1. Welcome! Please get out: Your lab notebook
Your “Discovering Patterns on the Periodic Table”
A writing utensil
Ask your partner:
“What is your favorite thing about the new school?”
Welcome!

2. Warm up
Answer #12 then compare you answers to number with your partner.
Which atom did you think would be bigger in size?
After looking at the cards you see that sodium has an atomic radius of 0.19 and chlorine has a radius of 0.10
Now try and answer #13a/b on “Discovering the Patterns on the Periodic Table”. Why do you think this is?

3. 11. Bohr Models
Na would have a low electronegativity and ionization energy because it doesn’t want to keep the valence electron and it doesn’t want to attract more electrons
Cl would have a high electronegativity and ionization energy because it doesn’t want to loose any electrons and it wants to attract another one
If one goes down the other has to as well. If you don’t want to attract electrons, then you want to loose them, so it can’t take a lot of energy to remove the electron

4. 12 + 13. Radius of Sodium Atom vs. Chlorine Atom
Atoms are neutral
Same # of p+ & e-
Why does Na have a larger atomic radius than Cl?
Holds them tighter
“More” Positive =
More Pull
Sodium Atom Chlorine Atom
11 protons protons
11 electrons electrons
17+
11+

5. In the notes section…
Put today’s date and title your notes “Periodic Table Basics”
I would also get out your periodic table and make notations on your table as well as we go along.

6. Location and Properties of…
Non-Metals
Metals?
Non-metals?
Metalloids?
Noble Gases?
Metals
Metals are on the left of the staircase they a) conduct heat and electricity, b) malleable, c) often shiny, and d) loose electrons in an ionic bond.
Non-metals are on the right of the staircase they have the opposite properties of non-metals and the gain electrons in an ionic bond.
Metalloids elements that touch the staircase – have characteristics of both metals and non-metals
Noble Gases – the far right column. These gases are considered to be inert/unreactive. They have fuller outer shells with 8 electrons therefore, they don’t react with any other elements

7. Groups/Families and Periods
Groups are columns, periods are rows!

8. - + Metals vs. Non- Metals Metals =Loser Non-Metals =Thieves
Positive = Ca+ions
Non-Metals =Thieves
Neg = Anions - +

10. Ion– charged particle (uneven # of p+ & e-)
Octet Rule- Atoms tend to gain/lose/share electrons to have 8 valence electrons.
Valence electrons– outer most electrons
Column 1 has 1 valence e –
Column 2 has 2 valence e-, etc.
Na would have a low electronegativity and ionization energy because it doesn’t want to keep the valence electron and it doesn’t want to attract more electrons
Cl would have a high electronegativity and ionization energy because it doesn’t want to loose any electrons and it wants to attract another one
If one goes down the other has to as well. If you don’t want to attract electrons, then you want to loose them, so it can’t take a lot of energy to remove the electron

11. Let’s make a foldable study guide…
Fold your paper “hamburger” style.
You will make two cuts to create three flips on your folded paper
Use color markers or color pencils on your foldable
Follow my example…

12. Atomic Radius: useful Decreases Decreases
More protons = tighter hold on electrons,
But
More electron shells = bigger atom

13. Electronegativity: Useful
Increases
Closer to F = hungrier for electrons
Column 8 is Full, so its electronegativity is 0

14. Ionization Energy: Useful
Increases
Closer to full, the stronger elements hold onto their electrons.

15. Tackle 14-20 With your group

16. Exit Task (in lab book!)
Phosphorus is an important element in making DNA and cell membranes!
What is its atomic #?
What is its mass #?
How many protons does a phosphorus atom have? electrons? neutrons?