Taking into account the definition of electronegativity and polarity of a chemical bond, the H-O bond is the bond with the higher polarity.
First, electronegativity is a chemical property that measures the ability of an atom to attract electrons in a bond. Those elements that have a greater capacity to attract electrons will be the most electronegative.
The polarity of a chemical bond occurs when there is an asymmetric distribution of the electron cloud of the bond around the two atoms that form said bond.
A polar bond has a non-uniform distribution of charges and has two poles (dipole) while a non-polar bond is characterized by having a uniform distribution of charges. The latter happens when both atoms have different electronegativity.
The Pauling scale is a classification of the electronegativity of atoms. So, the electronegativity of the elements is:
- C: 2.5
- O: 3.5
- F: 4
- H: 2.1
- N: 3
So the electronegativity difference of the bonds is:
- C-O: 3.5 - 2.5= 1
- F-F: 4 -4=0
- H-O: 3.5 - 2.1= 1.4
- N-H: 3 - 2.1= 0.9
Finally, since a larger electronegativity difference indicates a higher bond polarity, the H-O bond is the bond with the higher polarity.
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