Lewis structures (also known as Lewis dot structures or electron dot structures) are diagrams that represent the valence electrons of atoms within a molecule. It is used to show how electrons are arranged around individual atoms in a molecule. And electrons are shown as dots. In this activity, the complete dot structure is required, meaning that all bonds (lines) will need to be turned into dots. Here is an example:

Although both above Lewis structures can represent the molecular structure of carbon monoxide (CO) correctly, only the left one is required for this activity.

Use the Lewis diagram to draw for each hypothetical molecule shown below, and think critically about which molecule makes sense because each atom has a complete valence shell and each bond has the correct number of electrons.

Draw Lewis for both of them on your note (2pts), then mark or circle the nonsensical molecule on your note clearly (1pts). Take a picture to submit for grading.

2. Explain what makes the other molecule nonsensical, considering the number of bonds each type of atom can make. Your explanation has to be relevant to your drawing and specific to that molecular structure. (2pts)

Notice The Lewis diagram uses the correct number of valence electrons for each atom. And count how many dots (electrons) should be around each atom. And draw all valence electrons for each atom, including those valence electrons that are not being shared (forming bonds).