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 around the central atom (yellow sphere). There are 4 regions (two bonds and two lone pairs).

Step2: Determine molecular shape

For 4 regions of electron density (with two lone pairs), the molecular shape is bent with a bond angle of \(109.5^{\circ}\).

Step3: Check polarity

If all bonds are polar covalent, and the molecule has a bent shape (\(109.5^{\circ}\)), the bond dipoles do not cancel out, so the molecule is polar.

Answer:

1. E. 4
2. N. bent (\(109.5^{\circ}\))
3. U. yes