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 around the central atom. From the model, there are 4 regions.

Step2: Determine molecular shape

For 4 electron - density regions (assuming no lone pairs), the shape is tetrahedral.

Step3: Check polarity

If all bonds are polar covalent, in a tetrahedral molecule (e.g., \(CH_4\) - but if we assume all bonds are polar like \(CCl_4\) has non - polar overall due to symmetry, but if we consider a general case where substituents are different and polar, but in a regular tetrahedral arrangement (if all bonds are same polar bonds), the dipoles cancel out. Wait, no - wait, in a tetrahedral molecule with 4 identical polar bonds, the molecule is non - polar. But if we assume the model is \(CH_4\) - like (even though \(CH - H\) is not very polar, but if we take the concept). Wait, no - actually, for a tetrahedral molecule with 4 regions (assuming no lone pairs), if all bonds are polar covalent and identical, the molecule is non - polar because of symmetry.

Answer:

1. E. 4
2. J. tetrahedral
3. N. no