23 Questions
What is a Lewis base according to the Lewis definition?
An electron pair donor
What is the role of water in the reaction with HCl?
It acts as a Lewis base
What is the proton referred to as in the Lewis definition?
A Lewis acid
What is HCl considered a source of?
A Lewis acid
What is the relationship between HCl and H+ in the context of Lewis acid and base?
HCl is a source of a Lewis acid, which is H+
What is a Bronsted-Lowry acid?
A proton donor
What is the most common isotope of a neutral hydrogen atom?
One proton in the nucleus and one electron outside
What is the result of removing an electron from a neutral hydrogen atom?
A positively charged ion
What is the role of the oxygen in the reaction between HCl and water?
It accepts a proton from the HCl
What is the resulting ion when HCl donates a proton to water?
Hydronium ion
What is the charge on the oxygen in the hydronium ion?
+1
What is the resulting ion when HCl loses a proton?
Chloride ion
What is the role of the electron in magenta in the reaction between HCl and water?
It is left behind on the chlorine
What is the charge of the chloride ion in the reaction between HCl and water?
Negative
What is the role of HCl in the reaction between HCl and water?
Bronsted-Lowry acid
What is the difference between the conjugate acid-base pair HCl and Cl-?
One proton
What is the Lewis definition of an acid?
An electron pair acceptor
What is the hybridization of the boron atom in boron trifluoride?
sp2
What is the role of water in the reaction between boron trifluoride and water?
Lewis base
What is the formal charge of the oxygen atom in the product of the reaction between boron trifluoride and water?
+1
Which definition of acid-base reaction applies to the reaction between boron trifluoride and water?
Lewis
What is the role of the empty orbital in the boron atom in boron trifluoride?
Accepting a pair of electrons
What is the difference between the conjugate acid-base pair H2O and H3O+?
One proton
Study Notes
Bronsted-Lowry Definitions
- A Bronsted-Lowry acid is a proton donor, which means it donates an H+.
- A Bronsted-Lowry base is a proton acceptor, which means it accepts an H+.
Proton Explanation
- A proton is the nucleus of a hydrogen atom, which is one proton and one electron.
- When the electron is removed, the nucleus is left with just the proton, denoted as H+.
Acid-Base Reaction Example
- HCl is a Bronsted-Lowry acid, which donates a proton to water.
- Water acts as a Bronsted-Lowry base, accepting the proton.
- The reaction forms the hydronium ion (H3O+) and the chloride anion (Cl-).
Conjugate Acid-Base Pairs
- HCl and Cl- are a conjugate acid-base pair, with a one-proton difference.
- H2O and H3O+ are another conjugate acid-base pair, also with a one-proton difference.
Lewis Definitions
- A Lewis acid is an electron pair acceptor.
- A Lewis base is an electron pair donor.
Lewis Acid-Base Reaction Example
- Boron trifluoride (BF3) is a Lewis acid, which accepts a pair of electrons.
- Water acts as a Lewis base, donating a pair of electrons to form a bond with BF3.
- The reaction forms a bond between the oxygen and boron, with a +1 formal charge on the oxygen and a -1 formal charge on the boron.
Key Points
- The Lewis definition is more broad and can apply to acid-base reactions that don't involve H+.
- The Bronsted-Lowry definition only applies to reactions that involve H+.
- Both definitions can be used to describe the same reaction, but the Lewis definition is more general.
Learn about the definitions and concepts of Bronsted-Lowry acids and bases, including proton donors and acceptors, with a review of what a proton refers to.
Make Your Own Quizzes and Flashcards
Convert your notes into interactive study material.
