1. Beginning of the Year Warm Up
Chemistry II
Beginning of the Year Warm Up

2. Let's see what the sun baked out this summer!

3. Easy Ones! What is the chart thing on the wall?
Answer: Periodic Table
Bonus: How is it arranged?
Answer: By atomic number / by number of protons

4. Tell me what else you know about this thing ...

5. Other things to know:
Polyatomic Ions
Naming Compounds
Writing Compound Formulas
Identifying Charges on Ions
Any of these SCARE you???

6. Where to Start??
Our first topic is bonding… so you should remember the following items from Pre-AP or Chemistry I. If these first five slides made you sick, you are either going to have to study/review/ask for help/wake up your brain, or reconsider your schedule.

7. Periodic Trends What do you remember about Periodic trends?
Did you get it all?

8. Periodic Trends
Definition: a pattern of behavior on the periodic table
Defined for a group
Defined for a period
Some Examples:
Atomic Size:
Electronegativity:
Ionization Energy:

9. Periodic Trends Continued…
Atomic Size- atomic radius
increases down a group, decreases L-R across a period
Electronegativity- Ability of an atom to attract shared electrons "greed“
Decreases down a group, Increases L-R across a period
Ionization Energy- Energy needed to remove electrons from the atom

10. Next Topic: Valence Electrons
What do you remember about Valence Electrons?
Did you get it all?

11. Valence Electrons Outermost Electron(s) Control chemical activity
Can be shared
Can be transferred
Loss of electrons = positive ion
Gain of electrons = negative ion
Involved in bonding (sharing, transfer)

12. Atomic Models What do you remember about atomic models?
Did you get it all?

13. Atomic Models JJ Thomson “Plum Pudding Model”
Rutherford “Gold Foil Experiment”
Bohr “orbits, only worked for H”

14. Atomic Models continued
Current Model- Wave Mechanical Model
Mathematical representation
Orbital- area of probability- expect to find electrons
s/p/d/f sublevels
Electron configurations represent mathematical description

15. Electron Configurations
What do you remember about Electron Configurations?
Did you get it all?

16. Electron Configurations
Description of electron arrangement
wave mechanical model
quantum mechanical model
Orbital- probability zone
Pauli Exclusion Principle: no two electrons can have the same set of four quantum numbers
Quantum Numbers
Principle Energy Level
Sublevel- s, p, d, f
Orbital
Spin

17. Anatomy of a Standard Electron Configuration
Number of electrons in the sublevel
1s2
Sublevel:
Tells shape of orbital
Indicates how many electrons may be held
Principle Energy Level:
Tells distance from nucleus
Relative amount of energy
Number of sublevels in the P.E.L.
s - 2 electrons max.
p- 6 electrons max.
d- 10 electrons max.
f- 14 electrons max.

18. Abbreviated Configurations
Start with the previous noble gas in brackets
[He] 2s2 2p4
Continue with electron configuration from noble gas on
Previous noble gas symbol placed in brackets

19. Orbital Diagrams
Show the fourth quantum number- spin
1s s p

20. Practice Electron Configurations
Magnesium- atomic #12
Standard configuration
Abbreviated configuration
Orbital diagram

21. You should remember what you learned in Chemistry I or Pre AP !
If you do not, the items you will need most right now are:
recognize polyatomic ions (names, formulas and charges)
write formulas for compounds, write names for formulas
describe basic workings/organization of periodic table

22. Later you will need:
describe parts of a chemical equation : reactant, product, coefficients
describe basic parts of a solution: solvent, solute, concentration (molarity)
describe acids and bases

23. Assignment Electron Configuration Practice Worksheet Answer Key Page 1