Problem 1 a. Which compounds are Br0nsted-... [FREE SOLUTION]

Chapter 2: Problem 1

a. Which compounds are Br0nsted-Lowry acids: HBr, NH\(_3\) , CCl\(_4\)? b. Which compounds are Br0nsted-Lowry bases: CH\(_3\)CH\(_3\), (CH\(_3)_3\)CO\(^-\), HC =CH? c. Classify each compound as an acid, a base, or both: CH\(_3\)CH\(_2\)OH, CH\(_3\)CH\(_2\)CH\(_2\)CH\(_3\), CH\(_3\)CO\(_2\)CH\(_3\).

Short Answer

Expert verified

a) HBr is the Br酶nsted-Lowry acid. b) (CH鈧�)鈧僀O鈦� is the Br酶nsted-Lowry base. c) CH鈧僀H鈧侽H is both an acid and a base; others are neither.

Step by step solution

Understanding Br酶nsted-Lowry Acids

A Br酶nsted-Lowry acid is defined as a substance that can donate a proton (H鈦� ion). We need to analyze the given compounds: HBr, NH鈧�, CCl鈧�, to determine which can donate a proton. HBr is a well-known strong acid that readily donates a proton. NH鈧�, ammonia, usually acts as a base but does not donate a proton. CCl鈧�, carbon tetrachloride, does not have any hydrogen to donate, so it cannot act as a Br酶nsted-Lowry acid.

Identifying Br酶nsted-Lowry Bases

A Br酶nsted-Lowry base is a substance that can accept a proton. Let's evaluate the given compounds: CH鈧僀H鈧�, (CH鈧�)鈧僀O鈦�, HC鈮H. Ethane (CH鈧僀H鈧�) is a hydrocarbon and does not typically accept protons. The (CH鈧�)鈧僀O鈦� ion is a known base because it can accept protons to form (CH鈧�)鈧僀OH. HC鈮H, acetylene, can also act as a base in certain conditions where it's willing to accept a proton, but in typical conditions, it is considered acidic.

Classifying Provided Compounds as Acid, Base, or Both

For CH鈧僀H鈧侽H (ethanol), it can donate an H鈦� which classifies it as an acid, although weak, and can also accept H鈦� in certain situations acting as a weak base - thus can be considered both under certain reactions. CH鈧僀H鈧侰H鈧侰H鈧� (butane) is a saturated hydrocarbon and is neither an acid nor a base. CH鈧僀O鈧侰H鈧� (methyl acetate) does not readily donate or accept protons and is neither an acid nor a base in typical conditions.

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Key Concepts

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

Proton Donation

In the Br酶nsted-Lowry Acid-Base Theory, proton donation is an essential characteristic of acids. An acid is defined as a substance that donates a proton, or H鈦� ion, to another substance. This act of donating a proton classifies a compound as an acid. For example:

HBr (hydrogen bromide) is considered a strong Br酶nsted-Lowry acid. It readily donates its proton to other molecules, making it an effective proton donor.
CCl鈧� (carbon tetrachloride) and NH鈧� (ammonia) do not act as Br酶nsted-Lowry acids, as they do not donate protons. CCl鈧� can't donate protons because it lacks hydrogen atoms, while NH鈧� typically acts as a base.

This concept helps us differentiate acids in chemical reactions, especially when analyzing molecular interactions and predicting reaction outcomes.

Proton Acceptance

Proton acceptance is a key feature of bases in the Br酶nsted-Lowry theory. A base is defined as a substance that can accept a proton from an acid. When looking at base behavior under this theory:

The (CH鈧�)鈧僀O鈦� ion is a common example of a base because it eagerly accepts protons, forming (CH鈧�)鈧僀OH. This proton acceptance confirms its role as a Br酶nsted-Lowry base.
Acetylene (HC鈮H) can occasionally act as a base under specific conditions, but in neutral states, it's recognized as slightly acidic instead.
Conversely, CH鈧僀H鈧� (ethane) lacks the ability to accept protons, making it a non-base under typical circumstances.

Understanding proton acceptance is crucial for classifying bases and determining their reactivity with acids in different chemical environments.

Acid-Base Classification

Classifying substances as acids, bases, or both is integral in understanding their chemical roles. Br酶nsted-Lowry theory simplifies this classification based on proton donation and acceptance:

CH鈧僀H鈧侽H (ethanol) is an interesting example as it can both donate and accept protons. Due to its dual ability, it's considered both an acid and a base depending on the reaction conditions.
Butane (CH鈧僀H鈧侰H鈧侰H鈧�) is neither an acid nor a base as it doesn鈥檛 exhibit typical proton donating or accepting behavior. It represents a class of compounds known as hydrocarbons, neutral in acid-base terms.
Methyl acetate (CH鈧僀O鈧侰H鈧�) does not tend to participate in acid-base reactions under standard conditions, acting as neither an effective acid nor base.

This classification is vital in predicting how substances will interact in various chemical environments and reactions.

Organic Acids

Organic acids are characterized by having a hydrogen atom that can be donated as a proton. They usually contain a carboxylic group, R-COOH, which is responsible for their acidic behavior:

Acids like acetic acid (CH鈧僀OOH) illustrate this concept well, as they readily donate a proton from the carboxylic group.
In the context of Br酶nsted-Lowry, we see that compounds like ethanol (CH鈧僀H鈧侽H) can act as weak acids, depending on conditions, by donating their hydrogen as a proton.

Organic acids play a significant role in both natural processes and industrial applications, making the understanding of their proton-donating capability important for practical uses and chemical synthesis.

Organic Bases

Organic bases commonly contain nitrogen atoms or lone pairs of electrons, which facilitate the acceptance of protons:

Amine groups (found in compounds like NH鈧�, ammonia) are classic examples of organic bases. They can accept protons, forming ammonium ions (NH鈧勨伜).
Compounds such as (CH鈧�)鈧僀O鈦� also demonstrate base behavior by accepting protons to turn into their corresponding alcohol forms.
It鈥檚 important to note that not all organic compounds can act as bases. For example, hydrocarbons such as ethane (CH鈧僀H鈧�) do not exhibit proton accepting properties.

Understanding the basicity of different organic compounds helps in designing chemical reactions and developing new organic syntheses.

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a. Which compounds are Br0nsted-Lowry acids: HBr, NH\(_3\) , CCl\(_4\)? b. Which compounds are Br0nsted-Lowry bases: CH\(_3\)CH\(_3\), (CH\(_3)_3\)CO\(^-\), HC =CH? c. Classify each compound as an acid, a base, or both: CH\(_3\)CH\(_2\)OH, CH\(_3\)CH\(_2\)CH\(_2\)CH\(_3\), CH\(_3\)CO\(_2\)CH\(_3\).

Short Answer

Step by step solution

Understanding Br酶nsted-Lowry Acids

Identifying Br酶nsted-Lowry Bases

Classifying Provided Compounds as Acid, Base, or Both

Key Concepts

Proton Donation

Proton Acceptance

Acid-Base Classification

Organic Acids

Organic Bases

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