1. 1/13/16 Today I will describe the characteristics of an ionic bond
Warm Up – What is a compound?

2. Chemical Formulas and Bonding
Chapter 7
Chemical Formulas and Bonding

3. Bonding
Why if there are only 100 or so elements in nature, do we have so many different types of materials in the world?
Atoms combine together to form different materials!
Bonding – the combination of two or more atoms to form a compound
Two main types of bonds
Ionic
Covalent

4. Ionic Bonding
Why do clothes sometimes stick together when they come out of the dryer?
One has slight positive charge, one has slight negative charge
OPPOSITES ATTRACT!
Ionic Bond – occurs when oppositely charged ions are held together by electrical attraction caused by transferring electrons.

5. Ionic Compounds Ionic Compounds contain both metals and non-metals
Ionic compounds always form in set ratios
For example: 1 Li atom to 1 F atom

6. Ionic Compounds Properties –
High melting points
Strong Bonds
Brittle solids
Many are dissolvable in water
Dissolved or in liquid state – good electrical conductors
Solids cannot conduct electricity
**Ionic Compounds do not share the properties of the elements that they contain!
Soft silvery metal + highly poisonous gas  react to form table salt!

7. Ionic Compounds How do ions form? (REVIEW) Octet Rule!
Atoms tend to lose, gain or share electrons in order to acquire a full set of valence electrons!
In most cases, this is 8 valence electrons!!
H and He are the exception – they are full with 2!
When atoms complete their valence shell, they have the electron configuration of the closest noble gas.

8. 1/14

9. Ionic Compounds
Each unit of an ionic compound is called a FORMULA UNIT.

10. Lewis Dot Diagrams
Lewis Dot Diagram – a visual way to show an atom’s valence electrons 1 8 3 4 5 6 7
He=2 2

11. Lewis Dot Diagrams Li Be B C N O F Ne

12. Lewis Dot Diagrams
We can use the Lewis Dot Diagrams to see how atoms bond!

13. Na F NaF GaN Ga N Lewis Dot Diagrams Write the positive first!!! +1 -1-3 +3
GaN Ga N

14. Lewis Dot Diagrams +1 -2 Li S
Li2S +1 Li -1 +3
AlF3 Al F -1 F -1 F

15. Lewis Dot Diagrams +3 -2 In O
In2O3 +3 In -2 O -2 O

16. Criss Cross Method
Polyatomic Ion – an ion that consists of more than one atom
Name
Symbol
+ 1 Ions
ammonium ion
NH4+1
-1 Ions
cyanide
CN-1
hydroxide
OH-1
hypochlorite
ClO-1
chlorite
ClO2-1
chlorate
ClO3-1
perchlorate
ClO4-1
acetate
C2H3O2-1
permanganate
MnO4-1
nitrite
NO2-1
nitrate
NO3-1
hydrogen carbonate
(aka bicarbonate)
HCO3-1
hydrogen sulfate
HSO4-1
hydrogen sulfite
HSO3-1
thiocyanate
SCN-1
Name
Symbol
-2 Ions
carbonate
CO3-2
chromate
CrO4-2
dichromate
Cr2O7-2
hydrogen phosphate
HPO4-2
sulfite
SO3-2
sulfate
SO4-2
manganate
MnO4-2
oxalate
C2O4-2
-3 Ions
phosphite
PO3-3
phosphate
PO4-3

17. 1/15/16 Today I will determine formulas using the criss cross method.
Warm Up –
Using lewis dot diagrams, what compound would form between Ra and I?

18. Criss Cross Method
There is an easier way to determine what ionic compounds will form between two elements that works when lewis dots diagrams won’t.
Criss Cross Method!

19. Criss Cross Method
Criss Cross Method of formula writing utilizing charge. +1 +3
± 4 -3 -2 -1 +2

20. Criss Cross Method
What about the other elements?

21. Criss Cross Method Common Type II Ions Other Ions Name Symbol
Titanium (III)
Ti+3
Titanium (IV)
Ti+4
Chromium (II)
Cr+2
Chromium (III)
Cr+3
Manganese (II)
Mn+2
Manganese (IV)
Mn+4
Iron (II)
Fe+2
Iron (III)
Fe+3
Cobalt (II)
Co+2
Cobalt (III)
Co+3
Nickel (II)
Ni+2
Nickel (III)
Ni+3
Copper (I)
Cu+1
Copper(II)
Cu+2
Tin (II)
Sn+2
Tin (IV)
Sn+4
Lead (II)
Pb+2
Lead (IV)
Pb+4
Name
Symbol
Silver
Ag+1
Zinc
Zn+2

22. Criss Cross Method
Polyatomic Ion – an ion that consists of more than one atom
Name
Symbol
+ 1 Ions
ammonium ion
NH4+1
-1 Ions
cyanide
CN-1
hydroxide
OH-1
hypochlorite
ClO-1
chlorite
ClO2-1
chlorate
ClO3-1
perchlorate
ClO4-1
acetate
C2H3O2-1
permanganate
MnO4-1
nitrite
NO2-1
nitrate
NO3-1
hydrogen carbonate
(aka bicarbonate)
HCO3-1
hydrogen sulfate
HSO4-1
hydrogen sulfite
HSO3-1
thiocyanate
SCN-1
Name
Symbol
-2 Ions
carbonate
CO3-2
chromate
CrO4-2
dichromate
Cr2O7-2
hydrogen phosphate
HPO4-2
sulfite
SO3-2
sulfate
SO4-2
manganate
MnO4-2
oxalate
C2O4-2
-3 Ions
phosphite
PO3-3
phosphate
PO4-3

23. Criss Cross Method Criss Cross works with various types of compounds
#1. Binary ionic compounds – an ionic compound that consists of only two types of elements
Simple cation and a simple anion

24. Na F NaF Na F NaF Criss Cross Method+1 -1 Na F
NaF -1 +1 Na F
NaF 1 1
1. Write common ions, positive first
2. Criss Cross the numbers down
3. Write the numbers as subscripts without +/-
4. Don’t write ones! 5.

25. GaN Ga N Ga N GaN Lewis Dot Diagrams-3 +3
GaN Ga N -3 +3 Ga N
GaN 3 3
1. Write common ions, positive first
2. Criss Cross the numbers down
3. Write the numbers as subscripts without +/-
4. Don’t write ones!
5. Reduce to simplify!

26. Li S Li2S Li Li S Li2S Lewis Dot Diagrams+1 -2 Li S
Li2S +1 Li -2 +1 Li S
Li2S 2 1
1. Write common ions, positive first
2. Criss Cross the numbers down
3. Write the numbers as subscripts without +/-
4. Don’t write ones!
5. Reduce to simplify!

27. In O In2O3 In O O In O In2O3 Lewis Dot Diagrams +3 -2 +3 -2 -2 -2 +3 2

28. Let’s Try Some
Criss Cross #1

29. 1/20/16 Today I will use the criss cross method with polyatomic ions
Warm Up - Use criss cross to determine the formula of the compound that forms between:
a. Sr and P
b. Al and As
c. Rb and S

30. Polyatomic Ions
Polyatomic Ion – an ion that consists of more than one atom
You MUST know these polyatomic ions!
N-3
Monatomic ion
(charge from P.T.)
NO3-1
Polyatomic ion
(charge from sheet)

31. Criss Cross Method
Criss Cross will also work with compounds containing polyatomic ions
Polyatomic ions act like a single atom in ionic bonding!

32. Li PO4 Li3PO4 Criss Cross Method
#2 Ternary Ionic Compounds - compounds that include polyatomic ions (not binary because there are more than two atoms) -3 +1 Li
PO4
Li3PO4 3 1

33. ? Mg NO3 MgNO32 Mg(NO3)2 Criss Cross Method-1 +2 Mg
NO3
MgNO32 1 2
The number in the polyatomic ion never changes.
If a number needs to be added from criss cross to any polyatomic ion, that polyatomic ion goes into parentheses!
Mg(NO3)2

34. ? Sr OH SrOH2 Sr(OH)2 Criss Cross Method-1 +2 Sr OH
SrOH2 1 2
Sr(OH)2
If a number needs to be added from criss cross to any polyatomic ion, that polyatomic ion goes into parentheses!

35. Criss Cross Method -2 +1
NH4
CO3
(NH4)2CO3 2 1

36. Homework
Complete Criss Cross #2

37. 1/21/16
Today I will define covalent bonds and draw simple Lewis Structures.
Warm Up - Use criss cross to determine the compound that is formed between the following
Cs and N
Al and NO3
Be and PO3
Mg and P
Ba and CrO4

38. Covalent Bonding
Ionic Bond – occurs when oppositely charged ions are held together by electrical attraction caused by transferring electrons.
**We will consider an ionic bond to be any bond between a metal and a nonmetal OR any bond that contains a polyatomic ion!
Covalent Bond – occurs when electrons are shared between atoms.
**We will consider a covalent bond to be any bond between two non-metals!

39. Covalent Bonding
Each unit of a covalent compound is called a MOLECULE. (As opposed to ionic formula units)
Covalent compounds do NOT have a set ratio between elements. (Ionic AWLAYS does)
You CANNOT use criss cross or any other method to determine the formula! (You must with ionic compounds)
Covalent compounds form a wide range of substances with a wide range of properties!

40. Covalent Bonding CO
CO2
C12H22O11
C6H12O6

41. Covalent Bonding
Lewis Structure – structural formula that used dots and lines to describe bonding. (Based on Lewis Diagrams).
C6H12O6

42. F F C F F Covalent Bonding
Lets take a look at what happens when one carbon and four fluorines combine… F F C F F

43. F F C F F Covalent Bonding
Lets take a look at what happens when one carbon and four fluorines combine…
In a Lewis Structure, each pair of electrons becomes a line. F F C F F
Each pair of shared electrons is one covalent bond!

44. F F C F F Covalent Bonding
Lets take a look at what happens when one carbon and four fluorines combine…
***The shared pair counts as two electrons for both
In a Lewis Structure, each pair of electrons becomes a line. F F C F F
Note how each line is worth 2 electrons!
Each pair of shared electrons is one covalent bond!

45. Lewis Structures Steps to drawing simple Lewis Structures CF4
1. Count up the total number of valence electrons present.

46. Lewis Structures Steps to drawing simple Lewis Structures CF4
1. Count up the total number of valence electrons present.
C  4
x 1
= 4 v.e.
F  7
x 4
= 28 v.e.
= 32 v.e.

47. F F C F F Lewis Structures Steps to drawing simple Lewis Structures
2. Put the element with the lowest electronegativity in the center (This will usually be the first element written, except H cannot be center). Attach everything else to it with single bonds (one line). F
32 v.e. F C F F

48. F F C F F Lewis Structures Steps to drawing simple Lewis Structures
3. Add lone pairs to make octets. (Remember each bond is two electrons for each element!) F
32 v.e. F C F F

49. F F C F F Lewis Structures DONE!!
Steps to drawing simple Lewis Structures
CF4
4. Count up the total number of electrons drawn on! If it equals the total valence number, you are done! F
DONE!!
32 v.e. F C F F

50. Lewis Structures Steps to drawing simple Lewis Structures NH3
1. Count up the total number of valence electrons present.
N  5
x 1
= 5 v.e.
H  1
x 3
= 3 v.e.
= 8 v.e.

51. H H N H Lewis Structures Steps to drawing simple Lewis Structures NH3
2. Put the element with the lowest electronegativity in the center (This will usually be the first element written, except H can never go in the center). Attach everything else to it with single bonds (one line).
8 v.e. H H N H

52. H H N H Lewis Structures Steps to drawing simple Lewis Structures NH3
3. Add lone pairs to make octets. (Remember each bond is two electrons for each element!)
Ohhh…
H only wants two electrons!!!
H will only ever have one line and no dots in a Lewis Structure!
8 v.e. H H N H

53. H H N H Lewis Structures Steps to drawing simple Lewis Structures NH3
4. Count up the total number of electrons drawn on! If it equals the total valence number, you are done!
8 v.e. H H N H

54. Homework
Writing Simple Lewis Structures #1

55. 1/22/16 Today I will draw Lewis Structures with multiple bonds.
Warm Up – Draw the Lewis Structure for water (H2O)

56. Lewis Structures
Sometimes, double and triple covalent bonds will form!
H2CO H H C O

57. Lewis Structures
Sometimes, double and triple covalent bonds will form!
H2CO H H C O

58. Lewis Structures
H2CO
1. Count up the total number of valence electrons present.
H  1
x 2
= 2 v.e.
C  4
x 1
= 4 v.e.
O  6
x 1
= 6 v.e.
= 12 v.e.

59. H H C O Lewis Structures H2CO
2. Put the element with the lowest electronegativity in the center (This will usually be the first element written, except H can never go in the center). Attach everything else to it with single bonds (one line).
12 v.e. H H C O

60. H H C O Lewis Structures H2CO
3. Add lone pairs to make octets. (Remember each bond is two electrons for each element!)
12 v.e. H H C O

61. H H C O 14 v.e. ?? Lewis Structures H2CO
4. Count up the total number of electrons drawn on! If it equals the total valence number, you are done!
14 v.e. ??
12 v.e. H H C O

62. H H C O Lewis Structures H2CO
5. If you have used too many electrons, create double or triple bonds, by removing two pairs and creating one bond between them….then recount!
12 v.e. H H C O

63. Lewis Structures
C2H2
1. Count up the total number of valence electrons present.
C  4
x 2
= 8 v.e.
H  1
x 2
= 2 v.e.
= 10 v.e.

64. H C C H Lewis Structures C2H2
2. Put the element with the lowest electronegativity in the center (This will usually be the first element written, except H can never go in the center). Attach everything else to it with single bonds (one line).
10 v.e. H C C H

65. H C C H Lewis Structures C2H2
3. Add lone pairs to make octets. (Remember each bond is two electrons for each element!)
10 v.e. H C C H

66. H C C H Lewis Structures C2H2
4. Count up the total number of electrons drawn on! If it equals the total valence number, you are done!
10 v.e. H C C H

67. H C C H Lewis Structures C2H2
5. If you have used too many electrons, create double or triple bonds, by removing two pairs and creating one more bond….then recount!
10 v.e. H C C H

68. Cl O C Cl Lewis Structures Multiple Bonds – Never on H
Not usually on halogens
Most common with O, C, N
Try COCl2 Cl O C Cl

69. Homework
Writing Lewis Structures with Multiple Bonds #2

70. a. Rb and PO4 b. Al and OH c. B and N d. NH4 and O e. Sr and As
1/25/16
Today I will draw lewis structures of ions & other exceptions
Warm Up – Use criss cross to write formulas:
a. Rb and PO4
b. Al and OH
c. B and N
d. NH4 and O
e. Sr and As

71. Lewis Structures
Polyatomic Ions are covalently bonded within themselves.
Add or subtract electrons from the total valence number based on the charge!
NO3-1
N  5
x 1
= 5 v.e.
O  6
x 3
= 18 v.e.
= 23 v.e.
+ 1
= 24 v.e.

72. Lewis Structures
NO3-1
24 v.e.
26 electrons O O N O

73. Lewis Structures
NO3-1 -1
24 v.e. O O N O

74. Covalent Bonding
Several elements exist in nature covalently bonded to itself!
Diatomic molecules F F F2
Only when by itself (not in a bond with something else)

75. Diatomic Molecules

76. Homework
Lewis Structures #3 (Skip #10)

77. Today I will name ionic compounds
1/26/16
Today I will name ionic compounds
Warm Up – Draw the Lewis Structure for NI3

78. Naming Ionic Compounds
Ionic Compounds can be identified because they typically form between a metal and a non-metal OR contain a polyatomic ion!!
Rules for naming ionic compounds
Name the cation (metal or polyatomic ion)
Name the anion but…
If the anion is an element, change the ending to –ide
If the anion is a polyatomic ion, simply name it (no change)
3. Rule three to come!

79. Naming Ionic Compounds
Name the cation (metal or polyatomic ion)
Name the anion but…
If the anion is an element, change the ending to –ide
If the anion is a polyatomic ion, simply name it (no change)
CaO 
K2CO3 
Mg3P2 
calcium
oxide
potassium
carbonate
magnesium
phosphide

80. Naming Ionic Compounds
Write the formula and the name of the compound that forms between the following:
Tl and PO4
Na and S
NH4 and N
Be and PO3
TlPO4
thallium
phosphate
Na2S
sodium
sulfide
(NH4)3N
ammonium
nitride
Be3(PO3)2
beryllium
phosphite

81. Homework
Ionic Compounds – Formulas and Names #1

82. 1/27/16 Today I will name ionic compounds with Type II Cations
Warm Up – Name the following Compounds
KCl
BeBr2
Al2S3

83. Naming Ionic Compounds
Transition (and other Type II) Metals!
Some metals can form more than one charge!
These are called Type II cations!
This is typically seen in the transition metals (also, lead and tin)
Except zinc (always +2) and silver (always +1)
Rule #3! If a type II cation is present, place the charge of the ion in roman numerals in parenthesis after the cation name.

84. Naming Ionic Compounds
Type II Cations – formula from name
Iron(II) phosphate
Fe+2 PO4-3
Fe3(PO4)2

85. Naming Ionic Compounds
Type II Cations – name from formula
When naming an ionic compound from the formula, you must recognize the type II cations and give them a number by un-crisscrossing!
CoF2
Co2(SO3)3
FeO
SnO2
CuOH
Cobalt fluoride
(II)
Cobalt sulfite
(III)
Iron oxide
(II)
Tin oxide
(IV)
Copper hydroxide
(I)

86. Homework Ionic Compounds – Formulas and Names #2
(#3 is extra practice!)

87. 1/28/16 Today I will name covalent compounds Warm Up –
Name the following:
Ca(OH)2
AlCl3
NiS
Write the formulas for the following:
Calcium chloride
Lead(II) phosphide
Magnesium phosphate

88. Naming Covalent Compounds
Covalent Compounds can be identified because they typically form between two non-metals!!
Rules for naming covalent compounds
Name the first element
Name second element and change the ending to -ide
3. Add prefixes EXCEPT where the first element is a one! (When two vowels are together, you may eliminate one.)

89. Naming Covalent Compounds
prefix
number
mono- 1
di- 2
tri- 3
tetra- 4
penta- 5
hexa- 6
hepta- 7
octa- 8
nona- 9
deca- 10

90. Naming Covalent Compounds
Name the first element
Name the second element and change the ending to -ide
3. Add prefixes EXCEPT when the first element is one
N2O4 
PCl5 
NF3  di
nitrogen
tetr
oxide
phosphorus
penta
chloride
nitrogen
tri
fluoride

91. Naming Covalent Compounds
Write the name or formula of the following: CO
P2S5
SO2
carbon tetrachloride
carbon monoxide
diphosphorus pentasulfide
sulfur dioxide
CCl4

92. Mixed Naming
When naming, the first step is always to decide whether the compound is ionic or covalent.

93. Homework
Covalent Compounds – Formulas and Names

94. 1/29/16 Today I will practice naming compounds
Warm Up – Tell whether each of the following compounds is ionic or covalent:
a. CaCl2
b. SO3
c. NaOH
d. (NH4)3P
e. H2O2