Questions tagged [lewis-structure]

For questions about determining Lewis structures (or their validity) for different chemical species. Do not use this tag if your question is about determining [oxidation-state] or [formal-charges], use the other respective tags instead.

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Are bond orders always the same in isoelectronic diatomic species?

In my textbook of chemistry it is written that: In the Lewis description of covalent bond, the Bond order is given by the number of bonds between the two atoms of a molecule. ... ...
4
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0answers
566 views

What is an algorithm for drawing resonance structures?

Question What is an instance of a procedure for writing resonance structures for any given compound's name or structural formula? I would prefer any of these formats to represent the algorithm: ...
4
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1answer
191 views

Is it possible to use the school supplied algorithm to build the Lewis diagram of the iodate ion?

I am upgrading the grade 12 chemistry credit and have to use the school supplied algorithm to build the Lewis diagram of $\ce{IO3-}$ ion. It seems to me that iodine oxidation state in this ion should ...
4
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1answer
1k views

Are the Phosphate and Sulfate ion diagrams with double bonds an invalid picture?

Whenever you see an image of phosphate, it's always shown having 5 bonds. 3 single bonds to anionic oxygen atoms and a double bond to an extra neutral oxygen. Not only that, but they're shown being ...
3
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0answers
359 views

Can the Lewis dot structure of SO2 be experimentally verified?

I have just watched 2 different videos on the Lewis dot structure of sulfur dioxide, $\ce{SO2}$. One says it is $$\ce{O=S=O}$$ and the other says $$\ce{^-O-S^+=O <-> O=S^+-O-}$$ The first ...
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83 views

Linear algebra in Lewis structures?

In general, I have come across a phenomenon in chemistry where solutions to certain types of problems can often seem frustrating when trying to work out by hand, as they seem to depend on each other ...
2
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0answers
3k views

How can the formal charge of the B in the Lewis structure of BF4(-) ion be minus one?

How can the formal charge of the $\ce{B}$ in the lewis structure of $\ce{BF4-}$ ion be minus one ? I draw the lewis structure of $\ce{BF4-}$ ion such like the following: I put $\ce{B}$ in the ...
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41 views

Is bonds in CO is all 3 coordinate bonds or 2 covalent and 1 coordinate bonds?

Below image is as available in India's Class 11 NCERT Chemistry book vol 1 Page 104. I am confused as it states all 3 bonds are kind of coordinate bonds. Should it not start with 2 covalent bonds and ...
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0answers
39 views

Formal charge: size vs electronegativity?

My question is why size is not taken into consideration when deciding major contributors of resonance structures, particularly: why is the formal charge always assigned to the most electronegative ...
1
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0answers
294 views

How to rationalise the resonance structures of nitrogen dioxide?

The following image depicts resonance in $\ce{NO2}$ molecule: I don't know if it is obvious or not, but I'm puzzled by this structure. I've read about the structure of the $\ce{NO2}$ compound, but it ...
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2k views

Lewis structure of ClO radical

The commonly shown structure of the ClO radical described here has a single bond between the chlorine and oxygen atoms. In that structure, chlorine has a formal charge of 1, and oxygen has a formal ...
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0answers
6k views

Cyanide's Lewis structure - electronegativity or octet rule?

The formula for the cyanide ion is $\ce{CN-}$. That gives us a total of ten valence electrons to work with. There are two obvious ways to build the Lewis structure. $\ce{:^-C#N:}$ $\ce{:C=N^-::...
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558 views

Why do BF3 and NH3 react when B has an expanded octet in the adduct?

I know that some elements like sulfur are able to have an expanded octet due to vacant $\mathrm{d}$ orbitals. However, boron and nitrogen do not have any such vacant place so how is it that $\ce{NH3}$ ...
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37 views

Why is Cl2-P-O-Cl an unfavourable structure for POCl3?

Why is the structure $\ce{(Cl)2P - O - Cl}$ unfavourable compared to the two structures in the picture? The latter in the picture and the one I stated both have zero formal charge, so I don't really ...
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28 views

Correct representation of Lewis structure for sulphate ion

sulphate ion has tetrahedral geometry as predicted by VSEPR theory; the four S-O bonds are indistinguishable and have the same bond order, so the Lewis structure is better represented avoiding S=O ...
0
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0answers
79 views

What is the correct electron dot notation of carbon?

My book says that the dot notation for Lewis structure of carbon has 2 possible ways: two dots on the right, one on the top, one on the left one dot on all four sides Why are both of these correct? ...
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90 views

Lewis Structures and electron distribution with oxygen atom

I am a novice in chemistry. I don’t understand the way Lewis structure and how electrons are shared between elements. For instance As we know, Oxygen has six valence electrons that means it has ...
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0answers
1k views

Why isn't O=N-O-O the best lewis structure for NO3-?

I'm practicing lewis structures and I'm stuck on the one for NO3 -1 (nitrate ion). I understand that N has to be the central atom because it is the least electronegative, but I'm confused why all the ...
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51 views

How can nitrogen be quadruply bonded in tris(8-hydroxyquinoloinato)aluminum?

Nitrogen typically has five outer valence electrons. So how does a triply-bonded nitrogen in 8-hydroxyquinoline end up quadruply bonded in tris(8-hydroxyquinolinato)aluminum?
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1answer
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Structure of IO2F5(2-) dianion

This question came in my exam to draw the Structure of $\ce{[IO_2F_5]^2-}$ I am confused. Here's what I reasoned: Iodine will have hybridisation $\ce{sp^3d^3}$ so it will be pentagonal bi ...