Could someone please group these bonds under Polar and Non-Polar and also under hydrophobic and hydrophilic? C=O, C-H, O-P, and C-C

1 Answer
Sep 20, 2015

Answer:

Polar, nonpolar, polar, nonpolar.

Explanation:

You can determine the polarity of a bond by looking at the electronegativity of the atoms that make up tha bond.

More specifically, you need to examine the difference in electronegativity between the atoms that form the covalent bond.

Electronegativity is a measure of how good an atom that's part of a bond is at attracting the bonding electrons towards itself.

http://www.f.u-tokyo.ac.jp/~fukuyama/interactive_trial/virtual%20textbook/electronegativity/electronegativity.html

A polar covalent bond is formed when one of the two atoms is more electronegative than the other.

When this happens, the bonding electrons will spend more time surrounding the more electronegative atom, which will develop a partial negative charge.

The less electronegative atom will be "electron deprived", so it will develop a partial positive charge.

The difference in electronegativity, #Delta_(EN)#, between the two atoms will help you find the polarity of the molecule. A good rule of thumb to go by is

#Delta_(EN) < 0.5 -># nonpolar covalent bond

#0.5 < Delta_(EN) < 1.7 -> # polar covalent bond

#Delta_(EN)> 1.7 -># predominantly ionic bond

So, if you pair oxygen, #EN_O = 3.44#, and carbon, #EN_C = 2.55#, the difference in electronegativity will be

#Delta_EN = 3.44 - 2.55 = 0.89 -># polar covalent bond

The bond between carbon and hydrogen is considered nonpolar because you have

#Delta_(EN) = 2.55 - 2.20 = 0.35#

The bond between phosphorus and oxygen is polar covalent

#Delta_(EN) = 3.44 - 2.19 = 1.25#

The bond between two identical atoms will always be nonpolar covalent, because you essentially have

#Delta_(EN) = 2.55 - 2.55 = 0#