Lewis structure of IF5

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The Lewis structure of IF₅ contains five single bonds, with iodine in the center, and five fluorines on either side. There are three lone pairs on each fluorine atom, and one lone pair on the iodine atom.

Steps

By using the following steps, you can easily draw the Lewis structure of IF₅:

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Calculate formal charge and check stability (if octet is already completed on central atom)

Let’s one by one discuss each step in detail.

#1 Draw skeleton

In this step, first calculate the total number of valence electrons. And then, decide the central atom.

• Let’s calculate the total number of valence electrons

We know that… both iodine and fluorine are the group 17 elements. Hence, both iodine and fluorine have seven valence electrons.

Now IF₅ has one iodine atom and five fluorine atoms.

So the total number of valence electrons = valence electrons of iodine atom + (valence electrons of fluorine atom × 5)

Therefore, the total number of valence electrons = 7 + 35 = 42

• Now decide the central atom

The atom with the least electronegative value is placed at the center. By looking at the periodic table, we get the electronegativity values for iodine and fluorine as follows:

Electronegativity value of iodine = 2.66
Electronegativity value of fluorine = 3.98

Obviously, iodine is less electronegative than fluorine. Hence, assume that iodine is the central atom.

So now, put iodine in the center and fluorines on either side. And draw the rough skeleton structure for the Lewis structure of IF₅ something like this:

Also read: How to draw Lewis structure of SCl₂ (4 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since iodine is surrounded by five fluorines, use ten electrons to show five chemical bonds as follows:

Also read: How to draw Lewis structure of ClF₃ (4 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 42 valence electrons. And in the above structure, we have already used ten valence electrons. Hence, thirty-two valence electrons are remaining.

Two valence electrons represent one lone pair. So thirty-two valence electrons = sixteen lone pairs.

Note that iodine 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.

Also, make sure that you start marking these lone pairs on outside atoms first. And then, on the central atom.

The outside atoms are fluorines, so each fluorine will get three lone pairs. And the central atom (iodine) will get one lone pair.

So the Lewis structure of IF₅ looks something like this:

In the above structure, you can see that the octet is completed on the central atom (iodine), and also on the outside atoms. Therefore, the octet rule is satisfied.

After completing the octet, one last thing we need to do is, calculate the formal charge and check the stability of the above structure.

Also read: How to draw Lewis structure of PF₅ (4 steps)

#4 Calculate formal charge and check stability

The following formula is used to calculate the formal charges on atoms:

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

Collect the data from the above structure and then, write it down below as follows:

• For iodine atom

Valence electrons = 7
Nonbonding electrons = 2
Bonding electrons = 10

Formal charge = 7 – 2 – ½ (10) = 0

• For each fluorine atom

Valence electrons = 7
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 7 – 6 – ½ (2) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of IF₅ looks something like this:

In the above structure, you can see that the formal charges of both (iodine and fluorine) are zero. Therefore, this is the stable Lewis structure of IF₅.

And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.

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Related

• Lewis structure of SCl₂
• Lewis structure of ClF₃
• Lewis structure of PF₅
• Lewis structure of BeF₂
• Lewis structure of SCN^–

External video

• IF5 Lewis Structure: How to Draw the Lewis Structure for IF5 – YouTube • Wayne Breslyn

External links

• Lewis Structure for IF5 – The University of Maryland
• IF5 Lewis Structure (Iodine Pentafluoride) – Pinterest
• IF5 Lewis structure, molecular geometry, bond angle, hybridization – Topblogtenz
• IF5 Lewis Structure, Hybridization, Polarity, and Molecular Shape – Techiescientist
• Draw the Lewis structure for IF5 – Homework.Study.com
• IF5 Lewis Structure in 5 Steps (With Images) – Pediabay
• How to Draw the Lewis Dot Structure for IF5 – The Geoexchange
• Lewis Dot of Iodine Pentafluoride IF5 – Kent’s Chemistry
• Iodine Pentafluoride, IF5 Molecular Geometry & Polarity – Tutor-Homework.com
• How to draw IF5 Lewis Structure? – Science Education and Tutorials
• What is the molecular geometry of IF5? – Quora
• Molecular structure of IF5 – Physics Forums
• Write the correct Lewis structure for iodine pentafluoride, IF5 – Course Hero
• What is the correct Lewis structure for IF5? – Brainly
• Draw the Lewis structure with lowest formal charges, and determine the charge of each atom in IF5 – Quizlet