Bond Polarity
Jean Brainard, Ph.D.
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Printed: October 10, 2014
AUTHOR
Jean Brainard, Ph.D.
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C HAPTER
Chapter 1. Bond Polarity
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Bond Polarity
• Describe polar and nonpolar covalent bonds.
• Explain why some covalent compounds are polar.
Like the north and south poles of a bar magnet, Earth’s north and south magnetic poles—pictured above—are
opposites in terms of their magnetic fields. Some types of chemical bonds and chemical compounds have “poles”
similar to a bar magnet as well. But in the case of chemical bonds and compounds, the poles are opposites in terms
of their electric charge. These bonds and compounds are described as polar.
Polar and Nonpolar Covalent Bonds
Covalent bonds are chemical bonds between atoms of nonmetals that share valence electrons. In some covalent
bonds, electrons are not shared equally between the two atoms. These are called polar covalent bonds. The Figure
1.1 shows the polar bonds in a water molecule (H2 O). The oxygen atom attracts the shared electrons more strongly
than the hydrogen atoms do because the nucleus of the oxygen atom has more positively charged protons. As a
result, the oxygen atom becomes slightly negative in charge, and the hydrogen atoms become slightly positive in
charge. For another example of polar bonds, see the video at this URL: http://www.youtube.com/watch?v=1lnjg
81daBs
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FIGURE 1.1
In other covalent bonds, electrons are shared equally. These bonds are called nonpolar covalent bonds. Neither
atom attracts the shared electrons more strongly. As a result, the atoms remain neutral in charge. The oxygen (O2 )
molecule in the Figure 1.2 has two nonpolar bonds. The two oxygen nuclei have an equal force of attraction for
their four shared electrons.
FIGURE 1.2
Polar and Nonpolar Covalent Compounds
A covalent compound is a compound in which atoms are held together by covalent bonds. If the covalent bonds
are polar, then the covalent compound as a whole may be polar. A polar covalent compound is one in which there
is a slight difference in electric charge between opposite sides of the molecule. All polar compounds contain polar
bonds. But having polar bonds does not necessarily result in a polar compound. It depends on how the atoms are
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Chapter 1. Bond Polarity
arranged. This is illustrated in the Figure 1.3. In both molecules, the oxygen atoms attract electrons more strongly
than the carbon or hydrogen atoms do, so both molecules have polar bonds. However, only formaldehyde is a polar
compound. Carbon dioxide is nonpolar.
FIGURE 1.3
Q: Why is carbon dioxide nonpolar?
A: The symmetrical arrangement of atoms in carbon dioxide results in opposites sides of the molecule having the
same charge.
Summary
• In polar covalent bonds, electrons are not shared equally between the two atoms, so one atom is slightly
negative in charge and one is slightly positive in charge. In nonpolar covalent bonds, electrons are shared
equally so the atoms remain neutral in charge.
• Covalent compounds with polar bonds may be polar or nonpolar, depending on their arrangement of atoms.
Vocabulary
• polar: Having oppositely charged ends, as in polar covalent bond or polar covalent compound.
• nonpolar: Not having oppositely charged ends, as in nonpolar covalent bond or nonpolar covalent compound.
Explore More
Watch the video about polarity of molecules at the following URL, and then answer the questions below.
http://www.youtube.com/watch?v=LKAjTE7B2x0
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1. When does a polar covalent bond always produce a polar covalent compound?
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2. If a covalent compound has polar bonds and more than two atoms, what determines whether the compound is
polar?
3. Is water a polar compound? Why or why not?
4. Which of the following compounds are polar?
a.
b.
c.
d.
BF3
NH3
CCl4
CHCl3
Review
1. What are polar covalent bonds? Give an example.
2. Why are the covalent bonds in an oxygen molecule (O2 ) nonpolar?
3. Carbon (C) atoms attract electrons a little more strongly than hydrogen (H) atoms do. The illustration below
shows three covalent compounds containing only carbon and hydrogen atoms. Are the compounds polar or
nonpolar? Explain.
References
1. Christopher Auyeung. Polar bonds in a water molecule. CC BY-NC 3.0
2. Christopher Auyeung. Nonpolar bonds in carbon dioxide. CC BY-NC 3.0
3. Christopher Auyeung. Polarity of formaldehyde and carbon dioxide. CC BY-NC 3.0
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