What is the conjugate acid of each of the following bases? [The most basic atom is indicated.]
(a)

Verified step by step guidance

1. Step 1: Identify the base in the given structure. The base is the negatively charged carbon atom (CH₂⁻) in the ethyl anion (CH₃CH₂⁻).
2. Step 2: Recall the concept of conjugate acids and bases. A conjugate acid is formed when a base gains a proton (H⁺).
3. Step 3: Add a proton (H⁺) to the most basic atom, which is the negatively charged carbon atom in this case. This will neutralize the negative charge.
4. Step 4: Write the resulting chemical structure after the proton is added. The ethyl anion (CH₃CH₂⁻) becomes ethane (CH₃CH₃).
5. Step 5: Verify the result by checking that the conjugate acid (CH₃CH₃) is neutral and consistent with the addition of a proton to the base.

Key Concepts

Conjugate Acid-Base Pair

A conjugate acid is formed when a base accepts a proton (H+). In acid-base chemistry, every base has a corresponding conjugate acid, which is the species that results from the base gaining a proton. Understanding this relationship is crucial for predicting the behavior of substances in chemical reactions.

Basicity and Proton Affinity

Basicity refers to the ability of a substance to accept protons. The most basic atom in a molecule is typically the one with the highest electron density and the ability to stabilize the positive charge after accepting a proton. This concept is essential for identifying which atom in a given structure will form the conjugate acid.

Resonance Stabilization

Resonance stabilization occurs when a molecule can be represented by multiple valid Lewis structures, allowing for the delocalization of electrons. This delocalization can significantly affect the stability of the conjugate acid formed from a base, influencing its acidity and basicity. Recognizing resonance structures helps predict the strength of acids and bases.