1. Warm UP - Practice Write or name the following compounds
Ca(OH)2
7) Sr3(PO3)2
8) MgF2
9) LiBr
10) Mn2O7
Iron (III) Nitrite
2) Sodium Chloride
3) Silver Phosphate
4) Cadmium Oxide
5) Aluminum Phosphide

2. Practice 2) MgSO4 • 7 H2O 3) CrBr3• 6H2O 4) Pb(ClO3)2 • 3H2O
1) MnBr2• 4 H2O
2) MgSO4 • 7 H2O
3) CrBr3• 6H2O
4) Pb(ClO3)2 • 3H2O

3. 2) Cobalt(II) chloride hexahydrate 3) Mercury(II) nitrate monohydrate
Practice
1) Beryllium hydroxide octahydrate
2) Cobalt(II) chloride hexahydrate
3) Mercury(II) nitrate monohydrate
4) Tin(IV) chloride pentahydrate

4. Naming & Identifying Acids
All acids contain hydrogen
When acids are dissolved in water, H+ ions are generated
Acids that generate a lot of H+ are strong acids
Acids that generate only a small amount of H+ are weak acids

5. Strong Acids
HCl is a strong acid because no HCl molecules are in a water solution of HCl.
Because of the strong attraction between the water molecules and HCl molecules, every HCl molecule ionizes.

6. Naming & Identifying Acids Cont.
The formula for an acid is: HX
Where X = an anion

7. Naming Binary Acids
Naming Acids:
1. Begin with the regular name
Example HCl is Hydrogen Chloride
2. If the anion ends is “-ide,” add “hydro” as a prefix
3. Replace “-ide” with “-ic”and add acid
Example: HCl
Hydrogen chloride becomes hydrochloric acid
NOTE: It is only an acid with the ending ends in aqueous. If the compound is either gas, liquid, or solid it is not an acid, it is the normal compound.

8. Name the following binary acids
Answers:
1. Hydrofluoric Acid
2. Hydrobromic Acid
3. Hydroiodic Acid
1. HF
2. HBr
3. HI

9. Naming Ternary Acids Ternary acids contain polyatomic ions
To name acids (with 3 or more different elements):
1. Determine regular name of the compound
2. If the anion end in “-ite,” add “-ous” in place of “-ite” and add acid to the end
3. If the anion ends in “-ate,” add “-ic” in place of “-ate” and add acid to the end

10. Examples of Naming Ternary Acids
1. H2SO3
Name: Hydrogen Sulfite
Name of Acid: Sulfurous Acid
2. HNO3
Name: Hydrogen Nitrate
Name of Acid: Nitric Acid
Begin 3rd 4-28

11. Name the following ternary acids
1. H3PO4
2. H2CO3
3. H3PO3

12. Write formulas for the following acids:
1. Chlorous Acid
2. Acetic Acid

13. Warm Up Write the name or formula of the following
Mg(ClO4)2
Copper(II)nitrite
Na3(PO4)
Cu(OH)

14. Covalent Bonds
Covalent Bonds occur when electrons are shared between atoms
Covalent Bonds occur between nonmetals and nonmetals
Examples of Covalent Compounds:
H2O, SO2, CCl4

15. Covalent Compounds are molecular compound
A molecular compound is composed of only NONMETALS
Examples of molecular compounds CO
SF6
H2O

16. Determine if each of the following are molecular compounds
1. CCl4
2. CaCl2
3. Fe2O3
4. P2O5
5. PCl3
6. NH3
7. NaCl

17. Naming Binary Molecular Compounds
Molecular compounds are named using prefixes
You will only use prefixes when TWO NONMETALS are involved

18. Prefixes and Meaning
Mono Di
Tri
Tetra
Penta
1 atom
2 atoms
3 atoms
4 atoms
5 atoms

19. Prefixes and Meaning
Hexa
Hepta
Octa
Nona
Deca
6 atoms
7 atoms
8 atoms
9 atoms
10 atoms

20. Naming Molecular Compounds
With Molecular compounds, use Greek prefixes
The second atom still add “-ide” to its name
NOTE:
If the first element is a single element you do not have to use a prefix.
If the second element is a single element you MUST use a prefix

21. Naming Molecular Compounds
Example:
P2O5
SiCl4
CCl4

22. Write the correct formula for the following
nitrogen monoxide
carbon disulfide
dinitrogen trioxide
sodium nitrate
aluminum oxide
diboron tetrahydride
boron monocarbide

23. Warm-Up
Name or write the following Compounds
1) Sodium Acetate
2) MnO2
3) H3PO4
4) Hydrobromic Acid
5) Calcium Sulfate Pentahydrate
6) disulfur trihydride
7) CH4

24. Practice: Name or write out the following compounds
1. Se2Cl7
2. KMnO4 4 H2O
3. Tetracarbon hexasulfide
4. Al(OH)3
5. Pentanitrogen hexaoxide

25. Name the following compounds
1. SF6
2. N2O5
3. SO3
4. N2O3
5. NaCl

26. Practice Write the correct name for the following
MnO4 • 3 H2O
PH3
SO3
SnO
HCl(aq)
Li2S
H2SO4 (aq)

27. Name the following or write out the following formulas
1) Carbon tetrachloride ) NF3
2) Sulfur difluoride ) S4N4
3) SiO ) Silicon tetrachloride
4) ClF ) Chlorine trifluoride
5) SeO ) Fe(OH)3

28. Review: Determine the number of Valence electrons for the followingBr Sr Pb Fr P Rn

29. Dot Structures –Lewis structure
Dot Structures show the distribution of valence electrons around the nucleus
Rules:
1) Determine number of valence electrons
2) Write chemical symbol
3) Place valence electrons in each of the four directions (north, east, south, & west)

30. 5) Pair up electrons once there is one in each of the four directions
Dot Structures
4) Distribute one valence electron at a time
Do not pair (double up) any electrons until there is one electron in each of the four directions
5) Pair up electrons once there is one in each of the four directions

31. Example – Dot Structure for O
Step 1: O has 6 valence electrons
Step 2: Write chemical Symbol O

32. Example – Dot Structure for O
Step 3: Place valence electrons in each of the four directions (north, east, south, & west)
This is the correct answer!!!
Double up electrons now O
= e-
Place one in each direction first

33. Examples for you
Write Dot Structures for:
1) H
2) Ne
3) P
4) Ca
5) Al

34. Hydrogen Answer H
Note: You can place the electron in any direction you like when you have less than 4 electrons

35. Ne Answer Ne

36. P Answer P

37. Ca Answer Ca

38. Al Answer Al

39. Practice Determine the number of valence electron and draw the dot structure for the following
1) Rb
2) I
3) Te
4) Bi
5) Ra
6) Cl
7) S

40. Types of Covalent Bonds
There are three types of covalent bonds:
single, double, triple
Single Bonds- result when only 1 pair of electrons are shared

41. Types of Covalent BondsH H H

42. Double Bonds
A double bond involves two pairs of electrons being shared

43. Double Bonds Is when two electrons are being shared

44. Triple Bonds
Triple Bonds result when 3 pairs of electrons are shared N N N

45. Writing Lewis Dot Structures
In writing Lewis structures for covalent compounds, you must remember the following:
1. Determine the total number of valence electrons
2. The least electronegative element goes in the center
H is NEVER a center atom
Carbon is usually in the center

46. Writing Lewis Structures
3. Distribute 8 electrons around central atom
4. Place remaining atoms outside of central atom
5. Distribute any remaining electrons around outer atoms

47. Writing Lewis Structures
6. Use double or triple bonds to obey Octet Rule as needed
7. Check to make sure that every atom obeys the Octet Rule

48. Write Lewis Dot Structures for the following:
1. H2O
2. CO2
3. NH3
4. CBr4
5. SO2

49. Practice
Draw the Lewis Structures for the Following:
1) GeF4
2) COS
3) SeO3
4) HOF

50. Practice
Draw the following Lewis Structures
a. CH4
b. SCl2
c. HCN

51. Write Lewis structures for the following compounds: 1. H2S 6. NCl3
On Your Own (In Notes):
Write Lewis structures for the following compounds:
1. H2S NCl3
2. PH HCl
3. ClF CS2
4. NF SeF2
5. N2S

52. Practice
Write Lewis structures for the following molecules:
a. HCN d. PH3
b. CHCl e. SiO2
c. SeF2 f. CF4