Is NF3 an acid or a base?
Nitrogen trifluoride, or
Recall the definitions of acids and bases according to Lewis theory:
- A Lewis acid is an electron lone pair acceptor.
- A Lewis base is an electron lone pair donor.
Now let us observe the structure of the molecule in question, nitrogen trifluoride:
#"NF"_3# has a lone pair of electrons on the central nitrogen atom, giving it a trigonal pyramidal molecular geometry alongside the three#"N - F"# bonds. The molecule is also able to donate this electron pair (such as when it forms the complex tetrafluoroammonium ion,#"NF"_4^+# ).As such nitrogen trifluoride is a base according to Lewis theory. It is not able to accept electron pairs from other species and therefore is not a Lewis acid. This is not a hard-and-fast rule, as some species are capable of acting as both an acid and a base. This is known as amphoterism; water is an example of an amphoteric molecule.
It is very easy to apply Lewis theory to this example, and this theory is much more applicable in general than the alternative Brønsted–Lowry theory that discusses acid-base reactions in terms of the exchange of a proton - or an
#"H"^+# ion - in the process called protonation.
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NF3 is neither an acid nor a base; it is a neutral molecule.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- What is the conjugate acid of #HCO_3^-#?
- Why is there more than one definition of acid–base behavior?
- Consider the titration of #100# #ml# of #0.1# #M# #HCl# with #0.1# #M# #NaOH#. Calculate the #pH# of the solution at the following stages: ?
- What is the #pH# of a solution of #"sulfuric acid"# of #2xx10^-2*mol*L^-1# concentration?
- Why does a strong acid have a weak conjugate base, whereas a weak acid has a relatively strong conjugate base?

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