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5 months ago@Vocaloid

5 months agoyou'd add up the valence electrons as usual, add 1 more since we have a -1 charge, divide by 2 to get the total # of e' pairs, and arrange them following lewis structure rules

5 months agogive it a shot and i'll step in if you're getting stuck or want a solution check

5 months agoO added a -1 charge to the two o's wiTH A single bond

5 months agoI added *

5 months agoalmost nitrogen has a formal charge of 1 here since it normally has 5 valence electrons but only 4 bonds here and 0 lone pairs (5 - 4 - 0) = +1 so you need to add a + to the central nitrogen

5 months agoif you want to double-check yourself in the future, since NO3- has an overall charge of -1, the formal charges need to sum up to -1 if we only put two negative charges on the oxygens, that's an overall formal charge of -2, not -1, so we know we need to add a +1 somewhere

5 months agoFOr this I know the overall charge is -2 but I don't know where to put that

5 months agolike at the top

5 months agonotice the formal charges on the single-bond oxygen oxygen has 6 valence electrons. in its current state it has 6 lone electrons and 1 bond, so its formal charge is 6 - 6 - 1 = -1 so each of the single-bonded oxygens gets a -1 formal charge making the overall formal charge -2

5 months agoWhat is the formal charge on each of the atoms? Enter the formal charges in the same order as the atoms are listed. of HOFO

5 months agomay I see your lewis structure? as far as I know I don't think any of the atoms have formal charges

5 months ago|dw:1540348011551:dw|

5 months agoH-O-F-O

5 months agoah, if they want all single bonds then your solution would be correct

5 months agoB

5 months agodepends on what the structures are

5 months agowhatever structure puts more electrons on the more EN atom, in this case, oxygen, would be the right structure

5 months agoThese are the hints so I was going off of this

5 months agoThat it is better

5 months agoi still need to see what the structures are

5 months agoI got it lol thanks though

5 months agoand two dots on the p which I forgot

5 months agogood

5 months agoso to get the minus I would put it on the single oxygen right

5 months agoyup

5 months agoSO this would be a plus on the middle o

5 months agoyes, any other formal charges you can see?

5 months agominus on the single o

5 months agogood

5 months agominus on the single o

5 months agoyeah i messed up before it's supposed to have 2 double bonds not 1

5 months agootherwise, good, then add the formal charges on oxygen and chlorine

5 months agoso minus on the single o

5 months agoyeah that's it

5 months agochlorine shouldn't have one I messed up my structure before whoops

5 months agoIt says its incorrect and I need to check the electrons

5 months agoDid you overload an octet?

5 months agoBecause I see 5 bonds on Chlorine

5 months agochlorine has an expanded octet and should theoretically be able to take more than 4 bonds but try removing one of the double bonds to give chlorine a +1 FC

5 months agoand putting two dots on the one that I make a single bond right

5 months agoWell I learned something new about Lewis structures today, thanks Voca

5 months ago^^'
~~Okay I'm leaving now so you guys can discuss lol~~

yeah, Cl with 2 single bonds to O, 1 double bond to oxygen, formal charge -1 on the single bond oxygen, and +1 on the chlorine

5 months agoNope :/ still wrong

5 months agoyou need -1 on both single bonded oxygens

5 months agoStill wrong

5 months agohuh.

5 months agodo I add something to the double bonded one maybe

5 months agono, that one has formal charge 0 so it shouldn't need anything.

5 months agooh the one you have right now needs an electron pair on chlorine

5 months agoDraw the Lewis structures for the NO2− ion. Include all resonance structures.

5 months agowhat does resonance mean

5 months agothis is something to review but it means you need to draw all possible structures of NO2-

5 months ago|dw:1540350690550:dw| there, this is a better image

5 months agothese are both resonance structures because they're the same compound just with different distributions of charge

5 months agookay so is the structure I did now okay if it is I can make the second one to it

5 months agoyeah just don't forget formal charges if they ask for them

5 months agoyeah that should be it, lmk how it goes

5 months agoit was right!

5 months agowould triple bonds be +2?

5 months agoformula for formal charge: valence electrons - (number of bonds) - (number of lone pairs)

5 months agotry to apply it to the first nitrogen

5 months agoso 5 ve in n

5 months ago6 in o

5 months agoyes, keep going

5 months ago16

5 months ago16?? where is this coming from

5 months agothe n20

5 months agoyou don't have to add up the whole molecule; consider each atom individually

5 months agooh okay then 10

5 months agofor the first nitrogen what is valence electrons - (number of bonds) - (number of lone pairs)

5 months ago10-2-0=8

5 months agonitrogen has 5 valence electrons the nitrogen has 2 bonds and 4 lone pair electrons so 5 - 2 - 4

5 months ago-1

5 months agoyes try to apply this logic to the other atoms

5 months agofor clarity's sake *** valence electrons - (number of bonds) - (number of lone pair electrons) ***

5 months agookay so 5-2-4 again ? :S

5 months agofor the central nitrogen you have valence electrons = 5 4 bonds 0 lone pair electrons.

5 months ago1

5 months agogood try to see what you get for oxygen

5 months ago6-4?

5 months ago-0

5 months agoyou also have 2 bonds

5 months ago6-2-0=4

5 months ago6 valence electrons 2 bonds 4 lone electrons

5 months ago0

5 months agogood

5 months agoso -1 , +1 , 0 for structure A see what you get for the others

5 months agocheck C again

5 months ago0 and -1 switched

5 months agofirst nitrogen 5 valence 1 bond 6 lone electrons

5 months ago-2

5 months ago0

5 months agofor the next

5 months agogood central nitrogen is +1 as you stated check the oxygen now

5 months ago+1

5 months agogood so C = -2, +1 +1

5 months agoA

5 months agonot quite nitrogen is less electronegative so it will want a higher formal charge oxygen will want a lower formal charge

5 months agoc

5 months agoNo B

5 months agoon structure B, you have -1 +1 0 structure C = 0, +1, -1 C puts the +1 on the nitrogen and the -1 on the oxygen which is preferable to structure B

5 months agoyeah try re-doing them from the top for each of the single bond O's you have 6 valence electrons 6 lone electrons 1 bond

5 months agodouble bond 0 has +1and n has 0?

5 months agosingle bond O's: 6 - 6 - 1 double bond O's: 6 valence - 2 bonds - 4 lone electrons nitrogen: 5 valence electrons - 1 bond - 0 lone electrons

5 months agonitrogen: 5 valence electrons - 1 bond - 0 lone electrons is nt an option for 4

5 months ago*4 bonds

5 months ago5 valence electrons - 4 bond - 0 lone electrons

5 months agoyou need to swap them carbon always follows octet; boron and phosphorus violate the octet rule (boron only makes 3 bonds whereas phosphorus can make more than 4)

5 months agoco or cs

5 months agoco right

5 months agoboth of them have carbon as the central atom and thus follow the octet rule

5 months agouh as far as I know you'd just add up the oxygen formal charges and divide by 4

5 months ago