00 QUESTION 3 Many bonds are polar bonds due to the difference in electronegativities between the atoms involved in the bond. We saw earlier that bonds can be polar and therefore have a 5+ end and a 5- end. This creates an individual bond dipole. WHen dipoles are equal in magnitude but opposite in direction (like CO₂ below), the individual bond dipoles will cancel and the molecule is said to have no net dipole moment and is "a non-polar molecule". Water (also below), however, has bond dipoles that due to their orientation in space do not cancel and therefore lead to a molecular dipole (shown in green) and are "polar molecules". Which of the following moecules below will ALSO have a molecular dipole and are "polar molecules"? linear RECO A. BF3 B. CB4 C.CF2H2 D. NH3 E. H₂CO OF. IC1₂¹ -1 dipoles, cancel bent HD imolecule dipole

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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OD
QUESTION 3
Many bonds are polar bonds due to the difference in electronegativities between the atoms involved in the bond. We saw earlier that bonds
can be polar and therefore have a 5+ end and a 5- end. This creates an individual bond dipole. WHen dipoles are equal in magnitude but
opposite in direction (like CO₂ below), the individual bond dipoles will cancel and the molecule is said to have no net dipole moment and is
"a non-polar molecule". Water (also below), however, has bond dipoles that due to their orientation in space do not cancel and therefore
lead to a molecular dipole (shown in green) and are "polar molecules". Which of the following moecules below will ALSO have a molecular
dipole and are "polar molecules"?
A. BF3
B. CB4
C.CF2H2
D. NH3
E. H₂CO
F. IC1₂¹¹
-1
linear
CO
dipoles,
cancel
bent
HD
molecule
dipole
Transcribed Image Text:OD QUESTION 3 Many bonds are polar bonds due to the difference in electronegativities between the atoms involved in the bond. We saw earlier that bonds can be polar and therefore have a 5+ end and a 5- end. This creates an individual bond dipole. WHen dipoles are equal in magnitude but opposite in direction (like CO₂ below), the individual bond dipoles will cancel and the molecule is said to have no net dipole moment and is "a non-polar molecule". Water (also below), however, has bond dipoles that due to their orientation in space do not cancel and therefore lead to a molecular dipole (shown in green) and are "polar molecules". Which of the following moecules below will ALSO have a molecular dipole and are "polar molecules"? A. BF3 B. CB4 C.CF2H2 D. NH3 E. H₂CO F. IC1₂¹¹ -1 linear CO dipoles, cancel bent HD molecule dipole
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