Textbook Question
Consider the collection of nonmetallic elements: B, As, O, and I. (d) Which element would likely to participate in two covalent bonds?
11. Bonding & Molecular Structure
Chemical Bonds
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The electronegativity is 2.1 for H and 3.0 for N. Based on these electronegativities, the compound NH3 would be expected to:
A
Be ionic and contain H−.
B
Be ionic and contain H+.
C
Have polar covalent bonds with partial negative charge on N.
D
Have nonpolar covalent bonds.
Verified step by step guidance1
Electronegativity is a measure of an atom's ability to attract and hold onto electrons. In a bond, the atom with higher electronegativity will attract the shared electrons more strongly.
Compare the electronegativities of hydrogen (H) and nitrogen (N). Hydrogen has an electronegativity of 2.1, while nitrogen has an electronegativity of 3.0.
The difference in electronegativity between N and H is 3.0 - 2.1 = 0.9. This difference indicates that the bond between N and H is polar covalent, as it is significant but not large enough to be ionic.
In a polar covalent bond, the atom with the higher electronegativity (N) will have a partial negative charge (δ−), while the atom with the lower electronegativity (H) will have a partial positive charge (δ+).
Therefore, in NH₃, the nitrogen atom will have a partial negative charge due to its higher electronegativity, and the hydrogen atoms will have partial positive charges, resulting in polar covalent bonds.
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