1. Ch. 4 - The Periodic Table
III. Periodic Trends

2. A. Periodic Law
When elements are arranged in order of increasing atomic #, elements with similar properties appear at regular intervals.

3. B. Chemical Reactivity Families
within a group result in similar ______________ _____________

4. B. Chemical Reactivity _____________________________
________________________________
___________________________________

5. C. Other Properties Atomic Radius size ______________
© 1998 LOGAL
First Ionization Energy
Energy required to remove one
____________________.
© 1998 LOGAL
Melting/Boiling Point

6. D. Atomic Radius
Atomic Radius K Na Li Ar Ne

7. D. Atomic Radius
Atomic Radius
Increases to the _______ and ________

8. D. Atomic Radius
Atomic Radius
Decreases to the ________ and _____

9. D. Atomic Radius Why larger going down?
Higher _________ __________ have larger orbitals
________ - core e- block the attraction between the nucleus and the valence e-
Why smaller to the right?
____________ nuclear charge without additional shielding pulls e- in tighter

10. E. Ionization Energy
First Ionization Energy He Ne Ar Li Na K

11. E. Ionization Energy First Ionization Energy
Increases _____ and to the _________

12. E. Ionization Energy Why opposite of atomic radius?
In small atoms, e- are close to the nucleus where the attraction is ______________
Why small jumps within each group?
_____________ e- configurations don’t want to lose e-

13. F. Melting/Boiling Point
Highest in the ____________ of a period.

14. Examples
Which atom has the larger radius?
Be or Ba
Ca or Br Ba Ca

15. Examples
Which atom has the higher 1st I.E.? N
N or Bi
Ba or Ne Ne

16. Li or C Cr or Kr C Cr Examples
Which atom has the higher melting/boiling point?
Li or C
Cr or Kr C Cr