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Chapter 9: Problem 50

Do formal charges represent actual separation of charges?

Short Answer

Expert verified
No, formal charges do not represent actual separation of charges, but are a mathematical concept used to help chemists in understanding the distribution of electrons in a molecule.

Step by step solution

01

Define formal charges

Formal charges on an atom in a molecule are calculated by subtracting the number of valence electrons of the atom in isolation, from the number of valence electrons assigned to the atom in the molecule. It is a theoretical construct.
02

Describe the nature of formal charges

Formal charges are not actual charges, but a mathematical concept used to help chemists in predicting the distribution of electrons in a molecule. It doesn’t denote a separation of actual charges in any capacity. It merely assigns 'ownership' of bonding electrons to individual atoms. The value of formal charge can help to identify the most plausible Lewis structure for a molecule where there is more than one possible reasonable structure.
03

Summarize the understanding of formal charges

It's crucial to remember that formal charges are not true charges, but instead a theoretical construct useful for understanding molecular structures. When comparing between different Lewis structures for a same molecule, it is generally the structure with smallest formal charges on individual atoms (i.e., the structure with formal charges closest to zero) that is the more plausible representation of the actual molecule.

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Most popular questions from this chapter

Which of the following are ionic compounds? Which are covalent compounds? \(\mathrm{RbCl}, \mathrm{PF}_{5}, \mathrm{BrF}_{3},\) \(\mathrm{KO}_{2}, \mathrm{CI}_{4}\)

Write Lewis structures for \(\mathrm{SeF}_{4}\) and \(\mathrm{SeF}_{6}\). Is the octet rule satisfied for Se?

Four atoms are arbitrarily labeled \(D, \mathrm{E}, \mathrm{F},\) and \(\mathrm{G} .\) Their electronegativities are as follows: \(\mathrm{D}=3.8\), \(\mathrm{E}=3.3, \mathrm{~F}=2.8,\) and \(\mathrm{G}=1.3 .\) If the atoms of these elements form the molecules \(\mathrm{DE}, \mathrm{DG}, \mathrm{EG},\) and \(\mathrm{DF}\) how would you arrange these molecules in order of increasing covalent bond character?

Write Lewis structures for the following four isoelectronic species: (a) \(\mathrm{CO},(\mathrm{b}) \mathrm{NO}^{+},(\mathrm{c}) \mathrm{CN}^{-}\) (d) \(\mathrm{N}_{2}\). Show formal charges.

For each of the following pairs of elements, state whether the binary compound they form is likely to be ionic or covalent. Write the empirical formula and name of the compound: (a) I and \(\mathrm{Cl}\), (b) \(\mathrm{Mg}\) and \(\mathrm{F}\).
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