Question

Complete the sentences to explain why CO₂ and CCl₄ are both nonpolar even though they contain polar bonds.

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 ______

a. zero
b. one
c. two
d. three
e. four
f. linear
g. trigonal planar
h tetrahedral
i. trigonal pyramidal
j. bonds are only slightly polar
k. sum of the bond dipoles is zero
l. molecules are relatively small

Answer 1

CO₂ and CCl₄ are nonpolar because their molecular geometries cause the bond dipoles to cancel out, resulting in no net dipole moment.

Step-by-step explanation:

CO₂ and CCl₄ are both nonpolar molecules despite containing polar bonds because the sum of the bond dipoles is zero. In CO₂, the molecule is linear with two polar C=O bonds that are of equal strength and point in opposite directions, cancelling each other out. The molecule's nonpolarity arises from its symmetrical geometric shape, which, according to VSEPR theory, allows for the dipoles to negate one another. For CCl₄, the molecule has a tetrahedral shape where the four C-Cl dipole moments cancel each other out, again resulting in no net dipole moment and a nonpolar molecule.

The size of the molecules does not influence their polarity; rather, it is the arrangement of bonds and the resulting geometry that are crucial factors. While individual bonds may be polar due to differences in electronegativity between the bonded atoms, the molecular geometry plays a pivotal role in determining the overall polarity of the molecule.