Sketch the MO theory energy diagram for Na2. What is the bond order? a. 1 b. 1.5 c. 0 d. 0.5 e. 2

Fill in the Molecular Orbital Energy Diagram for the diatomic molecule Li₂. E lithiumA 2s- 1s. MO's 2s 02s 0* 1s 015 lithiumB 2s 1s

2. Use molecular orbital (MO) theory in description of the following molecules: Which of the following species has the greater bond enthalpy? These chemical species have the similar orbital structure to that of N2. CO, CO+

Molecular Orbital Theory -- Diatomics -- Electron Configuration Using the molecular orbital model, identify the correct (valence) electron configurations for the following diatomic species. A✓ N₂ CN+ Cv №₂+ Dv CN Fv F2 A. (025)2(02s*)2(2p)4(02p)²(12p*)1 B. (02s)2(02s+)2(02p)2(2p)4(π2p*)3 C. (025)²(025*)2(π2p)4(020)¹ D. (028)2(02s*)2(02p)2(2p)4(П2p*)2|| E. (025)²(025*)²(2p)4 F. (025)2(025*)2(020)²(2p)4(π2p*)4|| G. (025)²(02s*)2(2p)4(02p)²

For each of the following molecules, give the bond order, and describe them as paramagnetic or diamagnetic a. O2 b. N2 c. F2 d. N2- e. C2^(2-)

Referencing the diagrams on the next page, sketch molecular orbital diagrams, calculate bond order, and determine stability for the following 3 molecules: a. C2 (follows ordering in left-hand orbital diagram) b. O2 (follows ordering in right-hand orbital diagram) CO (follows ordering in left-hand orbital diagram) С. Atomic orbitals Atomic orbitals Atomic Molecular Atomic Molecular orbitals orbitals orbitals orbitals 2p 2p 2p 2p Energy T2p 2s 2s 2s 2s B2, C2, N2 Ог, Fz, Nez

22. Use the molecular orbital energy diagram shown to determine which of the following is most stable (has highest bond order). A. C₂² B. N₂2 C. B₂ D. C₂2 E. B₂2

B. Answer the next two questions about the Lewis structure of XYZ shown below. メー三 -YEz: I. What is the hybridization of the central atom? II. For all covalent bonds, specify the type of bond (o vs. T) and the atomic orbitals that overlap to form the bond. For example, in a molecule of H2, the only bond is o: H(s)-H(s).

Lewis structure of: 1. CO(2) 2. CH(2)Cl(2) 3. XeF(2) 4. BF(3) 5. NFBr(2)

This question is related to molecular orbital theory. а. Explain the key differences between valence bond theory and molecular orbital theory as models for bonding. b. When considering molecular orbital diagrams of homonuclear diatomic molecules (such as those shown below in part c), explain why atomic orbital energies are the same. How will this differ for heteronuclear diatomic molecules?