1. Unit II Note pack, pages 9-13
Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids
Unit II Note pack, pages 9-13

2. Ionic Compounds Writing Formulas for Binary Ionic Compounds
1. What are Binary Ionic Compounds?
Binary compounds have just 2 elements.
Binary ionic compounds have 2 elements that are from opposite sides of the table, a cation and an anion.
(metal) (nonmetal)

3. Ionic Compounds
Writing Formulas for Binary Ionic Compounds
2. What are the “rules” for writing Binary Ionic Compounds?
Write the metal (positive) ion first
Write the nonmetal (negative) ion last
The net charge for the compound must add up to zero (total positive + total negative = 0)
Use subscripts to indicate how many of each ion you need to “balance” the charge.
CrissCross Method

4. Ionic Compounds Practice Writing Formulas for Binary Ionic Compounds
Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT.

5. Ionic Compounds Practice Writing Formulas for Binary Ionic Compounds
Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT.
Mg Cl-  MgCl Magnesium Chloride

6. Ionic Compounds Practice Writing Formulas for Binary Ionic Compounds
Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT.
Mg Cl-  MgCl Magnesium Chloride
Write the formula for the binary ionic compound formed between sodium and oxygen. Then NAME IT.

7. Ionic Compounds Practice Writing Formulas for Binary Ionic Compounds
Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT.
Mg Cl-  MgCl Magnesium Chloride
Write the formula for the binary ionic compound formed between sodium and oxygen. Then NAME IT.
Na O-2  Na2O Sodium Oxide

8. Ionic Compounds Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)
Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT.

9. Ionic Compounds Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)
Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT.
Al S  Al2S Aluminum sulfide

10. Ionic Compounds Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)
Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT.
Al S  Al2S Aluminum sulfide
Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT.

11. Ionic Compounds Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)
Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT.
Al S  Al2S Aluminum sulfide
Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT.
Fe O-2  Fe2O Iron (III) oxide

12. Ionic Compounds Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)
Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT.
Al S  Al2S Aluminum sulfide
Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT.
Fe O-2  Fe2O Iron (III) oxide
Write the formula for the binary ionic compound between calcium and sulfur, and NAME IT.

13. Ionic Compounds Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)
Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT.
Al S  Al2S Aluminum sulfide
Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT.
Fe O-2  Fe2O Iron (III) oxide
Write the formula for the binary ionic compound between calcium and sulfur, and NAME IT.
Ca S-2  CaS Calcium sulfide

14. Polyatomic Ions (pg 10) What is a polyatomic ion?
a tightly bound group of atoms that behaves as a unit and carries a charge
B. What endings to polyatomic ions receive when naming them?
most polyatomic ions receive endings of either –ite or –ate.

15. Polyatomic ions
C. There are 3 important exceptions (to the end of their names), they are:
Ammonium cation (NH4+)
Two polyatomic ions end in –ide;
cyanide (CN-) and
hydroxide (OH-)

16. Polyatomic Ions
For “D”, see Chart 6.4
Example:
Ammonium NH4+

17. Ternary Ionic Compounds
Define ternary ionic compounds:
A compound that contains atoms of three, or more, different elements
Remember, they are still just two ions, and all rules from before still apply.
Write the formula for lithium nitrate, a ternary compound.
Li NO3-  LiNO3

18. Ternary Ionic Compounds
C. Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al CO3-2 
E. Write the formula for ammonium sulfate:
F. Write the formula for calcium phosphate:

19. Ternary Ionic Compounds
C. Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al CO3-2  Al2(CO3)3
E. Write the formula for ammonium sulfate:
F. Write the formula for calcium phosphate:

20. Ternary Ionic Compounds
C. Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al CO3-2  Al2(CO3)3
E. Write the formula for ammonium sulfate:
NH SO4-2 
F. Write the formula for calcium phosphate:

21. Ternary Ionic Compounds
C. Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al CO3-2  Al2(CO3)3
E. Write the formula for ammonium sulfate:
NH SO4-2  (NH4)2SO4
F. Write the formula for calcium phosphate:

22. Ternary Ionic Compounds
C. Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al CO3-2  Al2(CO3)3
E. Write the formula for ammonium sulfate:
NH SO4-2  (NH4)2SO4
F. Write the formula for calcium phosphate:
Ca PO4-3 

23. Ternary Ionic Compounds
C. Sometimes, we need to take more than one polyatomic ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al CO3-2  Al2(CO3)3
E. Write the formula for ammonium sulfate:
NH SO4-2  (NH4)2SO4
F. Write the formula for calcium phosphate:
Ca PO4-3  Ca3(PO4)2

24. Ternary Ionic Compounds
Do this one on your own, and compare with a partner.
Write the formula for beryllium carbonate.

25. Ternary Ionic Compounds
Do this one on your own, and compare with a partner.
Write the formula for beryllium carbonate.
Be CO3-2  BeCO3
Beryllium ion + carbonate  beryllium carbonate

26. Practice Problems, pg. 11
Write the formulas for compounds formed AND name the compound from these pairs of ions:
NH4+1, SO32-
Calcium ion, phosphate ion

27. (NH4)2SO3 Ammonium Sulfite
Practice Problems, pg. 11
Write the formulas for compounds formed AND name the compound from these pairs of ions:
NH4+1, SO32-
(NH4)2SO3 Ammonium Sulfite
Calcium ion, phosphate ion

28. (NH4)2SO3 Ammonium Sulfite
Practice Problems, pg. 11
Write the formulas for compounds formed AND name the compound from these pairs of ions:
NH4+1, SO32-
(NH4)2SO3 Ammonium Sulfite
Calcium ion, phosphate ion
Ca+2 + PO4-3  Ca3(PO4)2
Calcium phosphate

29. Practice Problems, pg. 11
Write the formulas for compounds formed AND name the compound from these pairs of ions:
Al3+, NO3-1
d. Potassium ion, chromate ion

30. Al(NO3)3 Aluminum Nitrate
Practice Problems, pg. 11
Write the formulas for compounds formed AND name the compound from these pairs of ions:
Al3+, NO3-1
Al(NO3)3 Aluminum Nitrate
d. Potassium ion, chromate ion

31. Al(NO3)3 Aluminum Nitrate
Practice Problems, pg. 11
Write the formulas for compounds formed AND name the compound from these pairs of ions:
Al3+, NO3-1
Al(NO3)3 Aluminum Nitrate
d. Potassium ion, chromate ion
K+ + CrO4-2  K2CrO4
Potassium chromate

32. Practice Problems, pg. 11 Write formulas for these compounds
Lithium hydrogen sulfate __________
Chromium (III) nitrite ______________
Mercury (II) bromide ______________
Ammonium dichromate ___________

33. Practice Problems, pg. 11 Write formulas for these compounds
Lithium hydrogen sulfate _LiHSO4__
Chromium (III) nitrite _____________
Mercury (II) bromide ______________
Ammonium dichromate ___________

34. Practice Problems, pg. 11 Write formulas for these compounds
Lithium hydrogen sulfate _LiHSO4___
Chromium (III) nitrite __Cr(NO2)3_____
Mercury (II) bromide _______________
Ammonium dichromate ____________

35. Practice Problems, pg. 11 Write formulas for these compounds
Lithium hydrogen sulfate _LiHSO4__
Chromium (III) nitrite __Cr(NO2)3__
Mercury (II) bromide __HgBr2___
Ammonium dichromate _(NH4)2Cr2O7_

36. Section 6.5 Molecular Compounds and Acids (pg. 12)
Binary Molecular Compounds
What is a binary molecular compound?
A compound composed of 2 nonmetallic elements.

37. Section 6.5 Molecular Compounds and Acids
Binary Molecular Compounds
We use prefixes when naming binary molecular compounds: Refer to Table 6.5 and fill in the following:
Number Prefix Number Prefix 6 7 8 9 10

38. Section 6.5 Molecular Compounds and Acids
Binary Molecular Compounds
We use prefixes when naming binary molecular compounds: Refer to Table 6.5 and fill in the following:
Number Prefix Number Prefix
mono hexa-
di hepta-
tri octa-
tetra nona-
penta deca-

39. Section 6.5 Molecular Compounds and Acids
Binary Molecular Compounds
How do we name binary molecular compounds?
Say the name of the first element, say the name of the second element, ending in ‘-ide’, and put the appropriate prefix in to indicate how many of each element there are in the formula:
If the prefix for the first element in a binary molecular compound is mono-, it may be dropped. However, it must be said if it is for the second element.
Don’t reduce the subscripts (like you did for binary ionic compounds)

40. Name these binary molecular compounds.
N2O -- ___________________
PCl3 -- ___________________
SF6 -- _____________________
OF2 -- _____________________
Cl2O8 -- ___________________
SO3 -- ____________________

41. Name these binary molecular compounds.
N2O -- _dinitrogen monoxide__
PCl3 -- ______________________
SF6 -- ________________________
OF2 -- _______________________
Cl2O8 -- _____________________
SO3 -- ______________________

42. Name these binary molecular compounds.
N2O -- _dinitrogen monoxide__
PCl3 -- _phosphorus trichloride_
SF6 -- ______________________
OF2 -- _____________________
Cl2O8 -- ____________________
SO3 -- ____________________

43. Name these binary molecular compounds.
N2O -- _dinitrogen monoxide__
PCl3 -- _phosphorus trichloride_
SF6 -- _sulfur hexafluoride___
OF2 -- _____________________
Cl2O8 -- _____________________
SO3 -- ____________________

44. Name these binary molecular compounds.
N2O -- _dinitrogen monoxide__
PCl3 -- _phosphorus trichloride_
SF6 -- _sulfur hexafluoride___
OF2 -- _oxygen difluoride___
Cl2O8 -- _dichlorine octoxide__
SO3 -- _sulfur trioxide___

45. Write the formulas for the following binary molecular compounds.
Nitrogen trifluoride ________________
Disulfur dichloride ________________
Dinitrogen tetraoxide _______________
Octoxygen dichloride _______________
Trinitrogen pentoxide _______________

46. Write the formulas for the following binary molecular compounds.
Nitrogen trifluoride ___NF3__________
Disulfur dichloride ________________
Dinitrogen tetraoxide ______________
Octoxygen dichloride _______________
Trinitrogen pentoxide _______________

47. Write the formulas for the following binary molecular compounds.
Nitrogen trifluoride ___NF3__________
Disulfur dichloride ___S2Cl2________
Dinitrogen tetraoxide ______________
Octoxygen dichloride ______________
Trinitrogen pentoxide ______________

48. Write the formulas for the following binary molecular compounds.
Nitrogen trifluoride ___NF3__________
Disulfur dichloride ___S2Cl2________
Dinitrogen tetraoxide __N2O4________
Octoxygen dichloride _______________
Trinitrogen pentoxide ______________

49. Write the formulas for the following binary molecular compounds.
Nitrogen trifluoride ___NF3__________
Disulfur dichloride ___S2Cl2________
Dinitrogen tetraoxide __N2O4________
Octoxygen dichloride __O8Cl2_______
Trinitrogen pentoxide __N3O5_______

50. Naming Acids (pg. 12, bottom)
What are acids?
Acids are compounds that produce H ions (H+) when dissolved in water
B. Write the chart that explains how to name acids: (next)

51. Naming acids

52. Name the following acids
Begin by finding the name of the anion (not the H) from the periodic Table or Table 6.4, then follow the naming flow chart.
HClO =___________________________ ________________________________
HClO4 = _________________________ ________________________________

53. Name the following acids
Begin by finding the name of the anion (not the H) from the periodic Table or Table 6.4, then follow the naming flow chart.
HClO = ClO is hypochlorite _so the name for this acid is… ______________
HClO4 =_________________________ _______________________________

54. Name the following acids
Begin by finding the name of the anion (not the H) from the periodic Table or Table 6.4, then follow the naming flow chart.
HClO = ClO is hypochlorite _so the name for this acid is hypochlorous acid
HClO4 = _________________________ ________________________________

55. Name the following acids
Begin by finding the name of the anion (not the H) from the periodic Table or Table 6.4, then follow the naming flow chart.
HClO = ClO is hypochlorite _so the name for this acid is hypochlorous acid
HClO4 = ClO4 is perchlorate, so the name for this acid is…______________

56. Name the following acids
Begin by finding the name of the anion (not the H) from the periodic Table or Table 6.4, then follow the naming flow chart.
HClO = ClO is hypochlorite _so the name for this acid is hypochlorous acid
HClO4 = ClO4 is perchlorate, so the name for this acid is perchloric acid

57. Practice naming the following acids:
HCl = _________________________
HClO3 = _______________________
HClO2 = _______________________
HClO = ________________________
HClO4 = _______________________
H2S = ____________________
H2SO3 = ___________________
H2SO4 = ___________________
HC2H3O2 = ____________________

58. Practice naming the following acids:
HCl = ____Hydrochloric acid__________
HClO3 = ___________________________
HClO2 = ___________________________
HClO = ____________________________
HClO4 = ___________________________
H2S = _____________________________
H2SO3 = ___________________________
H2SO4 = ___________________________
HC2H3O2 = _________________________

59. Practice naming the following acids:
HCl = ____Hydrochloric acid__________
HClO3 = ____Chloric acid_____________
HClO2 = ___________________________
HClO = ____________________________
HClO4 = ___________________________
H2S = _____________________________
H2SO3 = ___________________________
H2SO4 = ___________________________
HC2H3O2 = _________________________

60. Practice naming the following acids:
HCl = ____Hydrochloric acid__________
HClO3 = ____Chloric acid_____________
HClO2 = ____Chlorous Acid ___________
HClO = ____________________________
HClO4 = ____________________________
H2S = ______________________________
H2SO3 = ____________________________
H2SO4 = ____________________________
HC2H3O2 = __________________________

61. Practice naming the following acids:
HCl = ____Hydrochloric acid__________
HClO3 = ____Chloric acid_____________
HClO2 = ____Chlorous Acid ___________
HClO = ____Hypochlorous acid _______
HClO4 = ___________________________
H2S = _____________________________
H2SO3 = ___________________________
H2SO4 = ___________________________
HC2H3O2 = _________________________

62. Practice naming the following acids:
HCl = ____Hydrochloric acid__________
HClO3 = __Chloric acid_____________
HClO2 = __Chlorous Acid __________
HClO = ___Hypochlorous acid _______
HClO4 = __Perchloric acid __________
H2S = _____________________________
H2SO3 = ___________________________
H2SO4 = ___________________________
HC2H3O2 = _________________________

63. Practice naming the following acids:
HCl = ____Hydrochloric acid__________
HClO3 = ____Chloric acid_____________
HClO2 = ____Chlorous Acid ___________
HClO = ____Hypochlorous acid ________
HClO4 = ___Perchloric acid __________
H2S = _____Hydrosulfuric acid _________
H2SO3 = ____________________________
H2SO4 = ____________________________
HC2H3O2 = __________________________

64. Practice naming the following acids:
HCl = ____Hydrochloric acid__________
HClO3 = ____Chloric acid_____________
HClO2 = ____Chlorous Acid ______________
HClO = ____Hypochlorous acid ________
HClO4 = ___Perchloric acid __________
H2S = _____Hydrosulfuric acid _________
H2SO3 = ___Sulfurous acid __________
H2SO4 = ____Sulfuric acid_____
HC2H3O2 = ___Acetic acid_________

65. Write the formula for the following acids:
Nitric acid ______________________
Hydronitric acid _________________
Nitrous acid ____________________
Hydrocyanic acid ________________
Phosphoric acid _________________
Hydrobromic acid ________________
Acetic acid _____________________

66. Write the formula for the following acids:
Nitric acid _____HNO3_____________
Hydronitric acid __________________
Nitrous acid _____________________
Hydrocyanic acid _________________
Phosphoric acid __________________
Hydrobromic acid _________________
Acetic acid ______________________
Nitric acid _______________________

67. Write the formula for the following acids:
Nitric acid _____HNO3______________
Hydronitric acid _H3N______________
Nitrous acid ______________________
Hydrocyanic acid __________________
Phosphoric acid ___________________
Hydrobromic acid __________________
Acetic acid _______________________
Nitric acid ________________________

68. Write the formula for the following acids:
Nitric acid _____HNO3_____________
Hydronitric acid _H3N______________
Nitrous acid __HNO2_______________
Hydrocyanic acid _________________
Phosphoric acid ___________________
Hydrobromic acid __________________
Acetic acid _______________________
Nitric acid _______________________

69. Write the formula for the following acids:
Nitric acid _____HNO3______________
Hydronitric acid _H3N_______________
Nitrous acid __HNO2_______________
Hydrocyanic acid ___HCN___________
Phosphoric acid ___________________
Hydrobromic acid __________________
Acetic acid _______________________
Nitric acid ________________________

70. Write the formula for the following acids:
Nitric acid _____HNO3______________
Hydronitric acid _H3N_______________
Nitrous acid __HNO2________________
Hydrocyanic acid ___HCN___________
Phosphoric acid __H3PO4____________
Hydrobromic acid __________________
Acetic acid _______________________
Nitric acid ________________________

71. Write the formula for the following acids:
Nitric acid _____HNO3______________
Hydronitric acid _HN3_______________
Nitrous acid __HNO2______________
Hydrocyanic acid ___HCN___________
Phosphoric acid __H3PO4____________
Hydrobromic acid _HBr______________
Acetic acid _______________________
Nitric acid ________________________

72. Write the formula for the following acids:
Nitric acid _____HNO3______________
Hydronitric acid _HN3_______________
Nitrous acid __HNO2________________
Hydrocyanic acid ___HCN___________
Phosphoric acid __H3PO4____________
Hydrobromic acid _HBr______________
Acetic acid __HC2H3O2____________
Nitric acid ______________________

73. Write the formula for the following acids:
Nitric acid _____HNO3______________
Hydronitric acid _HN3_______________
Nitrous acid __HNO2________________
Hydrocyanic acid ___HCN___________
Phosphoric acid __H3PO4____________
Hydrobromic acid _HBr______________
Acetic acid __HC2H3O2____________
Nitric acid ___HNO3_______________