Question

# Is $\ce{BrCl3}$ polar molecule?

Solution

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We need to determine whether the $\ce{BrCl3}$ molecule is polar or nonpolar, and to do so, first we need to draw it's Lewis structure, and determine it's electron and molecular geometry.

Both bromine and chlorine are in the group 7A, so they have 7 valence electron each. The total number of valence electrons is:

$\ce{Total valence e- = 7e- + 3 \times 7e- = 28e-}$

Since bromine is the least electronegative element, we will place it in centre, and place chlorine atoms around it.

We have 28 valence electrons, so we will place 2 electrons between atoms, to form chemical bonds, and place the rest of them to complete the octet:

After doing so, we are still left with $2$ valence electrons. Since bromine is below period $2$, it can have an expanded octet (more than $8$ valence electrons), so we will place the remaining to electrons on it.