Single Choice

According to Lewis concept, an acid is a/an:

Aproton donor
Belectron pair donor
Cproton acceptor
Delectron pair acceptor.
Correct Answer

Solution

Lewis acids accept an electron pair. Lewis Acids are electrophilic meaning that they are electron attracting. When bonding with a base the acid uses its lowest unoccupied molecular orbital or LUMO.
• Various species can act as Lewis acids. All cations are Lewis acids since they are able to accept electrons. (e.g.,$$ Cu^{2+}, Fe^{2+}, Fe^{3+}$$)
• An atom, ion, or molecule with an incomplete octet of electrons can act as a Lewis acid (e.g.,$$ BF_3, AlF_3$$).
• Molecules where the central atom can have more than 8 valence shell electrons can be electron acceptors, and thus are classified as Lewis acids (e.g., $$SiBr_4, SiF_4$$).
• Molecules that have multiple bonds between two atoms of different electronegativities (e.g., $$CO_2, SO_2$$)

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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