1. Coloring the Periodic Table Families
6th Grade Science
Mr. Rohde
Part One

2. If only it was that easy…..

3. Learning Goal for This Unit
To describe the composition and structure of the Earth.

4. I made the PERIODIC TABLE !
I am Dmitri Mendeleev!
I made the PERIODIC TABLE !

5. Mendeleev
In 1869, Dmitri Ivanovitch Mendeléev created the first accepted version of the periodic table.
He grouped elements according to their atomic mass, and as he did, he found that the families had similar chemical properties. 
Blank spaces were left open to add the new elements he predicted would occur. 

6. Today, we are going to set up the periodic table into their groups
Today, we are going to set up the periodic table into their groups. Please have out these colors:
Orange
Green
Blue
Red
Yellow

7. Families on the Periodic Table
Elements on the periodic table can be grouped into families bases on their chemical properties.
Each family has a specific name to differentiate it from the other families in the periodic table.
Elements in each family
react differently with
other elements.

10. Families Periods Columns of elements are called groups or families.
Elements in each family have similar but not identical properties.
All elements in a family have the same number of valence electrons.
Each horizontal row of elements is called a period.
The elements in a period are not alike in properties.
The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas.

11. ALKALI METALS Group 1 Hydrogen is not a member, it is a non-metal
1 electron in the outer shell
Very reactive, esp. with water
Conduct electricity

12. ALKALINE EARTH METALS Group 2 2 electrons in the outer shell Reactive
Conduct electricity

13. TRANSITION METALS Groups in the middle
Good conductors of heat and electricity.
Some are used for jewelry..
Can bond with many elements

14. BORON FAMILY
Group 3
3 electrons in the outer shell
Most are metals

15. CARBON FAMILY
Group 4
4 electrons in the outer shell

16. NITROGEN FAMILY Group 5 5 electrons in the outer shell
Can share electrons to form compounds

17. OXYGEN FAMILY
Group 6
6 electrons in the outer shell

18. Halogens Group 7 7 electrons in the outer shell All are non-metals
Very reactive are often bonded with elements from Group 1

19. Noble Gases Group 8 Exist as gases Non-metals
8 electrons in the outer shell = Full
Not reactive with other elements

20. Rare Earth Metals
Some are Radioactive
Conduct electricity

21. Review Game: Click on this link to help you study your elements:

22. Now that we have set up the periodic table, let’s delve in 
Exit Ticket Time

23. Periodic Table Drawing the Elements
Part 2

24. Let’s start with a joke……
What do you do with a sick chemist?

25. If you can't helium, and you can't curium, then you might as well barium.

26. Learning Goal for This Unit
To describe the composition and structure of the Earth.

27. Bohr Diagrams Find your element on the periodic table.
Determine the number of electrons – it is the same as the atomic number.
This is how many electrons you will draw.

28. Bohr Diagrams Find out which period (row) your element is in.
Elements in the 1st period have one energy level.
Elements in the 2nd period have two energy levels, and so on.

29. C Bohr Diagrams Draw a nucleus with the element symbol inside.
Carbon is in the 2nd period, so it has two energy levels, or shells.
Draw the shells around the nucleus. C

30. C Bohr Diagrams Add the electrons. Carbon has 6 electrons.
The first shell can only hold 2 electrons. C

31. Bohr Diagrams
Since you have 2 electrons already drawn, you need to add 4 more.
These go in the 2nd shell. C

32. C Bohr Diagrams Check your work.
You should have 6 total electrons for Carbon. C

33. Copy this chart: Number of Shells Number of Electrons 1 2 8 3 18 4 325 6 7

34. Now you’re ready to draw Bohr diagrams for the Alkali metals.

35. Periodic Table of Elements
Part 3

36. Learning Goal for This Unit
To describe the composition and structure of the Earth.

37. Elements
The elements, alone or in combinations, make up our bodies, our world, our sun, and in fact, the entire universe.

40. Last week, you took a look at the Alkali metals
Last week, you took a look at the Alkali metals. We talked about the Valence electrons and how they are the electrons that react or mix with other mixtures or elements. Let’s see them in action.

41. Elements
Science has come along way since Aristotle’s theory of Air, Water, Fire, and Earth.
Scientists have identified 94 naturally occurring elements, and created about 24 others.

42. The most abundant element in the earth’s crust is oxygen.

43. All About the Periodic Table Article
When you read this article, please take notes on the three sections (structure, classification, and chemical properties).
We will be discussing this shortly.

44. Let’s unlock the information found on the Periodic Table!!!
The periodic table organizes the elements in a particular way. A great deal of information about an element can be gathered from its position in the period table.
Understanding the organization and plan of the periodic table will help you obtain basic information about each of the 117 KNOWN elements.
Let’s unlock the information found on the Periodic Table!!!

45. Key to the Periodic Table
Elements are organized on the table according to their atomic number, usually found near the top of the square.
The atomic number refers to how many protons an atom of that element has.

46. What’s in a square?
Different periodic tables can include various bits of information, but usually:
atomic number
symbol
atomic mass
number of valence (electrons the element shares) electrons
state of matter at room temperature.

47. Atomic Number
This refers to how many protons an atom of that element has.
No two elements, have the same number of protons.
Bohr Model of ________Atom
Wave Model

48. Atomic Mass Atomic Mass refers to the “weight” of the atom.
It is derived at by adding the number of protons with the number of neutrons.
This is a ________atom.
What is its atomic number? H

49. How to find the number of electrons, protons, and neutrons.
Electrons are the same as the Atomic number. This number also gives you the number of protons.
For neutrons, find the atomic mass (rounded to nearest whole number).
Atomic mass=Protons + Neutrons

50. Exit Ticket Time 
Today, you will be completing an exit ticket that asks you to:
Construct Bohr models
Describe protons, electrons, and neutrons
Calculate the number of protons, electrons, and neutrons that you would find in an element.

51. C Cu Symbols Carbon Copper All elements have their own unique symbol.
It can consist of a single capital letter, or a capital letter and one or two lower case letters. C
Carbon Cu
Copper

52. Common Elements and Symbols

53. Valence Electrons
The number of valence electrons an atom has may also appear in a square.
Valence electrons are the electrons in the outer energy level of an atom.
These are the electrons that are transferred or shared when atoms bond together.

55. Properties of Metals
Metals are good conductors of heat and electricity.
Metals are shiny.
A chemical property of metal is its reaction with water which results in corrosion.

56. Properties of Non-Metals
Non-metals are poor conductors of heat and electricity.
Solid non-metals are brittle and break easily.
They are dull.
Many non-metals are gases.
Sulfur

57. Properties of Metalloids
Metalloids (metal-like) have properties of both metals and non-metals.
They are solids that can be shiny or dull.
They conduct heat and electricity better than non-metals but not as well as metals.
Silicon

58. Exit Ticket:

59. Transition Metals:
Part 4

60. Learning Goal for This Unit
To describe the composition and structure of the Earth.

61. Opening Ceremony for Sochi Olympics?
Why would this be there?

62. Remember the rules for constructing Bohr Models:
Number of Shells
Number of Electrons 1 2 8 3 18 4 32 5 6 7

63. In order to start creating compounds and mixtures, we have one more part of the periodic table left to look at…….
The Transition Metals

64. Rules for constructing transition metals:
Every shell (excluding the last shell) should have electrons in pairs.
The same rule applies with the period telling us how many shells the element has.
There is NO rule for the number of Valence Electrons.

65. Please get out your individual white boards from your desk and lets get ready to construct some Bohr Models 
We’ll start with a review and then get into the Transition Metals.

66. Exit Ticket:
How many Valence Electrons are in the element Bromine (Halogen)?
Why was there a picture of the periodic table at the Olympics?
Construct a Bohr Model for the element Silver (47 electrons. 5th period. 108 mass)

67. Compounds and Mixtures
Part 5

68. Learning Goal for This Unit
To describe the composition and structure of the Earth.

69. Mixtures, elements, compounds
Scientists like to classify things.
One way that scientists classify matter is by its composition.
Ultimately, all matter can be classified as mixtures, elements and compounds.

70. Why isn’t it a good idea to classify matter by its phases?
Because one kind of substance can exist in more than one phase – such as H20. And matter changes phases rather easily.

71. What does it mean to be reactive?
Elements that are reactive bond easily with other elements to make compounds.
Some elements are only found in nature bonded with other elements.
What makes an element reactive?
An incomplete valence electron level.
All atoms (except hydrogen) want to have 8 electrons in their very outermost energy level
Atoms bond until this level is complete. Atoms with few valence electrons lose them during bonding.

72. Ionic vs Covalent Bonding
Ionic: electron(s) leave one atom & gained by another atom to satisfy both atoms’ octets, this results in the formation of ions. The resulting opposite charges attract each other.
Covalent: electrons are shared by two or more atoms to satisfy their octets.

73. How can you tell if a bond is IONIC or COVALENT?
Easy way:
All metals = metallic bond
Nonmetals and Metals = ionic bond
All nonmetals = covalent bond

74. The closer the elements are on the periodic table, their electronegativities are more similar… more likely to form covalent bonds
Farther away… greater difference in electronegativity… more likely to form ionic bonds.
Metal + nonmetal = usually ionic
Nonmetal + nonmetal = usually covalent.

75. 5

78. What is an ELEMENT? A substance composed of a single kind of atom.
Cannot be broken down into another substance by chemical or physical means.

79. What is a COMPOUND?
A substance in which two or more different elements are CHEMICALLY bonded together.

80. What is a MIXTURE?
Two or more substances that are mixed together but are NOT chemically bonded.

81. Element, Compound or Mixture?

82. Element, Compound or Mixture?

83. Element, Compound or Mixture?

84. Element, Compound or Mixture?

85. Element, Compound or Mixture?

86. Element, Compound or Mixture?