Which of the following acids would be classified as the strongest? 

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

Answer: (B)

Verified step by step guidance

1. Identify the acids given: CH\_4, H\_2Te, H\_2S, PH\_3, and BH\_3. These are hydrides of elements from different groups in the periodic table.
2. Recall that acid strength for binary acids (H-A) generally increases down a group in the periodic table because the bond strength between H and A decreases, making it easier to release H\^+ ions.
3. Locate the central atoms of these acids on the periodic table: C (group 14), P (group 15), B (group 13), S (group 16), and Te (group 16). Among these, H\_2Te and H\_2S are hydrides of group 16 elements.
4. Compare the acid strengths of H\_2S and H\_2Te. Since Te is below S in group 16, H\_2Te has a weaker H-Te bond and thus is a stronger acid than H\_2S.
5. Conclude that among the given options, H\_2Te is the strongest acid because it is a hydride of a heavier group 16 element, which leads to greater acidity.