# TeF6 Lewis structure

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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.

Contents

## Steps

Here’s how you can easily draw the TeF6 Lewis structure step by step:

#1 Draw a rough skeleton structure
#2 Mention lone pairs on the atoms
#3 If needed, mention formal charges on the atoms

Now, let’s take a closer look at each step mentioned above.

### #1 Draw a rough skeleton structure

• 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

• 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

### #2 Mention lone pairs on the atoms

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:

### #3 If needed, mention formal charges on the atoms

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.

In the above structure, you can see that the central atom (tellurium) forms an octet. And the outside atoms (fluorines) also form an octet. Hence, the octet rule is satisfied.

Therefore, this structure is the stable Lewis structure of TeF6.