Lewis Dot Structures

This week we learned about Lewis Dot Structures. It is defined as a structural representation of a given molecule where the dots show electron position and the lines show covalent bonds between atoms. The guidelines for drawing these structures are as followed:
1. Calculate the total number of valence electrons by adding all of the valence electrons for each atom in the molecule. (this is found on the periodic table)
2. Divide the total valence electrons by 2 to find the number of electron pairs in the molecule
3. Surround the central atom with 4 electron pairs. Use the remaining electron pairs to complete the octet around the other atoms. The only exception is hydrogen which only needs two
4. Electron pairs that are shared by atoms are called bonding electrons. the others are called lone pairs
5. If there are not enough electron pairs to provide each atom with an octet, move a nonbonding electron pair between two atoms that already share an electron pair.
Here are some examples:

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