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JEE Main & Advanced Sample Paper JEE Main Sample Paper-1

  • question_answer
    In a cubic dosed packed structure of mixed oxides, the lattice is made up of oxide ions, one eighth of tetrahedral/voids are occupied by divalent ions \[({{A}^{2+}})\], while one half of the octahedral voids are occupied by trivalent ions\[({{B}^{3+}})\]What is the formula of the oxide ?

    A) \[{{A}_{3}}{{B}_{2}}{{O}_{4}}\]                  

    B) \[{{A}_{2}}{{B}_{2}}{{O}_{4}}\]

    C) \[A{{B}_{2}}{{O}_{5}}\]                 

    D) \[A{{B}_{2}}{{O}_{4}}\]

    Correct Answer: D

    Solution :

     Let number of oxides = x Number of octahedral void = x Number of tetrahedral void = 2 x Number of \[{{A}^{2+}}\]ion \[=\frac{1}{8}.2x=\frac{x}{4}\] Number of \[{{B}^{3+}}\] ion \[=\frac{x}{2}\] \[\begin{matrix} {{A}^{2+}}: & {{B}^{3+}}: & {{O}^{2-}}  \\    \frac{x}{4}: & \frac{x}{2}: & x  \\    1 & 2 & 4  \\ \end{matrix}\] Hence, formula of oxide is \[A{{B}_{2}}{{O}_{4}}.\]


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