1. CHEMICAL BONDS

2. I. Chemical Compounds Compounds
Are made from more than one type of atom (element)
Are made during a chemical chg
Have properties different from the elements they are made of
Have constant compositions

3. Fe2O3 I. Chemical Compounds Chemical Formulas
Use symbols to represent the ratios of elements in a particular compound.
Element symbols
Subscripts
Fe2O3

4. 3. Practice Interpreting Formulas
B. Chemical Formulas
3. Practice Interpreting Formulas
NaCl
1 sodium atom; 1 chlorine atom
H2O
2 hydrogen atoms; 1 oxygen atom
Al2(SO4)3
2 aluminum atoms
3 sulfur atoms
12 oxygen atoms

5. Your Turn! Fe2O3 Pb(C2H3O2)2 Interpret each of the following
2 iron atoms
3 oxygen atoms
1 lead atom
4 carbon atoms
6 hydrogen atoms
4 oxygen atoms

6. I. Chemical Compounds
C. Atoms Combine
To become Stable
Atoms are stable when they have a full valence energy level
Octet rule: Usually 8 e-
Exception: He is stable w/ 2 e-
Atoms gain, lose or share e-
to achieve a full valence level
c. Atoms are held together by a chemical bond

7. I. Chemical Compounds C. Atoms Combine Noble gases Are inert
do not react because they already have a full valence energy level
(stable octet)

8. II. Ions A. Ions are atoms which 1. Have gained or lost e-
ELements to the Left of the Line Lose eLectrons
Neither
LOSE
GAIN

9. II. Ions
A. Ions are atoms which
1. Have gained or lost e-

10. II. Ions A. Ions are atoms which 1. Have gained or lost e-
You can predict the # of e- which will be gained or lost by looking at the family

11. Gains 3 e- Lose 1 e- Varies Lose 2 e- Gain 3 e- Gain 2 e- Gain 1 e-
Will P gain or lose electrons when forming an ion? How many?
Gains 3 e-

12. A. Ions are atoms which Formula= Na1+ Formula= Cl1-
Another name for charge is oxidation number
The formula for an ion includes its charge (oxidation number)
Na ion
Lost 1 e-
Formula= Na1+
Cl ion
Gained 1 e-
Formula= Cl1-

13. Review it Now!
Ions have a charge, atoms do not
What is the difference between an atom and an ion?
What is an oxidation number?
Write the oxidation number for each of the following ions:
a.  Li f. Al
b. K g. S
c. Mg h. Cl
d.  P i. Ne
e. B j. N
The charge on an ion 1+ 3+ 1+ 2- 2+ 1- 3- 3+ 3-

14. III.Compounds with Ionic Bonds
1.Are formed
a.between (+) and (-) ions
b.When one atom gains e- while the other loses e-
2.Compounds with ionic bonds are called ionic compounds

15. III.Compounds with Ionic Bonds
3. Ionic bonds are formed between a metal and a nonmetal!

16. Check Your Understanding!
Which of the following are ionic compounds?
1. KCl
2. CO2
3. LiF
4. CaCl2
Ionic
Not ionic
Ionic
Ionic

17. B. Formulas for Binary Cmpds
Step 1:Write the symbol of the (+) ion first, followed by the symbol of the (-) ion
Step 2: Determine the ox.# for each ion and write it above the symbols.
Step 3: Crisscross the charges and write them as subscripts.
Step 4: If the charges can be reduced, do so.

18. B. Formulas for Ionic Cmpds
Example #1: Ba and Cl

19. B. Formulas for Ionic Cmpds
Example #2: Be and P
Be3P2

20. BaS Ba2S2 B. Formulas for Ionic Cmpds Example #3: Ba and S
note subscripts can be reduced; do so!

21. Write the formula for each of the following compounds
Your Turn!
Write the formula for each of the following compounds
1. calcium with chlorine
2. potassium with bromine
3. lithium with sulfur
4. magnesium with phosphorus
5. aluminum with nitrogen
CaCl2
KBr
Li2S
Mg3P2
AlN

22. C. Naming Binary Cmpds
Step 1:Write the name of the positive element 1st.
Step 2:Write the name of the negative element 2nd.
Step 3:Add the ending -ide to the root of the second element.

23. calcium chloride C. Naming Binary Cmpds Example #1:
What is the formula name for CaCl2?
Step 1: calcium
Step 2: calcium chlorine
Step 3: calcium chloride
calcium chloride

24. Magnesium phosphide C. Naming Binary Cmpds Example #2:
What is the formula name for Mg3P2?
Step 1: magnesium
Step 2: magnesium phosphorus
Step 3: magnesium phosphide
Magnesium phosphide

25. Name each of the following
Your Turn!
Name each of the following
1. Li2S
2. KBr
3. BaS
4. Al2O3
5. Na3N
Lithium sulfide
Potassium bromide
Barium sulfide
Aluminum oxide
Sodium nitride

26. D. Formulas for Polyatomic Ionic Cmpds
Binary compounds are made of two kinds of elements.
Example: BaCl2
Polyatomic (ternary) compounds are made of three or more elements.
Examples:
K2SO4 Mg(ClO3)2

27. D. Formulas for Polyatomic Ionic Cmpds
Polyatomic ions are a group of covalently bonded atoms that act as one atom with a charge.

28. D. Formulas for Polyatomic Ionic Cmpds
Rules for Writing Formulas
Step 1:Write the symbol and ox. #
Step 2: Crisscross the charges and write them as subscripts.
Step 3: Make sure you put polyatomic ions in parentheses (if you need more than one).
Step 4: Make sure the subscripts are reduced.

29. Ca(NO3)2 D. Formulas for Ionic Cmpds Example #1: Calcium Nitrate
Ca2+ and NO31-
Ca2+ and NO31- 2
Ca2+ and (NO3) 2
Ca(NO3)2

30. Ca3(PO4)2 D. Formulas for Polyatomic Ionic Cmpds
Example #2: Calcium Phosphate
Ca2+ and PO43-
Ca2+ and PO43- 3 2
Ca and (PO4)2
Ca3(PO4)2

31. Your Turn! Write the formula for each of the following compounds
1. Sodium sulfate
2. Calcium hydroxide
3. Beryllium phosphate
4. Aluminum nitrate
Na2SO4
Ca(OH)2
Be3(PO4)2
Al(NO3)3

32. E. Naming Polyatomic Ionic Compounds
Rules for Naming
Polyatomic Compounds
Step 1:Write the name of the positive ion.
Step 2: Write the name of the negative ion .

33. Calcium nitrate E. Naming Polyatomic Ionic Cmpds Example #1: Ca(NO3)2

34. Aluminum phosphate E. Naming Polyatomic Ionic Cmpds Example #2: AlPO4

35. Your Turn! Name each of the following compounds Potassium sulfate
1. K2SO4
2. CaCO3
3. NaOH
4. NH4C2H3O2
Potassium sulfate
Calcium carbonate
Sodium hydroxide
Ammonium acetate

36. G. Special case ionic bonds: ACIDS
Acids are easy to recognize as compounds as they begin with the element hydrogen. As with other ionic bonds, acids fall into 2 categories, binary and ternary.

37. G. Special case ionic bonds: ACIDS
Examples of binary acids would include things like:
HF, HI, H2S and HCl
Examples of ternary acids would include things like:
H2SO4 and HNO3

38. G. Special case ionic bonds: ACIDS
Naming of binary acids
Step 1:Name the anion, changing the ending to “-ic”
Step 2: Add the prefix “hydro-”
Step 3: Slap acid on the end

39. G. Special case ionic bonds: ACIDS
Example #1: HF

40. G. Special case ionic bonds: ACIDS
Example #1: HF
“flourine” becomes

41. G. Special case ionic bonds: ACIDS
Example #2: HF
“flourine” becomes
“flouric” becomes

42. G. Special case ionic bonds: ACIDS
Example #1: HF
“flourine” becomes
“flouric” becomes
“hydroflouric” becomes

43. “hydroflouric acid” G. Special case ionic bonds: ACIDS Example #1: HF
“chlorine” becomes
“chloric” becomes
“hydrochloric” becomes
“hydroflouric acid”

44. G. Special case ionic bonds: ACIDS
Example #2: HCl

45. G. Special case ionic bonds: ACIDS
Example #2: HCl
“chlorine” becomes

46. G. Special case ionic bonds: ACIDS
Example #2: HCl
“chlorine” becomes
“chloric” becomes

47. G. Special case ionic bonds: ACIDS
Example #2: HCl
“chlorine” becomes
“chloric” becomes
“hydrochloric” becomes

48. “hydrochloric acid” G. Special case ionic bonds: ACIDS Example #2: HCl
“chlorine” becomes
“chloric” becomes
“hydrochloric” becomes
“hydrochloric acid”

49. Naming of ternary acids
G. Special case ionic bonds: ACIDS
Naming of ternary acids
Step 1:Name the polyatomic
Step 2: Change “-ate” to “-ic”
or “-ite” to “-ous”
Step 3: Slap acid on the end

50. “sulfuric acid” G. Special case ionic bonds: ACIDS Example #1: H2SO4
“sulfate” becomes
“sulfuric” becomes
“sulfuric acid”

51. G. Special case ionic bonds: ACIDS
Example #1: H2SO4

52. G. Special case ionic bonds: ACIDS
Example #1: H2SO4
“sulfate” becomes

53. G. Special case ionic bonds: ACIDS
Example #1: H2SO4
“sulfate” becomes
“sulfuric” becomes

54. “sulfuric acid” G. Special case ionic bonds: ACIDS Example #1: H2SO4
“sulfate” becomes
“sulfuric” becomes
“sulfuric acid”

55. G. Special case ionic bonds: ACIDS
Example #1: HNO2

56. G. Special case ionic bonds: ACIDS
Example #1: HNO2
“nitrite” becomes

57. G. Special case ionic bonds: ACIDS
Example #1: HNO2
“nitrite” becomes
“nitrous” becomes

58. “nitrous acid” G. Special case ionic bonds: ACIDS Example #1: HNO2
“nitrite” becomes
“nitrous” becomes
“nitrous acid”

59. Rules for Writing Formulas for binary acids
G. Special case ionic bonds: ACIDS
Rules for Writing Formulas for binary acids
Step 1: Does the name begin with
“hydro-”? If yes, then…
Step 2:Write the symbol for the
hydrogen ion followed by the
symbol for the second element
Step 3: Crisscross the charges and write them as subscripts.

60. G. Special case ionic bonds: ACIDS
Rules for Writing Formulas for binary acids
Example: hydrosulfuric acid

61. G. Special case ionic bonds: ACIDS
Rules for Writing Formulas for binary acids
Example: hydrosulfuric acid
H S-2

62. G. Special case ionic bonds: ACIDS
Rules for Writing Formulas for binary acids
Example: hydrosulfuric acid
H S-2

63. H2S G. Special case ionic bonds: ACIDS Example: hydrosulfuric acid
Rules for Writing Formulas for binary acids
Example: hydrosulfuric acid
H S-2
H2S

64. Rules for Writing Formulas for ternary acids
G. Special case ionic bonds: ACIDS
Rules for Writing Formulas for ternary acids
Step 1: Does the name begin with
“hydro-”? If no, then…
Step 2:Write the symbol for the
hydrogen ion followed by the
appropriate polyatomic ion
Step 3: Crisscross the charges and write them as subscripts.

65. Rules for Writing Formulas for binary acids Example: sulfuric acid
G. Special case ionic bonds: ACIDS
Rules for Writing Formulas for binary acids
Example: sulfuric acid

66. Rules for Writing Formulas for binary acids Example: sulfuric acid
G. Special case ionic bonds: ACIDS
Rules for Writing Formulas for binary acids
Example: sulfuric acid
H SO4-2

67. Rules for Writing Formulas for binary acids Example: sulfuric acid
G. Special case ionic bonds: ACIDS
Rules for Writing Formulas for binary acids
Example: sulfuric acid
H+1 SO4-2
H+1 SO4-2

68. Rules for Writing Formulas for binary acids Example: sulfuric acid
G. Special case ionic bonds: ACIDS
Rules for Writing Formulas for binary acids
Example: sulfuric acid
H+1 SO4-2
H+1 SO4-2
H2SO4

69. G. Special case ionic bonds: ACIDS
Name the chemical or write the symbol
1. HI
2. phosphoric acid
3. hydrobromic acid
4. H2SO3

70. G. Special case ionic bonds: ACIDS
Name the chemical or write the symbol
hydroiodic acid 1.
2. phosphoric acid
3. hydrobromic acid
4. H2SO3

71. G. Special case ionic bonds: ACIDS
Name the chemical or write the symbol
hydroiodic acid 1. 2.
3. hydrobromic acid
4. H2SO3
H3PO4

72. G. Special case ionic bonds: ACIDS
Name the chemical or write the symbol
hydroiodic acid 1. 2. 3.
4. H2SO3
H3PO4
HBr

73. G. Special case ionic bonds: ACIDS
Name the chemical or write the symbol
hydroiodic acid 1. 2. 3. 4.
H3PO4
HBr
sulfurous acid

74. IV.Compounds with Covalent Bonds
1.Are formed when atoms share e-

75. IV.Cmpds with Covalent Bonds
2.Are formed
Between two nonmetals

76. Your Turn!
State if each of the following compounds is ionic or covalent
1. CO2
2. MgS
3. Na2O
4. PI3

77. Your Turn!
State if each of the following compounds is ionic or covalent
1. CO2
2. MgS
3. Na2O
4. PI3
covalent

78. Your Turn!
State if each of the following compounds is ionic or covalent
1. CO2
2. MgS
3. Na2O
4. PI3
covalent
ionic

79. Your Turn!
State if each of the following compounds is ionic or covalent
1. CO2
2. MgS
3. Na2O
4. PI3
covalent
ionic
ionic

80. Your Turn!
State if each of the following compounds is ionic or covalent
1. CO2
2. MgS
3. Na2O
4. PI3
covalent
ionic
ionic
covalent

81. IV.Cmpds with Covalent Bonds
Writing Covalent Formulas
Greek Prefixes
mono- one
di- two
tri- three
tetra- four
penta- five
hexa- six
hepta- seven
octa- eight
nona- nine
deca- ten

82. B. Writing Covalent Formulas
2.Rules
Step 1: Write the symbol of the first nonmetal.
Step 2: Use the nonmetal’s prefix as a subscript

83. B. Writing Covalent Formulas
2.Rules
Step 3: Write the symbol of the second nonmetal.
Step 4: Use the nonmetal’s prefix as a subscript.
Note: If there is no prefix, there is no subscript.

84. C B. Writing Covalent Formulas 3.Practice problem #1
Write the formula for carbon dioxide C

85. C O B. Writing Covalent Formulas 3.Practice problem #1
Write the formula for carbon dioxide C O

86. C O B. Writing Covalent Formulas 2 3.Practice problem #1
Write the formula for carbon dioxide C O 2

87. No Prefix = No Subscript
B. Writing Covalent Formulas
3.Practice problem #1
Write the formula for carbon dioxide C O 2
No Prefix = No Subscript

88. B. Writing Covalent Formulas
3.Practice problem #2
Write the formula for dinitrogen trioxide

89. N B. Writing Covalent Formulas 3.Practice problem #2
Write the formula for dinitrogen trioxide N

90. N O B. Writing Covalent Formulas 3.Practice problem #2
Write the formula for dinitrogen trioxide N O

91. N O B. Writing Covalent Formulas 2 3 3.Practice problem #2
Write the formula for dinitrogen trioxide N O 2 3

92. B. Writing Covalent Formulas
3.Practice problem #3
Write the formula for dichlorine hexabromide

93. Cl B. Writing Covalent Formulas 3.Practice problem #3
Write the formula for dichlorine hexabromide Cl

94. Cl Br B. Writing Covalent Formulas 3.Practice problem #3
Write the formula for dichlorine hexabromide Cl Br

95. Cl Br B. Writing Covalent Formulas 2 6 3.Practice problem #3
Write the formula for dichlorine hexabromide Cl Br 2 6

96. Cl Br B. Writing Covalent Formulas 2 6 3.Practice problem #3
Write the formula for dichlorine hexabromide Cl Br 2 6
Note: Do Not Reduce subscripts!

97. Write formulas for the following compounds
Your Turn!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide

98. Write formulas for the following compounds
Your Turn!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
CCl4

99. Write formulas for the following compounds
Your Turn!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
CCl4
Cl3Br7

100. Write formulas for the following compounds
Your Turn!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
CCl4
Cl3Br7
N2O

101. Write formulas for the following compounds
Your Turn!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
CCl4
Cl3Br7
N2O CO

102. IV.Cmpds with Covalent Bonds
Naming Covalent Cmpds
Step 1: Name each element.
Step 2: Change the ending of the 2nd element to -ide
Step 3: Add Greek prefixes to indicate the # ofatoms of each element
Note: Do not use mono on the first element!

103. C. Naming Covalent Cmpds
2.Practice problem #1
Write the name for CO

104. C. Naming Covalent Cmpds
2.Practice problem #1
Write the name for CO
Carbon

105. C. Naming Covalent Cmpds
2.Practice problem #1
Write the name for CO
Carbon
Monoxide
oxygen

106. C. Naming Covalent Cmpds
2.Practice problem #1
Write the name for CO
Carbon
oxide
oxygen

107. C. Naming Covalent Cmpds
2.Practice problem #1
Write the name for CO
Carbon
Monoxide

108. C. Naming Covalent Cmpds
2.Practice problem #1
Write the name for CO
Carbon
Monoxide
Carbon Monoxide

109. C. Naming Covalent Cmpds
2.Practice problem #2
Write the name for Cl2O3
Dichlorine
trioxide
trioxide
oxide
Dichlorine trioxide

110. C. Naming Covalent Cmpds
2.Practice problem #2
Write the name for Cl2O3
chlorine

111. C. Naming Covalent Cmpds
2.Practice problem #2
Write the name for Cl2O3
chlorine
oxygen

112. C. Naming Covalent Cmpds
2.Practice problem #2
Write the name for Cl2O3
chlorine
oxide

113. C. Naming Covalent Cmpds
2.Practice problem #2
Write the name for Cl2O3
Dichlorine
chlorine
trioxide
trioxide
oxygen
oxide

114. C. Naming Covalent Cmpds
2.Practice problem #2
Write the name for Cl2O3
Dichlorine
chlorine
trioxide
trioxide
oxygen
oxide
Dichlorine trioxide

115. Write formulas for the following compounds
Your Turn!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide

116. Write formulas for the following compounds
Your Turn!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
CCl4

117. Write formulas for the following compounds
Your Turn!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
CCl4
Cl3Br7

118. Write formulas for the following compounds
Your Turn!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
CCl4
Cl3Br7
N2O

119. Write formulas for the following compounds
Your Turn!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
CCl4
Cl3Br7
N2O CO

120. Name the following compounds
Your Turn!
Name the following compounds
1. PBr5
2. NO
3. S2I3

121. Name the following compounds
Your Turn!
Name the following compounds
1. phosphorus pentabromide
2. NO
3. S2I3

122. Name the following compounds
Your Turn!
Name the following compounds
1. phosphorus pentabromide
2. nitrogen monoxide
3. S2I3

123. Name the following compounds
Your Turn!
Name the following compounds
1. PBr5
2. nitrogen monoxide
3. disulfur triiodide
phosphorus pentabromide

124. THAT’S ALL FOLKS!!!
Now you can name not only covalent bonds but binary and ternary ionic bonds, including acids. That being said, now…
GO DO!!!