Question

Give the number of lone pairs around the central atom and the geometry of the ion IBr2.
A. 3 lone pairs, linear
B. 2 lone pairs, bent
C. 0 lone pairs, linear
D. 1 lone pair, bent
E. 3 lone pairs, bent

Answer 1

Answer:

Option E!

Explanation:

If we were to draw the lewis dot structure for IBr2 -, we would first count the total number of valence electrons ( " available electrons " ). Iodine has 7 valence electrons, and so does Bromine, but as Bromine exists in 2, the total number of valence electrons would be demonstrated below;

$7 + 7 * ( 2 ) =\\7 + 14 + 1 =\\22 Electrons$

Don't forget the negative on the Bromine!

Now go through the procedure below;

1 ) Place Iodine in the middle and draw single bonds to each of the bromine.

2 ) Add three lone pairs on each of the Bromine's

3 ) Now we have 6 electrons left, if we were to exclude the electrons shared in the " single bonds. " This can be placed as three lone pairs on Iodine ( central atom )!

The molecular geometry can't be linear, as there are lone pairs on the atoms. This makes it bent.