Bond Order from Lewis.mpg

[MsEvilgenius101]

YOU ARE A SUPERSTARRR!!!!!!!!!!!!!!!!!!!­!!!!!!!!!!!!!!!!! YOU FUCKING ROCKKKK LOL! Can't thank you enough. However, what is the purpose of the bond order? Like what does it prove?

[EnderlePhD]

@MsEvilgenius101 The bond order indicates the type of bond. BO = 1 is a single bond, BO = 2 is a double bond, and BO = 3 is a triple bond. Any number in between is a combination thereof. Most students will see the importance of bond order when they learn molecular orbital diagrams because there the bond order is not as straightforward as this example.

[cfernandez1127]

thanks homie



[MrWelfare]

Thanks for the video! Do you mind me asking how I would find the bond order for a molecule such as nitryl chloride? O2NCl? Here, there is resonance with the chlorine and I don't think your method would work.

[EnderlePhD]

@MrWelfare Tell me what you think are all the viable resonance structures and I'll answer the question. It does get more difficult when the resonance structures don't contribute equally.

[MrWelfare]

@EnderlePhD thanks for the reply! But I got it figured out! I realized after that the formal charges in the Lewis Structure with the double bond on the Cl made that model unfavorable. After I ignored that one, I was able to get the NO bond order of 1.5 the same way you described above. Thanks again!!!

[MrVernalchung]

thank you guy

[chrisr8808]

Love this video thanks so much ,.....saved my homework

[sweetsmile493]

i dont like that method. i say use best resonance structure count total bonds and divide by number of outside atoms being bonded to.

[EnderlePhD]

@sweetsmile493 That's fine with me. Be careful because not all bonds are involved in the resonance so it is easy to mis-count depending on the given molecule.

[zebrazebra1990]

Thanks for explaining how to get bond order. If you don't mind could you explain what it actually is? sorry dumb question lol

[EnderlePhD]

@zebrazebra1990 Bond order gives you a method to calculate the type of bond. A bond order of 1 means there is one bond, or two electrons, shared between the atoms. A bond order of 2 means there is a double bond, or 4 electrons.

[oexnorth]

Is that chick in the front hot? Just wondering.

[mssca]

How do you do bond order when you DO NOT Have resonance like PCl3? plus my textbook says: OB=0.5*(no. of bonding e-no. of nonbonding e) Please help....

[EnderlePhD]

@mssca That formula is helpful if you are doing MO theory. If you are just looking at a Lewis structure, then the bond order is defined by the type of bond. For a single bond, the bond order is 1. For a double bond, the bond order is 2. For a triple bond, the bond order is 3.

[mssca]

@EnderlePhD,

For PCL3 I get BO=-3... can I even have a negative number at the first place? I am confused.

Thank you for the help.

[EnderlePhD]

@mssca Draw the Lewis structure and you will get P-Cl single bonds. A single bond means and bond order of one.

[jalonzo31]

The Bond Order is so EASY now!!!!

my professor wouldn't tell us, and expected us to figure it out from guessing

A+ for u

[730ize]

dude thanks, my teacher didn't tell us this, may be because she wants us to fail her hard test.

[Dakashizzlenizzle]

i wish you were my teacher, mine just gives us a note packet and then we go home and do bookwork... and im only a sophomore in highschool, god this sucks

[b1g1freeagain]

what thei dont rmemeber solving bond orders that way. that way seems like it would cause some errors. what if u forget to draw a resonance strucutre. shouldnt u use the molecular orbital diagram to solve for bond orders?

[EnderlePhD]

@b1g1freeagain You are right. Students must remember to draw all resonance structures to solve for the BO. In this case, drawing the Lewis then resonance structures is the easiest way. The MO diagram for a molecule like this one would be beyond the scope of general chemistry.

[purplepick1]

sweet, that makes sense!

[ErniesLament]

I know this is sort of irrelevant to the material you were presenting but the shouldn't the geometry have been drawn as trigonal planar since the N has no lone pair?

[EnderlePhD]

@ErniesLament If I had drawn the geometry, you are completely correct. It is trigonal planar. In this case, the geometry was not needed to solve the problem.

[y100269]

how big are your classes? my chem class has 600 students and we can't ask questions during class. we have to go to a resource room in the evening and ask a TA who is unaware of what we're learning.

[ammarhollywood]

He was talking to himself, its like if he intended to make everybody confused.

[EnderlePhD]

@ammarhollywood Which part confused you? I'm happy to clarify.

[yukipham18]

@EnderlePhD so it's okay for the N to not have 5 e- around it? because i'm only see 4 bonds around N, that's 8 e-, but 4 e- goes to the other 3 O's

[EnderlePhD]

@yukipham18 Correct. Good thinking! First, the N must have 8 electrons around to it to fulfill the octet - it does! Second, the formal charge on N is +1 (two of the O atoms are -1). While we prefer a formal charge of zero, either +1 or -1 works. In this case, these non-zero formal charges are the best we can do with the basic Lewis structure concept. From your comment, I'm guessing you learned a different style of drawing Lewis. If you want, check out my method on the other videos.

[EnderlePhD]

The oxygen atoms do have octets, or 8 surrounding electrons. Single bonded oxygen atoms have 2 electrons from the single bond and 6 lone pair electrons. Double bonded electrons have 4 electrons from the double bond and 4 from the lone pairs. Either way, it adds up to 8.

The nitrogen atom add 5 to the overall valence count of the nitrate ion. Each oxygen atom adds 6. The negative charge adds one. In the molecule the formal charges are 0.

Let me know if you need more explanation! Cheers!

[IMBLUESTREAK23]

why was the first one wrong? Formal charge?

[EnderlePhD]

If you keep three single bonds from N to O, then N does not have an octet. 2nd period elements like N always prefer an octet. I recommend always checking your octet first, then look at formal charge second.