Draw Lewis structures and MO diagrams for CN⁺ , CN, and CN^- . According to the Lewis model, which species is most stable?

Verified step by step guidance

1. Draw the Lewis structure for CN^+ by counting the total number of valence electrons. Carbon has 4 valence electrons and nitrogen has 5, but since there is a positive charge, subtract one electron. Distribute these electrons to satisfy the octet rule.
2. Draw the Lewis structure for CN by counting the total number of valence electrons. Carbon has 4 valence electrons and nitrogen has 5, making a total of 9 electrons. Distribute these electrons to satisfy the octet rule.
3. Draw the Lewis structure for CN^- by counting the total number of valence electrons. Carbon has 4 valence electrons and nitrogen has 5, but since there is a negative charge, add one electron. Distribute these electrons to satisfy the octet rule.
4. Construct the molecular orbital (MO) diagram for each species. Start by identifying the atomic orbitals of carbon and nitrogen, then combine them to form bonding and antibonding molecular orbitals. Fill the molecular orbitals with the appropriate number of electrons for CN^+, CN, and CN^-.
5. Compare the stability of CN^+, CN, and CN^- using the Lewis structures and MO diagrams. Consider factors such as the number of bonds, formal charges, and bond order to determine which species is most stable.

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 the arrangement of electrons and the overall stability of a molecule.

Molecular Orbital (MO) Theory

Molecular Orbital Theory describes the behavior of electrons in a molecule by considering the combination of atomic orbitals to form molecular orbitals. These orbitals can be bonding, antibonding, or non-bonding, and their occupancy determines the stability and reactivity of the molecule. MO diagrams visually represent these orbitals and their energy levels, providing insight into the electronic structure of the species.

Stability of Ions

The stability of ions, such as CN+, CN, and CN-, is influenced by factors like formal charge, electron configuration, and the presence of lone pairs. Generally, species with a formal charge close to zero and a full valence shell are more stable. Analyzing the Lewis structures and MO diagrams helps determine which ion has the most favorable electronic arrangement, thus indicating its stability.