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Chapter 7: Q103E (page 405)

Is the \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{BBC}}{{\rm{l}}_{\rm{2}}}\)molecule polar or nonpolar?

Short Answer

Expert verified

The molecule \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{BBC}}{{\rm{l}}_{\rm{2}}}\) is nonpolar.

Step by step solution

01

Definition of Concept

Dipole Moment: The separation of two electrical charges opposite in charge is measured by the dipole moment of any compound. It's calculated by multiplying the product of the two charges by the distance between them. The dipole moment is always shown in the direction of negative to positive charge.

The net dipole moment of the compounds determines the polarity of the compounds. A compound is non-polar if its net dipole moment is zero, while it is polar if it has a certain net dipole moment.

02

Find the molecule is polar or nonpolar

It is, in fact,\({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{BBC}}{{\rm{l}}_{\rm{2}}}\).

As shown in the figure below, it is trigonal planar around each B atom, and dipoles cancel each other out.

Therefore, it is non-polar.

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Most popular questions from this chapter

There are three possible structures for \({\rm{PC}}{{\rm{l}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{3}}}\)with phosphorus as the central atom. Draw them and discuss how measurements of dipole moments could help distinguish among them.

Question: Using the standard enthalpy of formation data in Appendix G, show how the standard enthalpy of formation of \({\rm{HCl(g)}}\) can be used to determine the bond energy.

From their positions in the periodic table, arrange the atoms in each of the following series in order of increasing electronegativity: (a)\({\rm{C, F, H, N, O}}\)(b)\({\rm{Br, Cl, F, H, I }}\)(c)\({\rm{F, H, O, P, S }}\)(d)\({\rm{Al, H, Na, O, P}}\)(e)\({\rm{Ba, H, N, O, As}}\).

Question: Using the bond energies in Table \({\rm{7}}{\rm{.2}}\), determine the approximate enthalpy change for each of the following reactions:

(a) \({{\rm{H}}_{\rm{2}}}{\rm{(g) + B}}{{\rm{r}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2HBr(g)}}\)

(b) \({\rm{C}}{{\rm{H}}_{\rm{4}}}{\rm{(g) + }}{{\rm{I}}_{\rm{2}}}{\rm{(g)}} \to {\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{I(g) + HI(g)}}\)

(c) \({{\rm{C}}_{\rm{2}}}{{\rm{H}}_4}{\rm{(g) + 3}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2C}}{{\rm{O}}_{\rm{2}}}{\rm{(g) + 2}}{{\rm{H}}_{\rm{2}}}{\rm{O(g)}}\)

How are single, double, and triple bonds similar? How do they differ?
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