1. A Review of General Chemistry

Formal Charges

1. A Review of General Chemistry

Formal Charges

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Calculating formal and net charge.

Calculate the formal charges of ALL atoms.

Practice this topic

Multiple Choice

Calculate the net charge of the molecule

Calculate the total charge of the molecule

What is the formal charge of the oxygen atom in the following structure (all bonds and lone pairs are drawn):

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Textbook Question

An atom with a formal charge does not necessarily have more or less electron density than the atoms in the molecule without formal charges. We can see this by examining the potential maps for H2O, H3O+, and HO−.

c. Which atom bears the formal positive charge in the hydronium ion? d. Which atom has the least electron density in the hydronium ion?

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a. Which atom bears the formal negative charge in the hydroxide ion? b. Which atom has the greater electron density in the hydroxide ion?

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LOOKING AHEAD In Chapter 3, we describe how the formal charge on an atom can be used to predict the number of lone pairs. Given the charge, or lack of charge, on each atom, fill in the electron pairs. (c)

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(••) By moving an electron pair, draw a better Lewis structure that minimizes formal charges. (b)

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(••) By moving an electron pair, draw a better Lewis structure that minimizes formal charges. (a)

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Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct. (c) BH⁻₄

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Calculate the formal charge of the indicated atom in the following molecules or ions. (f)

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Calculate the formal charge of the indicated atom in the following molecules or ions. (e)

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Draw the Lewis structure for the following molecules. Be sure to calculate the formal charge of each atom as a way of confirming your structure is correct. [To assist you, the central atom has been bolded where you might have trouble figuring it out on your own.] (c) CF₄

Calculate the formal charge of the indicated atom in the following molecules or ions. (d)

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Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct. (b) H⁺

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Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct. (d) AlCl⁻₄

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(a) Calculate the formal charge of the indicated atoms in the ions shown.

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Textbook Question

Calculate the formal charge on the non-hydrogen atoms in the molecules shown. Use the arrow-pushing formalism to 'move' an electron pair such that it is shared between two (formerly) charged atoms. Your arrow should account for the formation of the molecule on the right from the molecule on the left.

Based on the formal charge, determine how many lone pairs are on each indicated atom. (a)

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Give each atom the appropriate formal charge:

a. <IMAGE>

b. <IMAGE>

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Draw the missing lone-pair electrons and assign the missing formal charges for the following:

c. <IMAGE>

d. <IMAGE>

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Give each atom the appropriate formal charge:

c. <IMAGE>

d. <IMAGE>

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Draw the missing lone-pair electrons and assign the missing formal charges for the following:

a. <IMAGE>

b. <IMAGE>

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Textbook Question

For each of the following compounds and ions, 1. Draw a Lewis structure. 2. Show the kinds of orbitals that overlap to form each bond. 3. Give approximate bond angles around each atom except hydrogen. d. CH3CH=CH2

For each of the following structures, Draw a Lewis structure; fill in any nonbonding electrons. Calculate the formal charge on each atom other than hydrogen d. [(CH3)3O]+ e. CH3NC f. (CH3)4NBr

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Draw the Lewis structure for each of the following: d. +C2H5

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A. Draw a Lewis structure for each of the following: 1. CH3N2+ B. Draw a structure for each of the species that shows approximate bond angles. C. Which species have no dipole moment?

Draw the Lewis structure for each of the following: e. CH3NH3+

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(••) Draw the Lewis structure for the following molecular formulas.

(u) NH⁺₄

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Draw a Lewis structure for each of the following:

b. CO₃²⁻

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