Question

Draw the Lewis structures for each of the following ions or molecules. For each, give (i) the molecular shape, (ii) the electron pair geometry at the central atom, and (iii) the hybridization of the central atom.

(a) CO2
(b) NO2Cl
(c) ICl4-
(d) ICl5
(e) CH3I

Answer 1

(a) CO2: Linear, linear, sp

(b) NO2Cl: Trigonal pyramidal, tetrahedral, sp3

(c) ICl4-: Square planar, octahedral, sp3d2

(d) ICl5: Square pyramid, octahedral, sp3d

(e) CH3I: Tetrahedral, tetrahedral, sp3

Step-by-step explanation:

To determine the Lewis structures, molecular shapes, electron pair geometries, and hybridizations for each molecule or ion, we follow established principles of molecular geometry and valence bond theory.

For example, in CO2, the Lewis structure reveals a linear arrangement, resulting in a linear molecular shape, with a linear electron pair geometry at the central carbon atom, and sp hybridization. Similarly, NO2Cl exhibits a trigonal pyramidal shape, tetrahedral electron pair geometry, and sp3 hybridization around the central nitrogen atom.

Moving on to ICl4-, its Lewis structure indicates a square planar shape, octahedral electron pair geometry, and sp3d2 hybridization at the central iodine atom. For ICl5, the Lewis structure predicts a square pyramid shape, octahedral electron pair geometry, and sp3d hybridization. Lastly, CH3I has a tetrahedral molecular shape, tetrahedral electron pair geometry, and sp3 hybridization around the central carbon atom.