Give the formula and describe the strncture of a noble gas species which is isostructural with: `BrO_(3)^(-)`

Explanation

In `BrO_(3)^(-)`, O is more electronegative than Br. Therefore a negative charge stays on the O-atom. In `BrO_(3)^(-)`, there are two Br=O bond. According to VSEPR theory, double bonds do not contribute any electron, while single bonds contribute one electron towards the total number of electrons in the valence shell of the central atom. However, the double and single bonds, both contribute to one bond pair.
Thus total no. of electrons in the valence shell of central Br-atom `=7+2xx0+1xx1= 8`
`therefore` No. of electron-pairs around Br `=8/2=4`
Total number of bond pairs
`= 2xx1(Br=0)+1xx1 (Br--O^(-)) = 3` and total number of lone pairs = 4 - 3 = 1
Thus, `BrO_(3)^(-)` has 3 bond pairs and one lone pair. According to VSEPR theory. `BrO_(3)^(-)` should have a pyramidal geometry.
`XeO_(3)` is a noble gas compound having `8(8xx1+3xx0=8)` electrons in the valence shell of the central atom. It has 3 bond pairs and one lone pair like `BrO_(3)^(-)` Therefore `XeO_(3)` has a pyramidal geometry.