SbH3 Lewis structure

SbH₃ (stibine) has one antimony atom and three hydrogen atoms.

In SbH₃ Lewis structure, three single bonds around the antimony atom, with three hydrogen atoms attached to it, and on the antimony atom, there is one lone pair.

Alternative method: Lewis structure of SbH₃

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, antimony lies in group 15, and hydrogen lies in group 1.

Hence, antimony has five valence electrons and hydrogen has one valence electron.

Since SbH₃ has one antimony atom and three hydrogen atoms, so…

Valence electrons of one antimony atom = 5 × 1 = 5
Valence electrons of three hydrogen atoms = 1 × 3 = 3

And the total valence electrons = 5 + 3 = 8

Learn how to find: Antimony valence electrons and Hydrogen valence electrons

• Second, find the total electron pairs

We have a total of 8 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the total electron pairs = 8 ÷ 2 = 4

• Third, determine the central atom

Here hydrogen can not be the central atom. Because the central atom is bonded with at least two other atoms, and hydrogen has only one electron in its last shell, so it can not make more than one bond.

Hence, here we have to assume that the central atom is antimony.

Therefore, place antimony in the center and hydrogens on either side.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 4 electron pairs. And three Sb — H bonds are already marked. So we have to only mark the remaining one electron pair as a lone pair on the sketch.

Also remember that antimony is a period 5 element, so it can keep more than 8 electrons in its last shell. And hydrogen is a period 1 element, so it can not keep more than 2 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are hydrogens. But no need to mark on hydrogen, because each hydrogen has already two electrons.

So for antimony, there is one lone pair.

Mark the lone pair on the sketch as follows:

Formal charge

Use the following formula to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

For antimony atom, formal charge = 5 – 2 – ½ (6) = 0

For each hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

Here, both antimony and hydrogen atoms do not have charges, so no need to mark the charges.

Final structure

The final structure of SbH₃ comprises a central antimony atom linked to three hydrogen atoms through single covalent bonds. In this arrangement, the antimony atom satisfies the octet rule by forming three bonding pairs and retaining one lone pair, while each hydrogen atom achieves its stable duet state. This configuration is the most stable because it results in formal charges of zero for all participating atoms, representing the most energetically favorable state for the molecule. Consequently, this electronic distribution serves as the definitive and most accurate Lewis representation of stibine.

Next: C₃H₉N Lewis structure

External video

• How to Draw the Lewis Dot Structure for SbH3: Antimony trihydride (Stibane) – YouTube • Wayne Breslyn

External links

• https://homework.study.com/explanation/draw-a-lewis-structure-for-the-following-compound-include-all-lone-pair-electrons-sbh-3.html
• https://oneclass.com/homework-help/chemistry/6910020-lewis-dot-structure-for-sbh3.en.html