Question

answer the questions about the following model
there are 1 reds (regions of electron density) around the central atom
a. 0 b. 1 c. 2. d. 3 e. 4 f. 5 g. 6
the shape at the central atom is 2
h. diatomic i. linear j. trigonal planar k. bent (120°) l. tetrahedral
m. pyramidal n. bent (109.5°) o. see - saw p. hexahedral q. t - shape
r. octahedral s. square pyramidal t. square planar
if all of the bonds are polar covalent, is the molecule itself polar? 3
u. yes v. no

Explanation:

Step1: Count REDs

Count the number of electron - density regions (bonds and lone pairs) around the central atom. In the model, there are 4 regions.

Step2: Determine molecular shape

For 4 regions of electron density, if there are no lone pairs, the shape is tetrahedral (L).

Step3: Check polarity

In a tetrahedral molecule with all polar bonds, if the surrounding atoms are the same (symmetrical), the dipoles cancel out. But if there are different surrounding atoms (as in a general case where we assume no perfect symmetry due to lack of info about identical substituents), the molecule is polar.

Answer:

1. E. 4
2. L. tetrahedral
3. U. yes