1. Periodic Table Families
Some images are from
2008

4. 3/5/14 IQ
Discuss what happens when an energy level gets full with the amount of electrons it can hold

5. Energy Levels Electrons are arranged in energy levels.
Electrons with the lowest energy can be found in the energy level closest to the nucleus.
Energy levels can hold 2, 8, 18
The first 18 elements can hold:
1st level: 2 electrons
2nd level: 8 electrons
3rd level: 8 electrons
*When you get into higher numbered elements, we go to the 2,8,18 shells

6. Valence Electrons
Electrons in an atom are not all the same distance from the nucleus. Electrons farthest away from nucleus are called valence electrons.
Valence electrons are involved in chemical bonds.

7. Group 1: 1 valence electron
Group 2: 2 valence electrons
Group 13: 3 valence electrons
Group 14: 4 valence electrons
Group 15: 5 valence electrons
Group 16: 6 valence electrons
Group 17: 7 valence electrons
Group 18: 8 valence electrons -- except for helium, which has 2

8. The # of Valence electrons an atom has is dictated by the Group (vertical column) the element is in.

9. Examples: Mg= Group _2__ A so it has ____ valence electrons
Examples: Mg= Group _2__ A so it has ____ valence electrons. Li= Group _1__ A so it has ____ valence electrons.

10. Valence Electrons the Quick and Easy Way13 3A 5 B
Boron
Use the group number! 13 Al
Aluminum 31 Ga
Gallium
All of the elements in Group 13 or will have three valence electrons.

11. Valence Electrons the Quick and Easy Way
Determine the number of valence electrons.
Phosphorus
Argon
Lead
Barium
5 valence electrons
8 valence electrons
4 valence electrons
2 valence electrons

12. Electron Dot Diagram
Used to represent the valence electrons of an atom.
Elements can have between 1-8 valence electrons.
During a chemical bond the element usually ends up with either 0 or 8 valence electrons.

13. Determine the number of shells and the number of valence electrons for:
Carbon - C
2nd Period = 2 shells
4th Group =
4 valence
electrons

14. Determine the number of shells and the number of valence electrons for:
Sodium - Na
3rd Period = 3 shells
1st Group =
1 valence
electron

15. Write your answers on your handout.Ne
Name the element.
Number of shells ?
Valence electrons ?

16. Write your answers on your handout.Ne
Name the element.
Number of shells ?
Valence electrons ?
Neon
2nd Period = 2 shells
8th Group = 8 valence
electrons

17. Write your answers on your handout.
Name the element.
Number of shells ?
Valence electrons ?

18. Write your answers on your handout.
Name the element.
Number of shells ?
Valence electrons ?
Hydrogen
1st Period = 1 shell
1st Group = 1 valence
electron

19. Write your answers on your handout.Be
Name the element.
Number of shells ?
Valence electrons ?

20. Write your answers on your handout.Be
Name the element.
Number of shells ?
Valence electrons ?
Beryllium
2nd Period = 2 shells
2nd Group = 2 valence
electrons

21. Write your answers on your handout.
Name the element.
Number of shells ?
Valence electrons ?

22. Write your answers on your handout.
Name the element.
Number of shells ?
Valence electrons ?
Sulfur
3rd Period = 3 shells
6th Group = 6 valence
electrons

23. Write your answers on your handout.K
Name the element.
Number of shells ?
Valence electrons ?

24. Write your answers on your handout.K
Name the element.
Number of shells ?
Valence electrons ?
Potassium
4th Period = 4 shells
1st Group = 1 valence
electron

25. Write your answers on your handout.He
Name the element.
Number of shells ?
Valence electrons ?

26. Write your answers on your handout.He
Name the element.
Number of shells ?
Valence electrons ?
Helium
1st Period = 1 shell
8th Group = 2 valence
electrons
Helium is the exception in Group 8.
Since it has just one shell, that shell can only fit 2 electrons instead of 8.
It is in this group because all the elements have a full outer shell.

27. Chemical Bonds
Forms between two atoms when valence electrons move between them. The valence electrons may be transferred from one atom to another, or they may be shared.

28. If the valence shell is full, then the element is inert
If the valence shell is full, then the element is inert. If the valence shell isn't full, then the element is reactive, which means that it can form a bond with an atom of another element. Each atom shares its valence electrons in an attempt to complete its own valence shell.

29. Atoms tend to be most stable with a full outer shell
Atoms that do not have full outer shells will tend to gain or lose electrons, resulting in a full outer shell, creating stability

30. Drawing a Carbon Atom

31. IQ /3/14
Describe one way that the periodic table is arranged.

32. Modern Periodic Table
Period: Horizontal row. Properties of elements follow a repeating, or periodic pattern as you move across each row.
Family/Group: Vertical column. Elements in the same group often have similar chemical and physical properties
Elements are arranged by increasing atomic number (#of protons)

33. An element’s properties can be predicted from its location on the table.
Across the row or down a column the elements’ properties change in a predictable way.

34. We Do Together: Please get out a separate sheet of paper
Draw a model of each atom.
Lithium
Boron
Oxygen
Potassium
Include:
Correct number of protons and neutrons in the nucleus
Correct number of electrons, in their corresponding energy levels
IS YOUR LAST ENERGY LEVEL FULL? YES OR NO?
Use page 744 as a guide.

35. YOU DO: Classwork: On a separate sheet of paper, Draw a model of each atom.
Helium
Neon
Aluminum
Chlorine
Include:
Correct number of protons and neutrons in the nucleus
Correct number of electrons, in their corresponding energy levels
IS YOUR LAST ENERGY LEVEL FULL? YES OR NO?
Use page 744 as a guide.

36. IQ 3/10/14 What does a group tell you on the periodic table?
What does a period tell you?

37. Groups or Families Elements in a column.
Numbered 1 on left to 18 on right.
Elements in a group have similar characteristics.
They have the same number of valence electrons (electrons in the outermost shell/level).

38. Groups cont. Based on their chemical properties.
Each group has a specific name to differentiate it from other groups in the periodic table.
Elements in each group
react differently with
other elements.

39. Periods or Rows Contains a series of elements from different groups.
The elements have very different properties.
7 periods of elements.
7 electron shells
The elements change in a predictable way from left to right.
Most reactive to least reactive

40. Periods The elements in each period have the same number of shells
1st Period = 1 Shell
2nd Period = 2 Shells
3rd Period = 3 Shells
4th Period = 4 Shells

41. Groups Group 8 = 8 electrons Group 1 = 1 electron
Except for He, it has 2 electrons
Group 2 = 2 electrons
Each column is called a “group”
3, 4, 5, 6, 7
Each element in a group has the same number of electrons in their outer orbital, also known as “shells”.
The electrons in the outer shell are called “valence electrons”

42. IQ 3/11/14 Describe some characteristics about metals.
What are some common uses of metals?

43. Metals Found on the left of the zig-zag line.
Metals are based on physical properties of hardness, shininess, malleability, ductility.
Malleability means that it can be pounded into shapes.
Ductility means that the metal can be pulled out or drawn into a long wire.

44. Conductors – most metals can transmit heat and electricity easily.
Magnetic – several metals can be made into magnets or are attracted to magnets. (iron, cobalt, nickel)

45. Chemical Properties of Metals
Some very reactive – sometimes explosive others not reactive at all.
Metals on the left of the table, Family 1, are the most reactive and they become less and less reactive as you move right.

46. ALKALI METALS Group 1 Hydrogen is not a member, it is a non-metal
1 electron in the outer shell, which can be easily given away
Soft and shiny, silvery metals
Very reactive, esp. with water
Conduct electricity
Never found alone in nature, always in a compound.
Image:

47. ALKALINE EARTH METALS Group 2
2 valence electrons, which they can easily lose
White and malleable
Reactive, but less than Alkali metals
Conduct electricity
Not as reactive as Group 1 but more reactive than most metals.

48. TRANSITION METALS Groups in the middle
Good conductors of heat and electricity.
Some are used for jewelry.
The transition metals are able to put up to 32 electrons in their second to last shell.
Can bond with many elements in a variety of shapes.
Group 3 – 12
Form a bridge between the very reactive metals on the left side and the less reactive metals on the right.
Very similar so that it is difficult to detect differences from one column to the next.
Fairly stable, reacting slowly or not at all with air and water.

49. Metals in Mixed Groups
Groups 13 – 16 include: metals, nonmetals, metalloids.
The metals to the right of the transition metals are not as reactive as Groups 1 &2.

50. Bonding in Metals
Most have 1-3 valance electrons which they lose easily.
Usually lose the electron to a nonmetal and form ionic bonds.
Sometimes metallic bonding occurs – the positively charged ions are surrounded by a sea of electrons. The electrons can slide past each other . This is how they are malleable, ductile, and good conductors of electricity. Page 331.

51. For example, during the reaction of sodium with chlorine:
                            sodium (on the left) loses its one valence electron to chlorine (on the right),
   resulting in
                            a positively charged sodium ion (left) and a negatively charged chlorine ion (right).
The reaction of sodium with chlorine
Concept simulation - Reenacts the reaction of sodium with chlorine.
(Flash required)

52. Metal Facts Aluminum most abundant metal in the Earth’s crust.
Iron second most abundant. Metals must be dug or mined from earth’s crust.
Iron is most widely used metal (steel), cobalt is sometimes used in steel.
Nickel gives it the shiny color.

53. Nonmetals and Metalloids
Where are they located on the periodic table?
What are the properties of nonmetals and metalloids?

54. What is a Nonmetal?
17 Nonmetals located to the right of the zig-zag line on the PT.
Physical properties are the opposite of metals.

55. Physical Properties
Dull (non shiny), brittle (breaks easily), low densities, poor conductors of heat and electricity.
Many non metals are gases at room temperature

56. Chemical Properties
Most nonmetals form compounds. They gain/take or share electrons.
Family/Group 18 do not. This is because they have 8 valence electrons in their outermost energy level.
When nonmetals and metals react the valence electron moves from the metal to the nonmetal.

57. Find for each atom:
Atomic number Atomic mass
Group Period

59. Metalloids
Borders between metals and nonmetals and have characteristics of both metals and nonmetals
Semiconductor (able to conduct electricity at room temperature more easily than an insulator, but less easily than a metal)
Reactivity depends on properties of other elements in reaction

60. BORON FAMILY Group 3 3 electrons in the outer shell Most are metals
Boron is a metalloid

61. CARBON FAMILY Group 4 4 electrons in the outer shell
Contains metals, metalloids, and a non-metal Carbon (C)
4 valence electrons
Carbon is the only nonmetal.
All living things contain compounds that are made of carbon atoms.

62. NITROGEN FAMILY Group 5 5 electrons in the outer shell
Can share electrons to form compounds
Contains metals, metalloids, and non-metals
Group 15 – 5 valence electrons
Atmosphere is 80 % nitrogen

63. OXYGEN FAMILY Group 6 6 electrons in the outer shell
Contains metals, metalloids, and non-metals
ReactiveGroup 16, 6 valence electrons.
Usually gain or share 2 valence electrons.
Oxygen is a diatomic molecule
Oxygen is very reactive – it can combine with nearly all elements.
Most abundant element in the Earth’s crust, 2nd most abundant in the atmosphere.

64. Halogens Group 7 7 electrons in the outer shell All are non-metals
Very reactive are often bonded with elements from Group 1Group 17
contains fluorine, chlorine, bromine, iodine, astatine.
7 valence electrons, gains or shares one valence electrons when it reacts.

65. Noble Gases Group 8 Exist as gases Non-metals
8 electrons in the outer shell = Full
Helium (He) has only 2 electrons in the outer shell = Full
Not reactive with other elementsGroup 18, do not mix with others.
Do not gain, share, lose electrons.
Chemically stable because they have a full outer energy level.
Group 18 is the only family that consists of all nonmetals.

66. Rare Earth Metals Some are Radioactive
The rare earths are silver, silvery-white, or gray metals.
Conduct electricity

67. Iron, Cobalt, Nickel
First elements in groups 8,9, 10 called the iron triad.
The only ones known to create a magnetic field.

68. Hydrogen Alone in the upper left corner.
Simplest element – usually its atoms contain one proton and one electron.
Hydrogen is rarely found on Earth as an element. Usually combined with oxygen as water.