Consider the sulfine ion SO3^-2, what is the hybridization of the sulfur atom?

[DSNCSUN]

a) sp3
b)sp2
c)dsp3
d)d2sp3
e)sp

I understand that it's sp3 but it took too long to get to that answer first starting with giving an octet to sulfur and then expanding to see that a better structure works out with less charges on each atom. So any more efficient quicker way for this?

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[Ashish]

1> Count valence electrons of sulphur and oxygen ( 6 for both and a total of 26 (6x4 and 2= 26 total; you wanna get quick at knowing this. Recommend making periodic table your desktop background)
2> draw lewis structure and fill out octets for the surrounding atoms ( here 3 oxygens).
3> Give the remaining electrons to the central atom (sulphur here gets 2 additional electrons and has 3 "things" around it so total of 4 "things" around it. Thus sp3.

This is not lengthy process at all especially with some practice; although it appears so here 🤣

 

[DSNCSUN]

1> Count valence electrons of sulphur and oxygen ( 6 for both and a total of 26 (6x4 and 2= 26 total; you wanna get quick at knowing this. Recommend making periodic table your desktop background)
2> draw lewis structure and fill out octets for the surrounding atoms ( here 3 oxygens).
3> Give the remaining electrons to the central atom (sulphur here gets 2 additional electrons and has 3 "things" around it so total of 4 "things" around it. Thus sp3.

This is not lengthy process at all especially with some practice; although it appears so here 🤣

Thank you for the help, in the solutions of destroyer sulfur ends up having an expanded octet double bonding to one of the oxygens. although this detail is not necessary to answer the question in this particular case were you able to notice that? That's was what i meant when I said it would take long to figure that out. Thanks again

 

[zyzzbruh]

Don't worry about Sulfur making an octet, it's an exception. Just follow what Ashish said and assure your formal charges are correct.

 

[DAT Destroyer]

a) sp3
b)sp2
c)dsp3
d)d2sp3
e)sp

I understand that it's sp3 but it took too long to get to that answer first starting with giving an octet to sulfur and then expanding to see that a better structure works out with less charges on each atom. So any more efficient quicker way for this?

Be careful with this, you have made an error on the name. SO3 is sulfur trioxide . It is sp3 , trigonal planar. Sulfur loves to break the octet rule. so be generous with double bonds.So3-2 is a different specie, it is called the sulfite ion. Here the hybridization is sp3d because the lone pair resides on the sulfur atom.

Hope this helps..

Dr. Romano

 

[DSNCSUN]

Don't worry about Sulfur making an octet, it's an exception. Just follow what Ashish said and assure your formal charges are correct.

sometimes you get a large quantity for formal charge I remember the smaller the charge and the fewer the better and you would play around until you found the most stable resonance structure, how do avoid wasting time like that?

 

[asdf99]

Be careful with this, you have made an error on the name. SO3 is sulfur trioxide . It is sp3 , trigonal planar. Sulfur loves to break the octet rule. so be generous with double bonds.So3-2 is a different specie, it is called the sulfite ion. Here the hybridization is sp3d because the lone pair resides on the sulfur atom.

Hope this helps..

Dr. Romano

Hi Dr. Romano, the 2016 dat destroyed says that the Sulfur hybridization in the sulfite ion is sp3. However, I am having a little bit of trouble conceptualizing this. How is sulfur making a pi bond if it is sp3 hybridized?

I apologize if this is an obvious/easy question, but I'm just trying to wrap my head around it.

Thanks!

 

[Don Kim]

Hi Dr. Romano, the 2016 dat destroyed says that the Sulfur hybridization in the sulfite ion is sp3. However, I am having a little bit of trouble conceptualizing this. How is sulfur making a pi bond if it is sp3 hybridized?

I apologize if this is an obvious/easy question, but I'm just trying to wrap my head around it.

Thanks!

My guess is since there are four electron domains, it will be sp3, but since there is some double bond character due to resonance, the hybridization might be maybe half and half sp2/sp3.
But for the sake of getting the answer, I think just going by how many electron domains there are is the safer route, instead of just associating pi-bonds with non-sp3.
Another similar example I can think of is P4O10. Each phosphorus has 4 electron domains. (3 single bonds to oxygen, 1 double bond to oxygen = 5 total bonds) But this phosphorus is
till considered sp3 despite the double bond b/c there are 4 electron domains so the shape tetrahedral. But yeah, I agree this is a

 

[asdf99]

My guess is since there are four electron domains, it will be sp3, but since there is some double bond character due to resonance, the hybridization might be maybe half and half sp2/sp3.
But for the sake of getting the answer, I think just going by how many electron domains there are is the safer route, instead of just associating pi-bonds with non-sp3.
Another similar example I can think of is P4O10. Each phosphorus has 4 electron domains. (3 single bonds to oxygen, 1 double bond to oxygen = 5 total bonds) But this phosphorus is
till considered sp3 despite the double bond b/c there are 4 electron domains so the shape tetrahedral. But yeah, I agree this is a

Thanks bruh

 

[LuckBloodandSweat]

Didn't you take the DAT already? o__o

 

[DSNCSUN]

Didn't you take the DAT already? o__o

I love it so much I'm still working on destroyer.LOL this post is from the painful days of studying, May 26th

 

[LuckBloodandSweat]

Oh LMAO! Yeah I remember seeing your breakdown and I'm like no way this is happening, this dude already took it! Lol @ dead threads being revived xD

 

[DAT Destroyer]

Hi Dr. Romano, the 2016 dat destroyed says that the Sulfur hybridization in the sulfite ion is sp3. However, I am having a little bit of trouble conceptualizing this. How is sulfur making a pi bond if it is sp3 hybridized?

I apologize if this is an obvious/easy question, but I'm just trying to wrap my head around it.

Thanks!

Look at the structure drawn.......Go to the central S atom....Now.....draw a small circle around the S and the first oxygen...next do it for the second and third Oxygen. Now...draw a small circle from the S to the LONE ELECTRON pair......Thus you should see 4 " areas " of space.......In General Chemistry.......four areas of space means sp3 hybridization. If you had 5 areas of space as in PCl5...we have dsp3 hybridization...and in SF6...we have 6 areas of space from the central atom, hence d2sp3 hybridization . I have other problems like this...go over them all and learn the material. . If you are still stuck...let me know...I will try to scan it in for you.....if you are lost !!!

Hope this help

Dr. Romano