Podcast
Questions and Answers
What did the Arrhenius theory propose about acids?
What did the Arrhenius theory propose about acids?
- Acids are substances that accept protons.
- Acids can only exist in aqueous solutions. (correct)
- Acids are substances that can donate protons.
- Acids are only found in gaseous form.
According to the Bronsted-Lowry theory, what defines an acid?
According to the Bronsted-Lowry theory, what defines an acid?
- A substance that accepts protons.
- A substance that forms a cation in solution.
- A substance that can donate a proton. (correct)
- A substance that can only exist in gaseous form.
Which scientist proposed the Bronsted-Lowry theory of acids and bases?
Which scientist proposed the Bronsted-Lowry theory of acids and bases?
- Henrik Bronsted and James Lowry
- Johannes Bronsted and Thomas Lowry (correct)
- Niels Bohr
- Svante Arrhenius
What does the Bronsted-Lowry theory say about bases?
What does the Bronsted-Lowry theory say about bases?
In the reaction: HCl + H2O → H3O+ + Cl-, what role does HCl play?
In the reaction: HCl + H2O → H3O+ + Cl-, what role does HCl play?
What is the chemical formula for ammonia?
What is the chemical formula for ammonia?
Which theory allowed for substances to act both as acids and bases depending on the circumstance?
Which theory allowed for substances to act both as acids and bases depending on the circumstance?
What does the Bronsted-Lowry theory define an acid as?
What does the Bronsted-Lowry theory define an acid as?
In the Lewis theory, what is a Lewis acid?
In the Lewis theory, what is a Lewis acid?
What happens when ammonia (NH3) dissolves in water based on the text?
What happens when ammonia (NH3) dissolves in water based on the text?
Which ion is considered a Lewis acid in the given text?
Which ion is considered a Lewis acid in the given text?
What is formed when silver ion (Ag+) accepts electron pairs from ammonia according to the Lewis theory?
What is formed when silver ion (Ag+) accepts electron pairs from ammonia according to the Lewis theory?
In the Bronsted-Lowry theory, what is a base defined as?
In the Bronsted-Lowry theory, what is a base defined as?
What can be considered as a Lewis base?
What can be considered as a Lewis base?
What differentiates Lewis acids from Arrhenius acids?
What differentiates Lewis acids from Arrhenius acids?
Flashcards
Arrhenius theory of acids
Arrhenius theory of acids
Acids can only exist in aqueous solutions.
Bronsted-Lowry acid
Bronsted-Lowry acid
A substance that donates a proton (H+).
Who proposed the Bronsted-Lowry theory?
Who proposed the Bronsted-Lowry theory?
Johannes Bronsted and Thomas Lowry.
Bronsted-Lowry base
Bronsted-Lowry base
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Role of HCl in: HCl + H2O → H3O+ + Cl-
Role of HCl in: HCl + H2O → H3O+ + Cl-
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Chemical formula for ammonia
Chemical formula for ammonia
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Theory allowing substances to act as both acid and base.
Theory allowing substances to act as both acid and base.
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Bronsted-Lowry acid (defined)
Bronsted-Lowry acid (defined)
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Lewis acid
Lewis acid
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What happens when ammonia dissolves in water?
What happens when ammonia dissolves in water?
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Lewis acid (ion example)
Lewis acid (ion example)
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Product of Ag+ reacting with ammonia
Product of Ag+ reacting with ammonia
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Bronsted-Lowry base (defined)
Bronsted-Lowry base (defined)
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Lewis base
Lewis base
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Lewis vs. Arrhenius acids
Lewis vs. Arrhenius acids
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Study Notes
Arrhenius Acid and Base
- Proposed by Svante Arrhenius in 1887
- An acid is a substance that can give away a hydrogen atom in the form of an ion (H+) when dissolved in water, producing an aqueous acid
- Limitations: only applicable to aqueous solutions, does not account for acids in gaseous form, and substances that can act as both acids and bases
Bronsted-Lowry Acid and Base
- Proposed by Johannes Bronsted and Thomas Lowry in 1923
- An acid is a substance that can donate a proton (hydrogen atom that has lost its electron to become a positively charged ion of H+)
- A base is a substance that accepts protons
- Examples:
- Hydrogen chloride (HCl) dissolving in water, donating a proton to form H3O+ and Cl-
- Ammonia (NH3) accepting a proton from water to form NH4+ and OH-
Conjugate Acids and Bases
- Conjugate acid: an acid that forms when a base gains a proton
- Conjugate base: a base that forms when an acid loses a proton
- Every Bronsted-Lowry acid has a conjugate base, and every Bronsted-Lowry base has a conjugate acid
Lewis Acid and Base
- Proposed by G.N. Lewis in 1923
- An acid is a substance that accepts an electron pair to form a covalent bond
- A base is a substance that donates an electron pair to form a covalent bond
- Examples:
- Silver ion (Ag+) accepting electron pairs from ammonia to form a covalent bond
- Anion donating a pair of electrons to form a covalent bond
Key Points
- All Arrhenius acids and bases are also Bronsted-Lowry acids and bases, but not the opposite
- Bronsted-Lowry acid-base theory is more comprehensive and applicable to a wider range of substances
- Lewis acid-base theory is broader and encompasses substances that don't contain hydrogen at all
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Description
Learn about Johannes Bronsted and Thomas Lowry who developed the Bronsted-Lowry theory of acids and bases as an alternative to the Arrhenius theory. Explore how their theory expands the definition of acids and bases beyond aqueous solutions.
