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Chapter 8: Q46E (page 451)

True or false: Boron contains \({\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{1}}}\)valence electrons, so only one \({\rm{p}}\)- orbital is needed to form molecular orbitals.

Short Answer

Expert verified

The given statement is false.

Step by step solution

01

Molecular orbitals

The molecular orbital of an atom can be formed by the overlapping of atomic orbitals. During this process, the valence orbitals will participate.

02

Step 2: \({{\bf{B}}_{\bf{2}}}\) molecule

The molecular orbitals of\({B_2}\)are formed by the overlapping of valence atomic orbitals of each boron atom.

The valence orbitals in the boron are both 2s and 2p.

Hence, both 2s and 2p will participate in molecular orbital formation.

The given statement is false.

Molecular orbital diagram for \({B_2}\)

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Most popular questions from this chapter

Why is the concept of hybridization required in valence bond theory?

The bond energy of a C–C single bond averages \({\rm{347 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\); that of a

C ≡ C triple bond averages \({\rm{839 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\). Explain why the triple bond is not three times as strong as a single bond.

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?

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

Write Lewis structures for \({\rm{N}}{{\rm{F}}_{\rm{3}}}\) and \({\rm{P}}{{\rm{F}}_{\rm{5}}}\). On the basis of hybrid orbitals, explain the fact that \({\rm{N}}{{\rm{F}}_{\rm{3}}}\), \({\rm{P}}{{\rm{F}}_{\rm{3}}}\), and \({\rm{P}}{{\rm{F}}_{\rm{5}}}\) are stable molecules, but \({\rm{N}}{{\rm{F}}_{\rm{5}}}\) does not exist.
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