Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids

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Chemistry 102Section 6.4 Ionic Compounds

& Section 6.5 Molecular

Compounds and Acids

Unit II Note pack, pages 9-13

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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)

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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

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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.

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Ionic Compounds



Mg +2 + Cl- MgCl2 Magnesium Chloride

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Ionic Compounds




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

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Ionic Compounds




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

Na+ + O-2 Na2O Sodium Oxide

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Ionic Compounds


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

NAME IT.

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Ionic Compounds



NAME IT.

Al+3 + S-2 Al2S3 Aluminum sulfide

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Ionic Compounds



NAME IT.


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

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Ionic Compounds



NAME IT.



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

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Ionic Compounds



NAME IT.




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

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Ionic Compounds



NAME IT.




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

Ca+2 + S-2 CaS Calcium sulfide

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Polyatomic Ions (pg 10)

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.

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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-)

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Polyatomic Ions

• For “D”, see Chart 6.4

• Example:

• Ammonium NH4+

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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.

Li + + NO3- LiNO3

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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:

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



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


NH4+ + SO4

-2


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


NH4+ + SO4

-2 (NH4)2SO4


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


NH4+ + SO4

-2 (NH4)2SO4


Ca+2 + PO4-3

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


NH4+ + SO4

-2 (NH4)2SO4


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

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

Write the formula for beryllium carbonate.

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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

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Practice Problems, pg. 11

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

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a. NH4+1, SO3

2-

(NH4)2SO3 Ammonium Sulfite


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a. NH4+1, SO3

2-

(NH4)2SO3 Ammonium Sulfite


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

Calcium phosphate

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c. Al3+, NO3-1

d. Potassium ion, chromate ion

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c. Al3+, NO3-1

Al(NO3)3 Aluminum Nitrate


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c. Al3+, NO3-1

Al(NO3)3 Aluminum Nitrate


K+ + CrO4-2 K2CrO4

Potassium chromate

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2. Write formulas for these compounds

a. Lithium hydrogen sulfate __________

b. Chromium (III) nitrite ______________

c. Mercury (II) bromide ______________

d. Ammonium dichromate ___________

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a. Lithium hydrogen sulfate _LiHSO4__

b. Chromium (III) nitrite _____________

c. Mercury (II) bromide ______________

d. Ammonium dichromate ___________

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a. Lithium hydrogen sulfate _LiHSO4___

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

c. Mercury (II) bromide _______________

d. Ammonium dichromate ____________

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a. Lithium hydrogen sulfate _LiHSO4__

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

c. Mercury (II) bromide __HgBr2___

d. Ammonium dichromate _(NH4)2Cr2O7_

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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.

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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

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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-

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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)

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Name these binary molecular compounds.

A. N2O -- ___________________

B. PCl3 -- ___________________

C. SF6 -- _____________________

D. OF2 -- _____________________

E. Cl2O8 -- ___________________

F. SO3 -- ____________________

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A. N2O -- _dinitrogen monoxide__

B. PCl3 -- ______________________

C. SF6 -- ________________________

D. OF2 -- _______________________

E. Cl2O8 -- _____________________

F. SO3 -- ______________________

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B. PCl3 -- _phosphorus trichloride_

C. SF6 -- ______________________

D. OF2 -- _____________________

E. Cl2O8 -- ____________________

F. SO3 -- ____________________

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C. SF6 -- _sulfur hexafluoride___

D. OF2 -- _____________________

E. Cl2O8 -- _____________________

F. SO3 -- ____________________

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C. SF6 -- _sulfur hexafluoride___

D. OF2 -- _oxygen difluoride___

E. Cl2O8 -- _dichlorine octoxide__

F. SO3 -- _sulfur trioxide___

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Write the formulas for the following binary molecular compounds.

a. Nitrogen trifluoride ________________

b. Disulfur dichloride ________________

c. Dinitrogen tetraoxide _______________

d. Octoxygen dichloride _______________

e. Trinitrogen pentoxide _______________

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a. Nitrogen trifluoride ___NF3__________

b. Disulfur dichloride ________________

c. Dinitrogen tetraoxide ______________


e. Trinitrogen pentoxide _______________

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b. Disulfur dichloride ___S2Cl2________

c. Dinitrogen tetraoxide ______________

d. Octoxygen dichloride ______________

e. Trinitrogen pentoxide ______________

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c. Dinitrogen tetraoxide __N2O4________


e. Trinitrogen pentoxide ______________

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c. Dinitrogen tetraoxide __N2O4________

d. Octoxygen dichloride __O8Cl2_______

e. Trinitrogen pentoxide __N3O5_______

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Naming Acids (pg. 12, bottom)

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)

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Naming acids

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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 = _________________________ ________________________________

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

- HClO4 =_________________________ _______________________________

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

- HClO4 = _________________________ ________________________________

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

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

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Practice naming the following acids:

1. HCl = _________________________

2. HClO3 = _______________________

3. HClO2 = _______________________4. HClO = ________________________

5. HClO4 = _______________________

6. H2S = ____________________

7. H2SO3 = ___________________

8. H2SO4 = ___________________

9. HC2H3O2 = ____________________

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1. HCl = ____Hydrochloric acid__________

2. HClO3 = ___________________________

3. HClO2 = ___________________________4. HClO = ____________________________

5. HClO4 = ___________________________

6. H2S = _____________________________

7. H2SO3 = ___________________________

8. H2SO4 = ___________________________

9. HC2H3O2 = _________________________

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2. HClO3 = ____Chloric acid_____________

3. HClO2 = ___________________________4. HClO = ____________________________

5. HClO4 = ___________________________

6. H2S = _____________________________

7. H2SO3 = ___________________________

8. H2SO4 = ___________________________

9. HC2H3O2 = _________________________

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3. HClO2 = ____Chlorous Acid ___________4. HClO = ____________________________

5. HClO4 = ____________________________

6. H2S = ______________________________

7. H2SO3 = ____________________________

8. H2SO4 = ____________________________

9. HC2H3O2 = __________________________

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

5. HClO4 = ___________________________

6. H2S = _____________________________

7. H2SO3 = ___________________________

8. H2SO4 = ___________________________

9. HC2H3O2 = _________________________

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2. HClO3 = __Chloric acid_____________

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

5. HClO4 = __Perchloric acid __________

6. H2S = _____________________________

7. H2SO3 = ___________________________

8. H2SO4 = ___________________________

9. HC2H3O2 = _________________________

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

5. HClO4 = ___Perchloric acid __________

6. H2S = _____Hydrosulfuric acid _________

7. H2SO3 = ____________________________

8. H2SO4 = ____________________________

9. HC2H3O2 = __________________________

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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_________

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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 ______________________

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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 _______________________

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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 ________________________

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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 _______________________

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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 ________________________

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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 ________________________

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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 ________________________

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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 ______________________

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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

Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids