The pesticide Heptaclor can be synthesized using perchlorocyclopenta-1,3-diene and another five-membered-ring. Prove that Heptaclor is composed of these two rings.

What product(s) are expected from the following arrow-pushing formalism?

Show the mechanism of the following reaction using curved arrows.

Determine the type of each of the arrows displayed in the following arrow-pushing mechanism.

Type I: nucleophilic attack by a lone pair of electrons

Type II: heterolytic cleavage of a σ bond

Type III: nucleophilic attack by the π electrons

Type IV: dissociation of a π bond

Type V: formation of a π bond

Determine the identity of products that are formed in the reaction between each of the species given below with CH₃O⁻.
(i) CH₃CH₂OH
(ii) CH₃NH₃⁺

Consider the following acid-base reaction:

NH₃ + BF₃ ⇌ H₃N⁺—BF₃⁻

1. For all the reactants and products, draw Lewis structures.
2. Identify the nucleophile (base) and electrophile (acid) in the reaction.
3. Draw curved arrows to show the flow of electrons.
4. Determine if the reaction can be termed a Brønsted-Lowry acid-base reaction.

Consider the below-given reaction and answer each of the following questions.

(a) Which reactant is the acid, and which one is the base?

(b) Which is the most acidic proton in the acid?

(c) Which is the most electron-rich atom in the base?

Give an approximate pK_a value for each of the following acids using their  K_a values below:

1. Hydroiodic acid (HI), K_a = 3.2 × 10⁹

2. Ethanoic acid (CH ₃COOH), K_a = 1.8 × 10^-5

3. Oxalic acid (HO ₂C₂O₂H), K_a = 5.4 × 10^-2

4. Boric acid (H ₃BO₃), K_a = 5.8 × 10^-10

5. Carbonic acid (H ₂CO₃), K_a = 4.4 × 10^-7

6. Benzoic acid (C ₆H₅COOH), K_a = 6.3 × 10^-5

Calculate the K_eq (equilibrium constant) of the reaction given below.

Given the pK_a values, find the equilibrium constant K_eq (in 1 sig. fig.) for the following acid-base reaction: