A Lewis acid is any species that can accept a pair of electrons. A Lewis base is a species that can donate a pair of electrons to an electron acceptor. The bond formed in a Lewis acid/base reaction is called acoordinate covalent bond.
Background and Theory
Before delving into the specifics of the Lewis acid/base reaction, let's back up a bit, all the way to the Bronsted-Lowry Acid-Base theory. This theory focuses on acids and bases acting as proton donors and acceptors. However, this theory is very restrictive and sometimes doesn't adequately explain reactions, such as in solids and gases.
In 1923, G.N. Lewis proposed an alternative theory to describe acids and bases. His theory gave us an explanation of acids and bases based on structure and bonding. Through the use of the Lewis definition of acids and bases, chemists are now able to predict a wider variety of acid-base reactions. Lewis' theory used electrons instead of proton transfer and specifically stated that an acid is a species that accepts an electron pair while a base donates an electron pair.
The reaction of a Lewis acid and a Lewis base produces a coordinate covalent bond. You will often see a coordinate covalent bond shown as an arrow instead of a line in a Lewis structure. The arrow points from the donor atom to the acceptor atom.
A coordinate covalent bond is just a type of covalent bond in which one reactant gives its electron pair to another reactant. In this case, the Lewis base donates its electrons to the Lewis acid. The resulting product of this reaction is called an addition compound or more commonly, an adduct.
Lewis Acids
Various species can act as Lewis acids. Allcations are Lewis acids since they are able to accept electrons. Examples include copper (Cu2), iron (Fe2+ and Fe3+), and hydrogen ion (H+). An atom, ion, or molecule with an incomplete octet of electrons can accept electrons. Examples include boron trifluoride (BF3) and aluminum fluoride (AlF3).
Answers & Comments
Acid :- The compound which accepts a pair of electrons .
Base :- The compound which donates the pair if electron
A/c to bronsted- lowry concept :-
Acid :- The compound which donates H+ ions .
Base :- The compound which accepts H+ ions .
A/c to Arrehinus concept :-
Acid :- The compound which releases H+/H3O+ ions in its aq .
Base :- The compound which releases OH- ions in it's aq .
A Lewis acid is any species that can accept a pair of electrons. A Lewis base is a species that can donate a pair of electrons to an electron acceptor. The bond formed in a Lewis acid/base reaction is called acoordinate covalent bond.
Background and Theory
Before delving into the specifics of the Lewis acid/base reaction, let's back up a bit, all the way to the Bronsted-Lowry Acid-Base theory. This theory focuses on acids and bases acting as proton donors and acceptors. However, this theory is very restrictive and sometimes doesn't adequately explain reactions, such as in solids and gases.
In 1923, G.N. Lewis proposed an alternative theory to describe acids and bases. His theory gave us an explanation of acids and bases based on structure and bonding. Through the use of the Lewis definition of acids and bases, chemists are now able to predict a wider variety of acid-base reactions. Lewis' theory used electrons instead of proton transfer and specifically stated that an acid is a species that accepts an electron pair while a base donates an electron pair.
The reaction of a Lewis acid and a Lewis base produces a coordinate covalent bond. You will often see a coordinate covalent bond shown as an arrow instead of a line in a Lewis structure. The arrow points from the donor atom to the acceptor atom.
A coordinate covalent bond is just a type of covalent bond in which one reactant gives its electron pair to another reactant. In this case, the Lewis base donates its electrons to the Lewis acid. The resulting product of this reaction is called an addition compound or more commonly, an adduct.
Lewis Acids
Various species can act as Lewis acids. Allcations are Lewis acids since they are able to accept electrons. Examples include copper (Cu2), iron (Fe2+ and Fe3+), and hydrogen ion (H+). An atom, ion, or molecule with an incomplete octet of electrons can accept electrons. Examples include boron trifluoride (BF3) and aluminum fluoride (AlF3).
This is may be correct answer