TeF6 Lewis structure

TeF₆ (tellurium hexafluoride) has one tellurium atom and six fluorine atoms.

In TeF₆ Lewis structure, there are six single bonds around the tellurium atom, with six fluorine atoms attached to it, and on each fluorine atom, there are three lone pairs.

Alternative method: Lewis structure of TeF₆

Rough sketch

• First, determine the total number of valence electrons

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

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

Since TeF₆ has one tellurium atom and six fluorine atoms, so…

Valence electrons of one tellurium atom = 6 × 1 = 6
Valence electrons of six fluorine atoms = 7 × 6 = 42

And the total valence electrons = 6 + 42 = 48

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

• Second, find the total electron pairs

We have a total of 48 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 = 48 ÷ 2 = 24

• Third, determine the central atom

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

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

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

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 24 electron pairs. And six Te — F bonds are already marked. So we have to only mark the remaining eighteen 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 fluorine is a period 2 element, so it can not keep more than 8 electrons in its last shell.

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

So for each fluorine, there are three lone pairs, and for tellurium, there is zero lone pair because all eighteen electron pairs are over.

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 – 0 – ½ (12) = 0

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

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

Final structure

The final structure of TeF₆ comprises a central tellurium atom linked to six fluorine atoms through single covalent bonds. In this arrangement, the tellurium atom utilizes an expanded valence shell to accommodate twelve electrons, forming six bonding pairs with no remaining lone pairs. Within this layout, each of the six fluorine atoms successfully reaches a stable octet by maintaining three lone pairs alongside its single shared bond. This configuration 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 tellurium hexafluoride.

Next: SeF₅^– Lewis structure

External links

• https://homework.study.com/explanation/draw-the-lewis-structure-for-tef6-and-provide-the-following-information-a-number-of-bonding-electron-pairs-b-number-of-nonbonding-electron-pairs-c-electron-geometry-d-molecular-geometry-e-approximate-bond-angle.html
• https://www.bartleby.com/questions-and-answers/what-is-the-lewis-dot-structure-of-tef6/148bf1f3-74b9-4acf-b3a6-d94ada432fc3
• https://www.answers.com/Q/What_is_the_Lewis_structure_for_TeF6