Ch 9: Chemical Bonding II: Molecular Geometry and Bonding Theories

Question 1

Molecular polarity is a consequence of molecular ________.

Answer 1

geometry

p. 380

Question 2

An electron domain (or group) is…

Answer 2

…a lone pair or a bond, regardless of whether the bond is single, double, or triple.

Question 3

AXE nomenclature is used to assign geometries around the central atom. A, X, and E represent…

Answer 3

A = the central atom
X = # of bonding groups or domains attached to the central atom
E = lone pairs of e's on the central atom

Question 4

Since carbon and iodine are both 3 boxes away from F on the periodic table, it is difficult to tell which is more electronegative. Which one is less electronegative, and therefore should be the preferred central atom in a Lewis structure involving these atoms?

Answer 4

carbon

Question 5

The bond angle in NH3 is significantly smaller than the ideal bond angle of 109.5° because of the lone pair on the central atom. Which best explains why the bond angle in SO2 is very close to 120° despite there being a lone pair on the central atom?

A.) The double bonds in SO2 are not pushed apart by a lone pair as easily as the single bonds in NH3.
B.) The lone pair on the central atom in SO2 resides in an s orbital whereas the lone pair on the central atom in NH3 resides in a d orbital.
C.) The lone pair on the central atom in SO2 resides in a d orbital whereas the lone pair on the central atom in NH3 resides in an s orbital.
D.) The bonds in NH3 are stronger than the bonds in SO2.
E.) The bonds in NH3 are weaker than the bonds in SO2.

Answer 5

A.) The double bonds in SO2 are not pushed apart by a lone pair as easily as the single bonds in NH3.