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
the shape at the central atom is 2
f. diatomic g. linear h. trigonal planar i. bent (120°)
j. tetrahedral k. pyramidal l. bent (109.5°)
if all of the bonds are polar covalent, is the molecule itself polar? 3
m. yes n. no

Explanation:

Step1: Count REDs

Count the number of electron - density regions (bonds or lone pairs) around the central atom. In the model, there are 3 bonds (connected to red spheres), so there are 3 REDs.

Step2: Determine molecular shape

For 3 REDs with no lone pairs on the central atom (assuming the model represents a simple bonding situation without lone - pair representation in a basic sense for this problem), the molecular shape is trigonal planar.

Step3: Check polarity

In a trigonal planar molecule with all polar bonds, if the surrounding atoms are the same (as implied by the model with all red spheres likely representing the same atom), the bond dipoles cancel out. For example, in \(BF_3\) (a trigonal planar molecule with polar \(B - F\) bonds), the symmetry makes the molecule non - polar.

Answer:

1. D. 3
2. H. trigonal planar
3. N. no