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 (REDs) around the central atom. From the model, there are 4 REDs.

Step2: Determine molecular shape

For 4 REDs with no lone pairs (assuming the model shows 4 bonding pairs), the shape is tetrahedral.

Step3: Check polarity

In a tetrahedral molecule with all polar bonds, if the surrounding atoms are the same (as implied by the model's symmetry in terms of bonding pairs), the dipoles cancel out. But wait, no - in a tetrahedral molecule with all polar bonds (assuming the model is like \(CH_4\) - like with 4 identical bonds, but actually, if all bonds are polar covalent and the molecule is symmetric (tetrahedral with all 4 groups same), the molecule is non - polar. But wait, no - if the molecule has 4 identical polar bonds (e.g., \(CCl_4\)), the vector sum of bond dipoles is zero.

Answer:

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