I agree with Helen. Double bonds do not indicate expanded octets; they are often used in order to obey the octet rule. All lewis structures should obey the octet rule except for a few special cases.
1. Species with an odd number of electrons, otherwise known as free radicals. An example a free radical would be the lone electron on N in the compound NO. Here is a lewis structure for NO: http://i.ytimg.com/vi/NGo8aV3oMCk/maxresdefault.jpg
2. Elements such as boron that never satisfy the octet rule. An example would be BF3. Here: http://2012books.lardbucket.org/books/b
As you can see, the central atom (B) only has 6 electrons around it, rather than 8 to fulfill its octet.
3. Elements that have expanded valence shells, such as phosphorous and sulfur. They can accept more than 8 atoms. An example of this would be PF5. http://i.ytimg.com/vi/aqDYtjhSdBE/maxresdefault.jpg
Other than these three situations, I do not see why you would not obey the octet rule. Again, double or triple bonds still allow you to obey the octet rule.
I hope I interpreted your question correctly!