Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5

Chemistry 102

Section 6.4

Ionic Compounds

&

Section 6.5

Molecular Compounds and Acids

Unit II Note pack, pages 9-13

1

Ionic Compounds

A. 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)

2

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

3

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.

4

Ionic Compounds



Mg +2 + Cl  MgCl

2

Magnesium Chloride

5

Ionic Compounds



Mg +2 + Cl  MgCl

2


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

6

Ionic Compounds



Mg +2 + Cl  MgCl

2


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

Na + + O -2  Na

2

O Sodium Oxide

7

Ionic Compounds


(pg. 10)

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

NAME IT.

8

Ionic Compounds


(pg. 10)


NAME IT.

Al +3 + S -2  Al

2

S

3

Aluminum sulfide

9

Ionic Compounds


(pg. 10)


NAME IT.

Al +3 + S -2  Al

2

S

3


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

NAME IT.

10

Ionic Compounds


(pg. 10)


NAME IT.

Al +3 + S -2  Al

2

S

3



NAME IT.

Fe +3 + O -2  Fe

2

O

3

Iron (III) oxide

11

Ionic Compounds


(pg. 10)


NAME IT.

Al +3 + S -2  Al

2

S

3



NAME IT.

Fe +3 + O -2  Fe

2

O

3


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

NAME IT.

12

Ionic Compounds


(pg. 10)


NAME IT.

Al +3 + S -2  Al

2

S

3



NAME IT.

Fe +3 + O -2  Fe

2

O

3


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

NAME IT.

Ca +2 + S -2  CaS Calcium sulfide

13

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.

14

Polyatomic ions

C. There are 3 important exceptions (to the end of their names), they are:

Ammonium cation (NH

4

+ )

Two polyatomic ions end in –ide; cyanide (CN ) and hydroxide (OH )

15

Polyatomic Ions

• For “D”, see Chart 6.4

• Example:

• Ammonium NH

4

+

16

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 + + NO

3

 LiNO

3

17


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 +3 + CO

3

-2 

E. Write the formula for ammonium sulfate:

F. Write the formula for calcium phosphate:

18


C.



Al +3 + CO

3

-2  Al

2

( CO

3

)

3



19


C.



Al +3 + CO

3

-2  Al

2

( CO

3

)

3


NH

4

+ + SO

4

-2 


20


C.



Al +3 + CO

3

-2  Al

2

( CO

3

)

3


NH

4

+ + SO

4

-2  ( NH

4

)

2

SO

4


21


C.



Al +3 + CO

3

-2  Al

2

( CO

3

)

3


NH

4

+ + SO

4

-2  ( NH

4

)

2

SO

4


Ca +2 + PO

4

-3 

22


C.



Al +3 + CO

3

-2  Al

2

( CO

3

)

3


NH

4

+ + SO

4

-2  ( NH

4

)

2

SO

4


Ca +2 + PO

4

-3  Ca

3

( PO

4

)

2

23


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

Write the formula for beryllium carbonate.

24


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

Write the formula for beryllium carbonate.

Be

+2

+ CO

3

-2 

BeCO

3

Beryllium ion + carbonate  beryllium carbonate

25

Practice Problems, pg. 11

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

4

+1 , SO

3

2b. Calcium ion, phosphate ion

26



4

+1 , SO

3

2-

(NH

4

)

2

SO

3

Ammonium Sulfite b. Calcium ion, phosphate ion

27



4

+1 , SO

3

2-

(NH

4

)

2

SO

3

Ammonium Sulfite b. Calcium ion, phosphate ion

Ca +2 + PO

4

-3  Ca

3

(PO

Calcium phosphate

4

)

2

28


1. Write the formulas for compounds formed AND name the compound from these pairs of ions: c. Al 3+ , NO

3

-1 d. Potassium ion, chromate ion

29



3

-1

Al(NO

3

)

3

Aluminum Nitrate d. Potassium ion, chromate ion

30



3

-1

Al(NO

3

)

3

Aluminum Nitrate d. Potassium ion, chromate ion

K + + CrO

4

-2  K

2

CrO

Potassium chromate

4

31


2. Write formulas for these compounds a. Lithium hydrogen sulfate __________ b. Chromium (III) nitrite ______________ c. Mercury (II) bromide ______________ d. Ammonium dichromate ___________

32


2. Write formulas for these compounds a. Lithium hydrogen sulfate _ LiHSO

4

__ b. Chromium (III) nitrite _____________ c. Mercury (II) bromide ______________ d. Ammonium dichromate ___________

33



4

___ b. Chromium (III) nitrite __ Cr(NO

2

)

3

_____ c. Mercury (II) bromide _______________ d. Ammonium dichromate ____________

34



4

__ b. Chromium (III) nitrite __ Cr(NO

2

)

3

__ c. Mercury (II) bromide __ HgBr

2

___ d. Ammonium dichromate _(NH

4

)

2

Cr

2

O

7

_

35

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.

36


4

5

2

3


2.

We use prefixes when naming binary molecular compounds: Refer to Table 6.5 and fill in the following:

Number Prefix Number Prefix

1 6

7

8

9

10

37


4

5

2

3


2.

We use prefixes when naming binary molecular compounds: Refer to Table 6.5 and fill in the following:

Number Prefix Number Prefix

1 mono6 hexaditritetrapenta-

7

8

9

10 heptaoctanonadeca-

38



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)

39

Name these binary molecular compounds.

A. N

2

O -- ___________________

B. PCl

3

-- ___________________

C. SF

6

-- _____________________

D. OF

2

-- _____________________

E. Cl

2

O

8

-- ___________________

F. SO

3

-- ____________________

40


A. N

2

O -_ di nitrogen mon oxide__

B. PCl

3

-- _____________________ _

C. SF

6

-________________________

D. OF

2

-_______________________

E. Cl

2

O

8

-- _ __________________ __

F. SO

3

-______________________

41


A. N

2

O -_dinitrogen monoxide__

B. PCl

3

-_phosphorus tri chloride_

C. SF

6

-______________________

D. OF

2

-_____________________

E. Cl

2

O

8

-- ____________________

F. SO

3

-____________________

42


A. N

2


B. PCl

3

-_phosphorus trichloride_

C. SF

6

-_sulfur hexafluoride___

D. OF

2

-_____________________

E. Cl

2

O

8

-- _____________________

F. SO

3

-____________________

43


A. N

2


B. PCl

3

-_phosphorus trichloride_

C. SF

6

-_sulfur hexafluoride___

D. OF

2

-_oxygen difluoride___

E. Cl

2

O

8

-- _ dichlorine octoxide __

F. SO

3

-_sulfur trioxide___

44

Write the formulas for the following binary molecular compounds.

a. Nitrogen trifluoride ________________ b. Disulfur dichloride ___ ______ _______ c. Dinitrogen tetraoxide __ ______ _______ d. Octoxygen dichloride __ ______ _______ e. Trinitrogen pentoxide __ _______ ______

45


a. Nitrogen trifluoride ___NF

3

__________ b. Disulfur dichloride ________________ c. Dinitrogen tetraoxide ______________ d. Octoxygen dichloride _______________ e. Trinitrogen pentoxide _______________

46



3

__________ b. Disulfur dichloride ___ S

2

Cl

2

________ c. Dinitrogen tetraoxide ______________ d. Octoxygen dichloride ______________ e. Trinitrogen pentoxide ______________

47



3


2

Cl

2

________ c. Dinitrogen tetraoxide __ N

2

O

4

________ d. Octoxygen dichloride _______________ e. Trinitrogen pentoxide ______________

48



3


2

Cl

2

________ c. Dinitrogen tetraoxide __ N

2

O

4

________ d. Octoxygen dichloride __ O

8

Cl

2

_______ e. Trinitrogen pentoxide __ N

3

O

5

_______

49

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)

50

Naming acids

51

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 =___________________________

________________________________

HClO

4

= _________________________

________________________________

52




HClO = ClO is hypochlor ite _so the name for this acid is… ______________

HClO

4

=_________________________

_______________________________

53




HClO = ClO is hypochlor ite _so the name for this acid is hypochlorous acid

HClO

4

= _________________________

________________________________

54





HClO

4

= ClO

4 is perchlor ate , so the name for this acid is…______________

55





HClO

4

= ClO

4 is perchlor ate , so the name for this acid is perchloric acid

56

Practice naming the following acids:

1. HCl = _________________________

2. HClO

3

3. HClO

2

= _______________________

= _______________________

4. HClO = ________________________

5. HClO

4

7. H

2

SO

3

= _______________________

6. H

2

S = ____________________

= ___________________

8. H

2

SO

4

= ___________________

9. HC

2

H

3

O

2

= ____________________

57


1. HCl = ____ Hydrochloric acid __________

2. HClO

3

3. HClO

2

= ___________________________

= ___________________________

4. HClO = ____________________________

5. HClO

4

7. H

2

SO

3

= ___________________________

6. H

2

S = _____________________________

= ___________________________

8. H

2

SO

4

= ___________________________

9. HC

2

H

3

O

2

= _________________________

58



2. HClO

3

3. HClO

2

= ____ Chloric acid _____________

= ___________________________

4. HClO = ____________________________

5. HClO

4

7. H

2

SO

3

= ___________________________

6. H

2

S = _____________________________

= ___________________________

8. H

2

SO

4

= ___________________________

9. HC

2

H

3

O

2

= _________________________

59



2. HClO

3

3. HClO

2

= ____

= ____

Chloric acid _____________

Chlorous Acid ___________

4. HClO = ____________________________

5. HClO

4

7. H

2

SO

3

= ____________________________

6. H

2

S = ______________________________

= ____________________________

8. H

2

SO

4

= ____________________________

9. HC

2

H

3

O

2

= __________________________

60



2. HClO

3

3. HClO

2

= ____

= ____



4. HClO = ____ Hypochlorous acid _______

5. HClO

4

7. H

2

SO

3

= ___________________________

6. H

2

S = _____________________________

= ___________________________

8. H

2

SO

4

= ___________________________

9. HC

2

H

3

O

2

= _________________________

61



2. HClO

3

3. HClO

2

= __

= __


Chlorous Acid __________

4. HClO = ___ Hypochlorous acid _______

5. HClO

4

7. H

2

SO

3

= __ Perchloric acid __________

6. H

2

S = _____________________________

= ___________________________

8. H

2

SO

4

= ___________________________

9. HC

2

H

3

O

2

= _________________________

62



2. HClO

3

3. HClO

2

= ____

= ____



4. HClO = ____ Hypochlorous acid ________

5. HClO

4

7. H

2

SO

3

= ___ Perchloric acid __________

6. H

2

S = _____ Hydrosulfuric acid _________

= ____________________________

8. H

2

SO

4

= ____________________________

9. HC

2

H

3

O

2

= __________________________

63



2. HClO

3

3. HClO

2

= ____

= ____


Chlorous Acid ______________

4. HClO = ____ Hypochlorous acid ________

5. HClO

4

7. H

2

SO

3

= ___ Perchloric acid __________

6. H

2

S = _____ Hydrosulfuric acid _________

= ___ Sulfurous acid __________

8. H

2

SO

4

= ____

9. HC

2

H

3

O

2

Sulfuric acid

= ___ Acetic acid

_____

_________

64

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 ______________________

65


1. Nitric acid _____ HNO

3

_____________

2. Hydronitric acid __________________

3. Nitrous acid _____________________

4. Hydrocyanic acid _________________

5. Phosphoric acid __________________

6. Hydrobromic acid _________________

7. Acetic acid ______________________

8. Nitric acid _______________________

66



3

______________

2. Hydronitric acid _ H

3

N ______________

3. Nitrous acid ______________________

4. Hydrocyanic acid __________________

5. Phosphoric acid ___________________

6. Hydrobromic acid __________________

7. Acetic acid _______________________

8. Nitric acid ________________________

67



3

_____________


3

N ______________

3. Nitrous acid __ HNO

2

_______________

4. Hydrocyanic acid _________________

5. Phosphoric acid ___________________


7. Acetic acid _______________________

8. Nitric acid _______________________

68



3

______________


3

N _______________


2

_______________

4. Hydrocyanic acid ___ HCN ___________

5. Phosphoric acid ___________________


7. Acetic acid _______________________

8. Nitric acid ________________________

69



3

______________


3

N _______________


2

________________


5. Phosphoric acid __ H

3

PO

4

____________


7. Acetic acid _______________________

8. Nitric acid ________________________

70



3

______________

2. Hydronitric acid _ HN

3

_______________


2

______________



3

PO

4

____________

6. Hydrobromic acid _ HBr ______________

7. Acetic acid _______________________

8. Nitric acid ________________________

71



3

______________


3

_______________


2

________________



3

PO

4

____________


7. Acetic acid __ HC

2

H

3

O

2

____________

8. Nitric acid ______________________

72



3

______________


3

_______________


2

________________



3

PO

4

____________


7. Acetic acid __ HC

2

H

3

O

2

____________

8. Nitric acid ___ HNO

3

_______________

73

Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5

Ionic Compounds

Molecular Compounds and Acids

A compound that contains atoms of three, or more, different elements

Be

+ CO

BeCO

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Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5

Ionic Compounds

Molecular Compounds and Acids

A compound that contains atoms of three, or more, different elements

Be

+ CO

BeCO

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