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The Periodic Table of Elements
Study Guide
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As you go through this study guide, please have the periodic table that you were given. You will be filling it in as you go.

2. Next Year…
Next year you will be in 9th grade physical science. The periodic chart you have received will be very useful to you next year. As you go through this study guide, you will be filling it in with information that will be very helpful next year. You will want to hold on to your chart.

3. Test on the atom unit next week
The information you will be studying today will be on the test next week. Go through each slide carefully. You can always go back to slides that you don’t fully understand. Taking notes as you go is a very good idea. For the test next week, you will be allowed a “cheat sheet” (a 3x5 card that you will create in class from your notes)

4. An atom refresher Matter is anything that takes up space and has mass.
All matter is made of atoms
Atoms are the building blocks of matter, sort of how bricks are the building blocks of houses.
Elements are the alphabet to the language of molecules.
To make molecules, you must have elements.
Elements are made of atoms. While the atoms may have different weights and organization, they are all built in the same way.

5. Electrons have special rules….
You can’t just shove all of the electrons into the first orbit of an electron.
Electrons occupy something called shells or energy levels.
Only so many can be in any certain shell.
The number of shells an atom has relates to the period it is located in.
The group that an atom is in is related to how many electrons it has in its outer (valence) shell.
So let’s explore periods and groups in the next few slides.

6. Periodic Table
This table is a remarkable way to show the manifold relationships between differing kinds of elements
The modern table was devised in 1869 by Dimitri Mendeleyev
He arranged the elements by weight and by their chemical properties

7. Periodic Table
"...if all the elements be arranged in order of their atomic weights a periodic repetition of properties is obtained." - Mendeleyev
The next slide shows a few of the elements from the table.

9. Periods and Groups
Horizontal rows in the periodic table are called periods
Vertical columns are called groups
We will learn later why the elements can be arranged in this fashion based on the arrangements of the electrons outside the nucleus
Please note: Some Table of Elements show 18 groups, others show only 8 groups (the transition elements aren’t always considered to be in groups – you will see both ways in this study guide)

10. This shows 18 groups

11. This one shows 8 groups

12. Periods and Groups
Sizes of the atoms decrease as we move from left to right across a period (see the next slide)
This is due to the increasing number of protons in the nucleus, so the electrical attraction between the nucleus and the orbiting electrons gets stronger and pulls the electrons closer to the nucleus

14. Periods and Groups This property is called electronegativity
We can display the table to demonstrate other properties as well
As you move from left to right across a period, the ability of the atom to attract another electron increases (See next slide)
This property is called electronegativity

16. Periods Each row is called a “period”
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
Please make a note on your chart to help you remember that whatever period an element is in, that is how many shells it would have.

17. Groups Group 1 = 1 electron Group 2 = 2 electrons
Group 18 or 8 = Filled shells
Group 1 = 1 electron
Group 2 = 2 electrons
Except for He, it has 2 electrons
Group 13 or 3 = 3 electrons
Each column is called a “group”
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”

18. Transition Metals
Transition Metals have slightly different rules for shells and valence electrons.
This is something you will learn about in High School Chemistry.

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

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

21. 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

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

23. 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

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

25. 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

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. Review Li Lithium Protons = 3 3 7 Neutrons = 4 (7-3=4) + -
Electrons = 3
2 in the 1st shell, 1 in the 2nd shell
Neutrons = 4
(7-3=4)

28. Be sure to have all your answers on your study guide worksheet.
Remember, if you don’t understand a section, you can always go back and redo it.

29. Groups and Families
All the elements in a column have remarkably similar chemical properties
Some of the columns have been given special names to distinguish them (We call them families)
As you go through the families, very lightly color each family a different color. If you don’t have colored pencils with you, make a note to do it later when you do have them. (please…as you color the families, make sure it is very light and not so dark that you can’t see the numbers and symbol)

30. Please label the first group on your periodic table.
Alkalie Family
The first group (Group 1) is called the alkali metals or Alkalai Family. They are the most chemically reactive of all the metals.
This group does not include Hydrogen, however. Hydrogen is in its own group.
Each element in this family has one valence electron.
Generally, if members of this family form an ion, they would have a +1 charge because of their tendency to give away one electron.
Please label the first group on your periodic table.

31. Alkaline-Earth Family
The second group is the alkaline-earth metals. They are also very chemically reactive, but not as much as the group in the Alkali family.
Each element in this family has two valence electrons.
Generally, if members of this family form an ion, they would have a +2 charge because of their tendency to give away two electrons.
Please label the second group on your periodic table.

32. Transition Metals
The transition metals and aren’t considered a family and aren’t named. (remember some charts will call these Groups 3-12)
Members of this group generally have 1, 2 or 3 valence electrons.
Generally, if members of this family form an ion, they would have a +1 or +2 or +3 charge because of their tendency to give away one, two, or three electrons.
Make a small note on your table to help you remember they are called the transition metals.

33. Please label the this group on your periodic table.
Boron Family
Group 3 is the Boron Family. (13 on some charts)
Each element in this family usually has three valence electrons.
Generally, if members of this family form an ion, they would have a +3 charge because of their tendency to give away three electrons.
Please label the this group on your periodic table.

34. Please label the this group on your periodic table.
Carbon Family
Group 4 is the Carbon Family. (14 on some charts)
Carbon is the backbone of all living things, Silicon is the backbone of computerized things.
Each element in this family usually has four valence electrons.
Generally, if members of this family form an ion, they would have a -4 charge because of their tendency to attract four electrons.
Please label the this group on your periodic table.

35. Please label the this group on your periodic table.
Nitrogen Family
Group 5 is the Nitrogen Family. (15 on some charts)
Each element in this family usually has five valence electrons.
Generally, if members of this family form an ion, they would have a -3 charge because of their tendency to attract three electrons.
Please label the this group on your periodic table.

36. Please label the this group on your periodic table.
Oxygen Family
Group 6 is the Oxygen Family (16 on some charts)
Each element in this family usually has six valence electrons.
Generally, if members of this family form an ion, they would have a -2 charge because of their tendency to attract two electrons.
Please label the this group on your periodic table.

37. Please label the this group on your periodic table.
Halogen Family
Group 7 are the halogens (Salt Formers) Elements in this group are the most reactive of the non-metals. (17 on some charts)
Each element in this family usually have seven valence electron.
Generally, if members of this family form an ion, they would have a -1 charge because of their tendency to attract one electron.
Elements in this family have a tendency to chemically react strongly with metals. The product of that chemical reaction is a salt.
Please label the this group on your periodic table.

38. Please label the this group on your periodic table.
Noble Gas Family
Group 8 (18 on some charts) are the noble gases and are basically inert (inert means unable to chemically react with other elements)
Elements in this family all have filled valence shells.
Helium has just two electrons, and they fill its outer shell. The rest of the noble gases have 8 electrons in their outermost shells. (see the next slide)
These elements rarely or never form ions or join into chemical reactions.
Please label the this group on your periodic table.

39. Octet Rule
The Octet Rule states that atoms cannot have more than 8 electrons in their outermost shell.
So that means that starting with the fourth shell, the atom flips any extra electrons to the previous shell.
For example, Krypton is in the fourth shell:
- 2 electrons fill the first shell
- 8 electrons fill the second shell electrons fill the third shell (10 were flipped from the fourth shell)
- 8 electrons in the fourth shell

40. Electron Shell Examples Showing the Octet Rule
Zink (Zn) 2 electrons in the 1st shell 8 electrons in the 2nd shell 18 electrons in the 3rd shell 2 electrons in the 4th shell
Bromine (Br) 2 electrons in the 1st shell 8 electrons in the 2nd shell 18 electrons in the 3rd shell 7 electrons in the 4th shell

41. Please label the Rare Earth Elements
The Rare Earth Elements (or Inner transition metals) are in periods 6 and 7, and are pulled out to make the Table more compact.
Please label the Rare Earth Elements

42. Thought Questions Think carefully about your answers
Why are there only two elements in the first period?
Why are there eight elements in the second and third periods?
Why do we jump to eighteen in the fourth period?
Why are the chemical properties of a group so similar?