TeO3 Lewis Structure in 6 Steps (With Images)

So you have seen the above image by now, right?

Let me explain the above image in short.

TeO3 lewis structure has a Tellurium atom (Te) at the center which is surrounded by three Oxygen atoms (O). There are 3 double bonds between the Tellurium atom (Te) and each Oxygen atom (O). There are 2 lone pairs on all three Oxygen atoms (O).

If you haven’t understood anything from the above image of TeO3 lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of TeO3.

So let’s move to the steps of drawing the lewis structure of TeO3.

Steps of drawing TeO3 lewis structure

Step 1: Find the total valence electrons in TeO3 molecule

In order to find the total valence electrons in TeO3 molecule, first of all you should know the valence electrons present in tellurium atom as well as oxygen atom.
(Valence electrons are the electrons that are present in the outermost orbit of any atom.)

Here, I’ll tell you how you can easily find the valence electrons of tellurium as well as oxygen using a periodic table.

Total valence electrons in TeO3 molecule

→ Valence electrons given by tellurium atom:

Tellurium is a group 16 element on the periodic table. ^[1] Hence the valence electrons present in tellurium is 6.

You can see the 6 valence electrons present in the tellurium atom as shown in the above image.

→ Valence electrons given by oxygen atom:

Oxygen is group 16 element on the periodic table. ^[2] Hence the valence electrons present in oxygen is 6.

You can see the 6 valence electrons present in the oxygen atom as shown in the above image.

Hence, 

Total valence electrons in TeO3 molecule = valence electrons given by 1 tellurium atom + valence electrons given by 3 oxygen atoms = 6 + 6(3) = 24.

Step 2: Select the central atom

For selecting the center atom, you have to remember that the atom which is less electronegative remains at the center.

Now here the given molecule is TeO3 and it contains tellurium atom (Te) and oxygen atoms (O).

You can see the electronegativity values of tellurium atom (Te) and oxygen atom (O) in the above periodic table.

If we compare the electronegativity values of tellurium (Te) and oxygen (O) then the tellurium atom is less electronegative.

So here the tellurium atom (Te) is the center atom and the oxygen atoms (O) are the outside atoms.

Step 3: Connect each atoms by putting an electron pair between them

Now in the TeO3 molecule, you have to put the electron pairs between the tellurium atom (Te) and oxygen atoms (O).

This indicates that the tellurium (Te) and oxygen (O) are chemically bonded with each other in a TeO3 molecule.

Step 4: Make the outer atoms stable

Now in this step, you have to check the stability of the outer atoms.

Here in the sketch of TeO3 molecule, you can see that the outer atoms are oxygen atoms.

These outer oxygen atoms are forming an octet and hence they are stable. 

Also, in step 1 we have calculated the total number of valence electrons present in the TeO3 molecule.

The TeO3 molecule has a total 24 valence electrons and all these valence electrons are used in the above sketch of TeO3. 

Hence there are no remaining electron pairs to be kept on the central atom. 

So now let’s proceed to the next step.

Step 5: Check the octet on the central atom. If it does not have octet, then shift the lone pair to form a double bond or triple bond.

In this step, you have to check whether the central tellurium atom (Te) is stable or not.

In order to check the stability of the central tellurium (Te) atom, we have to check whether it is forming an octet or not.

Unfortunately, the tellurium atom is not forming an octet here. Tellurium has only 6 electrons and it is unstable.

Now to make this tellurium atom stable, you have to shift the electron pair from the outer oxygen atom so that the tellurium atom can have 8 electrons (i.e octet).

After shifting this electron pair, the central tellurium atom will get 2 more electrons and thus its total electrons will become 8.

You can see from the above picture that the tellurium atom is forming an octet as it has 8 electrons.

Now let’s proceed to the final step to check whether the lewis structure of TeO3 is stable or not.

Step 6: Check the stability of lewis structure

Now you have come to the final step in which you have to check the stability of lewis structure of TeO3.

The stability of lewis structure can be checked by using a concept of formal charge.

In short, now you have to find the formal charge on tellurium (Te) atom as well as oxygen (O) atoms present in the TeO3 molecule.

For calculating the formal charge, you have to use the following formula;

Formal charge = Valence electrons – (Bonding electrons)/2 – Nonbonding electrons

You can see the number of bonding electrons and nonbonding electrons for each atom of TeO3 molecule in the image given below.

For Tellurium (Te) atom:
Valence electrons = 6 (because tellurium is in group 16)
Bonding electrons = 8
Nonbonding electrons = 0

For double bonded Oxygen (O) atom:
Valence electrons = 6 (because oxygen is in group 16)
Bonding electrons = 4
Nonbonding electrons = 4

For single bonded Oxygen (O) atom:
Valence electrons = 6 (because oxygen is in group 16)
Bonding electrons = 2
Nonbonding electrons = 6

From the above calculations of formal charge, you can see that the tellurium (Te) atom has +2 charge and both the single bonded oxygen (O) atoms have -1 charges.

Because of this reason, the above obtained lewis structure of TeO3 is not stable. 

So we have to minimize these charges by shifting the electron pairs towards the tellurium atom.

After shifting the electron pairs from oxygen atom to tellurium atom, the lewis structure of TeO3 becomes more stable.

In the above lewis dot structure of TeO3, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of TeO3.

I hope you have completely understood all the above steps.

For more practice and better understanding, you can try other lewis structures listed below.

Try (or at least See) these lewis structures for better understanding:

About author

Jay Rana

Jay is an educator and has helped more than 100,000 students in their studies by providing simple and easy explanations on different science-related topics. He is a founder of Pediabay and is passionate about helping students through his easily digestible explanations.

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