This document discusses valence electrons and how to determine the number available for bonding using the periodic table. It defines valence electrons as those in the outermost shell or energy level available for bonding. It provides examples of how many valence electrons elements in different groups have, from 1 to 8. It also introduces Lewis dot structures as a way to represent an atom's valence electrons and provides examples of Lewis dot structures for period 2 elements.

1. Valence
Electrons:
ELECTRONS
AVAILABLE
FOR
BONDING

2. CA Standards
 Students know how to use the
periodic table to determine the
number of electrons available for
bonding.
 Students know how to draw Lewis
dot structures.

3. Definition
Valence electrons are electrons in
the outmost shell (energy level).
They are the electrons available
for bonding.

4. Group 1 (alkali metals) have 1
valence electron

5. Group 2 (alkaline earth metals)
have 2 valence electrons

6. Group 13 elements have 3
valence electrons

7. Group 14 elements have 4
valence electrons

8. Group 15 elements have 5
valence electrons

9. Group 16 elements have 6
valence electrons

10. Group 17 (halogens) have 7
valence electrons

11. Group 18 (Noble gases) have 8
valence electrons, except
helium, which has only 2

12. Transition metals (“d” block)
have 1 or 2 valence electrons

13. Lanthanides and actinides
(“f” block) have 1 or 2 valence
electrons

14. Dot Notations
An atom’s valence electrons can be represented
by Lewis dot notations.
1 valence e- 2 valence e- 3 valence e- 4 valence e-
X X X X
5 valence e- 6 valence e- 7 valence e- 8 valence e-
X X X X

15. Dot Notations – Period 2
Lewis dot notations for the valence electrons of
the elements of Period 2.
lithium beryllium boron carbon
Li Be B C
nitrogen oxygen fluorine neon
N O F Ne