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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

From their positions in the periodic table, arrange the atoms in each of the following series in order of increasing electronegativity: (a)\({\rm{As, H, N, P, Sb}}\)(b)\({\rm{Cl, H, P, S, Si}}\)(c)\({\rm{Br, Cl, Ge, H, Sr}}\)(d)\({\rm{Ca, H, K, N, Si}}\)(e)\({\rm{Cl, Cs, Ge, H, Sr}}\).

Predict the electron pair geometry and the molecular structure of each of the following molecules or ions:

(a)\({\rm{S}}{{\rm{F}}_{\rm{6}}}\)

(b)\({\rm{PC}}{{\rm{l}}_{\rm{5}}}\)

(c)\({\rm{Be}}{{\rm{H}}_{\rm{2}}}\)

(d) \({\rm{CH}}_{\rm{3}}^{\rm{ + }}\)

Question: Which bond in each of the following pairs of bonds is the strongest?

(a) \({\rm{C - C}}\) or \({\rm{C = C}}\)

(b) \({\rm{C - N}}\) or \({\rm{C}} \equiv {\rm{N}}\)

(c) \({\rm{C}} \equiv {\rm{O}}\) or \({\rm{C = O}}\)

(d) \({\rm{H - F}}\) or \({\rm{H - Cl}}\)

(e) \({\rm{C - H}}\) or \({\rm{O - H}}\)

(f) \({\rm{C - N}}\) or \({\rm{C - O}}\)

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select H2O. Switch between the “real” and “model” modes. Explain the difference observed.

Which of the following molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments?

  1. \({\rm{Cl}}{{\rm{F}}_{\rm{5}}}\)
  2. \({\rm{Cl}}{{\rm{O}}_{\rm{2}}}{\rm{ - }}\)
  3. \({\rm{TeC}}{{\rm{l}}_{\rm{4}}}^{{\rm{2 - }}}\)
  4. \({\rm{PC}}{{\rm{l}}_{\rm{3}}}\)
  5. \({\rm{Se}}{{\rm{F}}_{\rm{4}}}\)
  6. \({\rm{P}}{{\rm{H}}_{\rm{2}}}^{\rm{ - }}\)
  7. \({\rm{Xe}}{{\rm{F}}_{\rm{2}}}\)
See all solutions

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