Question

the lewis structure for the iodate ion, io3-, which is favored by the octet rule, should show ___ single bond(s), __ double bond(s), and ____ lone pair(s). 3, 0, 10 1, 3, 12 2, 1, 8 3, 0, 7 3, 2, 9

Explanation:

Step1: Determine valence electrons

Iodine (I) has 7 valence electrons, oxygen (O) has 6 valence electrons and there is a - 1 charge. So total valence electrons = 7+3×6 + 1=26.

Step2: Draw basic structure

Connect I to 3 O atoms with single - bonds first. This uses 6 electrons (3 single - bonds, 2 electrons per bond).

Step3: Distribute remaining electrons

We have 26 - 6=20 electrons left. Place 6 electrons as 3 lone - pairs on each of the 3 O atoms. This uses 18 electrons. The remaining 2 electrons are placed on the I atom as a lone - pair.

Step4: Check octet rule

In this structure, all atoms follow the octet rule. There are 3 single - bonds, 0 double - bonds. The total number of lone - pairs: 3 on each of 3 O atoms (9) and 1 on I atom, so 10 lone - pairs in total.

Answer:

3, 0, 10