Name: ___________________________________ Date: ___________________ Period: ______
Electron Configuration and Ions in the Periodic Table REVIEW WORKSHEET
Part 1: Valence Electrons
1.
Define Valence Electron:
Directions: In the following examples, circle the valence electrons and identify how many valence electrons are
present.
2. 1s22s22p2
3. 1s22s22p63s23p64s23d104p4
4. 1s22s22p63s23p64s23d104p1
5. 1s2 2s2 2p6 3s2 3p6 4s2
6. 1s2 2s2 2p6 3s2 3p6 4s2 3d104p5
7. 1s22s22p63s1
Directions: In the following examples, write the configuration first then circle and count the valence electrons.
8. Argon:
9. Boron:
10. Sulfur:
11. Lithium:
12. Complete the chart below.
Group 1A
Alkali
Metals
# of valence
electrons
Electron
Configuration
ending (outer
s and p
orbitals)
Group 2A
Alkaline
Earth
Metals
Group 3A
Boron
Group
Group 4A
Carbon
Group
Group 5A
Nitrogen
Group
Group 6A
Oxygen
Group
Group 7A
Halogens
Group 8A
Noble
Gases
13. The number of valence electrons is equal to the group number. Identify the number of valence electrons
for the following atoms:
a.
Neon: _____
d. Calcium: _____
b. Chlorine: _____
e.
Sulfur: _____
c.
f.
Potassium: _____
Aluminum: _____
Part 2: The Octet Rule
14. Define the octet rule: ______________________________________________________________
_______________________________________________________________________________
15. An octet is equal to ____ (#) electrons.
16. Group 18 already have a stable electron configuration as they have ____ electrons in their highest occupied
energy levels.
17. Atoms of __________________ (class of elements) tend to lose their valence electrons to leave a complete
octet in the next-lowest energy level. Atoms of ________________________ (class of elements) tend to
gain electrons or share electrons with another nonmetal to achieve a complete octet.
18. When the octet rule is satisfied, the outermost s and p ____________________ are filled.
19. The elements of the noble gas group satisfy the __________________ ______________ without forming
compounds. This is why they are considered unreactive.
20. Atoms in a stable compound achieve the nearest noble gas configuration by ________________ electrons
donating electrons, or by accepting electrons.
21. Atoms of nonmetals can achieve stable noble gas electron configuration by ______________ electrons. They
end up having a _______________________ charge.
22. Atoms of metals can achieve stable noble gas electron configuration by _____________________ electrons.
They end up having a _______________________ charge.
23. Identify whether the following atoms will want to lose electrons or if they will want to gain electrons. Pay
attention to whether the atom is a METAL or a NONMETAL. Follow the first example.
a.
Na (11): Lose
d. S (16): _____
g.
b. F (9): _____
e.
Mg (12): _____
h. Al (13): _____
c.
f.
N (7): ______
i.
K (19): _____
Ca (20): _____
Cl (17): _____
Part 3: Ion Formation
24. What is an ion? _________________________________________________________________
25. How is an ion produced? ___________________________________________________________
26. A positively charged ion is a ___________________. A negatively charged ion is a _________________.
27. Which group of elements is most likely to become cations? _______________________.
28. Which group of elements is most likely to become anions? _______________________.
29. Fill in the blanks to determine what charge an ion will have.
a.
When a neutral atom loses 1 electron, it will become an ion with a ______ charge.
b. When a neutral atom gains 2 electrons, it will become an ion with a ______ charge.
c.
When a neutral atom loses 2 electrons, it will become an ion with a ______ charge.
d. When a neutral atom gains 1 electron, it will become an ion with a ______ charge.
e.
When a neutral atom gains 3 electrons, it will become an ion with a ______ charge.
30. Complete the chart below.
Atom
Name
# of Valence
Electrons
Metal or
Nonmetal
Will it lose or
gain electrons?
# of e- to lose
or gain
Ion to be
formed
Fluorine (9)
Potassium (19)
Oxygen (8)
Aluminum ( )
Magnesium (12)
Nitrogen (7)
31. Write the electron configuration for each ion and determine what noble gas it represents
Ion
Mg 2+
Cl 1O 2Ba 2+
# of
electrons
in the ion
Electron Configuration
Noble Gas
the Ion is
representing