2. SnCl 4 3.N 2 O 3 a) calcium oxide c) tin(IV) chloride b) Dinitrogen trioxide

90. Mixed Practice 1.Dinitrogen monoxide 2.Potassium sulfide 3.Copper (II) nitrate 4.Dichlorine heptoxide 5.Chromium (III) sulfate 6.Iron (III) sulfite 7.Calcium oxide 8.Barium carbonate 9.Iodine monochloride

91. Mixed Practice 1.BaI 2 2.P 4 S 3 3.Ca(OH) 2 4.FeCO 3 5.Na 2 Cr 2 O 7 6.I 2 O 5 7.Cu(ClO 4 ) 2 8.CS 2 9.B 2 Cl 4

92. Name ‘Em! HI (aq)HI (aq) HClHCl H 2 SO 3H 2 SO 3 HNO 3HNO 3 HIO 4HIO 4

93. Write the Formula! Hydrobromic acidHydrobromic acid Nitrous acidNitrous acid Carbonic acidCarbonic acid Phosphoric acidPhosphoric acid Hydrotelluric acidHydrotelluric acid

94. Naming Ternary Compounds from Oxyacids The following table lists the most common families of oxy acids. one more oxygen atom most “common” one less oxygen two less oxygen HClO 4 perchloric acid HClO 3 chloric acid HClO 2 chlorous acid HClO hypochlorous acid H 2 SO 4 sulfuric acid H 2 SO 3 sulfurous acid H 3 PO 4 phosphoric acid H 3 PO 3 phosphorous acid H 3 PO 2 hypophosphorous acid HNO 3 nitric acid HNO 2 nitrous acid (HNO) 2 hyponitrous acid

96. Naming Simple Chemical Compounds Ionic (metal and nonmetal)Covalent (2 nonmetals) Metal Forms only one positive ion Forms more than one positive ion Nonmetal Use the name of element Use element name followed by a Roman numeral to show the charge First nonmetal Second nonmetal Before element name use a prefix to match subscript Use a prefix before element name and end with ide Single Negative Ion Polyatomic Ion Use the name of the element, but end with ide Use the name of polyatomic ion (ate or Ite)

97. Nomenclature PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion HC 2 H 3 O 2 Acetic Acid

98. Two nonmetalsMultiple-charge cationEverything else Roman numeral Polyatomic ions OK Roman numeral for name only Polyatomic ions Greek prefixes Charge Criss- Cross Rule Roman numeral OK Where would you file this? VCrO 4 BaO CBr 4 Nb(ClO 4 ) 5 SCl 2 Rb 2 SO 4 dinitrogen pentoxide platinum (IV) iodate ammonium chlorate potassium iodide nitrogen trichloride manganese (V) sulfide vanadium (II) chromate VCrO 4 N2O5N2O5 dinitrogen pentoxide barium oxide BaO Pt(IO 3 ) 4 platinum (IV) iodate carbon tetrabromide CBr 4 NH 4 ClO 3 ammonium chlorate niobium (V) perchlorate Nb(ClO 4 ) 5 KI potassium iodide sulfur dichloride SCl 2 NCl 3 nitrogen trichloride rubidium sulfate Rb 2 SO 4 Mn 2 S 5 manganese (V) sulfide PRACTICE

99. Learning Check Complete the names of the following binary compounds: Na 3 Nsodium ________________ KBrpotassium________________ Al 2 O 3 aluminum ________________ MgS_________________________

100. - calcium hydroxide - copper(II) sulfate - ammonium nitrate - cobalt(III) carbonate Ca(OH) 2 CuSO 4 NH 4 NO 3 Co 2 (CO 3 ) 3 Compounds containing polyatomic ions