# GeF4 Lewis structure

GeF4 (germanium tetrafluoride) has one germanium atom and four fluorine atoms.

In GeF4 Lewis structure, there are four single bonds around the germanium atom, with four fluorine atoms attached to it, and on each fluorine atom, there are three lone pairs.

Contents

## Steps

To properly draw the GeF4 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, germanium lies in group 14, and fluorine lies in group 17.

Hence, germanium has four valence electrons and fluorine has seven valence electrons.

Since GeF4 has one germanium atom and four fluorine atoms, so…

Valence electrons of one germanium atom = 4 × 1 = 4
Valence electrons of four fluorine atoms = 7 × 4 = 28

And the total valence electrons = 4 + 28 = 32

• Second, find the total electron pairs

We have a total of 32 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 = 32 ÷ 2 = 16

• Third, determine the central atom

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

Since germanium is less electronegative than fluorine, assume that the central atom is germanium.

Therefore, place germanium in the center and fluorines on either side.

• And finally, draw the rough sketch

### #2 Next, indicate lone pairs on the atoms

Here, we have a total of 16 electron pairs. And four Ge — F bonds are already marked. So we have to only mark the remaining twelve electron pairs as lone pairs on the sketch.

Also remember that germanium is a period 4 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 germanium, there is zero lone pair because all twelve electron pairs are over.

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 germanium atom, formal charge = 4 – 0 – ½ (8) = 0

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

Here, both germanium 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 (germanium) 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 GeF4.

Next: N2F4 Lewis structure