draw the lewis structure of brf₂⁺. be sure to include all lone pair electrons and nonzero formal charges.

Explanation:

Step1: Count valence electrons

Bromine (Br) has 7 valence electrons, each fluorine (F) has 7 valence electrons, and the ion has a +1 charge. So, $7 + 2\times7- 1=20$ valence electrons.

Step2: Determine central atom

Br is the central atom as it is less electronegative than F.

Step3: Connect atoms with single - bonds

Connect Br to each F with a single - bond. Each single - bond uses 2 electrons, so 4 electrons are used, and 16 electrons remain.

Step4: Add lone - pairs

Add lone - pairs to the outer atoms (F) first to satisfy the octet rule. Each F gets 3 lone - pairs. After adding lone - pairs to F, 4 electrons remain. Add these 4 electrons as 2 lone - pairs on Br.

Step5: Calculate formal charges

The formal charge on an atom is given by $FC = V - N - \frac{B}{2}$, where $V$ is the number of valence electrons, $N$ is the number of non - bonding electrons, and $B$ is the number of bonding electrons. For Br: $V = 7$, $N = 4$, $B = 4$, so $FC=7 - 4-\frac{4}{2}= + 1$. For each F: $V = 7$, $N = 6$, $B = 2$, so $FC = 7-6 - \frac{2}{2}=0$.

The Lewis structure has Br as the central atom with two single - bonds to F atoms, two lone - pairs on Br, and three lone - pairs on each F atom. There is a +1 formal charge on Br.

Answer:

Br is the central atom with two single - bonds to F atoms, two lone - pairs on Br, three lone - pairs on each F atom, and a +1 formal charge on Br.