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?
3. N3−
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1. A Review of General Chemistry
Electronegativity
Multiple Choice
Which molecule/s contain/snet dipoles?
A
c
B
d
C
both c and d
D
none of them
Verified step by step guidance1
Identify the molecular geometry of each molecule. Molecule c is a planar alkene with two fluorine atoms attached to the double-bonded carbons. Molecule d is a tetrahedral carbon with two fluorine atoms and two chlorine atoms attached.
Consider the electronegativity of the atoms involved. Fluorine is more electronegative than carbon, and chlorine is also more electronegative than carbon but less than fluorine.
For molecule c, analyze the symmetry. The molecule is symmetrical with fluorine atoms on opposite sides of the double bond, which can lead to cancellation of dipole moments.
For molecule d, examine the arrangement of atoms. The tetrahedral geometry with different atoms (F and Cl) leads to an asymmetrical distribution of electron density, resulting in a net dipole moment.
Conclude that molecule c, due to its symmetry, may not have a net dipole moment, while molecule d, due to its asymmetrical tetrahedral shape, is likely to have a net dipole moment.
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