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

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

4. 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

5. PROPERTIES OF IONIC COMPOUNDS FORMING NaCl FROM Na AND Cl 2 A metal atom can transfer an electron to a nonmetal. The resulting cation and anion are attracted to each other by electrostatic forces.

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

7. SOME IONIC COMPOUNDS Mg 2+ + N -3 ----> Mg 3 N 2 Sn 4+ + O 2- ----> SnO 2 calcium fluoride Ca 2+ + 2 F - ---> CaF 2

8. 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

9. MONATOMIC IONS

10. WRITING A FORMULA Steps: 1. Write the formula for the cation and anion (Don’t forget to include the charge of each ion) 2. Decide how many cations and anions are needed so that the sum of their charges balance out to be zero 3. Write the formula of the compound by writing the number of cations followed by the number of anions which you used in step #2.

11. IN CLASS PRACTICE barium chloride

12. Iron (II) oxide

13. LEARNING CHECK Write the correct formula for the compounds containing the following ions: 1. sodium sulfide a) NaS b) Na 2 Sc) NaS 2 2. aluminum chloride a) AlCl 3 b) AlCl c) Al 3 Cl 3. magnesium nitride a) MgN b) Mg 2 N 3 c) Mg 3 N 2

14. 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

15. NAMING COMPOUNDS 1.Separate the compound into its positive and negative parts (positive part will be the first element, negative part will be the second element) 2.Write the name of the cation and then the name of the anion Monatomic cation = name of the element Ca 2+ = calcium ion Monatomic anion = root + -ide Cl  = chloride CaCl 2 = calcium chloride Binary Ionic Compounds:

16. 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

17. 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!) 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

18. EXAMPLES OF OLDER NAMES OF CATIONS FORMED FROM TRANSITION METALS (YOU DO NOT HAVE TO MEMORIZE THESE)

19. NAMING BINARY IONIC COMPOUNDS Examples: NaCl ZnI 2 Al 2 O 3 sodium chloride zinc iodide aluminum oxide

20. IN CLASS PRACTICE ZnO

21. SrCl 2

22. Ag 2 S

23. NiP

24. LEARNING CHECK Complete the names of the following binary compounds: Na 3 Nsodium ________________ KBrpotassium________________ Al 2 O 3 aluminum ________________ MgS_________________________

25. 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________________________

26. 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)

27. 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

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. 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

31. 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

32. 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

33. 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)

34. 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.

35. 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

36. CCl 4 N 2 O SF 6 carbon tetrachloride dinitrogen monoxide sulfur hexafluoride MOLECULAR NOMENCLATURE: EXAMPLES

37. arsenic trichloride dinitrogen pentoxide tetraphosphorus decoxide AsCl 3 N 2 O 5 P 4 O 10 MORE MOLECULAR EXAMPLES

38. 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

39. 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

40. OVERALL STRATEGY FOR NAMING CHEMICAL COMPOUNDS.

41. A FLOW CHART FOR NAMING BINARY COMPOUNDS.

42. 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

43. 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

44. 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

45. 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

46. ACID NOMENCLATURE Acids  Compounds that form H + in water.  Formulas usually begin with ‘H’.  In order to be an acid instead of a gas, acids must be aqueous (dissolved in water) Examples:  HCl (aq) – hydrochloric acid  HNO 3 – nitric acid  H 2 SO 4 – sulfuric acid

47. ACID NOMENCLATURE REVIEW No Oxygen  w/Oxygen An easy way to remember which goes with which… “In the cafeteria, you ATE something ICky”

48. ACID NOMENCLATURE FLOWCHART

49. HBr (aq)HBr (aq) H 2 CO 3H 2 CO 3 H 2 SO 3H 2 SO 3 No oxygen, -ideNo oxygen, -ide Has oxygen, -ateHas oxygen, -ate Has oxygen, -iteHas oxygen, -ite  hydrobromic acid  carbonic acid  sulfurous acid ACID NOMENCLATURE

50. 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 -

51. NAME ‘EM! HI (aq) HCl H 2 SO 3 HNO 3 HIO 4

52. WRITE THE FORMULA! Hydrobromic acid Nitrous acid Carbonic acid Phosphoric acid

53. Nomenclature Summary Flowchart

54. NOW IT’S STUDY TIME DONE

55. 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)