SnCl2 Lewis structure

SnCl₂ [tin(Ⅱ) chloride] has one tin atom and two chlorine atoms.

In the SnCl₂ Lewis structure, there are two single bonds around the tin atom, with two chlorine atoms attached to it. Each chlorine atom has three lone pairs, and the tin atom has one lone pair.

Alternative method: Lewis structure of SnCl₂

Contents

Rough sketch

First, determine the total number of valence electrons

In the periodic table, tin lies in group 14, and chlorine lies in group 17.

Hence, tin has four valence electrons and chlorine has seven valence electrons.

Since SnCl₂ has one tin atom and two chlorine atoms, so…

Valence electrons of one tin atom = 4 × 1 = 4
Valence electrons of two chlorine atoms = 7 × 2 = 14

And the total valence electrons = 4 + 14 = 18

Learn how to find: Tin valence electrons and Chlorine valence electrons

Second, find the total electron pairs

We have a total of 18 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 = 18 ÷ 2 = 9

Third, determine the central atom

We have to place the least electronegative atom at the center.

Since tin is less electronegative than chlorine, assume that the central atom is tin.

Therefore, place tin in the center and chlorines on either side.

And finally, draw the rough sketch

SnCl2 Lewis Structure (Step 1) — Rough sketch of SnCl₂ Lewis structure | Image: Learnool

Lone pair

Here, we have a total of 9 electron pairs. And two Sn — Cl bonds are already marked. So we have to only mark the remaining seven electron pairs as lone pairs on the sketch.

Also remember that tin is a period 5 element, so it can keep more than 8 electrons in its last shell. And chlorine is a period 3 element, so it can keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are chlorines.

So for each chlorine, there are three lone pairs, and for tin, there is one lone pair.

Mark the lone pairs on the sketch as follows:

SnCl2 Lewis Structure (Step 2) — Lone pairs marked, and got the stable Lewis structure of SnCl₂ | Image: Learnool

Formal charge

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

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

For tin atom, formal charge = 4 – 2 – ½ (4) = 0

For each chlorine atom, formal charge = 7 – 6 – ½ (2) = 0

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

Final structure

The final structure of SnCl₂ contains a central tin atom linked to two chlorine atoms through single covalent bonds. Within this layout, the tin atom satisfies the octet rule by forming two bonds and retaining one lone pair, which results in a bent molecular geometry. In this configuration, each chlorine atom fulfills its octet by maintaining three lone pairs alongside its single shared bond. This arrangement represents the most stable state for the molecule because it results in a formal charge of zero for every atom involved. Accordingly, this specific electronic distribution serves as the definitive and most accurate Lewis representation of tin(Ⅱ) chloride (also known as stannous chloride).

Next: CH₃COO^– Lewis structure

External video

SnCl2 Lewis Structure – How to Draw the Lewis Structure for SnCl2 – YouTube • Wayne Breslyn

External links

Deep

Learnool.com was founded by Deep Rana, who is a mechanical engineer by profession and a blogger by passion. He has a good conceptual knowledge on different educational topics and he provides the same on this website. He loves to learn something new everyday and believes that the best utilization of free time is developing a new skill.