1. Please turn in: Any work if you were absent Please get out: Your lab notebook Your Discovering Patterns on the Periodic Table Packet A writing utensil Ask your partner: “What are you doing over the weekend?”

2.  Finish “Discovering Patterns on the Periodic Table” Packet  Basic Atomic Worksheet ◦ Z= Atomic # ◦ A=Mass #

3.  Title your these notes “Periodic Table Basics”

4.  Organized the 63 known elements into a table based on atomic mass  Russian professor/ scientist (1834-1907)

6.  Important patterns in each column/group  One of most important  Ionic Charges + / -

7. ◦ In #5-6 ONLY RECORD PATTERNS FOR:  ATOMIC RADIUS  ATOMIC MASS  IONIZATION ENERGY  ELECTRONEGATIVITY ◦ NO DRAWING NECCESARY

8.  Metals?  Non-metals?  Metalloids?  Noble Gases?

10.  Metals =Loser  Positive = Ca+ions  Non-Metals =Thieves  Neg = Anions

12. What determines the “identity” of an element? Protons = ID Mass = p + + n 0

13.  An atom of Cu has ◦ Protons? ◦ Neutrons? ◦ Electrons?  Atomic # = 29, so 29 protons  Mass # = 63.546 FIRST ROUND TO THE NEAREST WHOLE # 64, so 35 neutrons (64-29)  Same number as protons, 29 electrons!

14. Mass # (Always a whole #) Symbol of element Atomic #

15.  An atom of K has ◦ Protons? ◦ Neutrons? ◦ Electrons?  Atoms has 19 p +, 20 n, 19 e -,  An ion of K 1+ has ◦ Protons? ◦ Neutrons? ◦ Electrons?  Ion has 19 p + & 18 e -, because it has a charge of +1 19 K Potassium 39.10

17.  11. Bohr Models

18.  Atoms are neutral ◦ Same # of p + & e -  Why does Na have a larger atomic radius than Cl? ◦ Holds them tighter “More” Positive = More Pull SodiumAtom Chlorine Atom 11 protons 17 protons 11 electrons 17 electrons

20.  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.

21. Decreases More protons = tighter hold on electrons, But More electron shells = bigger atom Decreases

22. Increases Closer to F = hungrier for electrons Column 8 is Full, so its electronegativity is 0 0

23. Increases Closer to full, the stronger elements hold onto their electrons.

25.  Ionization Energy and Electronegativity decrease down each column. Why?  As atoms get bigger it is harder for the nucleus to hold electrons

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

27.  Get out “Discovering Patterns on the Periodic Table” and Gold PT  Who organized the first periodic table? ◦ Einstein ◦ Mendeleev ◦ Bryce ◦ Bohr ◦ Duty

28.  Atoms are neutral ◦ Same # of p + & e -  Ions are charged particles ◦ Uneven # of p + & e - ◦ Not neutral, either positive (cations) or negative (anions)  Isotopes ◦ Has a particular number of neutrons ◦ # on the PT is a WEIGHTED average!