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Chapter 1: Q10P (page 2)

Use the symbol 未+and 未+to show the direction of polarity of the bond between carbon and oxygen.

CH3-OH

Short Answer

Expert verified

H3C未+-O未-H

Step by step solution

01

Defining bond polarity

The distribution of positive and negative electrical charges over a bond is known as bond polarity. The bond polarity can be determined by comparing the difference in electronegativity between the atoms.

02

" width="9" height="19" role="math" style="max-width: none; vertical-align: -4px;" localid="1664883424373">Step2: Determining of role="math" localid="1664883414773" δ+ and δ+ over a bond.

The electronegativity of oxygen is 3.44 and that of carbon is 2.5. Out of two, oxygen being more electronegative develops a partial negative charge and carbon develops a partial positive charge. This separation in their charges makes them polar.

The direction of polarity is shown below.

The direction is always shown from positive to negative polarity. This is called the dipole moment

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Most popular questions from this chapter

Predict the approximate bond angle in

  1. The methyl cation
  2. The methyl radical
  3. The methyl anion

After examining the potential maps for LiH, HF and H2, answer the following questions:

  1. Which compounds are polar?
  2. Why does LiH have the largest hydrogen?
  3. Which compound has the hydrogen that would be most apt to attract a negatively charged molecule?

Rank the bonds from the most polar to least polar.

a. C - O,C - F,C - N

b. C - Cl > C - Br > C - I

c. H - O,H - N,H - C

d. C - H,C - C,C - N

Indicate the kind of molecular orbital (蟽 ,蟽 *,蟺 ,蟺 *) that results when the two atomic orbitals are combined:

Determine the partial negative charge on the fluorine atom in a C-F bond. The bond length is 1.39 1.39A* , and the bond dipole moment is 1.06D. The charge on an electron is 4.80猕�10-10esu.

See all solutions

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