1. Unit 3: Periodic Table and Atom Structure Comparing Atoms Periodic Table

2. Reading the Periodic Table WWWWhat information is shown? AAAAtomic Mass AAAAtomic Number EEEElement Symbol EEEElement Name

3. Periodic Table 47 Ag Silver 107.87 Atomic Number Element Name Atomic Mass Element Symbol Which is which?

4. Periodic Table 47 Ag Silver 107.87 Atomic Number Element Name Atomic Mass Element Symbol

5. Atomic Number  Number of Protons  What happens if you change the number of protons?  Change the element HUGE amounts of energy to add or remove. HUGE amounts of energy to add or remove.

6. Atomic Number  Begin @ 1  111  Why is there more than 111?  Heaviest elements are created by scientists.  WHY?

7. Periodic Table 47 Ag Silver 107.87 Atomic Number

8. Atomic Mass  Protons & Neutrons  Increase by amounts > 1  Different # of Neutrons in nucleus.  Neutrons don’t change charge of atom

9. Isotopes  Atoms with different amounts of neutrons. + + 0 0 + 0 -- - Hydrogen- proteium Hydrogen - deuterium Hydrogen- tritium A# M# 111 123

10. Periodic Table 47 Ag Silver 107.87 Atomic Mass

11. # 0f Neutrons?  Atomic Mass – Atomic Number 47 Ag Silver 107.87 108 -47 61 Neutrons

12. Nucleus OOOOpposites _ _ _ _ _ _ _ WWWWhy does the nucleus stay together? SSSStrong Nuclear Force SSSShort distance

13. Periodic Table 47 Ag Silver 107.87 Atomic Number Element Name Atomic Mass Element Symbol

14. Electrons ?  Equal to the Protons  Electron Cloud  Never in the same place  “Buzzing”  Arranged in energy levels

15. Electron Levels  Distance from nucleus increases energy.

16. Electron Levels  The higher the level the more electrons it can hold.

17. Electron Levels  Orbitals 2 8 8 18  We are only concerned with 8 per level

18. 1 2 (1)4(1)5(1)6(1)7 (1)8 (1)3 1 2 4 5 6 7 3 Columns 1-8, Group #’s tell you the # of electrons in the outer shell Period or row # 1-7, the number of electron shells

19. Types of Elements  Metals  Solid at room temp  Conduct heat & electricity  Shiny  bendable

20.  Non-Metals  Gasses or liquids at room temp  Do not conduct heat or electricity Types of Elements

21.  Metalloids  Next to the crooked line  Exhibit properties of metals & nonmetals nonmetals

22. Types of Elements  Transition Elements  Transitioning from metal to non-metal non-metal

23. Types of Elements  Halogens  Bond easily with groups 1 & 2 to make salts. to make salts. Most reactive Non-metals

24. Types of Elements  Noble Gasses  These gasses are inert; non-reactive

25. Types of Elements  Alkali Metals  Most Reactive Metals  React with water violently

26. Types of Elements  Alkaline Earth Metals  2nd most Reactive Metals  React with many things, just not as much as group 1

27. Why do atoms react?   Valance Electrons   Atoms are stable only when their outer shell (valance shell) is full.   Most of the time that means they need 8 valance electrons (Rule of Octet).   Atoms gain or lose electrons to become stable during a chemical reaction.

28. Why do atoms react?   Gaining or losing electrons requires the same amount of energy so…   Atoms will gain or lose electrons based on how many they have in their outer shell   Gaining or losing electrons results in a chemical bond being formed and that atom becomes an Ion (atom with a charge)

29. Drawing Atoms e-e- e-e- e-e- e-e- e-e- e-e- Sodium: Atomic #11 e-e- e-e- e-e- e-e- e-e-

30. Assignments:   Worksheets   “Unknown Elements”   “Elements you NEED to know”   Mr. Bunt will be coming around to grade your folder. BE READY!!!

31. Activity  Pick 4 elements and draw their structure.(5 min)  Move all desks to perimeter.  Class in 2 groups.  As a group pick an element and “ACT” out the arrangement of the sub atomic particles.  1 person can be the nucleus.  The other team guesses the element of the acting team

32. Electron Actors