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Chapter 8: Q5 CYL (page 433)

Label the molecular orbital shown as σ or Π, bonding or antibonding, and indicate where the node occurs.


Short Answer

Expert verified

It is called an σ orbital because it is placed along the internuclear axis. It's an antibonding orbital since there's a node that cuts the internuclear axis.

Step by step solution

01

Define bond

A bond is a long-term attraction between two atoms, molecules, or ions. Most bonding activity can be explained by the attraction of two electrical charges that are in opposition to one another.

02

Explanation

It is an σ orbital because it is placed along the internuclear axis. It is an antibonding orbital because a node bisects the internuclear axis.


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Most popular questions from this chapter

Explain why bonds occur at specific average bond distances instead of the atoms approaching each other infinitely close.

The main component of air is N2. From the molecular orbital diagram of N2, predict its bond order and whether it is diamagnetic or paramagnetic.

Methionine, \({\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{SC}}{{\rm{H}}_{\rm{2}}}{\rm{C}}{{\rm{H}}_{\rm{2}}}{\rm{CH}}\left( {{\rm{N}}{{\rm{H}}_{\rm{2}}}} \right){\rm{C}}{{\rm{O}}_{\rm{2}}}{\rm{H}}\), is an amino acid found in proteins. Draw a Lewis structure of this compound. What is the hybridization type of each carbon, oxygen, the nitrogen, and the sulfur?

Determine the bond order of each member of the following groups, and determine which member of each group is predicted by the molecular orbital model to have the strongest bond.

(a) \({{\rm{H}}_{\rm{2}}}{\rm{,}}{{\rm{H}}_{\rm{2}}}{\rm{ + ,H}}_{\rm{2}}^{\rm{ - }}\)

(b) \({{\rm{O}}_{\rm{2}}}{\rm{,O}}_{\rm{2}}^{{\rm{2 + }}}{\rm{,O}}_{\rm{2}}^{{\rm{2 - }}}\)

(c) \({\rm{L}}{{\rm{i}}_{\rm{2}}}{\rm{,B}}{{\rm{e}}_{\rm{2}}}{\rm{ + ,B}}{{\rm{e}}_{\rm{2}}}\)

(d) \({{\rm{F}}_{\rm{2}}}{\rm{,\;}}{{\rm{F}}_{\rm{2}}}{\rm{ + ,}}\;\;\;{\rm{F}}_{\rm{2}}^{\rm{ - }}\)

(e) \({{\rm{N}}_{\rm{2}}}{\rm{,\;N}}_{\rm{2}}^{\rm{ + }}{\rm{,}}\;\;\;{\rm{N}}_{\rm{2}}^{\rm{ - }}\)

Predict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions.

(a) \({\rm{N}}{{\rm{a}}_{\rm{2}}}^{{\rm{2 + }}}\)

(b) \({\rm{M}}{{\rm{g}}_{\rm{2}}}^{{\rm{2 + }}}\)

(c) \({\rm{A}}{{\rm{l}}_{\rm{2}}}^{{\rm{2 + }}}\)

(d) \({\rm{S}}{{\rm{i}}_{\rm{2}}}^{{\rm{2 + }}}\)

(e) \({\rm{P}}_{\rm{2}}^{{\rm{2 + }}}\)

(f) \({{\rm{S}}_{\rm{2}}}^{{\rm{2 + }}}\)

(g) \({{\rm{F}}_{\rm{2}}}^{{\rm{2 + }}}\)

(h) \({\rm{A}}{{\rm{r}}_{\rm{2}}}^{{\rm{2 + }}}\)
See all solutions

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