Solution Found!
For each of the following compounds: 1. Draw the Lewis structure. 2. Show how the bond
Chapter 2, Problem PROBLEM 2-3(choose chapter or problem)
For each of the following compounds: 1. Draw the Lewis structure. 2. Show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment. 3. Estimate whether the compound will have a large, small, or zero dipole moment. (a) NH4 + (b) O3 (a) NH4 + has four polar NH bonds. These bonds are probably more polarized than a typical NH bond, because the N in NH4 + bears a formal positive charge. Nevertheless, these four polar bonds have a symmetric tetrahedral arrangement so they cancel each other. dipoles cancel net dipole = 0 +N H H H H (b) Ozone (O3) is an sp2 hybrid structure, with a lone pair on the central oxygen atom. Therefore, O3 must be bent. The resonance structures imply partial negative charges on the outer oxygens and a partial positive charge on the central oxygen. The lone pair on the central oxygen cancels part, but not all, of the vector sum of the two OO dipoles. The resulting net dipole is relatively small.
Questions & Answers
QUESTION:
For each of the following compounds: 1. Draw the Lewis structure. 2. Show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment. 3. Estimate whether the compound will have a large, small, or zero dipole moment. (a) NH4 + (b) O3 (a) NH4 + has four polar NH bonds. These bonds are probably more polarized than a typical NH bond, because the N in NH4 + bears a formal positive charge. Nevertheless, these four polar bonds have a symmetric tetrahedral arrangement so they cancel each other. dipoles cancel net dipole = 0 +N H H H H (b) Ozone (O3) is an sp2 hybrid structure, with a lone pair on the central oxygen atom. Therefore, O3 must be bent. The resonance structures imply partial negative charges on the outer oxygens and a partial positive charge on the central oxygen. The lone pair on the central oxygen cancels part, but not all, of the vector sum of the two OO dipoles. The resulting net dipole is relatively small.
ANSWER:Problem 2-3
For each of the following compounds: 1. Draw the Lewis structure. 2. Show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment. 3. Estimate whether the compound will have a large, small, or zero dipole moment. (a) 
Step by Step Solution
Step 1 of 4
The structure that defines the arrangement of valence shell electrons existing in a particular molecule is named as “Lewis structure”. In this structure, the total valence electrons are identical to the total number of dots.