Chapter 9: Problem 54

Draw three resonance structures for the molecule \(\mathrm{N}_{2} \mathrm{O}\) in which the atoms are arranged in the order NNO. Indicate formal charges.

Short Answer

Expert verified

The three resonance structures for N2O (NNO arrangement) show different placements of electron pairs, leading to different distributions of formal charge in each structure. The first structure has formal charges of +1 on N (leftmost), 0 on N (middle) and -1 on O. The second structure presents formal charges of +1 on N (leftmost), 0 on both N (middle) and O. The third structure has formal charges of +1 on both N atoms and 0 on O.

Step by step solution

- Determine the central atom and draw the structure

The first atom in the given order, Nitrogen (N), is the leftmost atom, then another Nitrogen (N) in the middle, and Oxygen (O) is the rightmost. Connect all three atoms with single bonds. Subtract the total valence electrons used in bonding (6 electrons) from the total valence electrons available (16 electrons: 5 from each Nitrogen and 6 from Oxygen). There are 10 electrons left, which are placed as lone pairs on the atoms, starting from the outer atoms.

- Draw the first resonance structure

The first resonance structure places all the remaining 10 electrons on the Oxygen atom. Oxygen now has a complete octet (4 pairs of electrons; 2 pairs from bonds and 2 lone pairs). However, the left Nitrogen only has 3 electron pairs (1 from the bond and 1 lone pair), leading to a positive formal charge. The second Nitrogen has 4 electron pairs (1 from two bonds and 1 lone pair), and so does not carry any charge. Oxygen negatively charged due to having an extra pair of electrons.

- Draw the second resonance structure

The second resonance structure has one of the lone pairs on Oxygen forming a double bond with the second Nitrogen. This leaves Oxygen with 3 electron pairs (2 pairs from bonds and 1 lone pair). The second Nitrogen has a complete octet (4 electron pairs; 3 from bonds and 1 lone pair), while the first Nitrogen remains positively charged. Oxygen does not have any formal charge in this structure.

- Draw the third resonance structure

The third resonance structure has both lone pairs on Oxygen forming double bonds with the Nitrogen atoms. Oxygen now has a complete octet (4 electron pairs in bonds). The Nitrogen atoms have 3 electron pairs each (2 pairs from bonds and 1 lone pair), giving them both a positive formal charge.

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Draw three resonance structures for the molecule \(\mathrm{N}_{2} \mathrm{O}\) in which the atoms are arranged in the order NNO. Indicate formal charges.

Short Answer

Step by step solution

- Determine the central atom and draw the structure

- Draw the first resonance structure

- Draw the second resonance structure

- Draw the third resonance structure

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