The Periodic Table

1. The Periodic Table • After this slide, everything in this power point must be in your notes… you may abbreviate, as long as you will understand it as you prepare for tests etc.

2. Organization of the Periodic Table

3. 1. Overview of organization • a)Groups/ Families • i)Go up and down • ii)Similar chemical and physical properties • b)Periods • i)Rows, go across • ii)These elements follow a repeating pattern as you go across. • c)Classes of elements • i)Metals- • ii)Nonmetals- • Iii) Metalloids-

4. 2. Every element is unique! • a)      Symbol • i)        First letter must always be in capitols! (When there are 2 letters in the symbol the second is always in lower case!) • b)      Atomic Number • i)        Tells the number of protons in the nucleus • ii)      This number is unique to every element! • c) There are 92 (94) naturally occurring elements! Everything beyond that is created in a lab! (And not stable!...radioactive!)

5. 3. Electron configuration • a)Stable elements have full outer shell (only one group is stable)That would be 8 electrons total in that outer shell • b) Because, all but the noble gases do not have a full shell, most elements will gain or lose their valence electrons in reactions as they form compounds! • c) Valence electrons are the electrons in the outer energy level.

6. II) Grouping the Elements!

7. 1. Alkali Metals -Red • a)Group 1 • b)Very reactive- will often burn or give off gas when touched with water! • c)One valence electron! –Easily give away one electron. (This is why they are so reactive!) • d) Low density- all will float in water! http://video.google.com/videoplay?docid=-3103610687149839311#

8. 2. Alkaline Earth Metals -Orange • a)Group 2 • b)Very reactive, but less reactive than group 1 • c)Two valence electrons (Will lose the 2 valence electrons) • d) More dense than group 1 http://www.youtube.com/watch?v=wqErrNvns4o

9. 3. Transition Metals –Blue • a)Groups 3-12 • b)Less reactive than group 2 • c)1 or 2 valence electrons (will lose valence electrons) • d)Higher densities and melting points than groups 1 & 2 • e)Lanthanides & Actinides • i)These are part of periods 6 & 7 • ii) They are separated out in order to keep the periodic table from getting too wide!

10. A look @ the PT w/o the La & AC below!

11. 4. Boron Group –Yellow • a)Group 13 • b)3 valence electrons • loses the outer 3 electrons • Charge +3 • c) Reactive, because there is not a full outer shell they will bond with other elements, but they do not react violently!

12. 5. Carbon Group –White • a)Group 14 • b)4 valence electrons. They will either gain or lose 4 electrons. • c)Reactivity depends on the element. • d) *Carbon is the one element that all living things have in their atomic structure. We are able to date very old, once living things, by using radio carbon dating!

13. Carbon in action…

14. 6. Nitrogen Group –Gray • a)Group 15 • b)      5 valence electrons • gain 3 electrons • Charge of -3 • c)      More reactive than Group 14 • d) *Nitrogen makes up about 80% of the air that you breath!

15. 7. Oxygen Group –Brown • a)Group 16 • b)6 valence electrons • gain 2 electrons • a charge of -2 • c)Reactive elements • d)All but oxygen are solid at room temperature.

16. 8. Halogens –Green • a)Group 17 • b)7 valence electrons • gain 1 electron • a charge of -1 • c)Very reactive! Easily combine with metals to form compounds.

17. 9. Noble Gases –Purple • a)Group 18 • b)8 valence electrons • except for He that has 2! • c)Not reactive at all! • d)Do not gain or lose electrons! • e) Full outer shell.

18. What is going on with the attraction?

19. Homework! • Color code your white periodic table (as per the colors in the notes!) and put down important information… • Name of the group • …and a few facts • reactivity & the number of valance electrons!

20. Other things to include… • How to determine the number of • Protons • Neutrons • Electrons • Simple definitions… • Ions • Isotopes • Leave room for more stuff… we are nowhere near the end of Chemistry!