2. Nomenclature PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion HC 2 H 3 O 2 Acetic Acid Chemistry and Pre-AP Chemistry Ch 6 SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead of "Slides" in the print setup. Also, turn off the backgrounds (Tools>Options>Print>UNcheck "Background Printing")!

3. Chemical formula shows the kinds and numbers of atoms in the smallest representative unit of the substance.

4. Forms of Chemical Bonds There are 2 forms bonding atoms:There are 2 forms bonding atoms: Ionic—(binary) complete transfer of 1 or more electrons from one atom to another (one loses, the other gains)Ionic—(binary) complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) Covalent—(molecular) some valence electrons shared between atomsCovalent—(molecular) some valence electrons shared between atoms

5. Distinguish between the two types of compounds: Molecular or Covalent two or more NONMETALS low melting points low boiling points Ionic metal and a nonmetal solids at room temp high melting points electrically neutral

6. Common Names A lot of chemicals have common names as well as the proper IUPAC name.A lot of chemicals have common names as well as the proper IUPAC name. Chemicals that should always be named by common name and never named by the IUPAC method are:Chemicals that should always be named by common name and never named by the IUPAC method are: H 2 Owater, not dihydrogen monoxideH 2 Owater, not dihydrogen monoxide NH 3 ammonia, not nitrogen trihydrideNH 3 ammonia, not nitrogen trihydride

7. Diatomic molecules are those that contain two atoms. O2O2 Triatomic molecules are those that contain three atoms. O3O3 H2H2 H2OH2O

8. Examples: H2OH2OO2O2 CO 2 O3O3

9. 6.1 Introduction to Chemical Bonding Compound: the smallest electrically neutral unit of a substance that still has the properties of the substance. made up of two or more atoms that act as a unit.

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

11. Ions are atoms or groups of atoms that have a positive or a negative charge. are formed when an atom or group of atoms loses or gains electrons.

12. Cations positively charged ions electrons were lost metals usually form cations the name of a monatomic ion is the same as the element

13. Examples Mg 2+ Ag + Al 3+

14. Anions negatively charged ions electrons were gained nonmetals usually form anions monatomic anions end in –ide

15. Examples: Cl - P 3- O 2-

16. “We think positively about cats (cations) and negatively about ants (anions)!”

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

18. Example: Sodium loses an electron Na  ________________ Magnesium loses 2 electrons Mg  ____________ Chlorine Gains an electron Cl  _______________ Phosphorous gains 3 electrons P  _____________ Na + Mg 2+ Cl - P 3-

19. Ionic compounds composed of cations and anions usually a metal and a nonmetal electrically neutral solids at room temperature high melting points

20. Examples: NaCl NaF CaCl 2 metal nonmetal **The more positive element (metal) always comes first.

21. Properties of Ionic Compounds Forming NaCl from Na and Cl 2 A metal atom can transfer an electron to a nonmetal.A metal atom can transfer an electron to a nonmetal. The resulting cation and anion are attracted to each other by electrostatic forces.The resulting cation and anion are attracted to each other by electrostatic forces.

22. IONIC COMPOUNDS NH 4 + Cl - ammonium chloride, NH 4 Cl

23. Some Ionic Compounds Mg 2+ + N -3 ----> Mg 3 N 2 magnesium nitride Sn 4+ + O 2- ----> SnO 2 Tin (IV) oxide calcium fluoride Ca 2+ + 2 F - ---> CaF 2

24. Formulas of Ionic Compounds Formulas of ionic compounds are determined from the charges on the ions atoms ions     – Na  +  F :  Na + : F :  NaF     sodium + fluorine sodium fluoride formula Charge balance: 1+ 1- = 0

25. Monatomic Ions

26. Writing a Formula Write the formula for the ionic compound that will form between Ba 2+ and Cl . Solution: 1. Balance charge with + and – ions 2. Write the positive ion of metal first, and the negative ion Ba 2+ Cl  Cl  3. Write the number of ions needed as subscripts BaCl 2

27. Criss Cross Method Example: sodium chloride Na + Cl - 11 Na 1 Cl 1 =NaCl

28. magnesium iodide Mg 2+ I - 1 2 Mg 1 I 2 =MgI 2

29. magnesium nitride Mg 2+ N 3- 2 3 Mg 3 N 2

30. strontium selenide Sr 2+ Se 2- 22 Sr 2 Se 2 = SrSe

31. rubidium iodide aluminum oxide Rb + I - RbI Al 3+ O 2- Al 2 O 3

32. 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

33. 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

34. 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:

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

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

37. Solution Complete the names of the following binary compounds: Na 3 N KBr Al 2 O 3 MgS sodium nitride potassium bromide aluminum oxide magnesium sulfide

39. Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or 2+ 2+ or 3+ Cu +, Cu 2+ Fe 2+, Fe 3+ copper(I) ion iron(II) ion copper (II) ion iron(III) ion There are three exceptions: Zn 2+, Cd 2+, and Ag +

40. Examples: What is the formula for the following transition metals as ions? Copper (I) Iron (III) Lead (II) Manganese (III)

41. Names of Variable Ions These elements REQUIRE Roman Numerals because they can have more than one possible charge: anything except Group 1A, 2A, Ag, Zn, Cd, and Al (You should already know the charges on these!) Or another way to say it is: Transition metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral. FeCl 3 (Fe 3+ ) iron (III) chloride CuCl (Cu + ) copper (I) chloride SnF 4 (Sn 4+ ) tin (IV) fluoride PbCl 2 (Pb 2+ )lead (II) chloride Fe 2 S 3 (Fe 3+ )iron (III) sulfide

42. Examples of Older Names of Cations formed from Transition Metals (you do not have to memorize these)

43. When naming ionic compounds, simply name the ions as they appear in the formula. When naming ionic compounds containing a transition metal, include the Roman numeral representing the charge.

44. Example: AlCl 3 KBr FeCl 2 FeCl 3 aluminum chloride potassium bromide iron(II) chloride iron(III) chloride

45. 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________________________

46. Solution Complete the names of the following binary compounds with variable metal ions: iron ( II ) bromide copper ( I ) chloride tin (IV) oxide iron (III) oxide mercury (I) sulfide FeBr 2 CuCl SnO 2 Hg 2 S Fe 2 O 3

47. Sample ION QUIZ: Sodium: _______ Selenide: ______ Iron (III): _______ Tin (IV): _______

48. Poly Atomic Ions Tightly bound groups of atoms that behave as a unit and carry a charge These atoms are held together by shared electrons Ions ending in –ite or –ate contain oxygen. –ite ions have one less oxygen than –ate.

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

50. Example: (–ite ions have one less oxygen than –ate) SO 3 2-, sulfite NO 2 -, nitrite SO 4 2-, sulfate NO 3 -, nitrate

51. When writing formulas containing polyatomic ions, use parentheses around multiple polyatomic ions. Ammonium carbonate NH 4 + CO 3 2- 2 1 (NH 4 ) 2 CO 3

52. strontium hydroxide Sr 2+ OH - 12 Sr(OH) 2

53. calcium nitrate Ca 2+ NO 3 - 1 2 Ca(NO 3 ) 2

54. aluminum phosphite Al 3+ PO 3 3- 33 AlPO 3

55. 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)

56. 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

57. 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)

58. Solution 1. aluminum nitrate c) Al(NO 3 ) 3 2. copper(II) nitrate b) Cu(NO 3 ) 2 3. Iron (III) hydroxide c) Fe(OH) 3 4. Tin(IV) hydroxide a) Sn(OH) 4

59. Naming Ternary Compounds Contains at least 3 elements 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

60. 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

61. Solution 1. Na 2 CO 3 MgSO 3 MgSO 4 2.Ca(HCO 3 ) 2 CaCO 3 Ca 3 (PO 4 ) 2 c) sodium carbonate a)magnesium sulfite b)magnesium sulfate c)calcium bicarbonate a)calcium carbonate b) calcium phosphate

62. Mixed Practice! Name the following: 1.Na 2 O 2.CaCO 3 3.PbS 2 4.Sn 3 N 2 5.Cu 3 PO 4 6.HgF 2 1.Sodium oxide 2.Calcium carbonate 3.Lead (IV) sulfide 4.Tin (II) nitride 5.Copper (I) phosphate 6.Mercury (II) fluoride

63. Mixed Up… The Other Way Write the formula: 1.Copper (II) chlorate 2.Calcium nitride 3.Aluminum carbonate 4.Potassium bromide 5.Barium fluoride 6.Cesium hydroxide Cu(ClO 3 ) 2 Ca 3 N 2 Al 2 (CO 3 ) 3 KBr BaF 2 CsOH

64. Naming Molecular Compounds CH 4 methane BCl 3 boron trichloride CO 2 Carbon dioxide All are formed from two or more nonmetals. Ionic compounds generally involve a metal and nonmetal (NaCl)

65. 6.5 Molecular Compounds and Acids Binary Molecular Compounds When naming binary molecular compounds, prefixes are used to tell how many of each atom is in the formula. CO 2 carbon dioxide N 2 O 4 dinitrogen tetroxide

66. Molecular (Covalent) Nomenclature for two nonmetals Prefix System (binary compounds) 1.Less electronegative atom comes first. 2.Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Mono- is OPTIONAL on the SECOND element (in this class, it’s NOT optional!). 3.Change the ending of the second element to -ide.

67. PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 Molecular Nomenclature Prefixes

68. CCl 4 N 2 O SF 6 carbon tetrachloride dinitrogen monoxide sulfur hexafluoride Molecular Nomenclature: Examples

69. arsenic trichloride dinitrogen pentoxide tetraphosphorus decoxide AsCl 3 N 2 O 5 P 4 O 10 More Molecular Examples

70. 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

71. Solution CO carbon monoxide CO 2 carbon dioxide PCl 3 phosphorus trichloride CCl 4 carbon tetrachloride N 2 Odinitrogen monoxide

72. 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

73. Solution 1.P 2 O 5 2. Cl 2 O 7 3. Cl 2 c) diphosphorus pentoxide a) dichlorine heptoxide a) chlorine

74. Overall strategy for naming chemical compounds.

75. A flow chart for naming binary compounds.

76. 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

77. 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

78. 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 1.N 2 O 2.K 2 S 3.Cu(NO 3 ) 2 4.Cl 2 O 7 5.Cr 2 (SO 4 ) 3 6.Fe 2 (SO 3 ) 3 7.CaO 8.BaCO 3 9.ICl

79. 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 1.Barium iodide 2.Tetraphosphorus trisulfide 3.Calcium hydroxide 4.Iron (II) carbonate 5.Sodium dichromate 6.Diiodine pentoxide 7.Copper (II) perchlorate 8.Carbon disulfide 9.Diboron tetrachloride

80. Acid Nomenclature AcidsAcids Compounds that form H + in water.Compounds that form H + in water. Formulas usually begin with ‘H’.Formulas usually begin with ‘H’. In order to be an acid instead of a gas, binary acids must be aqueous (dissolved in water)In order to be an acid instead of a gas, binary acids must be aqueous (dissolved in water) Ternary acids are ALL aqueousTernary acids are ALL aqueous Examples:Examples: HCl (aq) – hydrochloric acidHCl (aq) – hydrochloric acid HNO 3 – nitric acidHNO 3 – nitric acid H 2 SO 4 – sulfuric acidH 2 SO 4 – sulfuric acid

81. Acid Nomenclature Binary  Ternary An easy way to remember which goes with which… “In the cafeteria, you ATE something ICky”

82. Acid Nomenclature Flowchart

83. HBr (aq)HBr (aq) H 2 CO 3H 2 CO 3 H 2 SO 3H 2 SO 3 2 elements, -ide2 elements, -ide 3 elements, -ate3 elements, -ate 3 elements, -ite3 elements, -ite  hydrobromic acid  carbonic acid  sulfurous acid Acid Nomenclature

84. hydrofluoric acidhydrofluoric acid sulfuric acidsulfuric acid nitrous acidnitrous acid 2 elements2 elements 3 elements, -ic3 elements, -ic 3 elements, -ous3 elements, -ous  HF (aq)  H 2 SO 4  HNO 2 Acid Nomenclature  H + F-  H + SO 4 2-  H + NO 2 -

85. Name ‘Em! HI (aq)HI (aq) HClHCl H 2 SO 3H 2 SO 3 HNO 3HNO 3 HIO 4HIO 4 Hydroiodic acid Hydrogen chloride (not aq!) Sulfurous acid Nitric acid Periodic acid

86. Write the Formula! Hydrobromic acidHydrobromic acid Nitrous acidNitrous acid Carbonic acidCarbonic acid Phosphoric acidPhosphoric acid Hydrotelluric acidHydrotelluric acid HBr (aq) HNO 2 H 2 CO 3 H 3 PO 4 H 2 Te (aq)

87. Nomenclature Summary Flowchart

88. Now You Should Be Able To… Identify common elements and compounds using scientific nomenclature. Use: Common system Stock system, Prefix system, IUPAC nomenclature acid nomenclature WITH: common monatomic ion, common polyatomic ions AND: Binary compounds Ionic Molecular Acids Ternary compounds Ionic Acids

89. Now You Should Be Able To… Demonstrate (students performing) the use of symbols, formulas, and equations in describing interactions of matter such as chemical and nuclear reactions. Write formulas and equations with: Words only Formula equations Symbols in equations like, aq, s, l, g, etc. Use Empirical and molecular formulas

90. Now it’s Study Time DONE

91. Rainbow Matrix Game Link on Chemistry Geek.com on Chemistry I page http://chemistrygeek.com/rainbow Use [ ] to represent subscripts since you can’t enter subscripts into the computer So H 2 O would be H[2]O And Al 2 (SO 4 ) 3 would be Al[2](SO[4])[3] Additional Polyatomic Ions (you do not have to memorize these, but they are in the game!) Borate = BO 3 -3 ; Silicate = SiO 4 -4 ; Manganate = MnO 4 -2 (permanganate is -1)