Lewis structure of GeCl4

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The Lewis structure of GeCl₄ contains four single bonds, with germanium in the center, and four chlorines on either side. There are three lone pairs on each chlorine atom, and the germanium atom does not have any lone pair.

Steps

By using the following steps, you can easily draw the Lewis structure of GeCl₄.

#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… germanium is a group 14 element and chlorine is a group 17 element. Hence, germanium has four valence electrons and chlorine has seven valence electrons.

Now GeCl₄ has one germanium atom and four chlorine atoms.

So the total number of valence electrons = valence electrons of germanium atom + (valence electrons of chlorine atom × 4)

Therefore, the total number of valence electrons = 4 + 28 = 32

• 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 germanium and chlorine as follows:

Electronegativity value of germanium = 2.01
Electronegativity value of chlorine = 3.16

Obviously, germanium is less electronegative than chlorine. Hence, assume that germanium is the central atom.

So now, put germanium in the center and chlorines on either side. And draw the rough skeleton structure for the Lewis structure of GeCl₄ something like this:

Also read: How to draw Lewis structure of C₂H₂F₂ (5 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since germanium is surrounded by four chlorines, use eight electrons to show four chemical bonds as follows:

Also read: How to draw Lewis structure of CH₂CHCN (5 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 32 valence electrons. And in the above structure, we have already used eight valence electrons. Hence, twenty-four  valence electrons are remaining.

Two valence electrons represent one lone pair. So twenty-four valence electrons = twelve lone pairs.

Note that germanium is a period 4 element, so it can keep more than 8 electrons in its last shell. And chlorine is a period 3 element, so it can 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 chlorines, so each chlorine will get three lone pairs. And the central atom (germanium) will not get any lone pair, because all twelve lone pairs are used.

So the Lewis structure of GeCl₄ looks something like this:

In the above structure, you can see that the octet is completed on the central atom (germanium), 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 TeBr₄ (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 germanium atom

Valence electrons = 4
Nonbonding electrons = 0
Bonding electrons = 8

Formal charge = 4 – 0 – ½ (8) = 0

• For each chlorine 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 GeCl₄ looks something like this:

In the above structure, you can see that the formal charges of both (germanium and chlorine) are zero. Therefore, this is the stable Lewis structure of GeCl₄.

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

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Related

• Lewis structure of C₂H₂F₂
• Lewis structure of CH₂CHCN
• Lewis structure of TeBr₄
• Lewis structure of GeH₄
• Lewis structure of HOF

External video

• How to Draw the Lewis Dot Structure for GeCl4: Germanium tetrachloride – YouTube • Wayne Breslyn

External links

• GeCl4 Lewis Structure in 6 Steps (With Images) – Pediabay
• draw the lewis structures of GeCl4, SeCl4, ICl4-, and ICl4+ – Chegg
• Germanium tetrachloride | GeCl4 | CID 66226 – National Institutes of Health (.gov)
• How many unbonded pairs of electrons do GeCl4 and AsH3 have? – Homework.Study.com
• What is the Lewis structure of germanium chloride? – Answers
• GeCl4 (Germanium Tetrachloride) Oxidation Number – ChemicalAid
• Germanium tetrachloride – Wikipedia
• What is the molecular geometry of GeCl4? – Bartleby