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.

Alternative method: Lewis structure of GeF₄

Rough sketch

• 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

Learn how to find: Germanium valence electrons and Fluorine valence electrons

• 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

Lone pair

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:

Formal charge

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.

Final structure

The final structure of GeF₄ comprises a central germanium atom connected to four fluorine atoms through single covalent bonds. In this configuration, the germanium atom satisfies the octet rule by forming four bonding pairs. Each fluorine atom also fulfills its octet by maintaining three lone pairs of its own alongside the single shared bond. This setup is the most stable because it results in formal charges of zero for all atoms involved, representing the most energetically favorable state for the molecule. Thus, this specific electronic distribution serves as the definitive and most accurate Lewis representation of germanium tetrafluoride.

Next: N₂F₄ Lewis structure

External links

• https://socratic.org/questions/what-is-the-lewis-structure-for-gef-4
• https://www.chegg.com/homework-help/draw-lewis-structures-cf4-gef4-gef62-predict-molecular-stru-chapter-19-problem-39e-solution-9780547054056-exc
• https://www.bartleby.com/questions-and-answers/draw-the-lewis-structure-for-gef4-and-h2se.-predict-which-molecule-is-polar./02db020c-6d0d-4654-92f0-327868d3adc0