Problem: Part A. Due to the small and highly electronegative nature of fluorine, the oxyacids of the this element are much less common and less stable than those of the other halogens. Bonding theory, however, does allow one to propose structures for these acids and use formal charges for the evaluation of these structures. For a molecule of fluorous acid, the atoms are arranged asHOFO. (Note: In this oxyacid, the placement of fluorine is an exception to the rule of putting the more electronegative atom in a terminal position.)What is the formal charge on each of the atoms? Enter the formal charges in the same order as the atoms are listed.Express your answers as charges separated by comma. For example, a positive one charge would be written as +1.Formal charge (FC) keeps track of which electrons an atom "owns" in a chemical bond with the equationFC =(valence e- in free atom) - (valence e- in bonded atom)When more than one valid Lewis structure can be drawn for a particular molecule, formal charge is used to predict the most favorable structure.A bonded atom is considered to "own" all its nonbonding electrons but only half of the bonding electrons because these are shared with another atom. Therefore, the formal charge formula can be rewritten as follows:null

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Part A. Due to the small and highly electronegative nature of fluorine, the oxyacids of the this element are much less common and less stable than those of the other halogens. Bonding theory, however, does allow one to propose structures for these acids and use formal charges for the evaluation of these structures. For a molecule of fluorous acid, the atoms are arranged asHOFO. (Note: In this oxyacid, the placement of fluorine is an exception to the rule of putting the more electronegative atom in a terminal position.)

What is the formal charge on each of the atoms? Enter the formal charges in the same order as the atoms are listed.

Express your answers as charges separated by comma. For example, a positive one charge would be written as +1.


Formal charge (FC) keeps track of which electrons an atom "owns" in a chemical bond with the equation

FC =(valence e- in free atom) - (valence e- in bonded atom)

When more than one valid Lewis structure can be drawn for a particular molecule, formal charge is used to predict the most favorable structure.

A bonded atom is considered to "own" all its nonbonding electrons but only half of the bonding electrons because these are shared with another atom. Therefore, the formal charge formula can be rewritten as follows:

null

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