XeF2 (Xenon Difluoride) Lewis structure (2024)

The XeF2 (xenon difluoride) is an uncommon compound because noble gases usually don’t react much due to their stability. This article explains the XeF2 Lewis structure and its characteristics.

XeF2 itself is a powerful substance that can both fluorinate and oxidize. Xenon, unlike other noble gases, can react and create different compounds like Xenon tetrafluoride (XeF4) and Xenon hexafluoride (XeF6). However, the XeF2 Lewis structure is the most stable among them.

Step-by-Step Guide to Drawing the Lewis Structure of XeF2

1. Determine the total number of valence electrons

• Xenon (Xe) is in Group 18 of the periodic table and has 8 valence electrons.
• Fluorine (F) is in Group 17 and has 7 valence electrons each.

Since we have two fluorine atoms, the total number of valence electrons is 8 (Xe) + 2(7) (F) = 22.

2. Identify the central atom

In XeF2, xenon (Xe) is the central atom since it is less electronegative than fluorine.

3. Place the central atom and connect it to the surrounding atoms

• Place xenon (Xe) in the center.
• Begin forming chemical bonds by placing pairs of electrons (dots or lines) between xenon and each fluorine atom.
• Use four valence electrons to create two chemical bonds: 2 between Xe and each F.

4. Distribute the remaining electrons around the atoms

• Start by placing the remaining electrons around the outer atoms (fluorine).
• Fluorine needs 8 electrons to achieve a stable octet (except for hydrogen, which needs 2 electrons). Since fluorine already has 1 bond (2 electrons), place 6 lone pairs (12 electrons) around each fluorine atom.
• Distribute the remaining electrons around the central atom (xenon). In this case, we have 22 – (4 + 12) = 6 remaining electrons.

5. Check if the central atom has an octet

Xenon (Xe) doesn’t play by the octet rule. Instead, it can hold more than 8 electrons.

Xenon sits in the fourth energy level and can use the 4d sublevel, which lets it hold more than 8 electrons. In XeF2, xenon is a bit different – it’s got 3 lone pairs and 2 pairs that bond to other atoms.

6. Verify formal charges

Calculate the formal charges for each atom in the molecule. Ensure that they are as close to zero as possible.

FC (Formal charge) = V (Number of valence electrons) – N (Number of nonbonding valence electrons) – B (total number of electrons shared in bonds)/2.

For Xenon atom: V = 8, B = 4, N = 6

FC = 8 – 6 – 4/2 = 0

For Xenon atom: V = 7, B = 2, N = 6

FC = 7 – 6 – 2/2 = 0

Each pair of bonding electrons (:) can be represented as a single bond (|). The final Lewis structure of XeF2 should look like this:

FAQs

1. What is the Lewis structure of XeF2?

The Lewis structure of XeF2 depicts the arrangement of atoms and valence electrons in a molecule of xenon difluoride. It shows xenon (Xe) as the central atom bonded to two fluorine (F) atoms.

2: How many valence electrons are in XeF2?

Xenon (Xe) has 8 valence electrons, and each fluorine (F) atom has 7 valence electrons. In XeF2, there are two fluorine atoms.
The total number of valence electrons in XeF2 is 8 (Xe) + 7 (F) * 2 (F) = 22 valence electrons.

3. Is the XeF2 molecule polar or nonpolar?

XeF2 is a nonpolar molecule. Its linear geometry and symmetric arrangement result in the cancellation of bond dipoles, giving it a net dipole moment of zero.

4. How is the Lewis structure of XeF2 determined?

The Lewis structure of XeF2 is determined through a step-by-step process involving the allocation of valence electrons, placement of atoms, formation of chemical bonds, and confirmation of octet completeness for each atom.

5. What is the molecular geometry of XeF2?

XeF2 has a linear molecular geometry, where the two fluorine atoms are positioned on opposite sides of the central xenon atom.

6. Are there any resonance structures in the Lewis structure of XeF2?

No, there are no resonance structures in the Lewis structure of XeF2. The arrangement of atoms and electrons is straightforward, with a single valid structure.

7. Is XeF2 a stable compound?

XeF2 is a stable compound under the appropriate conditions and is commonly used in laboratory and industrial settings.

8. Does xenon (Xe) in XeF2 follow the octet rule?

No, xenon (Xe) in XeF2 does not follow the octet rule. Xenon is in the noble gas group and, as such, can have an expanded valence shell. It can accommodate more than eight electrons in its valence shell due to its availability of d-orbitals. In XeF2, xenon forms a compound with two fluorine (F) atoms, and it has 10 valence electrons surrounding it, exceeding the typical octet (eight electrons) for main-group elements. This property of xenon to exceed the octet rule is known as an “expanded octet.”