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Chapter 9: Problem 42

Write Lewis structures for these ions: (a) \(\mathrm{O}_{2}^{2-}\), (b) \(\mathrm{C}_{2}^{2-},\) (c) \(\mathrm{NO}^{+}\), (d) \(\mathrm{NH}_{4}^{+}\). Show formal charges.

Short Answer

Expert verified
The four lewis structures are: (a) \(\mathrm{O}_{2}^{2-}\) with both oxygen atoms having an octet of electrons and each carrying a -1 charge, (b) \(\mathrm{C}_{2}^{2-}\) with both carbon atoms having an octet of electrons and each carrying a -1 charge, (c) \(\mathrm{NO}^{+}\) with nitrogen atom having 8 electrons (including bonding electrons) with +1 charge and oxygen atom has 7 electrons with -1 charge, (d) All atoms in \(\mathrm{NH}_{4}^{+}\) have completed their octet or duet (in case of hydrogen) and nitrogen carries a +1 charge.

Step by step solution

01

Lewis Structure and Formal Charges for \(\mathrm{O}_{2}^{2-}\)

First, calculate the total number of valence electrons. Oxygen atom has 6 valence electrons and as there are two atoms, total electrons are \(2*6 = 12\). As the ion carries overall 2- charge there are two additional electrons so the total number of electrons is \(12+2 =14\). Now, place the atoms and draw a single bond (representing two electrons) between them. Arrange the remaining electrons around the atoms to fulfill the octet rule.
02

Lewis Structure and Formal Charges for \(\mathrm{C}_{2}^{2-}\)

Every carbon has 4 valence electrons, so for two atoms, total valence electrons are \(2*4=8\). Due to overall 2- charge on ion, two additional electrons will add-up, making the total \(8+2=10\) electrons. Draw the atoms and place a triple bond (6 electrons) between them. Arrange the remaining electrons around the atoms to satisfy the octet rule.
03

Lewis Structure and Formal Charges for \(\mathrm{NO}^{+}\)

Nitrogen has 5 valence electrons and oxygen atom has 6. Therefore, the total number of valence electrons in \(\mathrm{NO}^{+}\) ion is \(5 + 6 -1 = 10\). We subtract one because there is a +1 charge on the ion. First draw the atoms together and put a single bond (two electrons) between N and O. Arrange the remaining electrons around the atoms to achieve the octet rule. Calculate the formal charges on each atom.
04

Lewis Structure and Formal Charges for \(\mathrm{NH}_{4}^{+}\)

Nitrogen has 5 valence electrons and as each hydrogen atom has 1 electron, the total sum of valence electrons from 4 hydrogen atoms is 4. The total number of valence electrons for \(\mathrm{NH}_{4}^{+}\) ion is \(5+4-1=8\). We subtract one due to the +1 charge on the ion. Draw N in the center surrounded by 4 H atoms. Use the 4 pairs of electrons to make single bond with hydrogen atoms. No left over electron remains. Calculate the formal charges on each atom.

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