Sodium amide (NaNH 2 ) dissociates to give a sodium cation (Na + ) and amide ion (NH 2 - ) a very strong base. In the following three equations, identify which definition of base is being exemplified. (c)

Welcome back, everyone consider the following reaction of the A ion and determine which definition of base is being demonstrated. Here, we're given a reaction between methyl cyclohexane, one ilium and the amide anion to produce one methyl cycle hex and one amine. Because the problem asks us to determine the definition of base, we have to recall that generally, we have three definitions in chemistry. So we can consider a base as one theory. The next one would be the Bron Laie theory. And the third one that we want to keep in mind is the Lewis theory, right. So in each case, we're considering base. So we have three theories and we want to tell exactly which one is applicable in this case, right. So bases dissociate and a solution to produce hydroxide. So an example would be sodium hydroxide dissociating in water would produce hydroxide. And therefore, it's an aria base. The Bronx theory tells us that bases are protein acceptor. So for example, when ammonia with a lone pair nitrogen gains a proton, it becomes the ammonium ion, right? So, ammonia and H three would be considered a bronze base because it's it can act as a proton acceptor in Lewis theory. However, it's a, a lot about the lone pair. So let's say we also have ammonia and that lone pair of electrons allows us to perform an acid based reaction based on the Lewis theory where base is a lone pair donor. So that lone pair can be incorporated into a free orbital of, let's say boring, right? Because it has a free orbital so boring can act as a lone pair acceptor and we can essentially form an adduct. So we can say we are forming born with a formal negative charge and now nitrogen will have a formal positive charge. So that's an example of a Lewis base where a base acts as a lone pair donor. And that's exactly what we are observing in this reaction. So just in case, let's define the theory, Lewis assets are loan pair acceptor and Louis bases are loan pair donors. In this case, we have our Carbo Canon, which is electron deficient because the Carbo Canon has three bonds and no lone pairs. That means we have a total of six valence electrons. So the carbo Ron lacks two electrons to have a complete and the a an has two lone pairs. Now, what's happening is that the lone pair on nitrogen attacks the carbo ion to form that carbon nitrogen bond. So nitrogen still has one of its lone pairs available, right? It's just not shown, but we can clearly see that the carbo ion is the Lewis acid because it's a long pair acceptor and the is the Lewis base because it's the lone pair donor. Now, the reason why the Bronx theory is not applicable is simply because we don't have any proton transfer, right? The base is a proton acceptor, but we have no proton that we're getting. Uh in other words, nitrogen is not gaining a proton from the acid. So it's not applicable. And for the re theory, it's a lot about dissociation and water. As we previously said, it's a lot about group one a basis. For example, such as sodium hydroxide, dissociating in water to produce hydroxide. Meaning the theory that is applicable here is the loose theory. Simply speaking, the aide and ion is the Lewis base because it's the lone pair donor in the given reaction. Thank you for watching.

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1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

3. Acids and Bases

Acids and Bases

Organic Chemistry

3. Acids and Bases

Acids and Bases

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Problem 7c

Textbook Question

Sodium amide (NaNH₂) dissociates to give a sodium cation (Na⁺) and amide ion (NH₂^-) a very strong base. In the following three equations, identify which definition of base is being exemplified.
(c)

Verified step by step guidance

Step 1: Recall the three main definitions of a base in chemistry: Arrhenius, Bronsted-Lowry, and Lewis. Each definition describes a base differently based on its behavior in a chemical reaction.

Step 2: Analyze the dissociation of sodium amide (NaNH₂) into sodium cation (Na⁺) and amide ion (NH⁻₂). The amide ion (NH⁻₂) is a very strong base. Consider how this ion interacts in the context of the three definitions.

Step 3: For the Arrhenius definition, a base is a substance that increases the concentration of hydroxide ions (OH⁻) in aqueous solution. Sodium amide does not directly produce OH⁻ ions, so this definition may not apply here.

Step 4: For the Bronsted-Lowry definition, a base is a proton acceptor. The amide ion (NH⁻₂) can accept a proton (H⁺) to form ammonia (NH₃), exemplifying the Bronsted-Lowry definition of a base.

Step 5: For the Lewis definition, a base is an electron pair donor. The amide ion (NH⁻₂) has a lone pair of electrons that can be donated to an electron-deficient species, demonstrating the Lewis definition of a base. Evaluate the equations provided to identify which definition is being exemplified in each case.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Brønsted-Lowry Base

A Brønsted-Lowry base is defined as a substance that can accept protons (H⁺ ions) in a chemical reaction. In the context of sodium amide, the amide ion (NH₂⁻) acts as a Brønsted-Lowry base by accepting protons from acids, thereby facilitating various acid-base reactions.

Lewis Base

A Lewis base is defined as a substance that can donate an electron pair to form a covalent bond. The amide ion (NH₂⁻) can also be considered a Lewis base because it has a lone pair of electrons that can be donated to electrophiles, participating in nucleophilic reactions.

Strong Base

A strong base is a substance that completely dissociates in solution to produce hydroxide ions (OH⁻) or other strong anions. Sodium amide is classified as a strong base because it dissociates completely in water to yield the highly reactive amide ion, which can deprotonate weak acids effectively.

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