The two types of bonds in the N2H4 molecule are found between Nitrogen and Nitrogen, and Nitrogen and Hydrogen. By using the elements’ electronegativity values and finding the difference between the two elements’ values, the type of bond can be determined.
N N N H
3.0 3.0 3.0 2.2
0 .8
Absolutely covalent Moderately covalent
Non-polar Polar
Because the N-N bond has an electronegativity difference of 0, the bond is absolutely covalent. Also, it is a non-polar bond because N and N have the same electronegativity value.
Because the N-H bond has an electronegativity difference of .8, the bond is moderately covalent. A polar bond occurs because one atom's electronegativity value has a larger electronegativity value than the other atom. In this case, the N atom has a larger electronegativity value than H, making the N-H bond polar.
Because the N-N bond has an electronegativity difference of 0, the bond is absolutely covalent. Also, it is a non-polar bond because N and N have the same electronegativity value.
Because the N-H bond has an electronegativity difference of .8, the bond is moderately covalent. A polar bond occurs because one atom's electronegativity value has a larger electronegativity value than the other atom. In this case, the N atom has a larger electronegativity value than H, making the N-H bond polar.
To determine the nature of each bond, use this value line. The values on this line represents the differences between the bond's elements' electronegativity values.
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