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. Each bond (single, double, or triple) or lone pair is a region. In the model, there are 4 regions of electron density around the central atom.

Step2: Determine molecular shape

For 4 regions of electron density and 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 (assuming symmetry as in a regular tetrahedral with all 4 bonds identical in a simple case like \(CH_4\) - like structure conceptually here), the dipoles cancel out. But wait, no - if all bonds are polar and it's a tetrahedral (e.g., if it was \(CH_3Cl\) - like but no, wait, if it's a symmetric tetrahedral in terms of bond vectors - actually, in a perfect tetrahedral with all 4 same polar bonds (e.g., \(CCl_4\) - like, but \(CCl_4\) has polar \(C - Cl\) bonds but is non - polar as dipoles cancel. Wait, no - the question says "if all of the bonds are polar covalent". If it's a regular tetrahedral (4 equivalent bonds), the vector sum of the bond dipoles is zero.

Answer:

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