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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 (A2+), while one half of the octahedral voids are occupied by trivalent ions(B3+)What is the formula of the oxide ?
- a)A3B2O4
- b)A2B2O4
- c)AB2O5
- d)AB2O4
Correct answer is option 'C'. Can you explain this answer?
Verified Answer
In a cubic dosed packed structure of mixed oxides, the lattice is made...
Let number of oxides = x Number of octahedral void = x Number of tetrahedral void = 2 x Number of
Hence, formula of oxide is AB2O4.
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Most Upvoted Answer
In a cubic dosed packed structure of mixed oxides, the lattice is made...
Understanding the Structure
In a cubic close-packed (ccp) structure of mixed oxides, the arrangement of ions is crucial for determining the chemical formula.
Ion Occupancy
- Oxide Ions (O2-): The lattice consists of oxide ions occupying the cubic structure.
- Divalent Ions (A2+): One eighth of the tetrahedral voids are occupied by divalent ions (A2+). Since there are 8 tetrahedral voids in a ccp structure, this means:
- Total A2+ ions = 8 * (1/8) = 1 A2+ ion
- Trivalent Ions (B3+): Half of the octahedral voids are occupied by trivalent ions (B3+). There are 4 octahedral voids in a ccp structure, so:
- Total B3+ ions = 4 * (1/2) = 2 B3+ ions
Calculating the Formula
Now, combining the contributions of A2+ and B3+ ions with the oxide ions:
- Oxide Ions (O2-): Each formula unit will need to balance the charges.
Charge Balance
- The total positive charge contributed by A2+ and B3+:
- A2+ contributes a charge of +2 (from 1 A2+ ion) = +2
- B3+ contributes a charge of +6 (from 2 B3+ ions) = +6
- Total positive charge = +2 + +6 = +8
- The total negative charge from oxide ions:
- Each oxide ion contributes -2 charge. Let the number of oxide ions be O.
- Total charge from oxide ions = -2O
To balance the total charges:
- Total positive charge (+8) must equal total negative charge (-2O).
Setting the equation:
+8 = -2O ==> O = 4
Final Formula
Thus, the formula based on the stoichiometry is A1B2O4, which can be simplified to AB2O4.
Therefore, the correct answer is option 'C': AB2O4.
In a cubic close-packed (ccp) structure of mixed oxides, the arrangement of ions is crucial for determining the chemical formula.
Ion Occupancy
- Oxide Ions (O2-): The lattice consists of oxide ions occupying the cubic structure.
- Divalent Ions (A2+): One eighth of the tetrahedral voids are occupied by divalent ions (A2+). Since there are 8 tetrahedral voids in a ccp structure, this means:
- Total A2+ ions = 8 * (1/8) = 1 A2+ ion
- Trivalent Ions (B3+): Half of the octahedral voids are occupied by trivalent ions (B3+). There are 4 octahedral voids in a ccp structure, so:
- Total B3+ ions = 4 * (1/2) = 2 B3+ ions
Calculating the Formula
Now, combining the contributions of A2+ and B3+ ions with the oxide ions:
- Oxide Ions (O2-): Each formula unit will need to balance the charges.
Charge Balance
- The total positive charge contributed by A2+ and B3+:
- A2+ contributes a charge of +2 (from 1 A2+ ion) = +2
- B3+ contributes a charge of +6 (from 2 B3+ ions) = +6
- Total positive charge = +2 + +6 = +8
- The total negative charge from oxide ions:
- Each oxide ion contributes -2 charge. Let the number of oxide ions be O.
- Total charge from oxide ions = -2O
To balance the total charges:
- Total positive charge (+8) must equal total negative charge (-2O).
Setting the equation:
+8 = -2O ==> O = 4
Final Formula
Thus, the formula based on the stoichiometry is A1B2O4, which can be simplified to AB2O4.
Therefore, the correct answer is option 'C': AB2O4.
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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 (A2+), while one half of the octahedral voids are occupied by trivalent ions(B3+)What is the formula of the oxide ?a)A3B2O4b)A2B2O4c)AB2O5 d)AB2O4Correct answer is option 'C'. Can you explain this answer?
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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 (A2+), while one half of the octahedral voids are occupied by trivalent ions(B3+)What is the formula of the oxide ?a)A3B2O4b)A2B2O4c)AB2O5 d)AB2O4Correct answer is option 'C'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about 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 (A2+), while one half of the octahedral voids are occupied by trivalent ions(B3+)What is the formula of the oxide ?a)A3B2O4b)A2B2O4c)AB2O5 d)AB2O4Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 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 (A2+), while one half of the octahedral voids are occupied by trivalent ions(B3+)What is the formula of the oxide ?a)A3B2O4b)A2B2O4c)AB2O5 d)AB2O4Correct answer is option 'C'. Can you explain this answer?.
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