Question

given the lewis structure of co₂, the central carbon atom has lone pair(s) of electrons and total electron groups. thus the molecular geometry is . given the lewis structure of ccl₄, the central carbon atom has lone pair(s) of electrons and total electron groups. thus the molecular geometry is . the reason both molecules are nonpolar is best explained because the . zero one two three four linear trigonal planar tetrahedral trigonal pyramidal bonds are only slightly polar sum of the bond dipoles is zero molecules are relatively small

Explanation:

Step1: Analyze \( \ce{CO2} \) Lewis Structure

The Lewis structure of \( \ce{CO2} \) is \( \ce{O=C=O} \). The central \( \ce{C} \) atom has 0 lone pairs (all valence electrons are in double bonds). The total electron groups (bonding groups, since no lone pairs) are 2 (two double bonds). For 2 electron groups (and 0 lone pairs), molecular geometry is linear.

Step2: Analyze \( \ce{CCl4} \) Lewis Structure

The Lewis structure of \( \ce{CCl4} \) has the central \( \ce{C} \) bonded to 4 \( \ce{Cl} \) atoms (single bonds). So, 0 lone pairs on \( \ce{C} \), and 4 total electron groups (four single bonds). For 4 electron groups (0 lone pairs), molecular geometry is tetrahedral.

Step3: Explain Nonpolarity

A molecule is nonpolar if the sum of bond dipoles is zero (symmetric geometry cancels dipoles). In \( \ce{CO2} \) (linear, symmetric) and \( \ce{CCl4} \) (tetrahedral, symmetric), the bond dipoles cancel, so sum of bond dipoles is zero.

Answer:

• For \( \ce{CO2} \): lone pairs = zero, total electron groups = two, molecular geometry = linear.
• For \( \ce{CCl4} \): lone pairs = zero, total electron groups = four, molecular geometry = tetrahedral.
• Reason for nonpolarity: sum of the bond dipoles is zero.