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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\({\rm{A}}{{\rm{B}}_{\rm{3}}}\), 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 that has each shape.

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

  1. \({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\,\)
  2. \({\rm{PC}}{{\rm{l}}_{\rm{4}}}{\rm{ - }}\)
  3. \({\rm{SnC}}{{\rm{l}}_{\rm{3}}}^{\rm{ - }}\)
  4. \({\rm{BrC}}{{\rm{l}}_{\rm{4}}}^{\rm{ - }}\)
  5. \({\rm{IC}}{{\rm{l}}_{\rm{3}}}\)
  6. \({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)
  7. \({\rm{S}}{{\rm{F}}_{\rm{2}}}\)

Write the electron configuration for the monatomic ions formed from the following elements (which form the greatest concentration of monatomic ions in seawater): (a) \({\rm{Cl}}\) (b) \({\rm{Na}}\) (c) \({\rm{Mg}}\)(d) \({\rm{Ca}}\) (e) \({\rm{K}}\) (f) \({\rm{Br}}\) (g) \({\rm{Sr}}\) (h) \({\rm{F}}\).

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

  1. \({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\)
  2. \({\rm{PC}}{{\rm{l}}_{\rm{4}}}^{\rm{ - }}\)
  3. \({\rm{SnCl}}_{\rm{3}}^{\rm{ - }}\)
  4. \({\rm{BrCl}}_{\rm{4}}^{\rm{ - }}\)
  5. \({\rm{IC}}{{\rm{l}}_{\rm{3}}}\)
  6. \({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)
  7. \({\rm{S}}{{\rm{F}}_{\rm{2}}}\)

Question: When a molecule can form two different structures, the structure with the stronger bonds is usually the more stable form. Use bond energies to predict the correct structure of the hydroxylamine molecule:
See all solutions

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