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Chapter 16: Problem 108

Which of the following is the stronger base: \(\mathrm{NF}_{3}\) or \(\mathrm{NH}_{3} ?\) (Hint: \(\mathrm{F}\) is more electronegative than \(\left.\mathrm{H} .\right)\)

Short Answer

Expert verified
\(\mathrm{NH}_{3}\) is the stronger base.

Step by step solution

01

Understanding Bases and Electronegativity

Bases are substances that can accept protons (H+ ions). The ability of a substance to act as a base is influenced by its electronegativity. Generally, the more electronegative an atom is, the less likely it is to donate an electron pair, hence less likely to act as a base.
02

Comparing Electronegativity

We are given that \(\mathrm{F}\) (Fluorine) is more electronegative than \(\mathrm{H}\) (Hydrogen). This means that \(\mathrm{F}\) is less likely to donate an electron pair compared to \(\mathrm{H}\). Therefore, the base with \(\mathrm{H}\), \(\mathrm{NH}_{3}\), has a higher probability of accepting a proton (H+) and thus behaving as a base.
03

Conclusion

From our analysis, we can deduce that \(\mathrm{NH}_{3}\) is a stronger base than \(\mathrm{NF}_{3}\) since it has atoms that are less electronegative, and hence more likely to donate an electron pair and accept a proton.

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Most popular questions from this chapter

Why do we normally not quote \(K_{\mathrm{a}}\) values for strong acids such as \(\mathrm{HCl}\) and \(\mathrm{HNO}_{3}\) ? Why is it necessary to specify temperature when giving \(K_{\mathrm{a}}\) values?

List four factors that affect the strength of an acid.

What are the Lewis definitions of an acid and a base? In what way are they more general than the Bronsted definitions?

How does the strength of an oxoacid depend on the electronegativity and oxidation number of the central atom?

List the factors on which the \(K_{\mathrm{a}}\) of a weak acid depends.
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