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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

Sketch the distribution of electron density in the bonding and antibonding molecular orbitals formed from two S orbitals and from two P orbitals.

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

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.)

Consider nitrous acid, \({\rm{HN}}{{\rm{O}}_{\rm{2}}}{\rm{(HONO)}}\). (a) Write a Lewis structure. (b) What are the electron pair and molecular geometries of the internal oxygen and nitrogen atoms in the \({\rm{HN}}{{\rm{O}}_{\rm{2}}}\) molecule? (c) What is the hybridization on the internal oxygen and nitrogen atoms in \({\rm{HN}}{{\rm{O}}_{\rm{2}}}\)?

The bonding molecular orbital in \({{\rm{H}}_2}\) is lower in energy than an electron in \({\rm{1s}}\) orbital because the bonding molecular is more stable.
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