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Chapter 7: Q20E (page 392)

Which is the most polar bond? (a) \({\rm{C - C}}\) (b) \({\rm{C - H}}\) (c) \({\rm{N - H}}\) (d) \({\rm{O - H}}\) (e) \({\rm{Se - H}}\) .

Short Answer

Expert verified

The most polar bond is: \({\rm{O - H}}\).

Step by step solution

01

Define Chemical Bonding

A chemical bond is a long-term attraction between atoms, ions, or molecules that allows chemical compounds to form.

02

Explanation

The polarity of a bond is determined by the electronegativity difference between two atoms creating it.

We'll start by looking at the electronegativity values of each element in fig. \({\rm{7}}{\rm{.6}}\), and then compute the electronegativity difference.

03

Finding which one is most polar bond?

a. As both atoms have the same electronegativity, the difference in electronegativity is \({\rm{0}}\).

Therefore, it is not the most polar bond.

04

Finding which one is most polar bond?

b.

\({\rm{C}}\) has an electronegativity of \({\rm{2}}{\rm{.5}}\) and \({\rm{H}}\) has an electronegativity of \({\rm{2}}{\rm{.1}}\), so the difference is \({\rm{0}}{\rm{.4}}\).

Therefore, it is not the most polar bond.

05

Finding which one is most polar bond?

c.

\({\rm{N}}\) has an electronegativity of \({\rm{3}}{\rm{.0}}\) and \({\rm{H}}\) has an electronegativity of \({\rm{2}}{\rm{.1}}\), so the difference is \({\rm{0}}{\rm{.9}}\).

Therefore, it is not the most polar bond.

06

Finding which one is most polar bond?

d.

\({\rm{O}}\) has an electronegativity of \({\rm{3}}{\rm{.5}}\) and \({\rm{H}}\) has an electronegativity of \({\rm{2}}{\rm{.1}}\), the difference is \({\rm{1}}{\rm{.4}}\).

Therefore, it is the most polar bond.

07

Finding which one is most polar bond?

e.

\({\rm{Se }}\)has an electronegativity is \({\rm{2}}{\rm{.4}}\) and \({\rm{H}}\) has an electronegativity is \({\rm{2}}{\rm{.1}}\), so the difference is \({\rm{0}}{\rm{.3}}\).

Therefore, it is not the most polar bond.

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Most popular questions from this chapter

A molecule with the formula\({\rm{A}}{{\rm{B}}_{\rm{2}}}\), in which A and B represent different atoms, could have one of three different shapes. Sketch and name the three different shapes that this molecule might have. Give an example of a molecule or ion for each shape.

The arrangement of atoms in several biologically important molecules is given here. Complete the Lewis structures of these molecules by adding multiple bonds and lone pairs. Do not add any more atoms.

What feature of a Lewis structure can be used to tell if a molecule鈥檚 (or ion鈥檚) electron-pair geometry and molecular structure will be identical?

What is the molecular structure of the stable form of \({\rm{FN}}{{\rm{O}}_{\rm{2}}}\) ? (\({\rm{N}}\)is the central atom.)

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. \({\rm{Xe}}{{\rm{F}}_{\rm{2}}}\)
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