Structure & Reactivity in Chemistry
Introduction to Molecules
IM11. Controversial Lewis structures
There is sometimes controversy in science. Argument
can be an important part of how we arrive at a better understanding of
things. In the context of molecules and structures, there have been
long-running controversies about how to draw certain phosphorus and sulfur
compounds. A look at that controversy can tell us some things about how
different chemists think about bonding. The controversy concerns how to draw, and think about,
the bonding in a number of "high-valent" sulfur and phosphorus compounds, in
which the sulfur or phosphorus atom is bonded to more than the usual number of
neighbours. Sulfate ion, SO42-, is an example
of a high-valent sulfur compound. Sulfur, like oxygen, frequently forms
two bonds. In sulfate, the sulfur is attached to four different atoms. We could draw that structure in two ways. A
structure that obeys the octet rule would have a single bond to each oxygen.
That would satisfy the octet of sulfur. In order to fill in the right
number of electrons for this group of atoms, each oxygen will have a negative
formal charge. Sulfur will have a charge of plus two.
Figure IM11.1. The structure of sulfate anion, SO42-,
closely following the octet rule.
A different way to draw the structure would include
double bonds between sulfur and two of the oxygen atoms. That structure
would have less charge separation than the other structure. However, the
sulfur would have twelve electrons in its valence shell, not eight. It
would exceed its octet.
Figure IM11.2. The structure of sulfate anion, SO42-,
minimizing charge separation. Can an atom have more than eight electrons in its valence
shell? Lots of them can, if they are further down the periodic table.
Whether sulfur and phosphorus can is much less clear. Frequently, the fact
that these are 3rd row atoms is considered significant. After all, the d
electrons begin in the third row. Perhaps sulfur and phosphorus can
accommodate extra electrons because they have d orbitals. The d orbitals
don't have any electrons in them, yet, so maybe they can accept some from other
aroms via bonds.
Figure IM11.3. The orbitals with principal quantum number, n = 3. Many theoretical chemists (including some experts in sulfur
and phosphorus chemistry) are convinced that this scenario just isn't
possible. The d level in these atoms is just too high in energy.
Other atoms can't possibly donate electrons to sulfur and phosphorus in this
way. And yet, many chemists (including some experts in sulfur and
phosphorus chemistry) still draw sulfate with double bonds. Why would they
make such a mistake? Partly, it has to do with experimental evidence.
Remember, "experimental" sounds wishy-washy and tentative to non-scientists, but
to a chemist the term really means "reality-based". One of the reasons
people draw double bonds in many sulfur and phosphorus compounds is that the
bonds simply behave like double bonds. That is, they are stronger and
shorter than single bonds. We might not think about those bonds in exactly the way
we think about double bonds in other situations, but the experimental evidence
says that there is some additional attraction between the sulfur and oxygen
atoms in these cases. There is additional evidence that sulfur and phosphorus
can "exceed the octet" or form "Lewis-disobedient" structures. Compounds
like phosphorus pentafluoride (PF5) clearly require more than four
bonds to phosphorus. Without five bonds, we would need to draw one of the
fluorides as an anion. It's certainly possible that this could be the true
structure, but there is evidence from X-ray crystallography that all of the
fluorines are attached to phosphorus in PF5, as well as in the
related PF6- anion (hexafluorophosphate, a very common
molecular ion in X-ray crystallographic studies). But those examples can also be drawn in other ways.
Are all five of the fluorines in PF5 really covalently bound, or are some of them ionic?
We could draw this structure in different ways, too.
Figure IM11.4. Two structures of phosphorus pentafluoride, PF5. Maybe we can think about sulfate in a similar way.
Are those S-O bonds stronger because of a covalent double bond, or are they
stronger because the covalent bond is augmented by an additional ionic
interaction between the sulfur and the oxygens?
Figure IM11.5. Ionic interaction vs. π-bonding in sulfate. So, maybe sulfur and phosphorus really can form additional
bonds. The bigger part of the controversy about the octet rule in sulfur and
phosphorus chemistry is a little too subtle to explore very deeply at this
point: it's whether sulfur can form a covalent double bond in these cases.
The issue has to do with ideas from molecular orbital theory, which is a later
chapter, and how well d orbitals can form "pi bonds" with the p orbital on
oxygen. Problem IM11.1. Fill in any missing lone pairs on the following
structures. Problem IM11.2. Indicate whether each of the structures in IM11.1. obeys
the octet rule. If not, provide a resonance structure that obeys the octet
rule. Problem IM11.3. Many oxyphosphorus compounds are commonly drawn in a way
that is inconsistent with the octet rule. Draw two structures for each of
the following compounds: one that obeys the octet rule but has higher charge
separation, and one that has lower charge separation but exceeds the octet on
phosphorus. (Note: in a few of the compounds, hydrogen is attached to
phosphorus, as suggested in the condensed formula.) a) H3PO4 or PO(OH)3
b) H3PO3 or HPO(OH)2 c)
H3PO2 or H2PO(OH) d) (CH3)3PO
e) (CH3O)PO Problem IM11.4. Draw two structures for each of the following compounds:
one that obeys the octet rule but has higher charge separation, and one that has
lower charge separation but exceeds the octet on chlorine.
a) hypochlorite, ClO- b)
chlorite, ClO2-
c) chlorate, ClO3-
d) perchlorate, ClO4- Problem IM11.5. Draw two structures for each of the following compounds:
one that obeys the octet rule but has higher charge separation, and one that has
lower charge separation but exceeds the octet on sulfur. a) sulfite, SO32-
b) sulfate, SO42-
c) thiosulfate, S2O32-
d) disulfate, S2O72-
e) persulfate or peroxomonosulfate, SO52- Problem IM11.6. Global warming is a controversial topic in society but
there is not a great deal of controversy about it in the scientific community.
A summary of evidence can be found at the
National Oceanic and Atmospheric
Administration's website. Explain some of the evidence that global warming is
occurring and is linked to human activity. Why do you think there is
little debate about these ideas among scientists, but lots of debate in the US
public as a whole? This site was written by Chris P. Schaller, Ph.D., College of Saint Benedict / Saint John's
University (retired) with contributions from other authors as noted. It is freely
available for educational use.
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Reactivity in Organic, Biological and Inorganic Chemistry
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