ACTIVITY VII- CHEMISTRY 2012-13
ELECTRON ARRANGEMENT DETERMINES THE CHEMICAL BEHAVIOR OF
ATOMS
IONIC BONDS ARE ATTRACTIONS BETWEEN IONS OF OPPOSITE
CHARGE
A. MATERIALS:
1. Three different colors of M&M’s
2. Cup, bowl, or Ziplocs bag
3. Periodic table
4. Atomic model handout
B. PROCEDURE- 20 minutes
1. Use the paper atomic models and M&M’s to build a fluorine atom and a
hydrogen atom.
2. Answer questions below:
a. Does the hydrogen atom have a full outer electron shell? If not
how many electrons does it need to fill its outer energy level?
b. Is the hydrogen atom currently neutral? Explain
c. Does the Fluorine atom have a full outer electron shell? If not
how many electrons does it need to fill its outer energy level?
d. Is the Fluorine atom currently neutral? Explain
e. Would you consider the hydrogen atom and fluorine atom
stable or unstable? Why?
3. STOP AND WAIT FOR CLASS DISCUSSION
4. Move an electron from hydrogen to fluorine to form two stable atoms
(ions).
a. How many protons and electrons does hydrogen now
have?
b. Will the hydrogen be neutral, positively charged, or
negatively charged? Explain.
c. Is the hydrogen more or less stable now?
d. How many protons and electrons does Fluorine now have?
e. Will the Fluorine be neutral, positively charged, or
negatively charged? Explain.
f. Is the Fluorine more or less stable now?
g. Which atom gained an electron and which atom gave up an
electron?
5. STOP AND WAIT FOR CLASS DISCUSSION
6. Students should build LiCl, MgO and BeS, NaCl and draw before and
after diagrams of each.
7. ANSWER QUESTIONS BELOW:
a. In each of the molecules you’ve modeled, which atom has become the cation
(positively charged ion), and which is the anion (the negatively charged ion)?
b. Which elements of the periodic table tend to become negative ions (have the
greatest potential for acquiring electrons)? Why?
c. Which elements of the periodic table tend to be positive ions (have the
weakest ability to retain their electrons)? Why?
d .Which columns would combine well in order for both to be more stable?
e. Which elements on the periodic table tend to make ionic bonds?
f. How does electronegativity correlate with ionic bonding?
8.STOP AND WAIT FOR CLASS DISCUSSION
9. Check for understanding
a. How do atoms behave?
b. Which subatomic particle determines how an atom behaves when
it encounters another atom?
c. How many electrons can the first energy level hold?
d. How many electrons can the second energy level hold?
e. How many electrons can the third energy level hold if it is the
outermost energy level?
f. Which energy level determines behavior of an atom?
g. What can you say about an atom with a full outer energy level?
h. What can you say about an atom with an unfilled outer energy
level?
I. What is one way an unstable atom will become stable?
j. What is the attraction force in ionic bonds?
10. WHOLE CLASS DISCUSSION