1. Bell Ringer How many groups are on the periodic table?
How many periods are on the periodic table?
How many elements are on the current periodic table?
Elements on the left of the staircase are classified as what?
Elements on the staircase are classified as what, because?
Elements on the right of the staircase are classified as what?

2. Chemical Bonds
Chapter 6

3. Making bonds
Bonding gives the molecule completely different chemical properties than its parent elements.
Ex: Salt (NaCl)
Sodium is a metal that is violently reactive with water. 
Chlorine is a highly toxic, greenish-colored gas. 
Bonding stabilizes these two elements.

4. Valence Electrons
Valence electron: an electron that is in the highest occupied energy level of an atom
-Each Valence e- has an e- charge
Group # = Valence #
Think about your Bohr Model

5. Valence e- and e- charges
All valence electrons have charges
Group# valence e- e-charge
Group1A
Group2A
Group3A
Group4A
Group5A
Group6A
Group7A
Group8A

7. Visualize and Understand the RelationshipBe O

8. Bonding Atoms bond between their _________ e-
Represented in a ___________ dot diagram.
This show the relationship of bonding between elements.

9. Electron Configuration
***Valence Electrons in the highest energy level***
Group A 1, 2, 3-8
Electron Dot Diagrams show the number of valence electrons
Write the symbol
Place a LARGE dot for each valence electron
1 dot on each side before pairing them up
end

10. Electron Configuration
end

11. Electron Configuration
Draw diagrams for the following: Sr
How many Valence electrons?
What is the charge of this electron?
end

12. Draw diagrams for the following:Si
How many Valence electrons?
What is the charge of this electron?

13. Draw diagrams for the following:Cl
How many Valence electrons?
What is the charge of this electron?

14. Lewis Dot Diagram
Fill in your Lewis Dot Structure Worksheet.

15. E- charges Most metals have _______ charges
Most non-metals have a _______ charge
L of staircase mostly (___) charge
R of staircase mostly (___) charge

16. Metals and Non
Metals, with only a few electrons in the outer energy level, tend to ____ electrons
 Non-metals, which lack only one or two electrons in the outer energy level have a tendency to _____ electrons.

17. Chemical Formulas

18. Chemical Formulas Chemical Formula NaCl CO2 MgCl2 Na3P
Subscripts show the number of atoms of each element in the compound
1 atom = No Subscript!
NaCl
CO2
MgCl2
Na3P
end

19. Chemical Formulas How many total atoms are in each of these:
TRY ON YOUR OWN!
H2SO4
KNO3
Fe2O3
Hg2Cl2
end

20. On your Own Worksheet Problems 1-8
Label the element and the # of atoms

21. Chemical Formulas Polyatomic Ions OH-, PO43-
Last page of your Reference Tables!!!
More than 1 Polyatomic Ion =
Write inside ( )
Put a subscript OUTSIDE
end

22. Chemical Formulas
Ba(OH)2
Cu (NO3)2
NH4NO3
(NH4)2O

23. Chemical Formulas How many total atoms are in each of these: Cu(NO3)2
end

24. How many total atoms are in each of these:
KMnO4

25. How many total atoms are in each of these:
Al2(SO4)3

26. How many total atoms are in each of these:
(NH4)3PO4

27. How many total atoms are in each of these:
Mg(C2H3O2)2

28. Counting Atoms
Worksheet 1-9

29. Worksheet On Back of Worksheet Identify and Count Atoms
Grab a book and copy onto your worksheet or a separate sheet of paper the following vocabulary words:
Electron Dot Diagram
Ion
Chemical Bond
Chemical Formula
Molecule
Crystal
Polyatomic Ion
When you are done, I want to check your work.

30. Bell Ringer Draw a Lewis Dot Structure for the following elements: FSi Mg
What is an ion?

31. Bonding

32. Electron Configuration
All atoms want 8 valence electrons
8 valence = Stable (DO NOT REACT)
Noble Gases
To get 8 valence, atoms can either:
Transfer Electrons:
Lose Electrons to drop an energy level
Gain Electrons till they have 8
Share Electrons with other atoms, so everyone has 8
end

33. Chemical Bonding Chemical Bond 3 types Ionic (Metal and Nonmetal)
Covalent (Nonmetal and Nonmetal)
Metallic (Metal and Metal)
end

34. Chemical Bonding Identify the following as ionic or covalent
CaCl LiBr
CO SO3
H2O CH4
end

35. Classify on Own
BaS Na2O3
K2O NaF
MgO N4Cl
HCl KI

36. Ionic Bonding Ionic Bonding Cation Anion
Metal and Nonmetal (or polyatomic ion)
Electrons are TRANSFERRED from the cation to the anion
Cation
Positive (a Metal)
Has Lost Electrons
Anion
Negative (a Nonmetal)
Has Gained Electrons
end

37. Ionic Bonding Ions have the same electrons as Noble Gases
Making them stable
Metals (Groups 1 to 13) become like the noble gas Before the element
Na  Lose 1 e-  Ne
Sr  Lose 2 e-  Kr
end

38. Ionic Bonding Changing the # of e- makes the atom an ION
Nonmetals (Groups 15 to 17) become like the noble gas After the element
O  Gain 2 e-  Ne
I  Gain 1 e-  Xe
Changing the # of e- makes the atom an ION
Has a charge called an Oxidation State
end

39. Ionic Bonding Oxidation States follow the # of Valence Electrons
Group:
Valence e-:
Oxidation #: ±
end

40. Ionic Bonding
Show the transfer of electrons with an Electron Dot Diagram
sodium chloride (NaCl)
Na + Cl 
[ ]+
[ ]- Na Cl
end

41. Bonding
Draw Electron Dot Diagrams for: KF
MgO
MgCl2
end

42. Bonding
On Own Complete Diagram Worksheet

43. Periodic Table Activity
Online to Complete in place of article assignment this week!

44. Bell Ringer Draw and electron diagram for Table Salt.
What is a bond between a metal and non-metal called?
What is a bond between two non-metals called?
What is a cation?
What is an anion?
Lab Safety Tip #

45. Naming Ionic Compound Naming Ionic Compounds: 3 steps
Name the Cation (the metal)
Name the Anion (the nonmetal)
Change the Ending on the anion to –ide
IGNORE THE SUBSCRIPTS!!!
NaBr
Sodium
Bromine
Sodium
Bromide
end

46. Naming Ionic Compounds
Name the following:
BaS
MgF2
Ca3N2
end

47. Naming Ionic Compounds
Complete the following on “Names of Ionic Compounds’ worksheet
1 9
2 13
8 16
6 18
8 19 25

48. Naming Ionic Compounds
More than 2 elements = POLYATOMIC ION!!!
LOOK AT YOUR REFERENCE TABLE!!!
Follow the same steps to name the compound
Get the polyatomic’s name from the reference tables!
DON’T change the ending of a polyatomic ion
NaNO3
Sodium
Nitrate
end

49. Naming Ionic Compounds
Name the following:
KOH
NaC2H3O2
(NH4)2O
Sr3(PO4)2
end

50. Naming Ionic Compounds
Complete on “Names of Ionic Compounds”
# 3, 4, 5, 7, 11, 12, 14, 15, 17, 21, 24

51. Writing Ionic Formulas
Writing formulas:
3 steps:
Write the positive ion, with charge
Write the negative ion, with charge
Cross the charges to get subscripts
Do NOT put the “+” or “-”
end

52. Writing Ionic Formulas
Write the formulas for the following:
Beryllium Phosphide
Calcium Fluoride
Lithium Iodide
Strontium Sulfide
end

53. Writing Ionic Compounds
Complete numbers 1-10 on “Writing Binary Formulas”

54. Writing Ionic Formulas
Remember: Polyatomic Ions ARE A GROUP
When you cross charges, the subscript applies to the WHOLE GROUP
USE ( )
end

55. Writing Ionic Formulas
Write the formula for the following:
Potassium Nitrate
Barium Chromate
Aluminum Acetate
Ammonium Sulfate
end

56. Transition Metals Transition Metals have 2 valence electrons
But they have Many Oxidation States
So we write their names differently
end

57. Transition Metals Follow the same steps to write the formula
The metal's charge is the Roman Numeral
Vanadium (III) Sulfide
V S2-
V2S3
Metal's Charge
end

58. Transition Metals Write formulas for the following:
Osmium (V) Fluoride
Silver (I) Nitride
Technetium (VII) Phosphate
end

59. Transition Metals
When naming you MUST put the charge as a Roman Numeral!
To figure out the charge, uncross the subscripts!
Fe2O3
Fe O2-
iron (III) oxide
end

60. Transition Metals
Name the following:
HgF2
Hf2S5
Y3P7
end

61. Naming Ionic Compounds
Complete the following on “Naming Binary Compounds (Ionic)”

62. Bell Ringer Silver (I) oxide Copper (I) bromide Copper (II) bromide
Iron (II) oxide
Iron (III) oxide
Chromium (II) chloride
Chromium (III) chloride
Mercury (I) Iodide
Manganese (II) oxide

63. Covalent Bonding Naming and Writing Formulas

64. Covalent Bonding Covalent Bond
Nonmetal and Nonmetal
Atoms SHARE electrons
7 nonmetals that never exist by themselves.
Form pairs with each other
Called Diatomics (H, N, O, F, Cl, Br, I)
end

65. Covalent Bonding
The number of electrons shared create different types of bonds
2 shared electrons — single bond
4 shared electrons = double bond
6 shared electrons ≡ triple bond
end

66. Naming Covalent Molecules
Number
Prefix 1
Mono- 2
Di- 3
Tri- 4
Tetra- 5
Penta- 6
Hexa- 7
Hepta- 8
Octa- 9
Nona- 10
Deca-
When naming Covalent Molecules:
Use a prefix for the first element
If it is 1, do NOT use a prefix
Name the first element
Use a prefix for the second element
Always!!!
Name the second element AND change the ending to –ide
end

67. Naming Covalent Molecules
Practice:
As2O3
N2H4
CCl4 SO
end

68. Naming Covalent Molecules
Complete 9-16 on “Naming Covalent Compounds”
SKIP #4

69. Writing Covalent Formulas
Writing formulas:
Write the symbol of the first element
Use the prefix for the subscript
Write the symbol of the second element
end

70. Formulas of Covalent Molecules
Practice:
Disulfur trioxide
Dinitrogen monoxide
Phosphorus pentachloride
Diphosphorus pentoxide
Carbon dioxide
end

71. Complete 'Naming Covalent Compounds Worksheet' 1-8

72. Try 1-20 on your own under Formulas and Nomenclature of Covalent Compounds

73. USE YOUR EDUCREATION APP
MIXED REVIEW
USE YOUR EDUCREATION APP

74. Finish on Front of worksheet On the Back Complete the chapeter review problems from the book, when you are done, turn it into the box! IF TIME…WORK ON BONDING DRY LAB