The Electron
Name__________________________________
Period_________________________________
1. On a periodic table group 1A (the reactive alkali metals) have one valence electron. How many
electrons do the following groups have? 2A______3A______ 4A______ 5A______ 6A______ 7A
______
2. Potassium (K ) is the 4th element down in group 1A alkali metals. How many valence electrons do
Potassium have_________?
3. Aluminum (Al) is the 2nd element down in group 3A. How many valence electrons do Al
have_________?
4. Octet rule: elements will gain or lose electrons to achieve the stable electron configuration of the
nearest Noble gas. Lithium in group 1A will___________(gain, lose) an electron(s) to be like the
nearest Noble gas. Bromine (Br) will___________(gain, lose) an electron to be like the nearest
Nobel gas.
5. Octet rule is also used to explain why elements are likely to form bonds by their position on the
periodic table. Sodium (Na) is in group 1A. Na will bond with elements in group _________to
achieve a stable electron configuration. Beryllium (Be) from group 2A will bond with elements in
group _________to achieve a stable electron configuration.
6. Lewis dot represents the number of_________________electrons that an element has. Rubidium
(Rb) is in group 1A so it will have a box with the symbol “Rb” and show that it has
___________electron(s).
7. For each of the following groups the Lewis Dot model will have how many dots around its box.
2A______3A______ 4A______ 5A______ 6A______ 7A ______
8. Bohr diagrams represent the number of electron in planetary orbits around a positive nucleus.
The___________(groups, periods) determines the number of Bohr planetary orbits.
9. The element Carbon (C) with an atomic number of 6 has ___________electrons in its outer most
orbital.
10. The element Silicon (Si) with an atomic number of 14 has ___________electrons in its outer most
orbital.
11. Using periods and groups for a reference, Sulfur (S) will have___________ valence electrons and a
total of ___________orbitals.
12. Using periods and groups for a reference, Calcium (Ca) will have___________ valence electron(s)
and a total of ___________orbitals.
13. Aluminum has an atomic number of 13, the first Bohr orbital can hold 2 electrons. How many
electrons are in the second orbital____________? How many are in the third orbital____________?
14. F1- is and anion which means it grabs one valence electron from another atom. If you were going to
represent this with a Lewis dot model, how many electrons would be around your box containing
the symbol “F1- ”_________________?
15. The cation of Calcium (Ca2+) would be _______________(larger, smaller) than the stable element
Calcium (Ca).
Draw the Bohr Diagrams (including the number of protons, neutrons, and electrons) for Carbon, Sodium,
and Aluminum.