Draw the Lewis structure for IO2 and give the number of electrons in each species.

To draw the Lewis structure for IO₂, we first need to determine the total number of valence electrons available for bonding.

Iodine (I) is in group 17 of the periodic table, so it has 7 valence electrons. Each oxygen (O) is in group 16 and has 6 valence electrons. Therefore, for IO₂:

• 1 Iodine = 7 electrons
• 2 Oxygen = 2 × 6 = 12 electrons
• Total = 7 + 12 = 19 valence electrons

Next, we place the iodine atom in the center since it is less electronegative than oxygen. We connect the iodine to each oxygen atom with a single bond. Each single bond uses 2 electrons, so:

• 2 bonds × 2 electrons = 4 electrons
• Remaining electrons = 19 – 4 = 15 electrons

Now we distribute the remaining electrons to satisfy the octet rule for the oxygen atoms first. Each oxygen requires 8 electrons for a full valence shell, which they can achieve by forming double bonds with iodine after placing lone pairs:

• For the first oxygen, we create a double bond, which accounts for 4 electrons (2 from iodine and 2 from oxygen), and we place 4 remaining electrons as two lone pairs on the oxygen.
• For the second oxygen, we do the same and create another double bond with iodine, using another 4 electrons, and placing the other 4 remaining electrons as two lone pairs on this second oxygen as well.

This results in the Lewis structure of IO₂ being:

I:O::O

Where I is iodine double-bonded to two oxygen atoms, and each oxygen has two lone pairs of electrons.

Now, let’s count the total number of electrons in each species:

• Iodine (I) has 7 valence electrons and will share 4 for double bonds, so retains 3 lone electrons under the octet rule.
• Each oxygen in IO₂ has 6 valence electrons, forms 4 with iodine, and holds 4 as lone pairs, satisfying the octet rule.

Each species then is:

• Iodine (I): 7 – 4 (bonded) = 3 lone electrons
• Oxygen (O) in IO₂: 6 – 4 (4 shared) = 2 lone pairs (4 electrons each)

In summary:

• Total valence electrons in IO₂: 19
• Iodine: 7 valence, 3 lone electrons (not involved in bonding)
• Oxygen 1 and Oxygen 2: both have 6 valence, 2 lone pairs each

This is a complete representation of the Lewis structure for IO₂ along with the number of electrons in each species.