If you used a triple bond then the formal charges have changed and are no longer neutral which is preferred. Plus if you didn't add the lone pairs and just placed a triple bond the number of electrons would be off. You'll see the below image explains why it had to be a double bond. 

When you aren't sure of the structure always check if you have the correct number of electrons (octet rule) and if the formal charges are neutral. Neutral structures want every atom to have a neutral formal charge. When there is a net charge of let's say -1 then the more electronegative atom will have the negative formal charge. 

When removing a proton we are looking at the area that has a full positive charge or a partial positive charge. We saw this with the full positive charge on the N and partial positive charge on the pi bonds. 

We also know to remove a H from the more electronegative atom because it will hold a negative charge better than a C. Carbons do not like being negative they are most happy when neutral. 

We don't have downloads on this, but in most textbooks you'll find lists of the different prefixes. Several of them also have them in the back in the appendix. 

Aliyah Arias When you are drawing the MO diagram you add the electrons then when you are looking for the bond order yes you subtract the bonding orbitals - the anti-bonding orbitals. This is why we get 2-2 which is 0 on top. 

You could have had the lone pair on the wedged and the hydrogen on the dashed, that's fine too. As long as you keep with the pattern of the rest of the bonds how they all go dashed then wedged. You could have also drawn the bonds all going wedged then dashed. 

Were you referring to the Helium (He) example? If so, recall that we are adding the outside 1s orbitals  electrons and He has 2 electrons in each 1s orbital. Since we have two 1s orbitals for He2 this is why there is a total of 4 electrons in the center. 2 in the bonding and 2 in the anti-bonding. 

If you have any examples of the questions you are thinking of please feel free to post that in the Homework Help group and our team can help you out. Click on the "ochem-homework-help" on the bottom left. Seeing the questions you are referring to, helps us know what to add to better help you and other students 👍

Yes it's in the below video:

The numbers refer to the location of the ethyl group, by saying "3,3" we are saying the location of the ethyl carbons. Both ethyls are at carbon 3 so 3,3. While it's the "diethyl" portion of the name that refers to their being 2 ethyl groups. 

Jen - Chemmunity Team Elvia Castillo, after you finish this video I recommend watching and trying out the practice problems in the below video. You'll find more examples with nitrogen and oxygen and some trick questions to look out for.