Draw the Lewis structure for NO+ . Is the nitrogen– oxygen bond in NO+ longer, shorter, or the same length as the nitrogen–oxygen bond in NO? Explain. Draw the Lewis structure for NO+ .

Verified step by step guidance

1. Identify the total number of valence electrons for NO^+. Nitrogen (N) has 5 valence electrons, oxygen (O) has 6 valence electrons, and the positive charge indicates the loss of one electron, so the total is 5 + 6 - 1 = 10 electrons.
2. Place the nitrogen and oxygen atoms next to each other, as they will form a bond. Start by drawing a single bond between N and O, which uses 2 electrons, leaving 8 electrons to distribute.
3. Distribute the remaining electrons to satisfy the octet rule, starting with the more electronegative atom, oxygen. Place 6 electrons (3 lone pairs) on oxygen, and 2 electrons (1 lone pair) on nitrogen.
4. Check if the octet rule is satisfied for both atoms. Nitrogen has 5 electrons (1 lone pair and 2 from the bond), and oxygen has 8 electrons (3 lone pairs and 2 from the bond). To satisfy the octet for nitrogen, form a double bond by moving one lone pair from oxygen to form a second bond with nitrogen.
5. Compare the bond order of NO^+ and NO. NO^+ has a bond order of 3 (triple bond), while NO has a bond order of 2. A higher bond order typically indicates a shorter bond length, so the N-O bond in NO^+ is shorter than in NO.

Key Concepts

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for predicting molecular geometry, bond lengths, and the overall reactivity of the molecule.

Bond Length

Bond length is the distance between the nuclei of two bonded atoms. It is influenced by the type of bond (single, double, or triple) and the atoms involved. Generally, as the number of shared electron pairs increases, the bond length decreases, leading to shorter and stronger bonds. This concept is crucial for comparing bond lengths in different molecules.

Formal Charge

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and the number of bonds. It helps in determining the most stable Lewis structure by minimizing formal charges across the molecule. In the case of NO+ and NO, analyzing formal charges can provide insight into the stability and bond characteristics of the nitrogen-oxygen bond.