TeCl2 Lewis structure

TeCl₂ (tellurium dichloride) has one tellurium atom and two chlorine atoms.

In TeCl₂ Lewis structure, there are two single bonds around the tellurium atom, with two chlorine atoms attached to it. Each chlorine atom has three lone pairs, and the tellurium atom has two lone pairs.

Alternative method: Lewis structure of TeCl₂

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, tellurium lies in group 16, and chlorine lies in group 17.

Hence, tellurium has six valence electrons and chlorine has seven valence electrons.

Since TeCl₂ has one tellurium atom and two chlorine atoms, so…

Valence electrons of one tellurium atom = 6 × 1 = 6
Valence electrons of two chlorine atoms = 7 × 2 = 14

And the total valence electrons = 6 + 14 = 20

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

• Second, find the total electron pairs

We have a total of 20 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 = 20 ÷ 2 = 10

• Third, determine the central atom

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

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

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

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 10 electron pairs. And two Te — Cl bonds are already marked. So we have to only mark the remaining eight electron pairs as lone pairs on the sketch.

Also remember that tellurium 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 tellurium, there are two lone pairs.

Mark the lone pairs 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 tellurium atom, formal charge = 6 – 4 – ½ (4) = 0

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

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

Final structure

The final structure of TeCl₂ contains a central tellurium atom connected to two chlorine atoms through single covalent bonds. In this layout, the tellurium atom satisfies the octet rule by forming two bonding pairs and retaining two lone pairs. Each chlorine atom also fulfills its octet by maintaining three lone pairs of its own alongside the single shared bond. This setup is the most stable because it results in formal charges of zero for all atoms, representing the most energetically favorable state for the molecule. As a result, this specific electronic distribution serves as the definitive and most accurate Lewis representation of tellurium dichloride.

Next: CH₂I₂ Lewis structure

External video

• How to Draw the Lewis Dot Structure for TeCl2: Tellurium dichloride – YouTube • Wayne Breslyn

External links

• https://www.numerade.com/questions/draw-lewis-dot-structures-for-the-molecules-listed-here-a-mathrmtecl_2-b-mathrmhi-c-mathrmasbr_3-d-o/
• https://www.chegg.com/homework-help/questions-and-answers/question-1-1-pts-lewis-structure-tecl2-total-number-valence-electrons-select-central-atom–q71316166