1. Periodic Table Folding Exercise Draw a Line as shown on this chart and the one on the wall.

2. Periodic Table Folding Exercise Fold the chart so that only the first 2 columns are showing.

3. Periodic Table Folding Exercise Bring the new edge back over to the front of the chart and connect the column starting with Be to the column that starts with B.

4. Periodic Table Folding Exercise

5. A column goes up and down. A row goes side to side. This is a column. This is a row

6. Periodic Table Folding Exercise Write (above the Column numbers) the Valence Numbers: +1, +2, +3, +4, -3, -2, -1, 0. At the end of Row 1, write 2 At the end of Row 2, write 2,8 At the end of Row 3, write 2, 8, 8 At the end of Row 4, write 2, 8, 18, 8

7. Periodic Table Folding Exercise Elements to the LEFT of the line are METALS. Elements to the RIGHT of the line are NON- METALS. Metal + Non-Metal has IONIC Bond Non-Metal + Non-Metal has COVALENT Bond

8. Periodic Table Folding Exercise Period = Row # = number of e- orbits around atomic nucleus for atoms of all elements in that Period. Numbers at end of each row indicate Maximum number of e- allowed in each orbit.

9. Periodic Table Folding Exercise The Column Numbers that have an ‘A’ indicate the number of e- in the outermost orbit. The Valence numbers indicate the charge on an atom of that element when it has achieved a full outer orbit.

10. How to Use This Info 1 Look at any element in the ‘A’ columns. The column number (eg., 7A) tells you how many electrons are in the outermost orbit of a neutrally charged atom of that element. Remember: Neutrally charged means the same number of protons (p+) and electrons (e-) are present.

11. How to Use This Info 2 Look at any element in any row. The row number tells you how many electron orbits are around the nucleus of a neutrally charged atom of any element in that row. Look at the end of row numbers (rows 1-4). The end of row numbers tells you the maximum number of electrons allowed in each orbit for elements in that row.

12. How to Use This Info 3 Orbit 1  Can only ever have a max of 2 e - ’s Orbit 2  Can have a max of 8 e - ’s Orbit 3  Can have a max of 8 e - ’s {for our purposes} Orbit 4  Can have a max of 8 e - ’s Remember: An atom is only STABLE if it has 8 electrons in the outer orbit.

13. How to Use This Info 4 In the following ionic compound: Na + CL - Na starts with 11 protons and 11 electrons as follows: Orbit 1  2, Orbit 2  8, Orbit 3  1 Cl starts with 17 protons and 17 electrons as follows: Orbit 1  2, Orbit 2  8, Orbit 3  7

14. How to Use This Info 5 Due to their Electronegativity difference Cl is going to not only attract electrons but will also take them away. Na will give away its 1 outer electron. When Na gives away its 1 e - in Orbit 3 to Cl, the new outer orbit is Orbit 2 with 8 e - ’s making Na stable. When Cl takes the e- from Na and adds it to its outer orbit, Orbit 3 then has 8 e - ’s making Cl stable.

15. Element Symbols You Must Memorize CHOPKINS CaFe, Mighty good, with NaCl C=CarbonH=HydrogenO=Oxygen P=PhosphorousK=PotassiumI=Iodine N=NitrogenS=SulfurCa=Calcium Fe=IronMg=Magnesium Na=SodiumCl=Chlorine