In the Lewis structure for ICl2-, how many lone pairs of electrons are around the central iodine atom

In the Lewis structure for ICl2-, how many lone pairs of electrons are around the central iodine atom? Group of answer choices 4 1 0 2 3

The Correct Answer and Explanation is:

To determine the number of lone pairs of electrons around the central iodine atom in the Lewis structure for ICl₂⁻, follow these steps:

1. Determine the total number of valence electrons:
   • Iodine (I) is in Group 17 of the periodic table, so it has 7 valence electrons.
   • Each chlorine (Cl) atom is also in Group 17, so each chlorine contributes 7 valence electrons.
   • The ion has a negative charge (ICl₂⁻), which means it has gained one electron, adding 1 more valence electron.
   • Therefore, the total number of valence electrons is: (7 from iodine)+2×(7 from chlorine)+1 (from the negative charge)=22 electrons.(7 \, \text{from iodine}) + 2 \times (7 \, \text{from chlorine}) + 1 \, (\text{from the negative charge}) = 22 \, \text{electrons}.(7from iodine)+2×(7from chlorine)+1(from the negative charge)=22electrons.
2. Distribute the electrons in the structure:
   • Place iodine in the center since it is the least electronegative atom. Each chlorine atom will form a single bond with iodine.
   • Two single bonds between iodine and the two chlorine atoms use 4 electrons (2 electrons per bond).
   • The remaining 18 electrons (22 total electrons – 4 electrons used in bonds) will be placed as lone pairs.
3. Complete the octet for each atom:
   • Each chlorine atom needs 6 more electrons to complete its octet. So, place 3 lone pairs (6 electrons) around each chlorine atom.
   • After placing these electrons, 12 electrons are used for the chlorines.
4. Place the remaining electrons around iodine:
   • Iodine now has 4 electrons involved in bonds, and it has 18 electrons remaining. Distribute these 18 electrons around the iodine atom.
   • Iodine can hold more than 8 electrons in its valence shell because it is in period 5, and therefore can have an expanded octet. Place 3 lone pairs of electrons around iodine.

Thus, there are 3 lone pairs of electrons around the central iodine atom in ICl₂⁻.

Correct answer: 3