IBr3 Lewis structure

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IBr₃ (iodine tribromide) has one iodine atom and three bromine atoms.

In IBr₃ Lewis structure, there are three single bonds around the iodine atom, with three bromine atoms attached to it. Each bromine atom has three lone pairs, and the iodine atom has two lone pairs.

Steps

To properly draw the IBr₃ Lewis structure, follow these steps:

#1 Draw a rough sketch of the structure
#2 Next, indicate lone pairs on the atoms
#3 Indicate formal charges on the atoms, if necessary

Let’s break down each step in more detail.

#1 Draw a rough sketch of the structure

• First, determine the total number of valence electrons

In the periodic table, both iodine and bromine lie in group 17.

Hence, both iodine and bromine have seven valence electrons.

Since IBr₃ has one iodine atom and three bromine atoms, so…

Valence electrons of one iodine atom = 7 × 1 = 7
Valence electrons of three bromine atoms = 7 × 3 = 21

And the total valence electrons = 7 + 21 = 28

Learn how to find: Bromine valence electrons

• Second, find the total electron pairs

We have a total of 28 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 = 28 ÷ 2 = 14

• Third, determine the central atom

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

Since iodine is less electronegative than bromine, assume that the central atom is iodine.

Therefore, place iodine in the center and bromines on either side.

• And finally, draw the rough sketch

#2 Next, indicate lone pairs on the atoms

Here, we have a total of 14 electron pairs. And three I — Br bonds are already marked. So we have to only mark the remaining eleven electron pairs as lone pairs on the sketch.

Also remember that iodine is a period 5 element, so it can keep more than 8 electrons in its last shell. And bromine is a period 4 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 bromines.

So for each bromine, there are three lone pairs, and for iodine, there are two lone pairs.

Mark the lone pairs on the sketch as follows:

#3 Indicate formal charges on the atoms, if necessary

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

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

For iodine atom, formal charge = 7 – 4 – ½ (6) = 0

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

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

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

Therefore, this structure is the stable Lewis structure of IBr₃.

Next: B₂ Lewis structure

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External links

• https://www.bartleby.com/questions-and-answers/draw-the-lewis-structure-for-iodine-tribromide-ibr3.-what-is-the-molecular-geometry-of-this-molecule/2133af36-150a-4690-ac13-bb395fa9a45f
• https://www.chegg.com/homework-help/questions-and-answers/lewis-structure-ibr3-central-atom–molecular-polar-nonpolar-identify-intermolecular-forces-q28406979
• https://www.numerade.com/ask/question/what-is-the-lewis-structure-for-ibr3-with-the-central-atom-of-i-is-the-molecular-polar-or-nonpolar-identify-the-intermolecular-forces-present-63972/