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General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343

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BuyFindarrow_forward

General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

Using electronegativities, decide which of the following bonds is most polar: C─O, C─S, H─Br.

Interpretation Introduction

Interpretation:

The given following bonds is most polar has to be explained using electro negativity method.

Concept introduction:

  • Electronegativity is an important concept.  You will use it to recognize bond individuality, dipole moment, intermolecular bonding, and many other properties of molecules that you will study later on.  Electronegativity is the ability of an atom to attract electrons in a chemical bond.
  • Electronegativity increases moving to the right in the periodic table and decreases down a group.
  • The difference in electro negativities of the two atoms gives a rough guide to the type of bond to expect.  The difference is 0.5 or less, the bond is essentially covalent.  When the difference is greater than 1.8, the bond is considered ionic.  The polar covalent bond as a result would lie within electronegativity differences of 0.6 and 1.8.
Explanation

The greater the electro negativity difference, the more polar is the bond. The elements have the following electro negativities: H = 2.1, C = 2.5, S = 2.5, Br = 2.8, O = 3

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