Chemical Bonding Worksheet With Answers Page 4
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617.
Make a chart showing periodic trends for ionization energy, electron
affinity, electro-negativity, and atomic size, include their relationship to metals
and nonmetals.
Check notes and handouts for Periodic Trend Table.
18.
Fluorine has the highest electro-negativity, what does that tell you about the
element fluorine?
It strongly attracts an electron.
19.
How does a metal ion size compare to its original atom? How does a
nonmetallic ion compare to its original nonmetal?
Metals are smaller than the original atom. (They lose electrons.)
Non-metals are larger than the original atom. (They gain electrons.)
20.
Distinguish between a polar and non-polar bond, and a polar and non-polar
molecule. Use examples in your discussion.
Polarity is measured on a scale of electro-negativity (the electron
disparity between two elements that are combined in a compound). The
more electrons you take from your partner element in the bonding process,
the greater your negative charge, and the greater your electro-negativity.
There are three terms to describe the polarity of a given molecular bond:
Ionic, Polar covalent, and Non-polar covalent.
Ionic is the most polar - essentially, one atom physically takes electrons
from another atom, creating a huge electron disparity between the two
atoms. This tends to happen in molecules where one atom has very few
valence electrons and the other has a lot of valence electrons. Sodium
chloride (NaCl) is a good example of an ionic bond.
Polar covalent is the mid-range - technically closer to ionic. This happens
when one atom attempts to take electrons from its partner, but cannot quite
attract them all to itself. The result is a covalent bond between the two
atoms where the valence electrons are "shared," but the sharing is unequal.
One atom pulls the "shared" electrons a little closer to itself. Polar
covalent bonds usually occur between very electronegative elements;
hydrogen paired with elements like oxygen and fluorine almost always
creates polar covalent bonds. A good example of a polar covalent bond is
found in water (H
O).
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Non-polar covalent is the least polar - in fact, it is not polar at all. This
occurs when valence electrons are shared equally between two atoms.
There is little or no tendency for either atom to pull any of the electrons
toward itself. Non-polar covalent bonds can often be seen in molecules
with two non-metals. Methane (CH
) is an example of a non-polar
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covalent bond
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