Lewis Dot Structures
Name:______________________
Period:____
Helpful hints for Ionic Bonds
1. Identify that the compound is made of a metal and a nonmetal.
2. Draw the metal and non metal with the correct valence electrons as dots.
3. Then draw the correct number of each type of element so that the dots are completely removed from all
the metals and completely fill the non-metals.
4. Circle and x out the lost electrons, show an arrow moving them to the non metals, then circle the new
electrons on the non metals.
5. Write down the charges on the newly formed ions.
Example: Na2S
AlF3
Rb2Se
Li2S
PbI4
CaO
K 3N
Helpful hints For Covalent Bonds
1. Identify that the compound is made of all non-metals.
2. Sum the valence electrons for each atom in the compound so you know how many the image can have.
3. Write the symbols for the atoms to show which atoms are attached to which, and connect them with a
single bond. Think symmetrically, and do not create rings.
4. Place the dots in pairs around the atoms until you have used all the dots allowed in step 2. (Remember,
hydrogen obeys the duet rule, so it only needs two electrons.)
5. Count the dots to make sure you have the right number, then check to see if everyone is full.
6. If an atom is short electrons, move a pair from a full atom into a double bond so they both have eight.
Examples
H 2O2
CO2
PF3
NH3
CH4
SO3