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Question #44127

Difficulty: 8/10 | 🟢 Free

The Question

Consider the following species at standard conditions: Tribromooctoxide (\ce{Br3O8}), Tetrathionate ion (\ce{S4O6^{2-}}), and Carbon suboxide (\ce{C3O2}). Let $x_1, x_2,$ and $x_3$ be the actual oxidation state of an individual central atom in the homonuclear chains of \ce{Br3O8}, \ce{S4O6^{2-}}, and \ce{C3O2}, respectively. Let $y_1, y_2,$ and $y_3$ be the actual oxidation state of an individual terminal atom in the homonuclear chains of the same respective species. Calculate the value of $(x_1 + x_2 + x_3) \times (y_1 + y_2 + y_3)$ .

Options

A.
52
B.
66
C.
84
D.
17

Check Your Answer

Correct Answer

Step-by-Step Solution

Explanation

How the Examiner Thinks

Mechanism_Trap

Don't get tricked by the process! Learn the mechanical traps used in competitive exam questions.

Concepts Behind This Question

Oxidation State Extremes|Average vs. Actual Oxidation State|Bond Angle Variations

Why This Question Is Tricky

Common Mistakes

This question targets the 'Average vs.

Actual Oxidation State' trap.

Students frequently rely on the arithmetic mean formula (e.g., +16/3 for Br in Br3O8 or +2.5 for S in S4O6^2-) without considering the structural reality of homonuclear bonds.

By asking for the specific oxidation states of central vs. terminal atoms, the problem forces the student to draw the correct Lewis structures and assign formal oxidation states based on electronegativity differences, punishing those who assume delocalized or averaged electronic states.

Quick Facts About This Question

Question Information

Subject	Chemistry
Chapter	Redox Reactions - Class 11 Part 2
Concept	Oxidation State Extremes
Difficulty	8
Cognitive Load	7
Target Solve Time	160 sec
Access	Free