Single Choice

Which of the following is not a Lewis acid

A$$BF_3$$
Correct Answer
B$$FeCl_3$$
C$$SiF_4$$
D$$C_2H_4$$

Solution

A Lewis acid is defined as an electron-pair acceptor. it can accept a pair of electrons from a Lewis base.
The boron in BF_3 is electron poor and has an empty orbital, so it can accept a pair of electrons, making it a Lewis acid.
FeCl3 is a Lewis acid. because it can accept an electron pair from a Lewis base.
SiF4 can act as a Lewis acid because Si can expand its octet.
C2H4 is CH2=CH2, it has one double bond that means it has pi electrons. It is electron rich. thus, C2H4 is a Lewis base due to availability of electons as a pi bond.
thus, D is the correct answer.

SIMILAR QUESTIONS

Acids, Bases and Salts

Which one of the following is not a base?

Acids, Bases and Salts

The gaseous phase neutralisation reaction can be explained only on the basis of:

Acids, Bases and Salts

Which one of the following is not a Lewis Acid?

Acids, Bases and Salts

Identify the incorrect statement out of the following :

Acids, Bases and Salts

According to the Lewis acid-base concept:

Acids, Bases and Salts

Which of the following is a Lewis acid?

Acids, Bases and Salts

Which of the following fluoro-compounds is most likely to behave as a Lewis base?

Acids, Bases and Salts

Which of these is least likely to act as a Lewis base?

Acids, Bases and Salts

Classify the following species into Lewis acids and Lewis bases and show how these act as Lewis acid/base: (a) $$\displaystyle { OH }^{ - }$$ (b) $$\displaystyle { F }^{ - }$$ (c) $$\displaystyle { H }^{ + }$$ (d) $$\displaystyle { BCl }_{ 3 }$$.

Acids, Bases and Salts

Why does boron triflouride behave as a Lewis acid ?

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