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 REDs.

Step2: Determine molecular shape

For 4 REDs with no lone pairs, the molecular shape is tetrahedral.

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 we assume a general case (since no info on surrounding atoms' identity, but based on common tetrahedral polar - non - polar rules: if all bonds are polar and no lone pairs, a regular tetrahedral (e.g., \(CH_4\) is non - polar if we consider \(C - H\) as slightly polar in a sense, but if we assume all bonds are polar and same surrounding atoms), the molecule is non - polar.

Answer:

1. E. 4
2. L. tetrahedral
3. V. no