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