Questions: Question 33 of 39 Consider the following two compounds. Which of the compounds is more acidic? Compound A Compound B Which factor applies here? Induction Resonance Orbital Atom Bearing a Charge

Question 33 of 39 Consider the following two compounds. Which of the compounds is more acidic? Compound A Compound B Which factor applies here? Induction Resonance Orbital Atom Bearing a Charge
Transcript text: Question 33 of 39 Consider the following two compounds. Which of compounds is more acidic? Compound $A$ Compound B Which factor applies here? Induction Resonance Orbital Atom Bearing a Charge
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Solution

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Solution Steps

Step 1: Comparing Acidity

Compound A is more acidic than Compound B. Acidity increases as you go down the periodic table within a group. Sulfur is below oxygen on the periodic table, and since the sulfur atom is larger than the oxygen atom, the negative charge is more stabilized on the sulfur, making it a weaker base, and consequently, Compound A (with the SH group) a stronger acid.

Step 2: Identifying the Relevant Factor

The factor that explains the difference in acidity is the orbital in which the negative charge resides after deprotonation.

Final Answer:

Compound A is more acidic due to orbital effects.

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