This assignment can be found in Google Docs: Chemistry for Majors Assignment: 8
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- How is a [latex]\pi[/latex] bond different from a double bond?
- This module touches on a review concept: bond energy. (Figure 1, in 8.1). Does it take energy to break a bond, or does it take energy to make a bond? Explain your understanding of this in two sentences.
- Using valence bond theory, sketch the atomic orbitals involved in bonding Cl2 and HCl.
- How many [latex]\sigma[/latex] and [latex]\pi[/latex] bonds are present in the molecule CO2?
- Give the shape associated with each hybrid orbital set: (a) sp (b) sp3d2 (c) sp3 (d) sp2
- Threonine (CH3CHOHCHNH2COOH) is an amino acid found in many proteins. The Lewis structure is shown above. Find the hybridization of each non-terminal atom (each carbon, oxygen, and nitrogen).
- Write the Lewis structure for nitric acid (HNO3). Identify the VSEPR geometry for each atom. Then find the hybridization for each atom.
- Draw the molecular orbitals formed by: (a) two s orbitals overlapping (b) two p orbitals overlapping
- Reminder- orbitals are conserved- you get out the same number of orbitals that you start with.
- Predict the valence electron molecular orbital configurations for the following and state whether the ion will form. (a) F2 (b) F2+ (c) F2– (d) Al2
- Calculate the bond order for a molecule with this configuration: (σ2s)2(σ∗2s)2(σ2px)2(π2py,π2pz)3(π∗2py,π∗2pz)1