What’s the Lewis structure for XeCl3 -1?

In HSO3- Lewis structure Sulfur is least electron electronegative atom and goes in the center of the Lewis structure.

For the Lewis structure for HSO3- you should take formal charges into account to find the best Lewis structure for the molecule. Also note that you should put the HSO4- Lewis structure in brackets with as 1- on the outside to show that it is an ion with a negative one charge.

In the Lewis structure for HSO3- there are a total of 26 valence electrons.

HCO3- is essentially an H+ and a CO3 2- combined. CO3 2- contained 24 valence electrons with a structure consisting of a C bonded to 3 O’s. The C is sp2 hybridized and is resonance stabilized with 2 C-O and 1 C=O.

Xe = 8 electrons,

4[F] = 4 electrons

Total electrons in XeF4 =Xe (8) + F (4) = 12 e-

Electron pairs = 6

bond pair = 4

lone pairs = 2

sigma pair = 4

Geometry = octahedral

shape = square planar

Actually Lewis and I don’t get alone very well but this should be what it looks like.

Cl is one electron short of the 8 surrounding the atom

* *
* Cl *
* x
* *

Oxigen is two short of the 8

* *
* O x
* *
x *

* is electron x is free place
Cl is not neutral, it is Cl- one e- more and so is ClO-

** **
* Cl ** O *
* ** *
**

Are you sure it’s a 3- charge? A 1- is easy to explain, a C bonded to three N atoms, octets on all the atoms with one nonbonded electron pair on all C and N atom but that is only 26 electrons and not 28 which the 3- would require.

I thought i could by extrapolation from XeF2 and XeF4…but i have not been able to except wonder if it is a possible compound. Is there a XeF3–1 likewise ?

I am gonna own this saying, “ i do not believe the compounds above are able to become ionic in nature the way both you and i have written Xe(halide3)-1 them”

XeF2, XeF4, and XeF6 all exist….but XeF-1, XeF3–1, and XeF5–1 for me are concept ideas for discussion only and still i need help on this one if i am incorrect here where i have landed.

☆ [[ see William von Bencem’s answer !

I added this comment AFTER checking answers from others. I answer first, then check what others have written. Sure i could check first….but you learn better when you ‘act the fool’…..i’m not afraid to learn ot make mistakes]] ☆

Xe has noble gas electron configuration s2p2p2p2 so it has to expand its octet to s2p2p1p1d1d1 to accommodate the 3 Cl atoms. The shape of the hybridization is octahedral. Three Cl atoms are bonded to three single electrons and one electron is added to the remaining single electron to give the negative charge on the ion. There are two possible shapes for the molecule, two polar and one equatorial Cl or two equatorial and one polar. Both molecules are polar.