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Chapter 8: Problem 35

(a) Construct a Lewis structure for \(\mathrm{O}_{2}\) in which each atom achieves an octet of electrons. (b) How many bonding electrons are in the structure? (c) Would you expect the \(\mathrm{O}-\mathrm{O}\) bond in \(\mathrm{O}_{2}\) to be shorter or longer than the \(\mathrm{O}-\mathrm{O}\) bond in compounds that contain an \(\mathrm{O}-\mathrm{O}\) single bond? Explain.

Short Answer

Expert verified
The Lewis structure for \(\mathrm{O}_{2}\) consists of a double bond between the two oxygen atoms, with each atom fulfilling the octet rule. There are 4 bonding electrons in this structure. The O-O bond in \(\mathrm{O}_{2}\) is shorter than the O-O bond in compounds containing an O-O single bond due to the increased electron density and stronger attractive force between the atoms in a double bond.

Step by step solution

01

Determine the total number of valence electrons

For a molecule of \(\mathrm{O}_{2}\), we have two oxygen atoms, each of which has 6 valence electrons (oxygen is in Group 16). The total number of valence electrons available for bonding is therefore 2 × 6 = 12.
02

Construct a Lewis structure for \(\mathrm{O}_{2}\) that satisfies the octet rule

To construct a Lewis structure for \(\mathrm{O}_{2}\), we must have each oxygen atom fulfill the octet rule (having 8 electrons in its outer shell). Since both the oxygen atoms have six valence electrons each that are not involved in bonding, we can begin by forming a single bond (using 2 electrons) between the two atoms. However, a single bond does not fulfill the octet rule for both atoms. Therefore, we need a double bond to complete the octet requirement. The resulting Lewis structure for \(\mathrm{O}_{2}\) is: O = O Each oxygen atom has 2 electrons in the double bond, plus six additional electrons in their outer shell, satisfying the octet rule.
03

Count the bonding electrons in the Lewis structure

In the Lewis structure for \(\mathrm{O}_{2}\), there is a double bond between the two oxygen atoms. A double bond consists of two pairs of electrons, so there are 4 bonding electrons in total.
04

Compare the O-O bond length in \(\mathrm{O}_{2}\) to that of an O-O single bond

In a double bond, such as the one in \(\mathrm{O}_{2}\), the electron density between two atoms is greater than in a single bond. This increased electron density leads to a stronger attractive force between the positively charged nuclei and the negatively charged electrons. Consequently, double bonds are shorter and stronger than single bonds between the same atoms. Therefore, we can conclude that the O-O bond in \(\mathrm{O}_{2}\) is shorter than the O-O bond in compounds that contain an O-O single bond.

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