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Chapter 16: Problem 59

Draw Lewis structures that show how electron pairs move and bonds form and break during the autoionization of water. Label the appropriate \(\mathrm{H}_{2} \mathrm{O}\) molecules as the Lewis acid and Lewis base.

Short Answer

Expert verified
Answer: In the autoionization process, one water molecule acts as a Lewis base, donating a hydrogen atom with its electron pair to the other water molecule, which acts as a Lewis acid. This process results in the formation of a hydronium ion (H鈧僌鈦�) and a hydroxide ion (OH鈦�).

Step by step solution

01

Draw the Lewis structure of a water molecule

To draw the Lewis structure of a water molecule (\(\mathrm{H}_{2} \mathrm{O}\)), first, arrange the atoms: the central atom (oxygen) is bonded to two hydrogen atoms. The oxygen atom has 6 valence electrons, and each hydrogen has 1 valence electron. Oxygen forms two single bonds with the hydrogen atoms, and it's left with two lone pairs of electrons. Lewis structure for water: O / \ H H
02

Identify a molecule as a Lewis acid and another as a Lewis base

In autoionization, one water molecule will act as a Lewis acid by accepting an electron pair, and the other will act as a Lewis base by donating an electron pair. In this case, the oxygen atom of the Lewis acid molecule will accept the electron pair from a hydrogen atom of the Lewis base molecule.
03

Draw the Lewis structures showing the movement of electron pairs and bonds formation and breakage during autoionization

During the autoionization process, the electron pair from an oxygen-hydrogen bond of one water molecule (Lewis base) is donated to the oxygen of another water molecule (Lewis acid), forming a hydronium ion (\(\mathrm{H}_{3} \mathrm{O}^{+}\)) and a hydroxide ion (\(\mathrm{OH}^{-}\)). The Lewis structures showing this process are: Lewis base Lewis acid O O / \ / \ H H + H H |---| Movement: v Hydronium ion Hydroxide ion O O /|\ / \ H H H H ..
04

Label the structures as Lewis acid and Lewis base

Now, we can label the water molecules as the Lewis acid and Lewis base in the initial reaction: Lewis base Lewis Acid O O / \ / \ H H + H H Overall, the autoionization process of water involves one water molecule acting as a Lewis base, donating a hydrogen atom with its electron pair to the other water molecule as a Lewis acid, resulting in the hydronium and hydroxide ions.

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Most popular questions from this chapter

A cook dissolves a teaspoon of baking soda (NaHCO \(_{3}\) ) in a cup of water and then discovers that the recipe calls for a tablespoon, not a teaspoon. If the cook adds two more teaspoons of baking soda to make up the difference, does the additional baking soda change the pH of the solution? Explain why or why not.

Why is \(\mathrm{BF}_{3}\) a Lewis acid but not a Bronsted-Lowry acid?

Draw Lewis structures that show how electron pairs move and bonds form and break in the following reaction, and identify the Lewis acid and Lewis base. $$ \mathrm{SeO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{H}_{2} \mathrm{SeO}_{4}(a q) $$

Buffer A contains nearly equal concentrations of its conjugate acid-base pair. Buffer \(\mathrm{B}\) contains the same total concentration of acidic and basic components as buffer \(\mathrm{A}\) but B has twice as much of its weak acid as its conjugate base. Which buffer experiences a smaller change in \(\mathrm{pH}\) when a. the same small quantity of strong base is added to both? b. the same small quantity of strong acid is added to both?

What volume of \(0.100 M\) HCl is required to titrate \(250 \mathrm{mL}\) of \(0.0100 M \mathrm{Na}_{2} \mathrm{CO}_{3}\) to the first equivalence point?
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