2. Chemistry Chapter 7 Chemical Formulas and Chemical Compounds

3. Elements combine to form bonds Covalent Bonds -Electrons are shared -Usually between two non- metals EXAMPLE: carbon dioxide Ionic Bonds -Electrons are transferred -Usually between a metal and a non-metal or polyatomic ions EXAMPLE: sodium chloride Different systems of naming depending on the type of bond…BE CAREFUL!

4. Ions Ions Cation: A positive ion Cation: A positive ion Mg 2+, NH 4 + Mg 2+, NH 4 + Anion: A negative ion Anion: A negative ion Cl -, SO 4 2- Cl -, SO 4 2- Ionic Bonding: Force of attraction between oppositely charged ions. Ionic Bonding: Force of attraction between oppositely charged ions.

5. Predicting Ionic Charges Group 1: Lose 1 electron to form 1+ ions H+H+H+H+ Li + Na + K+K+K+K+

6. Na How many valence electrons does Na have?Does Na satisfy the octet rule? Bohr Model of Sodium How can we satisfy the octet rule?Now does Na satisfy the octet rule? How many protons does Na have? Protons: 11 How many electrons does Na have? Electrons: 11 What’s the net charge on Na? × +1 = 11 × -1 = -11 0 Now, how many electrons does Na have? Electrons: 10 × -1 = -10 +1 +

7. Predicting Ionic Charges Group 2: Loses 2 electrons to form form 2+ 2+ ions Be 2+ Mg 2+ Ca 2+ Sr 2+ Ba 2+

8. Mg Bohr Model of Magnesium How many valence electrons does Mg have?Does Mg satisfy the octet rule?How can we satisfy the octet rule?Now does Mg satisfy the octet rule? What is the net charge of Mg? Protons: 12 × +1 = 12 × -1 = -10 Electrons: 10 +2

9. Predicting Ionic Charges Group 13: Loses 3 Loses 3 electrons to form 3+ ions B 3+ Al 3+ Ga 3+

10. Al Bohr Model of Aluminum How many valence electrons does Al have?Does Al satisfy the octet rule?How can we satisfy the octet rule?Now does Al satisfy the octet rule? What is the net charge of Al? Protons: 13 × +1 = 13 × -1 = -10 Electrons: 10 +3

11. Predicting Ionic Charges Group 14: Lose 4 electrons or gain 4 electrons? Neither! Group 14 elements rarely form ions.

12. Predicting Ionic Charges Group 15: Gains 3 electrons Gains 3 electrons to form 3- ions to form 3- ions N 3- P 3- As 3- Nitride Phosphide Arsenide

13. P Bohr Model of Phosphorous How many valence electrons does P have? Does P satisfy the octet rule?How can we satisfy the octet rule? Now does P satisfy the octet rule? What is the net charge of P? Protons: 15 × +1 = 15 × -1 = -18 Electrons: 18 -3

14. Predicting Ionic Charges Group 16: Gains 2 electrons to form 2- ions O 2- S 2- Se 2- Oxide Sulfide Selenide

15. S Bohr Model of Sulfur How many valence electrons does S have? Does S satisfy the octet rule? How can we satisfy the octet rule?Now does S satisfy the octet rule? What is the net charge of S? Protons: 16 × +1 = 16 × -1 = -18 Electrons: 18 -2

16. Predicting Ionic Charges Group 17: Gains 1 electron Gains 1 electron to form 1- ions to form 1- ions F 1- Cl 1- Br 1- Fluoride Chloride Bromide I 1- Iodide

17. Cl Bohr Model of Chlorine How many valence electrons does Cl have?Does Cl satisfy the octet rule? How can we satisfy the octet rule? Now does Cl satisfy the octet rule? What is the net charge of Cl? Protons: 17 × +1 = 17 × -1 = -18 Electrons: 18

18. Predicting Ionic Charges Group 18: Stable Noble gases Stable Noble gases do not form ions! do not form ions!

19. Pause for a Cause #1 What is the oxidation number of each of the following elements? Ba Al S Br N F K

20. Predicting Ionic Charges Groups 3 - 12: Many transition elements have more Many transition elements have more than one possible oxidation state. than one possible oxidation state. Iron (II) = Fe 2+ Iron (III) = Fe 3+

21. Predicting Ionic Charges Groups 3 - 12: Some transition elements have only one Some transition elements have only one possible oxidation state. possible oxidation state. Zinc = Zn 2+ Silver = Ag + Cadmium = Cd 2+ Memorize

23. Polyvalent Elements and Their Charges to Memorize Copper Polyvalent ElementSymbolCharge Cu +1,+2 Lead Pb +2,+4 Iron Fe+2,+3 Mercury Hg,Hg 2 +1,+2 Tin Sn +2,+4 Chromium Cr +2,+3 Cobalt Nickel Co Ni ManganeseMn +2,+3

24. Polyatomic Ions to Memorize! +1 -2 Ammonium NH 4 +1 Acetate C 2 H 3 O 2 -1 Bromate BrO 3 -1 Chlorate ClO 3 -1 Chlorite ClO 2 -1 Cyanide CN -1 Bicarbonate HCO 3 -1 Hydroxide OH -1 Nitrate NO 3 -1 Nitrite NO 2 -1 Iodate IO 3 -1 Permanganate MnO 4 Hydrogen Sulfate HSO 4 Carbonate CO 3 -2 Chromate CrO 4 -2 Dichromate Cr 2 O 7 -2 Oxalate C 2 O 4 -2 Peroxide O 2 -2 Sulfate SO 4 -2 Sulfite SO 3 -2 Arsenate AsO 4 -3 Phosphate PO 4 -3 -3 Hand out Table

25. Writing Ionic Compound Formulas Example: Barium nitrate 1. Write the formulas for the cation and anion, including CHARGES! Ba NO 3 2. Check to see if charges are balanced. (If so, skip to step 5) 3. Balance charges, if necessary, using subscripts. A. Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion. B. Use parentheses if you need more than one of a polyatomic ion. Not balanced! ( ) 2 4. Check the subscripts and divide them by their largest common factor to give the smallest possible whole- number ratio. 5. Write the formula without the charges. 2+ - Ba(NO 3 ) 2

26. Writing Ionic Compound Formulas Example: Ammonium sulfate 1. Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. (If so, skip to step 5) 3. Balance charges, if necessary, using subscripts. A. Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion. B. Use parentheses if you need more than one of a polyatomic ion. 4. Check the subscripts and divide them by their largest common factor to give the smallest possible whole-number ratio. 5. Write the formula without the charges. NH 4 SO 4 Not balanced! ( ) 2 + 2- (NH 4 ) 2 SO 4

27. Let’s Practice 1. potassium nitrate 2. sodium sulfate 3. calcium hydroxide 4. ammonium sulfite 5. calcium phosphate 6. aluminum chromate 7. lithium bromide 8. sodium peroxide

28. Pause for a Cause #2 Page 251 16. Write formulas for each of the following compounds: a.sodium fluoride b.calcium oxide c.potassium sulfide d.magnesium chloride e.aluminum bromide f.lithium nitride

29. Writing Ionic Compound Formulas Example: Copper II carbonate 1.Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. (If so, skip to step 5) 5. Write the formula without the charges. Cu 2+ CO 3 2- They are balanced! CuCO 3

30. Writing Ionic Compound Formulas Example: Iron (III) chloride 1. Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. (If so, skip to step 5) 3. Balance charges, if necessary, using subscripts. A. Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion. B. Use parentheses if you need more than one of a polyatomic ion. 4. Check the subscripts and divide them by their largest common factor to give the smallest possible whole- number ratio. 5. Write the formula without the charges. FeCl Not balanced! 3 3+ - FeCl 3 Names ending in –ide usually, but not always, represent an element from the periodic table.

31. Writing Ionic Compound Formulas Example: Chromium III sulfide 1. Write the formulas for the cation and anion, including CHARGES! 2. Check to see if charges are balanced. (If so, skip to step 5) 3. Balance charges, if necessary, using subscripts. A. Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion. B. Use parentheses if you need more than one of a polyatomic ion. 4. Check the subscripts and divide them by their largest common factor to give the smallest possible whole-number ratio. 5. Write the formula without the charges. CrS Not balanced! 3 3+ 2- Cr 2 S 3 2

32. Write formulas for each of the following compounds. 1. Chromium III hydroxide 2. Mercury I chloride 3. Tin IV chloride 4. Iron II chromate 5. Cobalt II sulfide 6. Copper I sulfate 7. Iron III oxide Let’s Practice

33. Pause for a Cause #3 Writing Formulas of Compounds that have Roman Numerals Write the formulas for the following compounds:  Lead II nitrate  Iron II Sulfite  Mercury I Chloride  Tin II Chlorate  Chromium III Dichromate  Mercury II Phosphate  Cobalt II Acetate

34. Naming Covalent Binary Compounds - Compounds between two nonmetals - Compounds between two nonmetals -First element in the formula is named first. -First element in the formula is named first. -Second element is named as if it were an -Second element is named as if it were an anion. anion. -Use prefixes -Use prefixes -Only use mono on second element - -Only use mono on second element -

35. P 2 O 5 = CO 2 = CO = N 2 O = diphosphorus pentoxide carbon dioxide carbon monoxide dinitrogen monoxide 1 – mono 2 – di 3 – tri 4 – tetra 5 - penta 6 – hexa 7 – hepta 8 – octa 9 – nona 10 – deca

36. If given the formula…….. 1 st determine if the compound is a binary (molecular) compound – If all the elements in the compound are non-metals or metalloids the compound is a binary compound. – Use prefixes to name the compound. – CHARGES DON’T MATTER, DON’T WRITE CHARGES!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!! !!!!! – DON’T SWITCH THE PREFIXES!!!!!!!!!!!!!!!!!!!!

37. Pause for a Cause #4 Write the formula of the following compounds ( WRITE WHAT YOU SEE DO NOT CHECK OXIDATION STATE!) a.Phosphorus Pentachloride b.Carbon Tetrafluoride c.Dinitrogen Pentaoxide d.Tetraphosphorous Decaoxide e.Carbon Monoxide f.Carbon Disulfide

38. Sourvelis’s Rules For Naming Look at the first element in the compound. If the first element is… 1. A group 1 or 2 metal, or if it is Ag, Zn, Al, Cd, simply name the compound. NaCl  Sodium Chloride 2. A transitional metal all the way to the left of the metalloid line, use roman numerals. Fe 2 O 3  Iron (III) Oxide 3. A metalloid or nonmetal use prefixes. N 2 O 5  Dinotrogen Pentoxide 4. is hydrogen name it like an acid. HCl  Hydrochloric acid. Exception Acetic acid C 2 H 3 O 2 H 5. a carbon atom, name it as an organic molecule. ex. C 2 H 6  ethane Mixed Review Sheet

39. Naming Ionic Compounds Using Rule 1 Naming Ionic Compounds Using Rule 1 1. Cation first, then anion 1. Cation first, then anion 2. Monatomic cation = name of the element 2. Monatomic cation = name of the element Ca 2+ = calcium ion Ca 2+ = calcium ion 3. Monatomic anion = root + -ide 3. Monatomic anion = root + -ide Cl - = chloride Cl - = chloride CaCl 2 = calcium chloride CaCl 2 = calcium chloride 4. For polyatomic ions, use the name of that polyatomic ion.

40. Let’s Practice!! Name the following compounds: MgCl 2 Ag 2 O Ca(OH) 2 SrS KClO 3 NH 4 OH KClO 2 Magnesium Chloride Silver Oxide Calcium Hydroxide Strontium Sulfide Potassium Chlorate Ammonium Hydroxide Potassium Chlorite

41. Pause for a Cause #5 Name the following compounds: K 2 CrO 4 Ca(MnO 4 ) 2 Zn(HCO 3 ) 2 Mg 3 N 2 Na 2 O 2 Ba 3 (PO 4 ) 2 AgCl

42. If given the formula…….. And the compound is not a binary compound, name the compound like an ionic compound. – Use roman numerals if the first element is a transitional element or to the left of the metalloid line. (Exceptions Ag, Zn, Cd)

43. Naming Ionic Compounds Using Roman Numerals Naming Ionic Compounds Using Roman Numerals Example: PbCl 2 Lead can be a Pb 2+ or Pb 4+ cation PbCl 2 = lead (II) chloride How do you know??? Some metals have multiple oxidation states (Groups 3-12 and to the left of the metalloid line)

44. How do we know that lead was +2? PbCl 2 What is the charge of chlorine ion? How many chlorine ions does PbCl 2 have? What’s the total charge of the chlorine ions? -2 Compounds are neutral, so what must the charge of lead be in order to balance the -2 charge of chlorine? +2 The oxidation number of lead is +2.

45. Let’s try Fe 2 O 3 What is the charge of oxygen ion? How many oxygen ions does Fe 2 O 3 have? What’s the total charge of the oxygen ions? What must the charge of iron be in order to balance the -6 charge of the oxygens? Fe O 2 3 -2 -6 +6 +3 Iron III Oxide The oxidation number of iron is +3.

46. Let’s practice!!! Name the following compounds: CuO CoF 3 SnI 4 FeS Copper II Oxide Cobalt III Fluoride Tin IV Iodide Iron II Sulfide

47. If given the name….. If the compound is not a binary compound (contains polyatomic ions), use the rules for writing ionic compounds. – Make sure to use the correct charges. – Make sure you don’t change the subscripts of the polyatomic ions. – THE ANSWER DOES NOT HAVE ANY CHARGES!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!

48. Name the following compounds: Pb(ClO 3 ) 2 Co 2 O 3 Fe 2 (Cr 2 O 7 ) 3 NiBr 2 MnSO 4 SnO Hg 2 Cl 2 Fe(HCO 3 ) 3 Pause for a Cause #6

49. If given the name….. 1 st check for prefixes. – If prefixes are present, the compound is probably a binary compound. – DON’T WORRY ABOUT CHARGES, DON’T WRITE CHARGES, JUST WRITE WHAT YOU SEE!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!! – ***Remember some polyatomic ions have prefixes (bicarbonate, dichromate, dimercury). Write these like ionic compounds.

50. Pause for a Cause #7 Name the following compounds using prefixes: OF 2 SiO 2 SO 3 P2O5P2O5 BF 3 XeF 4

51. Quiz: Name the formula AgC 2 H 3 O 2 FeCl 3 N 2 O 4 Cr 2 O 3 FeCl 2

52. Quiz: Write the Formula sulfur tetrachloride ammonium carbonate chromium (III) oxide sodium peroxide Antimony (III) Chloride

53. Acid Nomenclature AcidsAcids –Compounds that form H + in water. –Formulas usually begin with ‘H’. –Exception is acetic acid CH 3 C00H Examples:Examples: –HCl (aq) – hydrochloric acid –HNO 3 – nitric acid –H 2 SO 4 – sulfuric acid

54. Acid Nomenclature Binary  Ternary 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 3 H 2 CO 3 H 2 SO 3 H 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 acid hydrofluoric acid sulfuric acid sulfuric acid nitrous acid nitrous 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. Binary Acids HF(aq) - HCl(aq) - HBr(aq) - HI(aq) - H 2 S(aq) - hydrofluoric acid hydrochloric acid hydrobromic acid hydriodic acid hydrosulfuric acid Exception, HI the “o” in hydro is left off for HI(aq), so its name is hydriodic acid. HCl(aq)  HCl(gas)

59. Name ‘Em! H 2 SO 3H 2 SO 3 HNO 3HNO 3 H 3 PO 4 CH 3 COOH sulfurous acid nitric acid phosphoric acid acetic acid

60. Write the Formula! Hydrobromic acidHydrobromic acid Nitrous acidNitrous acid Carbonic acidCarbonic acid Phosphoric acidPhosphoric acid HBr HNO 2 H 2 CO 3 H 3 PO 4

61. Straight Chains –Hydrocarbons linked in a straight chain C 8 H 18 Cyclochains –Hydrocarbon interlinked in a ring structure C 6 H 12

62. Hydrocarbons - molecules that possess hydrogen and carbon Alkanes – hydrocarbons with only C-C single bonds. Example: Butane CH 3 CH 2 CH 2 CH 3 C 4 H 10 C n H 2n+2 Alkenes – hydrocarbons with C=C double bonds. Example: Butene CH 3 CH=CHCH 3 C 4 H 8 C n H 2n Alkynes – hydrocarbons with C C triple bonds. Example: Butyne CH 3 C CCH 3 C 4 H 6 C n H 2n-2 Alcohols – R-OH (-OH is hydroxyl group, NOT hydroxide) Example: CH 3 OH Methanol

63. Basic Naming of Hydrocarbons Hydrocarbon names are based on: 1) type, 2) # of carbons, 3) side chain type and position 1) name will end in -ane, -ene, or -yne 2) the number of carbons is given by a “prefix” 1 meth- 2 eth- 3 prop- 4 but- 5 pent- 6 hex- 7 hept- 8 oct- 9 non- 10 dec- Actually, all end in a, but a is dropped when next to a vowel. E.g. a 6 C alkene is hexene Q - What names would be given to these: 7C, 9C alkane 2C, 4C alkyne 1C, 3C alkene heptane, nonane ethyne, butyne methene, propene

64. Mnemonic for First Four Prefixes First four prefixes Meth- Eth- Prop- But- Monkeys Eat Peeled Bananas

65. ? Decade Decimal Decathalon Other Prefixes Pent Hex Hep Oct Non Dec

66. Organic Compounds Containing Oxygen An alcohol is a compound obtained by substituting a hydroxyl group (-OH) for an –H atom on a carbon atom of a hydrocarbon group. Some examples are methanolethanolpropanol

67. Practice-Give the name or formula a.Butane b.Pentene c.Methanol d.C 2 H 4 e.C 7 H 15 OH 1, 3, 5-Cyclohexene Cyclopentane