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Chapter 2: Problem 63

Classify each species as a Lewis acid, a Bronsted-Lowry acid, both, or neither. a. H\(_3\)O\(^+\) b. Cl\(_3\)C\(^+\) c. BCl\(_3\) d. BF\(_4{^-}\)

Short Answer

Expert verified
H extsubscript{3}O extsuperscript{+}: both Lewis and Bronsted-Lowry acid; Cl extsubscript{3}C extsuperscript{+}: Lewis acid; BCl extsubscript{3}: Lewis acid; BF extsubscript{4} extsuperscript{-}: neither.

Step by step solution

01

Identify Lewis Acid

A Lewis acid is a species that can accept an electron pair. Examine each species to see if it has an incomplete octet or a positive charge that allows it to accept electrons.
02

Identify Bronsted-Lowry Acid

A Bronsted-Lowry acid is a species that can donate a proton (H extsuperscript{+}) to another species. Analyze if any of the species contains hydrogen atoms that can be donated.
03

Classify H extsubscript{3}O extsuperscript{+}

Hydronium ion (H extsubscript{3}O extsuperscript{+}) can donate a proton, making it a Bronsted-Lowry acid. As it can also accept an electron pair when it donates a proton to revert to H extsubscript{2}O, it's also a Lewis acid. Thus, it is both a Lewis acid and a Bronsted-Lowry acid.
04

Classify Cl extsubscript{3}C extsuperscript{+}

The carbocation Cl extsubscript{3}C extsuperscript{+} has an incomplete octet and a positive charge, allowing it to accept electrons, thus acting as a Lewis acid. It cannot donate protons, so it is not a Bronsted-Lowry acid. Therefore, it is a Lewis acid.
05

Classify BCl extsubscript{3}

Boron trichloride (BCl extsubscript{3}) has an incomplete octet on the boron and can accept an electron pair, which qualifies it as a Lewis acid. It cannot donate protons as it has no hydrogen atoms, so it is not a Bronsted-Lowry acid. Thus, it is a Lewis acid.
06

Classify BF extsubscript{4} extsuperscript{-}

The tetrafluoroborate anion (BF extsubscript{4} extsuperscript{-}) is a stable species with a complete electron octet and cannot accept an electron pair or donate a proton. Hence, it is neither a Lewis acid nor a Bronsted-Lowry acid.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Lewis Acid
A Lewis acid is essential in acid-base chemistry as it focuses on the ability to accept an electron pair. This type of acid is central in understanding how certain chemical reactions occur.
  • Characteristics: Typical indicators of Lewis acids include the presence of an incomplete octet or a positive charge on the atom.
  • Examples: Boron trichloride (BCl extsubscript{3}) and trichloromethyl cation (Cl extsubscript{3}C extsuperscript{+}) are classic Lewis acids. Their lack of a full electron octet allows them to readily accept electrons from another species.
By recognizing these factors, you can quickly identify whether a molecule qualifies as a Lewis acid or not.
Bronsted-Lowry Acid
The Bronsted-Lowry concept provides insights by defining acids based on their ability to donate protons. This viewpoint shifts the focus from electron pair acceptance to proton donation.
  • Characteristics: A Bronsted-Lowry acid must have at least one hydrogen atom capable of being donated as a proton (H extsuperscript{+}).
  • Examples: Hydronium ion (H extsubscript{3}O extsuperscript{+}) is a typical Bronsted-Lowry acid because it can release a proton to revert to water (H extsubscript{2}O).
This approach emphasizes the role of hydrogen atoms and their contributions to acidic behavior.
Electron Pair Acceptor
The term 'electron pair acceptor' is closely associated with Lewis acids in acid-base chemistry. Understanding this concept clarifies why certain reactions occur.
  • Definition: An electron pair acceptor is any atom or molecule capable of receiving an electron pair, leading to the formation of a new bond.
  • Importance: Recognizing a molecule as an electron pair acceptor explains its reactivity and interaction with other species.
  • Examples: The positive charge in compounds like Cl extsubscript{3}C extsuperscript{+} and the electron-deficient boron in BCl extsubscript{3} make them prime candidates to accept electrons and form bonds.
Grasping this concept aids in visualizing and predicting chemical interactions.
Proton Donor
In the realm of Bronsted-Lowry acids, a proton donor denotes the heart of their definition. Comprehending this concept simplifies the classification of acids within numerous reactions.
  • Definition: A proton donor is any species that can release a proton (H extsuperscript{+}) during a reaction.
  • Role in Reactions: Proton donors play a critical role in initiating reactions by donating hydrogen ions, often forming a new species or compound.
  • Examples: Species like H extsubscript{3}O extsuperscript{+} act as proton donors since they can provide a proton to other substances.
Focusing on proton donation offers a practical method for identifying acids in typical chemical processes.

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Most popular questions from this chapter

Draw the product formed when the Lewis acid (CH\(_3\)CH\(_2)_3C^+\) reacts with each Lewis base: (a) H\(_2\)O; (b) CH\(_3\)OH; (c) (CH\(_3)_2\)O; (d) NH\(_3\); (e) (CH\(_3)_2\)NH.

Rank the following compounds in order of increasing acidity. a. NH\(_3\), H\(_2\)O, HF e. CH\(_3\)OH, CH\(_3\)NH\(_2\), CH\(_3\)CH\(_3\) b. HBr, HCI, HF f. HCI, H\(_2\)O, H\(_2\)S c. H\(_2\)O, H\(_3\)O\(^+\). Ho- g. CH\(_3\)CH\(_2\)CH\(_3\), CICH\(_2\)CH\(_2\)OH, CH\(_3\)CH\(_2\)OH d. NH\(_3\), H\(_2\)O, H\(_2\)S h. HC = CCH\(_2\)CH\(_3\), CH\(_3\)CH\(_2\)CH\(_2\)CH\(_3\), CH\(_3\)CH = CH CH\(_3\)

What is the conjugate base of each acid? a. HCN b. HCO\(_3{^-}\) c. (CH\(_3)_2\)NH\(_2\) d. HC= CH e. CH\(_3\)CH\(_2\)COOH f. CH\(_3\)SO\(_3\)H

Which compounds are Lewis bases? a. NH\(_3\) b. CH\(_3\)CH\(_2\)CH\(_3\) c. H\(^-\) d. H-C =C-H

Explain the apparent paradox. HBr is a stronger acid than HCI, but HOCI is a stronger acid than HOBr.
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