Based on the properties of the compounds in the interactive, predict whether the given compounds behave as electrolytes or as no
1 answer:
You might be interested in
Answer:
C) SO₂
Explanation:
The figure below shows — clockwise from the upper left — BH₃, CCl₄, SO₂. CO₂, and PCl₅.
You must draw the Lewis structures of the molecules and then use VSEPR theory to figure out their molecular shape.
A) BH₃
BH₃ has a trigonal planar geometry.
It is nonpolar because of symmetry.
The bond dipole of the vertical B-H bond balances the equal and opposite resultant of the two downward-pointing B-H bonds.
BH₃ is nonpolar.
B) CCl₄
CCl₄ has a tetrahedral geometry.
The resultant of the two C-Cl bond dipoles on the right balances the equal and opposite resultant of the two C-Cl bond dipoles on the right.
CCl₄ is nonpolar.
C) SO₂
The Lewis structure shows that the central S atom has two S=O double bonds and a lone pair.
The electron pair geometry is trigonal planar and the molecular geometry is bent.
There is a net resultant of the S=O bond dipoles.
SO₂ is polar.
D) CO₂
CO₂ has a linear geometry with two C=O bonds pointing in opposite directions.
The bond dipoles cancel, so
CO₂ is nonpolar.
E) PCl₅
PCl₅ has a trigonal bipyramidal geometry.
The axial P-Cl bond dipoles cancel, as do the equatorial trigonal planar ones.
PCl₅ is nonpolar.
