Ionic Compounds with Fruit Loops! (We’ll do the first two together)
1. Make the electron dot structure for the Rubidium atom using one color Fruit Loop.
2. Make the electron dot structure for the Bromine atom using a second color Fruit Loop.
3. Which of the preceding atoms tend to lose electrons? How many?
4. Which of the preceding atoms tend to gain electrons? How many?
5. Show the electron(s) leaving one atom and moving to the other atom so each atom forms an ion that has an octet of electrons.
6. How many of each atom are needed to demonstrate #5 above?
7. Draw orbital notations for all atoms involved and show which electrons from which sublevel
(s, p, d, f) of each atom. Where is the electron being lost and where will the electron end up? Show this on the orbital notations.
8. Why is this now a stable arrangement?
9. Write the charge of each ion.
10. Write the formula unit using the ratio of ions formed.
11. Repeat the procedure with: a. Potassium and Oxygen b. Calcium and Sulfur c. Magnesium and Nitrogen d. Potassium and Iodine e. Aluminum and Oxygen f. Sodium and Phosphorus g. Lithium and Nitrogen h. Aluminum and Chlorine

Covalent Bonds with Fruit Loops! (We’ll do a couple together)
1. Make the electron dot structure for one Chlorine atom with one color fruit loop.
2. Make the electron dot structure for a second Chlorine atom with a second color.
3. Show how the electrons are shared between the two Cl atoms so that each atom forms the stable noble gas configuration. Remember when electrons are shared, they belong to both atoms.
4. Draw orbital notations for both chlorine atoms and show which electrons from which sublevel (s, p, d, f) of each atom are being shared. How many different orbitals with in this sublevel are involved in the sharing? Show, using the orbital notations, the orbitals involved in the sharing.
5. Use the fruit loops to help you draw the electron dot notation that illustrates the bonding.
Show the shared electrons between the two atoms first! Remember to only include valence electrons! (The fruit loops)
6. Draw a structural formula of this molecule.
7. Write the molecular formula of this molecule.
8. Repeat steps 1-7 using the following molecules: a. Oxygen molecule (two oxygen atoms) b. Nitrogen molecule (two nitrogen atoms) c. Hydrogen chloride (one hydrogen atom {one color} and one chlorine {second color} atom) d. Water molecule (two hydrogen atoms {color 1) and one oxygen atom {color 2}) e. Ammonia (one nitrogen atom {color 1} and three hydrogen atoms {color 2})
9.
For the Oxygen molecule “How would you expect the strength of this bond to compare to that of the bond between the Cl atoms?”
10. For the Nitrogen molecule “How would you expect the strength of this bond to compare to that of the bond between the O atoms?”