Which of the following acids would be classified as the strongest? 
a) CH₄             b) H₂Te            c) H₂S             d) PH₃             e) BH₃

• A. CH₄
• B. H₂Te
• C. H₂S
• D. PH₃
• E. BH₃

Answer: (B)

Verified step by step guidance

1. Identify the acids given in the problem: CH4, H2Te, H2S, PH3, and BH3.
2. Understand that acid strength generally increases with the ability to donate protons (H+ ions).
3. Consider the electronegativity and size of the central atom bonded to hydrogen in each compound. Strong acids typically have a more electronegative and larger central atom.
4. Locate the central atoms in the periodic table: C (carbon), Te (tellurium), S (sulfur), P (phosphorus), and B (boron). Note that Te is below S in the same group, indicating it is larger and less electronegative.
5. Conclude that H2Te is the strongest acid among the options because tellurium is larger and less electronegative, making it easier to donate H+ ions compared to the other compounds.