Textbook Question
a. Draw a Lewis structure for each of the following:
b. Draw a structure for each of the species that shows approximate bond angles.
c. Which species have no dipole moment?
2. HNO3
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1. A Review of General Chemistry
Electronegativity
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Which molecule/s contain/snet dipoles?
A
a
B
b
C
both a and b
D
none of them
Verified step by step guidance1
Identify the molecular structure of each compound. Molecule a is a linear hydrocarbon chain, and molecule b is water (H2O).
Understand the concept of dipole moments. A dipole moment occurs when there is a separation of charge due to differences in electronegativity between atoms in a molecule.
Analyze molecule a. Hydrocarbons like alkanes are generally nonpolar because the C-H bonds have very similar electronegativities, resulting in no significant dipole moment.
Analyze molecule b. Water (H2O) has a bent shape due to the two lone pairs on the oxygen, and the O-H bonds are polar because oxygen is more electronegative than hydrogen. This results in a net dipole moment.
Conclude which molecules have net dipoles. Molecule a does not have a net dipole moment, while molecule b does due to its polar bonds and molecular geometry.
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