2. Nomenclature PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion HC 2 H 3 O 2 Acetic Acid Chemistry : Chapter 9

3. Forms of Chemical Bonds There are 3 forms bonding atoms:There are 3 forms bonding atoms: Ionic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains)Ionic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) Covalent—some valence electrons shared between atomsCovalent—some valence electrons shared between atoms Metallic – holds atoms of a metal togetherMetallic – holds atoms of a metal together Most bonds are somewhere in between ionic and covalent.

4. 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

5. 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

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

7. 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.

8. http://www.angelo.edu/faculty/kbou drea/demos/sodiu m_chlorine/sodiu m_chlorine.htmhttp://www.angelo.edu/faculty/kbou drea/demos/sodiu m_chlorine/sodiu m_chlorine.htm

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

10. 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

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

12. Monatomic Ions

13. 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

14. 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

15. 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

16. 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:

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

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

19. 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

20. 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

21. 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

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

23. 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________________________

24. 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

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

26. You can make additional polyatomic ions by adding a H + to the ion! CO 3 -2 is carbonate HCO 3 – is hydrogen carbonate H 2 PO 4 – is dihydrogen phosphate HSO 4 – is hydrogen sulfate Polyatomic Ions

27. 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)

28. 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

29. 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)

30. 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

31. 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

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. 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

34. 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

35. 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

36. 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)

37. 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.

38. 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

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

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

41. 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

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

43. 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

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

45. Overall strategy for naming chemical compounds.

46. A flow chart for naming binary compounds.

47. 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

48. 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

49. 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

50. 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

53. 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

54. Acid Nomenclature Review No Oxygen  w/Oxygen An easy way to remember which goes with which… “In the cafeteria, you ATE something ICky”

55. Acid Nomenclature Flowchart

56. 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

57. 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 -

58. 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

59. 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)

60. Nomenclature Summary Flowchart

61. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. This flowchart provides you with a sequence of questions for naming a compound when you know its formula. Practicing Skills: Chemical Names and FormulasPracticing Skills: Chemical Names and Formulas Binary molecular Use prefixes in the name. Q = Group A? Name the ions. Q = Metal? Name the ions. yes no Name the ions; use a Roman numeral with the cation. Q = Group A? Name the ions; use a Roman numeral with the cation. Acid Review the rules given in Table 9.5. yes Q = H? > 2 Elements? no QxRyQxRy

62. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Apply the general formula Q x R y to each compound. Q and R can be atoms, monatomic ions, or polyatomic ions. Practicing Skills: Chemical Names and FormulasPracticing Skills: Chemical Names and Formulas Binary molecular Use prefixes in the name. Q = Group A? Name the ions. Q = Metal? Name the ions. yes no Name the ions; use a Roman numeral with the cation. Q = Group A? Name the ions; use a Roman numeral with the cation. Acid Review the rules given in Table 9.5. yes Q = H? > 2 Elements? no QxRyQxRy

63. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. For example, to name HNO 3, let H = Q and NO 3 = R. Follow the first arrow down to the question “Q = H?” The answer is yes, so the compound is an acid. Follow the rules for naming acids. Practicing Skills: Chemical Names and FormulasPracticing Skills: Chemical Names and Formulas Binary molecular Use prefixes in the name. Q = Group A? Name the ions. Q = Metal? Name the ions. yes no Name the ions; use a Roman numeral with the cation. Q = Group A? Name the ions; use a Roman numeral with the cation. Acid Review the rules given in Table 9.5. yes Q = H? > 2 Elements? no QxRyQxRy

64. Bases Ionic so Name the element followed by Hydroxide. NaOH KOH Ba(OH) 2

65. Now it’s Study Time DONE