Draw the lewis structure (electron- dot diagram ) of each of the four species

GeCl4, SeCl4, ICI4-, ICI4+, Draw the lewis structure (electron- dot diagram ) of each of the four species. Show all valence electron in your structure.

The correct answer and explanation is :

Here’s the correct Lewis structure for each species and a 300-word explanation.

1. Lewis Structures:

1. Germanium Tetrachloride (GeCl₄)

Valence Electrons: Ge (4) + Cl (4×7) = 32
Structure:
Ge is the central atom.
Forms four single bonds with Cl.
Each Cl has three lone pairs.
Ge has no lone pairs.
Shape: Tetrahedral
Total valence electrons shown: 32

        Cl
        |
    Cl—Ge—Cl
        |
        Cl

2. Selenium Tetrachloride (SeCl₄)

Valence Electrons: Se (6) + Cl (4×7) = 34
Structure:
Se is the central atom.
Forms four single bonds with Cl.
Se has one lone pair.
Each Cl has three lone pairs.
Shape: See-saw
Total valence electrons shown: 34

         Cl
         |
  Cl—Se—Cl
         |
         Cl
        (lone pair on Se)

3. Tetrachloroiodate Ion (ICl₄⁻)

Valence Electrons: I (7) + Cl (4×7) + 1 (extra e⁻) = 36
Structure:
I is the central atom.
Forms four single bonds with Cl.
I has two lone pairs.
Each Cl has three lone pairs.
Shape: Square planar
Total valence electrons shown: 36

   Cl     Cl
    \   /
     I
    /   \
   Cl     Cl
  (2 lone pairs on I)

4. Tetrachloroiodate Ion (ICl₄⁺)

Valence Electrons: I (7) + Cl (4×7) – 1 (lost e⁻) = 34
Structure:
I is the central atom.
Forms four single bonds with Cl.
I has one lone pair.
Each Cl has three lone pairs.
Shape: See-saw
Total valence electrons shown: 34

         Cl
         |
   Cl—I—Cl
         |
         Cl
        (1 lone pair on I)

2. Explanation (300 Words):

The Lewis structures of these molecules and ions help predict their molecular shapes and reactivity based on the VSEPR (Valence Shell Electron Pair Repulsion) Theory.

GeCl₄ adopts a tetrahedral shape because the four Cl atoms are symmetrically arranged around Ge, which has no lone pairs. This results in sp³ hybridization with bond angles of 109.5°.
SeCl₄ has a see-saw shape due to the presence of one lone pair on selenium. Lone pairs repel bonding pairs more strongly, distorting the angles to around 102° and 87°.
ICl₄⁻ is a square planar species because the central iodine has two lone pairs. Lone pairs prefer opposite positions to minimize repulsion, leading to an sp³d² hybridization and bond angles of 90°.
ICl₄⁺ also adopts a see-saw geometry, similar to SeCl₄, due to the presence of one lone pair on iodine. It experiences distortions in bond angles due to lone-pair repulsions.

These structures follow the octet rule except for iodine and selenium, which can expand their octets due to available d orbitals. The negative charge in ICl₄⁻ adds an extra electron, stabilizing the square planar geometry, while the positive charge in ICl₄⁺ results in one fewer electron, affecting electron distribution.

By analyzing the electron distribution and hybridization, we predict bond angles and shapes, which are essential for understanding their physical and chemical properties.