what is the lewis structure for BrF2+ and the number of valence
The correct answer and explanation is:
Lewis Structure of BrF₂⁺ and Valence Electrons Calculation
Valence Electrons Calculation:
- Bromine (Br) Contribution: Bromine belongs to Group 17 and has 7 valence electrons.
- Fluorine (F) Contribution: Each fluorine atom also belongs to Group 17 and has 7 valence electrons. Since there are two fluorine atoms, the total contribution from fluorine is 2 × 7 = 14 valence electrons.
- Cation (+1) Effect: Since BrF₂⁺ has a +1 charge, it means one electron is lost from the total count.
Total valence electrons calculation: 7(Br)+(2×7)(F)−1(for +1 charge)=7+14−1=20 valence electrons.7 (Br) + (2 \times 7) (F) – 1 (\text{for +1 charge}) = 7 + 14 – 1 = 20 \text{ valence electrons}.
Lewis Structure Construction:
- Central Atom Selection: Bromine is less electronegative than fluorine, so it is the central atom.
- Bonding: Two fluorine atoms are bonded to bromine via single bonds. This uses up 2 × 2 = 4 electrons.
- Remaining Electrons: After bonding, 16 electrons remain.
- Lone Pairs Assignment:
- Fluorine atoms need 3 lone pairs each (total 2 × 6 = 12 electrons).
- The remaining 4 electrons are placed as two lone pairs on bromine.
Molecular Geometry & Formal Charge:
- Formal Charge Calculation:
- Br: 7−(4+2)=+17 – (4 + 2) = +1
- F: 7−(6+1)=07 – (6 + 1) = 0
- Structure Shape: Bent (T-Shaped) due to lone pairs and the AX₂E₃ arrangement (based on VSEPR theory).
Now, generating the image for the Lewis structure of BrF₂⁺:
Here is the Lewis structure of BrF₂⁺. The diagram shows bromine in the center with two fluorine atoms bonded via single bonds, two lone pairs on bromine, and a +1 charge indicated. The molecular geometry follows a T-shape due to the electron repulsions. Let me know if you need further explanations!
