1. Unit One

2. Notes One Unit One Two Classes of Elements Periodic Table Info?
What Are Stable Elements?
Stabilizing Sodium
Stabilizing Oxygen
Sodium Loses electrons to Oxygen
Oxidation Numbers
Key Elements and Examples

3. Two Classes of Elements
What are the Two Main Classes of Elements?
Metals and Nonmetals (Stair-Step)

4. What information doe the Periodic Table give us?
Atomic Number
# Protons = # of Electrons
Electron structure
Mass Number = # P + # N

5. What Makes Elements Stable?
Which orbitals?
Eight Electrons……
Highest S and P……
Noble Gases (electronically stable)
He, Ne, Ar, Kr, Xe, and Rn
Lose or Gain to get 8e-1 (to become stable)
Do metals Lose or Gain electrons?
Do nonmetals Lose or Gain electrons?
Which Family?
(Lose)
(Gain)

6. Stabilizing Sodium How many electrons does sodium have? 11Na
What is Sodium’s Short-Hand Element?
10Ne
How many Valence Electrons for Sodium?
1e-1
What is the shorthand electron configuration?
Sodium loses/gain how many electrons?
Na Na+1 + e Oxidation or reduction?
(protons) + (electrons)=charge 1
[10Ne] 3s
(+11)
(-10) +1

7. Stabilizing Oxygen How many electrons does oxygen have? 8O
What is oxygen’s Short-Hand Element?
2He
How many Valence Electrons for oxygen?
6e-1
What is the shorthand electron configuration?
Oxygen loses/gains how many electrons?
2e-1
O + 2e-1 O Oxidation or reduction?
(protons) + (electrons)=charge
[2He] 2s 2 2p 4
(+8)
(-10) -2

8. Sodium Loses electrons to Oxygen
Na Na+1 + e-1 (Stable Like Neon) Ox or Red?
O + 2e-1 O (Stable Like Neon) Ox or Red?
How many sodium atoms are needed to satisfy oxygen’s electron hunger?
2e-1 means
How many oxygen atoms are needed to satisfy sodium’s electron loss?
Na2O
High Electronegativity
two Na
Low Electronegativity
One O

9. Oxidation Numbers Fe+2 Fe+3 S-2 S+4 S+6 All elements Lose or Gain e-1.
Some have multiple loss or gain possibilities.
Fe+2
Fe+3
S-2
S+4
S+6

10. Key Elements (99%) H+1 H-1 (99%)O-2 O-1
(Always) Li+1, Na+1, K+1, Rb+1, Cs+1, Fr+1
(Always) Be+2, Mg+2, Ca+2, Ba+2, Sr+2, Ra+2
(Always) Al+3
(with only a metal) F-1, Cl-1, Br-1, I-1
(NO3-1) ion is always +5
(SO4-2) ion is always +6

11. Example One Find the oxidation numbers. Al2S3 Algebra is useful!
Al+3 key element
2(+3) + 3(S)=0
S= -2
2(Al) +
3(S)=

12. Example Two Find the oxidation numbers. Ca(NO3)2 Algebra is useful !
Ca+2 and O-2 key elements
(+2)+2(N)+6(-2)=0
(+2)+2(N)+(-12)=0
2(N)+(-10)=0
2(N)=10
N= +5
(Ca)+
2(N)+
6(O)=

13. Finding Oxidation #’s for Compounds+1 -2 +1 +4 -2
H2O
H2CO3 +1 +5 -2 -3 +1 +4 -2
H3PO4
(NH4)2CO3 +2 +5 -2 +1 +5 -2
Ca3(AsO4)2
HNO3 +1 +6 -2 +3 +6 -2
H2SO4
Fe2(SO4)3 +1 +6 -2 +2 +7 -2
Hg2SO4
Ba(ClO4)2 +3 +4 -2 +1 +6 -2
Na2Cr2O7
Al2(CO3)3

14. Now it is time for class work !!!
A101: paper practice (Work Together)
CA101 : computer assignment
Both will be due at beginning of class next time
Ready Set Break !!!

15. Notes Two Unit One Naming Inorganic Salts Example One
Example One Thinking
Example Two
Computer Assignment One

16. Naming Inorganic Salts
TWO parts to the name
1) Cation
2) Anion
Cation Examples
Ca+2
Al+3
Fe+2
Na+1
Anion Examples
Cl-1
NO3-1
SO4-2
N-3
Positive
Negative

17. Example One Iron(II) Fe+2 Iron(III) Fe+3 Name the formula Fe2(CrO4)3
Step #1 Find The + Ion(s).
Iron(II) Fe+2
Iron(III) Fe+3

18. Example One
Step #2 Find The - Ion(s)
Chromate CrO4-2

19. Example One Fe2(CrO4)3 Fe+2 Iron(II) Fe+3 Iron(III) CrO4-2 Chromate
(+2) + Y
(-2) = X
(+3) + Y
(-2) =
X=1
Y=1
X=2
Y=3 1
(+2) + 1
(-2) = 2
(+3) + 3
(-2) = Fe
CrO4
Fe2(CrO4)3

20. Example Two Al2(CO3)3 Al+3 Aluminum CO3-2 Carbonate Aluminum Carbonate
(+3) + Y
(-2) =
X=2
Y=3 2
(+3) + 3
(-2) =
Al2(CO3)3

21. Computer Assignment One/Two
NAMING IONIC COMPOUNDS LEVELs ONE AND TWO

22. Writing a Formula From a Name
(Cation+?)X(Anion-?)Y X
(+?) + Y
(-?) =
If X or Y is 2 or greater...
Lowest Whole Number Ratio
and the ion is polyatomic.
Ba+2 Cr2O Hg Pb+4
( )_( )_
Lithium Nitrate
Li+1 1
NO3-1 1
LiNO3
( )_( )_
Hydrogen Phosphate
H+1 3
PO4-3 1
H3PO4
( )_( )_
Ammonium carbonate
NH4+1 2
CO3-2 1
(NH4)2CO3
( )_( )_
Calcium Arsenate
Ca+2 3
AsO4-3 2
Ca3(AsO4)2
( )_( )_
Iron(III) periodate
Fe+3 1
IO4-1 3
Fe(IO4)3
( )_( )_
Mercury(I) Sulfate
Hg2+2 2
SO4-2 2
Hg2SO4
( )_( )_
Barium Perchlorate
Ba+2 1
ClO4-1 2
Ba(ClO4)2
( )_( )_
Sodium Dichromate
Na+1 2
Cr2O7-2 1
Na2Cr2O7
( )_( )_
Lead(IV) Sulfate
Pb+4 2
SO4-2 4
Pb(SO4)2

23. Notes Three Unit One Standard Amounts One Gopher One Mole Formula mass
Percent Composition
Empirical Formula

24. Standard Amounts How many dollars is… A) 120 pennies? 1.2 dollars
B) 2 quarters?
0.5 dollars
C) 15 nickels?
0.75 dollars
How many dozens is…
D) 48 eggs?
4 dozen
E)18 apple fritters
1.5 dozen

25. One Gopher One Gopher equals 12 items
What is the mass of one gopher of…
A) white beads?
2.81g/G
B) blue beads?
0.50g/G
C) orange Beads?
1.67g/G

26. Seven Rows
Eight Rows

27. One Gopher(12 items) In Six groups
(1) How many gophers of beads are in… (2) How many beads are in… A) ___g B) ___g C) ___g D) ___g E) ___g F) ___g
2.00
48 beads
4.00G
3.49
15 beads
1.24G
2.51
18 beads
1.50G
27 beads
3.75
2.25G
1.75
3.50G
42 beads
5.82
2.07G
25 beads

28. One Mole N O C One mole is 6.022x10+23 items.
Each element on the period table has a mass per mole. N
14.0g
6.022x10+23atoms O
16.0g
6.022x10+23atoms C
12.0g
6.022x10+23atoms
How many moles are in each?
How many atoms are in each? N
7.0g
÷14.0g/m
=0.50m
x6.022x10+23atoms/m
=3.01x10+23atoms O
4.0g
÷16.0g/m
=0.25m
x6.022x10+23atoms/m
=1.51x10+23atoms C
18.0g
÷12.0g/m
=1.50m
x6.022x10+23atoms/m
=9.03x10+23atoms

29. Calculations Bases on Chemical Formulas
Formula mass (Molecular Mass or Gram-Formula Mass)
Empirical Formula
Percent Composition

30. Rounding Atomic Mass C 12.011 12.0 Fe 55.847 55.8 O 15.9994 16.0 Bi
209.0 K
39.1 Au
197.0 Os
190.23
190.2 Mg
24.3 Na
23.0

31. Formula Mass Example One
Calculate the formula mass for 1 mole of C6H12O6. E #
Mass C
6 x
12.0 =
72.0
12.011 H
12 x
1.0 =
12.0
1.0079 O
6 x
16.0 =
96.0
180.0g/mol
How many molecules of C6H12O6 is 180.0g/mol?
6.022x10+23 molecules

32. Empirical Formula Example One
What is the empirical (simplest) formula containing 36.8% N, 63.2% O?
1) Calculate moles of each element. E Q
Mass
Mass N
36.8 g ÷
14.0 =
2.63 mol N O
63.2 g ÷
16.0 =
3.95 mol O
2) Calculate the lowest ratio. E
Moles
Lowest Ratio N
2.63 mol N ÷
2.63 mol =
1.00 O
3.95 mol O ÷
2.63 mol =
1.50
3) Write the formula
X by 2 to get whole numbers
N2O3

33. Percent Composition Example One
Calculate the percentage composition of H2O.
1)Calculate the formula mass for 1 mole of H2O E #
Mass H
2 x
1.0 =
2.0
1.0079 O
1 x
16.0 =
16.0
18.0g/mol
2) Divide each contribution by the total mass. H
2.0 ÷
18.0 =
( x 100) = 11%
0.11
Answer O
16.0 ÷
18.0 =
0.889
( x 100) = 88.9%
3) Add the percentages to check work.
11%
88.9%
100.%

34. Empirical Formula Example Two
What is the empirical (simplest) formula containing 69.58% Ba, 6.090% C, 24.32% O?
1) Calculate moles of each element. E Q
Mass
Mass Ba
69.58 g ÷ =
mol Ba C
6.090 g ÷ =
mol C O
24.32 g ÷ =
mol O
2) Calculate the lowest ratio. E
Moles
Lowest Ratio Ba
mol ÷
mol =
1.000 C
mol ÷
mol =
1.001 O
mol ÷
mol =
3.00
3) Write the formula
X by 1 to get whole numbers
BaCO3

35. Percent Composition Example Two
Calculate the percentage composition of Fe(ClO4)3.
1)Calculate the formula mass for 1 mole of Fe(ClO4)3. E #
Mass
55.847 Fe
1 x
55.8 =
55.8
35.453 Cl
3 x
35.5 =
106.5 O
12 x
16.0 =
192.0
354.3g/mol
2) Divide the each contribution by the total mass. Fe
55.8 ÷ =
( x 100) = 15.8%
0.1575 Cl
106.5 ÷ =
( x 100) = 30.06%
0.3006
Answer O
192.0 ÷ =
( x 100) = 54.19%
0.5419
3) Add the percentages to check work.
15.8 %
30.1 %
54.2 %
100.1%

36. Formula Mass Example Three
Calculate the formula mass for 1 mole of Al2O3 E #
Mass Al
2 x
27.0 =
54.0 O
3 x
16.0 =
48.0
102.0g/mol
How many molecules of Al2O3 is102.0g/mol?
6.022x10+23 molecules

37. Formula Mass Example Two
Calculate the formula mass for 1 mole of CaCO3. E #
Mass
40.078 Ca
1 x
40.1 =
40.1
12.011 C
1 x
12.0 =
12.0 O
3 x
16.0 =
48.0
100.1g/mol
How many molecules of CaCO3 is100.1g/mol?
6.022x10+23 molecules