1. LecturePLUS Timberlake1 ChemIH: Chapters 6 & 7 Covalent Bonding Def: bonds btwn 2 or more nonmetals Nonmetals have high EN values so electrons must be shared Compounds w/covalent bonds are called molecular compounds. We will learn about 4 types of molecular cpds.

2. 1. Acids Acids are covalent compounds that act like ionic compounds. They have H+ as the “cation”. LecturePLUS Timberlake2

3. Acids There are 3 types of acids. They are named based on the type of ANION they contain: 1.Anion = element 2.Anion = polyatomic ion that ends in “ate” 3.Anion = polyatomic ion that ends in “ite” LecturePLUS Timberlake3

4. Acids 1. If anion is an element, name of acid is “hydro____ic acid” where blank is filled with root of element name Ex: HCl LecturePLUS Timberlake4 Hydrochloric acid

5. Acids 2. If anion is a polyatomic ion that ends in “-ate”, name of acid is “____ic acid” where blank is filled with root of polyatomic ion name Ex: HClO 3 LecturePLUS Timberlake5 chloric acidClO 3 = “chlorate”

6. Acids 3. If anion is a polyatomic ion that ends in “-ite”, name of acid is “____ous acid” where blank is filled with root of element name Ex: HClO 2 LecturePLUS Timberlake6 chlorous acidClO 2 = “chlorite”

7. Acids, Summary LecturePLUS Timberlake7 Type of Anion Naming ruleExample ElementHydro___ic acidHCl: hydrochloric acid Polyatomic “-ate” ____ic acidHClO 4 : perchloric acid Polyatomic “-ite” ____ous acidHClO: hypochlorous acid

8. Covalent Bonding single bond shares 1 pair electrons- ex:H 2 double bond shares 2 pairs electron-ex:O 2 triple bond shares 3 pairs electrons-ex: N 2 LecturePLUS Timberlake8

9. 9 Covalent Bonding By sharing e-s, atoms obtain NGC, which makes them more stable than they were by themselves. H  +  H H : H = H  H = H 2 hydrogen molecule

10. LecturePLUS Timberlake10 Learning Check Indicate whether a bond between the following would be (I) Ionic OR (C) covalent ____A. sodium & oxygen ____B. nitrogen & oxygen ____C. phosphorus & chlorine ____D. calcium & sulfur ____E. chlorine & bromine

11. LecturePLUS Timberlake11 Solution Indicate whether a bond between the following would be (I) Ionic OR (C) covalent IA. sodium and oxygen CB. nitrogen and oxygen CC. phosphorus and chlorine ID. calcium and sulfur CE. chlorine and bromine

12. There are 4 types of molecular substances we will learn about. LecturePLUS Timberlake12

13. LecturePLUS Timberlake13 2. Diatomic Elements Elements that exist as atom pairs : H 2, O 2, N 2, Cl 2, Br 2, I 2, F 2, They are given the name of the element. octets          N  +  N   N ::: N   triple bond

14. LecturePLUS Timberlake14 Learning Check Use the name of the element to name a diatomic molecules. H 2 hydrogen N 2 nitrogen Cl 2 _______________ O 2 _______________ I 2 _______________

15. LecturePLUS Timberlake15 Solution Use the name of the element to name the following diatomic molecules. H 2 hydrogen N 2 nitrogen Cl 2 chlorine O 2 oxygen I 2 iodine

16. LecturePLUS Timberlake16 2. Binary Covalent Compounds Two nonmetals (def of binary covalent) 1.Name each element 2.End the last element in -ide 3.Add prefixes to show how many atoms of each (except when there’s only 1 atom of the 1 st element listed) PREFIXES mono1 hexa6 di2hepta7 tri3octa8 tetra4nona9 penta5deca10

17. LecturePLUS Timberlake17 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

18. LecturePLUS Timberlake18 Solution CO carbon monoxide CO 2 carbon dioxide PCl 3 phosphorus trichloride CCl 4 carbon tetrachloride N 2 Odinitrogen monoxide

19. LecturePLUS Timberlake19 Learning Check A.P 2 O 5 1) phosphorus oxide 2) phosphorus pentoxide 3) diphosphorus pentoxide B.Cl 2 O 7 1) dichlorine heptoxide 2) dichlorine oxide 3) chlorine heptoxide C. Cl 2 1) chlorine 2) dichlorine 3) dichloride

20. LecturePLUS Timberlake20 Solution A.P 2 O 5 3) diphosphorus pentoxide B.Cl 2 O 7 1) dichlorine heptoxide C. Cl 2 1) chlorine

21. 3. Hydrocarbons-A Type of Binary Covalent Compound Def: hydrocarbons are made of hydrogen & carbon They are named by the number of carbon atoms a molecule contains. They are important as fuels.

22. Hydrocarbons The table below lists only hydrocarbons w/single bonds\ The names all end w/ “ane” CH 4 methaneC 6 H 14 hexane C 2 H 6 ethaneC 7 H 16 heptane C 3 H 8 propaneC 8 H 18 octane C 4 H 10 butaneC 9 H 20 nonane C 5 H 12 pentaneC 10 H 22 decane

23. Writing Formulas for Molecular Compounds 1. Analyze the name of the compound 2. Identify the type of compound (diatomic? binary? hydrocarbon?) 3. Reverse the process used to name it so you can determine the formula. LecturePLUS Timberlake23

24. Tips for Identifying TYPE of Molecular Compound IF THE NAME HAS:TYPE OF COMPOUND HOW TO WRITE FORMULA Just the name of 1of Diatomic Element H 2, O 2, N 2, Cl 2, the following elements: Br 2, I 2, F 2 (HONClBrIF) Prefixes Binary (2 elements) Turn prefixes into Ends in “-ide” subscripts. (Write them after element symbol) Ends in “-ane” Hydrocarbon Look it up on list of hydrocarbons! LecturePLUS Timberlake24

25. Common v. Formal Names Formal Names follow the rules we have learned for naming compounds. Common Names are ones that don’t follow these rules. –Ex: water=

26. Frequently Used Common Names Water = H 2 O Ammonia = NH 3

27. LecturePLUS Timberlake27 Covalent Bonds in NH 3 Bonding pairs H  H : N : H  Lone pair of electrons

28. Allotropes Def: molecules of the same element that differ in structure Ex 1: Carbon…graphite, charcoal, Buckminsterfullerine (“bucky ball”)= C 64 Ex 2: O 2 (oxygen) and O 3 (ozone)

29. Q:Why do we have to specify the number of atoms of each element in a covalent compound? A: Atoms of the same elements can combine in different ratios. Ex: C & O CO CO 2

30. Writing Formulas for Covalent Compounds 1. Identify it as a covalent: containing only nonmetals. 2. Determine what type of covalent it is: diatomic elementbinary hydrocarbon (ends in –ane)acid/base 3. Reverse the naming process. LecturePLUS Timberlake30

31. STOP HERE!!! LecturePLUS Timberlake31

32. Naming Ionic Compounds Binary Ionic Ionic Compounds contain- ing Polyatomic Ions. Ionic Cpds containing Transition Metals LecturePLUS Timberlake32

33. PLEASE NOTE: IF YOU ARE UNABLE TO IDENTIFY IONIC & COVALENT COMPOUNDS, YOU WILL BE LOST!!! PLEASE SEE ME IMMEDIATELY TO GET CAUGHT UP. LecturePLUS Timberlake33

34. LecturePLUS Timberlake34 Ionic Bonding & Electronegativity Nonmetals have high EN’s. Metals have low EN’s. Bonds between a metal & a nonmetal involve transfers of e-s b/c of the big difference in EN!

35. Binary Ionic Compounds Binary= 2 elements Ionic= 1 metal & 1 nonmetal LecturePLUS Timberlake35

36. Naming Binary Ionic Compounds 1. Name the cation, which is the given the name of the element. 2. Name the anion, which is given the name of the element, w/the ending changed to “–ide.” LecturePLUS Timberlake36

37. PRACTICE Naming Binary Ionic Compounds 1. Na║Cl 2. Na = “sodium” 3. Cl = “chloride” (full name is “sodium chloride”) LecturePLUS Timberlake37

38. PRACTICE Naming Binary Ionic Compounds 1. Li 2 O 2 & 3. ____║____= ______ ______ ( cation (anion (cation name) (anion name) symbol) symbol) LecturePLUS Timberlake38

39. MORE PRACTICE Naming Binary Ionic Compounds-p __ of I.N. 1.KF 2.CaF 2 3.Al 2 O 3 LecturePLUS Timberlake39

40. Naming Ionic Compounds w/ Polyatomic Ions DEF: Charged particles containing more than 1 type of atom. Ex: SO 4 2- LecturePLUS Timberlake40

41. Naming Ionic Compounds w/ Polyatomic Ions 1.Identify the cation & the anion. (Draw a line between the 2 ions) 2.Name the cation, then the anion (find polyatomics on Table 5.3, p 159 of text). That’s it! LecturePLUS Timberlake41

42. PRACTICE :Naming Ionic Compounds w/ Polyatomic Ions EX: Na 2 SO 4 ____║____= ______ ______ ( cation (anion (cation name) (anion name) symbol) symbol) LecturePLUS Timberlake42

43. Naming Ionic Compounds w/ Polyatomic Ions Most polyatomic ions are anions. LecturePLUS Timberlake43

44. A Couple of Important Exceptions w/Polyatomic Ions Important Exception #1: there are 2 cations that contain NO METALS: NH 4 + (ammonium) H 3 O + (hydronium) (this can be tricky b/c we have always identified ionic compounds because they start with a metal cation.) LecturePLUS Timberlake44

45. A Couple of Important Exceptions w/Polyatomic Ions Important Exception #2: Some anions contain metals. Ex: MnO 4 - = permanganate Cr 2 O 7 2- = dichromate (this can be tricky b/c anions are usually a nonmetal) LecturePLUS Timberlake45

46. Copy Table 5.2 into Notes LecturePLUS Timberlake46

47. Naming Ionic Cpds Containing Transition Metals Ex: NiO 2 1.Determine the total # of negative charges in a unit of the compound: Ex: O 2- & O 2- = 4 total - charges 2. Determine the charge on the cation that will give you 4 total + charges Ex: Ni 4+ 3. Write the cation & anion names. Write cation with the oxidation # written as a Roman numeral in parentheses: Ex: nickel (IV) oxide LecturePLUS Timberlake47

48. Writing Formulas for Binary Ionic Compounds 1. Identify the ionic charge (“oxidation number”) on the cation & anion. LecturePLUS Timberlake48

49. Writing Formulas for Binary Ionic Compounds ELEMENTOXIDATION # Group 11+ Group 22+ Group 133+ Group 144+ or 4- Group 153- Group 162- Group 171- LecturePLUS Timberlake49

50. Practice Predicting Oxidation #s Li O Mg F B LecturePLUS Timberlake50

51. Writing Formulas for Binary Ionic Compounds 2. A compound has NO CHARGE on it, so a formula unit (the smallest ratio of cations to anions) must have equal numbers of + & - charges. (use the LCM) LecturePLUS Timberlake51

52. Cross-Over Method You can use this to write formulas. Take the charge on the cation and use it as the subscript on the anion Take the charge on the anion and use it as the subscript on the cation Reduce the subscripts, if necessary LecturePLUS Timberlake52

53. Using the LCM to Write Ionic Formulas Ex: Li & F Ex: Li & O Ex: Al & O LecturePLUS Timberlake53

54. ANSWERS LiF Li 2 O Al 2 O 3 LecturePLUS Timberlake54

55. Writing Formulas for I.Cpds Containing Polyatomic Ions Determine the cation & anion Determine the oxidation # on each ion. (oxidation #s for polyatomics are found on Table 5.2) Write a balanced formula –If there is more than 1 of an ion, use parentheses, then a subscript LecturePLUS Timberlake55

56. Writing Formulas for I.Cpds Containing Polyatomic Ions Ex: see Practice Problems, p 162 3. Write the formula for the compound formed from the following pairs of ions a) ammonium & sulfite ions IONS: NH 4 + & SO 3 2- NH 4 + FORMULA: (NH 4 ) 2 SO 3 LecturePLUS Timberlake56

57. Practice Problems, cont. from p 16 2of text 3b) 3c) 3d) 4a) 4b) 4c) 4d) LecturePLUS Timberlake57

58. Transition Metals QUESTION: What was strange about the e- configurations of transition metals? LecturePLUS Timberlake58 ANSWER: Their d sublevels overlap with the other sublevels in the next higher main E.L.

59. Oxidation #s of Transition Metals The d sublevel e-s are so close to the actual valence e-s, they sometimes act like valence e-s! See Table 5.4 on p 164 of text: Common Ions of Select Transition Metals Ex: Fe 2+ & Fe 3+ Write the e- configuration LecturePLUS Timberlake59

60. e- Configuration for Fe Fe=26 e-s 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 Valence e-s=4s 2 BUT, some 3d e-s can be lost too! NOTE: Students found this a bit confusing, or at best minimally helpful. Explain, but do not belabor the e- config. LecturePLUS Timberlake60

61. Writing Formulas for Ionic Cpds containing Transition Metals 1. Identify the cation & anion 2. Determine the oxidation #s on the cation & anion –The oxidation # of the cation is given in the name ex: Nickel (IV) = Ni 4+ –The Roman numeral is the oxidation# 3. Write a formula w/ 0 charge. LecturePLUS Timberlake61

62. Distillation Def: process of separating ionic & covalent compounds by heating them till the covalent compound evaporates. –The ionic compound remains in the flask –The covalent compound can be cooled & collected in a separate container. –This process is called distillation

63. LecturePLUS Timberlake63 Learning Check Match each set with the correct name: A. Na 2 CO 3 1) magnesium sulfite MgSO 3 2) magnesium sulfate MgSO 4 3) sodium carbonate B.Ca(HCO 3 ) 2 1) calcium carbonate CaCO 3 2) calcium phosphate Ca 3 (PO 4 ) 2 3) calcium bicarbonate

64. LecturePLUS Timberlake64 Solution A. Na 2 CO 3 3) sodium carbonate MgSO 3 1) magnesium sulfite MgSO 4 2) magnesium sulfate B.Ca(HCO 3 ) 2 3) calcium bicarbonate CaCO 3 1) calcium carbonate Ca 3 (PO 4 ) 2 2) calcium phosphate

65. LecturePLUS Timberlake65 Learning Check A. aluminum nitrate 1) AlNO 3 2) Al(NO) 3 3) Al(NO 3 ) 3 B. copper(II) nitrate 1) CuNO 3 2) Cu(NO 3 ) 2 3) Cu 2 (NO 3 ) C. Iron (III) hydroxide 1) FeOH2) Fe 3 OH3) Fe(OH) 3 D. Tin(IV) hydroxide 1) Sn(OH) 4 2) Sn(OH) 2 3) Sn 4 (OH)

66. LecturePLUS Timberlake66 Solution A. aluminum nitrate 3) Al(NO 3 ) 3 B. copper(II) nitrate 2) Cu(NO 3 ) 2 C. Iron (III) hydroxide 3) Fe(OH) 3 D. Tin(IV) hydroxide 1) Sn(OH) 4