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Chapter 8: Q45E (page 451)

A friend tells you that the \({\rm{2s}}\)orbital for fluorine starts off at a much lower energy than the \({\rm{2s}}\) orbital for lithium, so the resulting \({{\rm{\sigma }}_{{\rm{2s}}}}\) molecular orbital in \({{\rm{F}}_{\rm{2}}}\) is more stable than in \({\rm{L}}{{\rm{i}}_{\rm{2}}}\). Do you agree?

Short Answer

Expert verified

Yes, it is agreed.

Step by step solution

01

Definition of diatomic molecule

A diatomic molecule is a molecule that consists of only two atoms of the same or different chemical elements

02

 Evaluating \({{\bf{F}}_{\bf{2}}}\) is more stable than \({\bf{L}}{{\bf{i}}_{\bf{2}}}\)

Yes, i agree. The \(2s\) Fluorine orbits start at much lower energies \(2s\) this is because fluorine is smaller than lithium and is orbital lithium \(2s\) The orbit of fluorine is closer to the nucleus than lithium and is more stable. Therefore, the result is \({\sigma _{2s}}\)molecular orbital in \({F_2}\)is more stable than in \({\rm{L}}{{\rm{i}}_{\rm{2}}}\).

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Most popular questions from this chapter

For the first ionization energy for an \({{\rm{N}}_2}\) molecule, what molecular orbital is the electron removed from?

Sulfuric acid is manufactured by a series of reactions represented by the following equations:

\(\begin{array}{l}{{\rm{S}}_{\rm{8}}}{\rm{(s) + 8}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {\rm{8S}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}}\\{\rm{2S}}{{\rm{O}}_{\rm{2}}}{\rm{(g) + }}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2S}}{{\rm{O}}_{\rm{3}}}{\rm{(g)}}\\{\rm{S}}{{\rm{O}}_{\rm{3}}}{\rm{(g) + }}{{\rm{H}}_{\rm{2}}}{\rm{O(l)}} \to {{\rm{H}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}{\rm{(l)}}\end{array}\)

Draw a Lewis structure, predict the molecular geometry by VSEPR, and determine the hybridization of sulfur for the following:

(a) circular \({{\rm{S}}_{\rm{8}}}\)molecule

(b) \({\rm{S}}{{\rm{O}}_{\rm{2}}}\)molecule

(c) \({\rm{S}}{{\rm{O}}_{\rm{3}}}\)molecule

(d) \({{\rm{H}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\)molecule (the hydrogen atoms are bonded to oxygen atoms)

What charge would be needed on \({{\rm{F}}_{\rm{2}}}\) to generate an ion with a bond order of \({\rm{2}}\)?

Another acid in acid rain is nitric acid, HNO3, which is produced by the reaction of nitrogen dioxide, NO2, with atmospheric water vapor. What is the hybridization of the nitrogen atom in NO2? (Note: the lone electron on nitrogen occupies a hybridized orbital just as a lone pair would.)

How are the following similar, and how do they differ?

(a) 蟽 molecular orbitals and 蟺 molecular orbitals

(b) 蠄 for an atomic orbital and 蠄 for a molecular orbital (c) bonding orbitals and antibonding orbitals
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