Advertisements
Advertisements
Question
Answer the following in one sentence :
Why cations are Lewis acids?
Advertisements
Solution
Cations are electron-deficient species and can accept an electron pair. Hence, cations are Lewis acids.
APPEARS IN
RELATED QUESTIONS
Answer the following in brief :
What is meant by conjugate acid-base pair?
Label the conjugate acid-base pair in the following reaction:
\[\ce{CO^2-_3 + H2O ⇌ OH- + HCO^-_3}\]
Answer the following in brief :
Write a reaction in which water acts as a base.
Answer the following in brief :
Ammonia serves as a Lewis base whereas AlCl3 is Lewis acid. Explain.
The theory which explain amphoteric nature of water is ______.
Classify the following species into Lewis acids and Lewis bases.
| Cl- | |
| `"NH"_4^+` | |
| BCl3 | |
| NH3 |
The conjugate acid of \[\ce{HSO^-_4}\] is ____________.
Identify the CORRECT statement.
In which oxidation state, group 15 elements act as Lewis base?
According to the Bronsted-Lowry theory, an acid is a substance that ____________.
Conjugate base for Bronsted acids H2O and HF are ___________.
Which of the following fluro compounds is most likely to behave as a Lewis base?
Which of the following can act as Lowry – Bronsted acid as well as base?
Discuss the Lowry – Bronsted concept of acids and bases.
Identify the conjugate acid-base pair for the following reaction in an aqueous solution.
\[\ce{HS^-_{( aq)} + HF ⇌ F^-_{( aq)} + H2S_{(aq)}}\]
Identify the conjugate acid-base pair for the following reaction in an aqueous solution.
\[\ce{HPO^{2-}_4 + SO^{2-}_3 ⇌ PO^{3-}_4 + HSO^-_3}\]
Identify the conjugate acid-base pair for the following reaction in an aqueous solution.
\[\ce{NH^+_4 + CO^{2-}_3 ⇌ NH3 + HCO^-_3}\]
Name one amphoteric solvent.
Which of the following species is amphoteric in nature?
The species which will behave both as conjugate acid and conjugate base is ______.
Define conjugate acid-base pair.
What are the limitations of Arrhenium theory?
According to Lowry-Bronsted concept, base is a substance which acts as ______.
Identify the conjugate acid-base pairs in the reaction,
\[\ce{CH3COOH(aq) + NH3(aq) <=> NH^+_4(aq) + CH3COO^-(aq)}\]
Define acids according to Bronsted-Lowry theory.
