1. Bellringer: 3/7/2018
**Get out the periodic table you colored and answer the following:
Where can you find the halogens?
What is the most reactive nonmetal
What 2 elements are liquid at room temperature?
STOTD
**Have you turned in your Unit 3 Packet?

2. The Periodic Table By 1860 scientists had discovered 63 elements
But there was no good way to organize them
Scientists had to memorized everything
This was changed by Mendeleev
end

3. The Periodic Table Mendeleev’s Periodic Table:
Elements with similar properties were placed in the same column
The mass of the elements increased along each row
end

4. The Periodic Table
Mendeleev left several blank spaces in his periodic table
For elements that had not been discovered yet
He correctly predicted the properties of these elements based on the elements around them
end

5. The Periodic Table The Modern Periodic Table:
Based on Mendeleev’s table
Similar Properties are in the Same Column
Columns are called Groups
Numbered 1 to 18 (from left to right)
Atomic Numbers increase going across the table
Rows are called Periods
Numbered 1 to 7 (from top to bottom)
end

6. The Periodic Table This is the full Periodic Table
As you can see it is REALLY long
Way too long to fit on a page
end

7. The Periodic Table
To make everything fit on 1 page, the Lanthanides and Actinides are moved to the bottom
end

8. The Periodic Table Metals Left of the stair-step line
Francium (Fr) is the most reactive
Moving away from Fr, metals become less reactive
Good conductors of electricity and heat
Mostly solids at room temperature
High melting and boiling points
Malleable and ductile
end

9. The Periodic Table Nonmetals Right of the stair-step line
Fluorine (F) is the most reactive nonmetal
Moving away from F, nonmetals become less reactive
Poor conductors of heat and electricity
Mostly gases at room temperature
Low melting and boiling points
Not malleable and not ductile
end

10. The Periodic Table Metalloids Touching the stair-step line
Have properties between metals and nonmetals
Depends on the temperature
end

11. The Periodic Table: Group Names
Alkali Metals
Lanthanide and Actinide Series
Group 1
At the bottom of the table
EXTREMELY REACTIVE!
All are radioactive
Alkaline Earth Metals
Halogens
Group 2
Group 17
Transition Metals
Highly Reactive
Groups 3 to 12
Noble Gases
Have a wide variety of properties
Group 18
Extremely Unreactive
THEY DO NOTHING!
end

12. The Periodic Table Atomic Size Valence Electrons
Francium (Fr) is the largest atom
Helium (He) is the smallest atom
The closer to Fr, the larger the atom
Valence Electrons
Electrons in the highest energy level
Give Elements their Chemical Properties
Group:
# of
Valence:
end

13. Chemical Bonds
Chapter 6

14. Chemical Formulas Chemical Formula CO2 NaCl MgCl2 Na3P
Shows what elements are in a compound
If there is more than 1 atom of an element we add subscripts to show how many
CO2
NaCl
MgCl2
Na3P
1 C and 2 O
1 Na and 1 Cl
O C O
1 Mg and 2 Cl
CO2
3 Na and 1 P
end

15. Chemical Formulas 7 5 3 8 4 How many total atoms are in each of these:
H2SO4
KNO3
CaCl2
C2H6
H2O2
H2O
Fe2O3
Hg2Cl2 7 5 3 8 4 O
H O S O H H
H2SO4
end

16. Chemical Formulas Some compounds have large groups of atoms
Polyatomic Ions
OH-, PO43-, NO3-, NH4+
Last page of your Reference Tables!!!
If there is more than 1 Polyatomic Ion,
Write the group inside ( )
And put a subscripts outside to tell how many
end

17. Chemical Formulas Ba(OH)2 Cu (NO3)2 NH4NO3 (NH4)2O 1 Ba 1 Cu 2 OH
end

18. Chemical Formulas
How many total atoms are in each of these:
Cu(NO3)2
KMnO4
Ba(OH)2
NH4Br
Ca3(PO4)2
Al2(SO4)3
(NH4)3PO4
Mg(C2H3O2)2 9 6 5 13 17 20 15
end

19. Bellringer: How many atoms are in the following: STOTD H2SO4 KNO3
CaCl2
C2H6
STOTD

20. Electron Configuration
Valence Electrons
Valence Electrons are found in the highest energy level
Electron Dot Diagrams are used to show the number of valence electrons
Write the symbol for the element
Place large dots around the symbol to represent each valence electron
Put 1 dot on each side before pairing them up
end

21. Valence Electrons “1,2, skip a few…”
Transition Metals beat to their own drum!

22. Electron Configuration
Draw diagrams for the following: Sr Si Cl
end

23. Bellringer: Draw an electron dot diagram for Sulfur.
Count the total atoms:
CaCO3
KBr
Mg(NO3)2
3. STOTD

24. What is a valence electron?
Bellringer:
What is a valence electron?
Draw a Bohr model for carbon-13. How many valence electrons does it have?
STOTD

25. Electron Configuration
All atoms want to have 8 valence electrons
Atoms with 8 valence do not react with other things
In order to get 8 valence atoms can either:
Transfer Electrons:
Lose Electrons
Gain Electrons till they have 8
Share Electrons with other atoms, so everyone has 8
end

26. Chemical Bonding Chemical Bond 3 types
The force that holds atoms or ions together
3 types
Ionic
Metal and Nonmetal (Including Polyatomic Ions)
Covalent
Nonmetal and Nonmetal
Metallic
Metal and Metal
end

27. Chemical Bonding I C I C Identify the following as ionic or covalent
CaCl LiBr
CO SO3
H2O CH4
BaSO Na2CO3
K2O NaF
MgO NH4Cl
HCl KI I C I C
end

28. Ionic Bonding Ionic Bonding Holds cations and anions together
Between a metal and a nonmetal (or polyatomic ion)
Electrons are transferred from the cation to the anion
Cation
Metal
Anion
Nonmetal
end

29. Cation
A positively charged atom, usually a metal
Has Lost Electrons
Anion
A negatively charged atom, usually a nonmetal
Has Gained Electrons

30. Ionic Bonding Groups 1, 2, 13 lose electrons/cations
Group 14 can either gain or lose electrons
Groups 15, 16, 17 gain electrons/anions
As the number of electrons changes the atom becomes an ion (has a charge)
This charge is called an Oxidation State
end

31. Ionic Bonding Oxidation States follows the # of Valence Electrons
There is a PT trend for Oxidation states!
Oxidation States follows the # of Valence Electrons
Group
Oxidation ve
end

32. Ionic Bonding
We can show the transfer of electrons using an Electron Dot Diagram
Start with sodium chloride (NaCl)
Na + Cl 
[ ]+
[ ]- Na Cl
Draw Electron Dot Diagrams for: KF
MgO
MgCl2
end

33. Bellringer: What is an oxidation state?
What is the oxidation state for group 1 elements?
How are cations and anions different?
STOTD

34. Ionic Bonding
Ionic Compounds form a structure called a Crystal Lattice
The cations and anions alternate to form a cube
Cl-
Na+
end

35. Naming Ionic Compound Naming Ionic Compounds is easy.
There are 3 steps
Name the Cation (the metal)
Name the Anion (the nonmetal)
Change the Ending on the anion to –ide
Sodium
Bromine
Bromide
Sodium
NaBr
Name the following:
BaS
MgF2
Ca3N2
end

36. Write the names of the following compounds:
KCl
BeO
Na3P
LiBr

37. Naming Ionic Compounds
If there are more than 2 elements,
YOU HAVE A POLYATOMIC ION!!!
LOOK AT YOUR REFERENCE TABLE!!!
Follow the same steps to name the compound
Get the polyatomic’s name from the reference tables!
But don’t change the endings for polyatomic ions
NaNO3
Sodium
Nitrate
Name the following:
(NH4)2O
KOH
Sr3(PO4)2
NaC2H3O2
end

38. Bellringer:
Explain the difference between an ionic bond and a covalent bond.
How would you name the following compounds:
CaCl2
Ba(NO3)2
STOTD
**ELEMENT QUIZ TODAY
** IONIC BONDING QUIZ FRIDAY

39. Writing Ionic Formulas
To write formulas from the names:
There are 3 easy steps:
Write the positive ion, with charge
Write the negative ion, with charge
Cross the charge numbers to get your subscripts
Do NOT put the “+” or “-”
Write the formulas for the following:
Beryllium Phosphide
Calcium Fluoride
Lithium Iodide
Strontium Sulfide
end

40. Writing Ionic Formulas
Watch out for Polyatomic Ions
Follow the same steps to write the formula
Remember: The polyatomic ion IS A GROUP
When you cross charges, the subscript applies to the WHOLE GROUP
Write the formula for the following:
Potassium Nitrate
Barium Chlorate
Aluminum Acetate
Ammonium Sulfate
end

41. Bellringer: What is the chemical formula for Francium Sulfide?
What is the chemical formula for Aluminum Phosphate?
What is the name of SrCl2?
What is the name of Mg(OH)2?
STOTD
**Ionic bonding quiz on Friday

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

43. 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

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

45. 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

46. Transition Metals
Name the following:
HgF2
Hf2S5 YP
end

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

48. HW
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 Manganese (III) oxide

49. Bellringer:
Compare and contrast metals and nonmetals. Be sure to mention the differences in their properties.
How are transition metals different from all of the other elements on the periodic table.
STOTD

50. Bellringer: Name the following: Write formulas for the following:
Ca(OH)2
MgO
Ti2S3
Write formulas for the following:
Potassium chloride
Barium phosphate
Iron (II) bromide
***STOTD

51. Bellringer: Identify each bond as either covalent or ionic:
N2O
CaS
CO2
Draw an electron dot diagram for iodine.
How many atoms of sodium are there in sodium phosphide?
STOTD

52. Covalent Bonding Covalent Bond
Between a nonmetal and a nonmetal
Atoms SHARE electrons
There are 7 nonmetals that never exist by themselves.
form pairs with each other
These are called the Diatomics (H, N, O, F, Cl, Br, I)
BrIN-Cl-HOF
Look for the 7 on the P.T.
end

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

54. Covalent Bonding
Show the electrons being shared with an Electron Dot Diagram
Start with chlorine (Cl2)
Cl + Cl  Cl Cl
end

55. Covalent Bonding
Draw the Electron Dot Diagrams for: H2 N2

56. Covalent Bonding Atoms never share electrons equally
These are called Polar Molecules
1 side is negative
Has the electrons
And 1 side is positive
It doesn’t have the electrons
end

57. 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

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

59. Naming Covalent Molecules
Complete 1-10 on “Naming Molecular Compounds”

60. Writing Covalent Formulas
Writing the formula for covalent molecules is easy:
Write the symbol of the first element
Use the prefix to write the subscript
Write the symbol of the second element
end

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

62. Bellringer: Name the following: Write formulas for the following:
As2O3
N2H4
BaO
K3PO4
Write formulas for the following:
Dinitrogen monoxide
Phosphorus pentachloride
Francium Phosphide
Magnesium Sulfate
STOTD

63. Metallic Bonding Metallic Bond
Between metals
In metallic bonds valence electrons are shared between all of the atoms in the substance
A “sea of electrons”
end

64. Metallic Bonding
The more valence electrons metals have to share the stronger the metallic bond will be
Because there is a sea of electrons metals are malleable and conduct electricity
Alloy
Mixture of 2 or more elements
1 element must be a metal
Alloys with specific properties can be created by mixing different types of elements in different amounts
end

65. Properties of Ionic Bonds
Conduct electricity when dissolved
Not Malleable
Not flammable
High melting point and high boiling point
Form a crystal

66. Properties of Covalent Bonds
Will not conduct electricity
Malleable
Flammable
Low melting point and boiling point
Have many structures