Answer :

pstnonsonjoku

Answer:

explanation and image attached

Explanation:

Our aim is to draw a structure of XeO2F2 whith the least formal charges. We must remember that the compound has 34 valence electrons.

To obtain the least formal charges then Xe must have a total of twelve electrons on its valence shell instead of eight.

The other atoms around the central Xe atom are arranged as shown in the image attached.

Image Credit: UCLA

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annyksl

The correct Lewis structure allows all the atoms involved in the bond to have eight electrons in the valence layer.

You can see this structure in the image attached below.

We can arrive at this answer because:

  • According to the Lewis structure, atoms must achieve electronic stability, by getting eight electrons in the valence layer.
  • Therefore, covalent bonds are very important, as it allows atoms to share electrons, so that they achieve stability.
  • Within the Lewis structure, each little ball around the atom symbol represents an electron in the valence layer and each trace represents the sharing of one more electron.

In this case, we can observe the figure below and count the number of electrons that each atom reaches with the covalent bond between them. This will show us that each has eight electrons, which is the correct structure for [tex]X_eO_2F_2[/tex].

More information:

https://brainly.com/question/11439067?referrer=searchResults

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