1 Chemistry Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 10-14

1

ChemistrySection 6.4 Ionic Compounds

& Section 6.5 Molecular

Compounds and Acids

Unit II Note pack, pages 10-14

2

Ionic Compounds

A. Writing Formulas for Binary Ionic Compounds1. 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

A. Writing Formulas for Binary Ionic Compounds

2. What are the “rules” for writing Binary Ionic Compounds?

a. Write the metal (positive) ion first

b. Write the nonmetal (negative) ion last

c. The net charge for the compound must add up to zero (total positive + total negative = 0)

d. Use subscripts to indicate how many of each ion you need to “balance” the charge.

e. 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



Mg +2 + Cl- MgCl2 Magnesium Chloride

6

Ionic Compounds




Write the formula for the binary ionic compound formed between sodium and oxygen. Then NAME IT.

7

Ionic Compounds




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


(pg. 10)

Write the formula for the binary ionic compound between aluminum and sulfur, and NAME IT.

9

Ionic Compounds


(pg. 10)Write the formula for the binary ionic compound between aluminum

and sulfur, and NAME IT.

Al+3 + S-2 Al2S3 Aluminum sulfide

10

Ionic Compounds





Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT.

11

Ionic Compounds


(pg. 10)Write the formula for the binary ionic compound between aluminum and

sulfur, and NAME IT.



Fe+3 + O-2 Fe2O3 Iron (III) oxide

12

Ionic Compounds







Write the formula for the binary ionic compound between calcium and sulfur, and NAME IT.

13

Ionic Compounds


(pg. 10)Write the formula for the binary ionic compound between aluminum and

sulfur, and NAME IT.




Write the formula for the binary ionic compound between calcium and sulfur, and NAME IT.

Ca+2 + S-2 CaS Calcium sulfide

Please do the Practice Problems in the Note Pack,

pg. 11.

14

15

Polyatomic Ions (pg 11)

A. 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.

16

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-)

17

Polyatomic Ions

• For “D”, see Chart 6.4

• Example:

• Ammonium NH4+

With the person next to you, please do the “Reminder” at the

top of page 12.

18

19

Ternary Ionic Compounds

A. 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.

B. Write the formula for lithium nitrate, a ternary compound.

20






Li + + NO3-

21






Li + + NO3- LiNO3

22

Ternary Ionic CompoundsC. 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+3 + CO3-2

E. Write the formula for ammonium sulfate:

F. Write the formula for calcium phosphate:

23




Al+3 + CO3-2 Al2(CO3)3



24




Al+3 + CO3-2 Al2(CO3)3


NH4+ + SO4

-2


25




Al+3 + CO3-2 Al2(CO3)3


NH4+ + SO4

-2 (NH4)2SO4


26




Al+3 + CO3-2 Al2(CO3)3


NH4+ + SO4

-2 (NH4)2SO4


Ca+2 + PO4-3

27




Al+3 + CO3-2 Al2(CO3)3


NH4+ + SO4

-2 (NH4)2SO4


Ca+2 + PO4-3 Ca3(PO4)2

28


G. Do this one on your own, and compare with a partner.

Write the formula for beryllium carbonate.

29


G. Do this one on your own, and compare with a partner.

Write the formula for beryllium carbonate.

Be+2 + CO3-2 BeCO3

Beryllium ion + carbonate beryllium carbonate

30

Practice Problems, pg. 10

1. Write the formulas for compounds formed AND name the compound from these pairs of ions:

a. NH4+1, SO3

2-

b. Calcium ion, phosphate ion

31



a. NH4+1, SO3

2-

(NH4)2SO3 Ammonium Sulfite


32



a. NH4+1, SO3

2-

(NH4)2SO3 Ammonium Sulfite


Ca+2 + PO4-3 Ca3(PO4)2

Calcium phosphate

33



c. Al3+, NO3-1

d. Potassium ion, chromate ion

34



c. Al3+, NO3-1

Al(NO3)3 Aluminum Nitrate


35



c. Al3+, NO3-1

Al(NO3)3 Aluminum Nitrate


K+ + CrO4-2 K2CrO4

Potassium chromate

36


2. Write formulas for these compounds

a. Lithium hydrogen sulfate __________

b. Chromium (III) nitrite ______________

c. Mercury (II) bromide ______________

d. Ammonium dichromate ___________

37



a. Lithium hydrogen sulfate _LiHSO4__

b. Chromium (III) nitrite _____________

c. Mercury (II) bromide ______________

d. Ammonium dichromate ___________

38



a. Lithium hydrogen sulfate _LiHSO4___

b. Chromium (III) nitrite __Cr(NO2)3_____

c. Mercury (II) bromide _______________

d. Ammonium dichromate ____________

39



a. Lithium hydrogen sulfate _LiHSO4__

b. Chromium (III) nitrite __Cr(NO2)3__

c. Mercury (II) bromide __HgBr2___

d. Ammonium dichromate _(NH4)2Cr2O7_

40

Section 6.5 Molecular Compounds and Acids (pg. 12)

A. Binary Molecular Compounds

1. What is a binary molecular compound?

A compound composed of 2 nonmetallic elements.

41

Section 6.5 Molecular Compounds and Acids

A. Binary Molecular Compounds2. We use prefixes when naming binary molecular

compounds: Refer to Table 6.5 and fill in the following:

Number Prefix Number Prefix

1 6

2 7

3 8

4 9

5 10

42


A. Binary Molecular Compounds2. We use prefixes when naming binary molecular

compounds: Refer to Table 6.5 and fill in the following:

Number Prefix Number Prefix

1 mono- 6 hexa-

2 di- 7 hepta-

3 tri- 8 octa-

4 tetra- 9 nona-

5 penta- 10 deca-

43


A. Binary Molecular CompoundsHow 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)

44

Name these binary molecular compounds.

A. N2O -- ___________________

B. PCl3 -- ___________________

C. SF6 -- _____________________

D. OF2 -- _____________________

E. Cl2O8 -- ___________________

F. SO3 -- ____________________

45


A. N2O -- _dinitrogen monoxide__

B. PCl3 -- ______________________

C. SF6 -- ________________________

D. OF2 -- _______________________

E. Cl2O8 -- _____________________

F. SO3 -- ______________________

46



B. PCl3 -- _phosphorus trichloride_

C. SF6 -- ______________________

D. OF2 -- _____________________

E. Cl2O8 -- ____________________

F. SO3 -- ____________________

47




C. SF6 -- _sulfur hexafluoride___

D. OF2 -- _____________________

E. Cl2O8 -- _____________________

F. SO3 -- ____________________

48




C. SF6 -- _sulfur hexafluoride___

D. OF2 -- _oxygen difluoride___

E. Cl2O8 -- _dichlorine octoxide__

F. SO3 -- _sulfur trioxide___

49

Write the formulas for the following binary molecular compounds.

a. Nitrogen trifluoride ________________

b. Disulfur dichloride ________________

c. Dinitrogen tetraoxide _______________

d. Octoxygen dichloride _______________

e. Trinitrogen pentoxide _______________

50


a. Nitrogen trifluoride ___NF3__________

b. Disulfur dichloride ________________

c. Dinitrogen tetraoxide ______________


e. Trinitrogen pentoxide _______________

51



b. Disulfur dichloride ___S2Cl2________

c. Dinitrogen tetraoxide ______________

d. Octoxygen dichloride ______________

e. Trinitrogen pentoxide ______________

52




c. Dinitrogen tetraoxide __N2O4________


e. Trinitrogen pentoxide ______________

53




c. Dinitrogen tetraoxide __N2O4________

d. Octoxygen dichloride __O8Cl2_______

e. Trinitrogen pentoxide __N3O5_______

54

Naming Acids (pg. 14, top)

A. 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)

55

Naming acids

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 =___________________________ ________________________________

- HClO4 = _________________________ ________________________________

57



- HClO = ClO is hypochlorite _so the name for this acid is… ______________

- HClO4 =_________________________ _______________________________

58



- HClO = ClO is hypochlorite _so the name for this acid is hypochlorous acid

- HClO4 = _________________________ ________________________________

59




- HClO4 = ClO4 is perchlorate, so the name for this acid is…______________

60




- HClO4 = ClO4 is perchlorate, so the name for this acid is perchloric acid

61

Practice naming the following acids:

1. HCl = _________________________

2. HClO3 = _______________________

3. HClO2 = _______________________4. HClO = ________________________

5. HClO4 = _______________________

6. H2S = ____________________

7. H2SO3 = ___________________

8. H2SO4 = ___________________

9. HC2H3O2 = ____________________

62


1. HCl = ____Hydrochloric acid__________

2. HClO3 = ___________________________

3. HClO2 = ___________________________4. HClO = ____________________________

5. HClO4 = ___________________________

6. H2S = _____________________________

7. H2SO3 = ___________________________

8. H2SO4 = ___________________________

9. HC2H3O2 = _________________________

63



2. HClO3 = ____Chloric acid_____________

3. HClO2 = ___________________________4. HClO = ____________________________

5. HClO4 = ___________________________

6. H2S = _____________________________

7. H2SO3 = ___________________________

8. H2SO4 = ___________________________

9. HC2H3O2 = _________________________

64




3. HClO2 = ____Chlorous Acid ___________4. HClO = ____________________________

5. HClO4 = ____________________________

6. H2S = ______________________________

7. H2SO3 = ____________________________

8. H2SO4 = ____________________________

9. HC2H3O2 = __________________________

65




3. HClO2 = ____Chlorous Acid ___________4. HClO = ____Hypochlorous acid _______

5. HClO4 = ___________________________

6. H2S = _____________________________

7. H2SO3 = ___________________________

8. H2SO4 = ___________________________

9. HC2H3O2 = _________________________

66



2. HClO3 = __Chloric acid_____________

3. HClO2 = __Chlorous Acid __________4. HClO = ___Hypochlorous acid _______

5. HClO4 = __Perchloric acid __________

6. H2S = _____________________________

7. H2SO3 = ___________________________

8. H2SO4 = ___________________________

9. HC2H3O2 = _________________________

67




3. HClO2 = ____Chlorous Acid ___________4. HClO = ____Hypochlorous acid ________

5. HClO4 = ___Perchloric acid __________

6. H2S = _____Hydrosulfuric acid _________

7. H2SO3 = ____________________________

8. H2SO4 = ____________________________

9. HC2H3O2 = __________________________

68




3. HClO2 = ____Chlorous Acid ______________4. HClO = ____Hypochlorous acid ________

5. HClO4 = ___Perchloric acid __________

6. H2S = _____Hydrosulfuric acid _________

7. H2SO3 = ___Sulfurous acid __________

8. H2SO4 = ____Sulfuric acid_____

9. HC2H3O2 = ___Acetic acid_________

69

Write the formula for the following acids:

1. Nitric acid ______________________2. Hydronitric acid _________________3. Nitrous acid ____________________4. Hydrocyanic acid ________________5. Phosphoric acid _________________6. Hydrobromic acid ________________7. Acetic acid _____________________8. Nitric acid ______________________

70


1. Nitric acid _____HNO3_____________2. Hydronitric acid __________________3. Nitrous acid _____________________4. Hydrocyanic acid _________________5. Phosphoric acid __________________6. Hydrobromic acid _________________7. Acetic acid ______________________8. Nitric acid _______________________

71


1. Nitric acid _____HNO3______________

2. Hydronitric acid _H3N______________3. Nitrous acid ______________________4. Hydrocyanic acid __________________5. Phosphoric acid ___________________6. Hydrobromic acid __________________7. Acetic acid _______________________8. Nitric acid ________________________

72


1. Nitric acid _____HNO3_____________

2. Hydronitric acid _H3N______________

3. Nitrous acid __HNO2_______________4. Hydrocyanic acid _________________5. Phosphoric acid ___________________6. Hydrobromic acid __________________7. Acetic acid _______________________8. Nitric acid _______________________

73


1. Nitric acid _____HNO3______________

2. Hydronitric acid _H3N_______________

3. Nitrous acid __HNO2_______________4. Hydrocyanic acid ___HCN___________5. Phosphoric acid ___________________6. Hydrobromic acid __________________7. Acetic acid _______________________8. Nitric acid ________________________

74


1. Nitric acid _____HNO3______________

2. Hydronitric acid _H3N_______________

3. Nitrous acid __HNO2________________4. Hydrocyanic acid ___HCN___________

5. Phosphoric acid __H3PO4____________6. Hydrobromic acid __________________7. Acetic acid _______________________8. Nitric acid ________________________

75


1. Nitric acid _____HNO3______________

2. Hydronitric acid _HN3_______________

3. Nitrous acid __HNO2______________

4. Hydrocyanic acid ___HCN___________

5. Phosphoric acid __H3PO4____________

6. Hydrobromic acid _HBr______________

7. Acetic acid _______________________

8. Nitric acid ________________________

76


1. Nitric acid _____HNO3______________


3. Nitrous acid __HNO2________________4. Hydrocyanic acid ___HCN___________

5. Phosphoric acid __H3PO4____________6. Hydrobromic acid _HBr______________

7. Acetic acid __HC2H3O2____________8. Nitric acid ______________________

77


1. Nitric acid _____HNO3______________


3. Nitrous acid __HNO2________________

4. Hydrocyanic acid ___HCN___________

5. Phosphoric acid __H3PO4____________

6. Hydrobromic acid _HBr______________

7. Acetic acid __HC2H3O2____________

8. Nitric acid ___HNO3_______________

Documents

1 Chemistry Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 10-14