Question

Identify the Lewis acid and Lewis base in each reaction:
(a) $Fe_3^+ + 2H_2O \leftrightarrow FeOH_2^++ H_3O^+ Lewis Acid , Lewis Base$
(b) $H_2O + H^- \leftrightarrow H_2 + OH^- Lewis Acid , Lewis Base$
(c) $4CO^+ Ni \leftrightarrow Ni(CO)_4 Lewis Acid , Lewis Base$

Answer 1

Answer:

Explanation:

A Lewis acid is defined as a chemical species that contains an empty orbital which accepts an electron pair from a Lewis base to.

A Lewis base is defined as any species that has a filled orbital containing an electron pair which is not involved in bonding but forms a dative bond with a Lewis acid.

A. Fe3+ + 2H2O --> FeOH2+ + H30+

Fe3+ - Lewis acid

H2O - Lewis base

B. H2O + H- --> H2 + OH-

H- - Lewis acid

H2O - Lewis base

C. 4CO + Ni --> Ni(CO)4

CO - Lewis base

Ni - Lewis acid

Answer 2

Answer:

The answers to the question are

(a)

• Fe₃⁺ = Lewis acid

• H₂O = Lewis base

(b)

• H₂O = Lewis acid

• H⁻ = Lewis base

(c)

• CO⁺ = Lewis acid

• Ni = Lewis base

Explanation:

Lewis theory of acids states that

An acid is a substance that accepts a pair of electrons an i doing so forms a covalent bond with the group that supplies the electrons

A Lewis base is a substance that donates an unshared pair of electrons to a recipient species with which the  electrons can be shared

(a) Here Fe₃⁺ is the Lewis acid as it accepts an electron pair from H₂O which is amphoteric an so can act either as a Lewis base or acid

Fe₃⁺ = Lewis acid

H₂O = Lewis base

(b) H₂O + H⁻ → H₂ + OH⁻

Here the water accepts a pair of electrons from H⁻ anion hence it is the Lewis acid while H⁻ anion donates a pair of electrons acting as the Lewis base

H₂O = Lewis acid

H⁻ = Lewis base

(c) 4CO⁺ +Ni ↔ Ni(CO₄) Here we have

CO⁺ = Lewis acid

Ni = Lewis base