Home
Class 12
CHEMISTRY
Al crystallises in cubic shape unit cell...

Al crystallises in cubic shape unit cell and with edge length 405pm and density 2.7g/cc. Predict the type of crystal lattice.

Text Solution

Verified by Experts

`"Density"=(("No. of atoms")xx("Molecular weight")xx1.67xx10^(-27)"kg")/("Volume of unit cell")`
`2.7xx10^(3)kg//m^(3)=((n)xx27xx1.67xx10^(-27))/((4.05xx10^(-10))^(3))rArrn~4`
Hence, the possible crystal lattice is FCC.
Promotional Banner

Topper's Solved these Questions

  • THE SOLID STATE

    VMC MODULES ENGLISH|Exercise EXAMPLE|20 Videos

  • THE SOLID STATE

    VMC MODULES ENGLISH|Exercise EXERCISE - A|10 Videos

  • THE SOLID STATE

    VMC MODULES ENGLISH|Exercise IMPECCABLE|49 Videos

  • SURFACE CHEMISTRY

    VMC MODULES ENGLISH|Exercise PRACTICE EXERCISE|9 Videos

  • THEORY OF SOLUTIONS

    VMC MODULES ENGLISH|Exercise JEE Advanced (Archive)|31 Videos

Similar Questions

Explore conceptually related problems

Al (atomic mass =27) crystallises in a cubic system with edge length (a) equal to 4Å its density is 2.7 g//cm^(3) The type of the unit cell is:

Suppose the mass of a single Ag atoms is 'm' Ag metal crystallises in fcc lattice with unit cell edge length 'a' The density of Ag metal in terms of 'a' and 'm' is:

Sodium crystallises in a cubic lattice and the edge length of the unit cell is 430 pm. Calculate the number of atoms in the unit cell. (Atomic mass Na = 23 amu, Density of Na = 0.9623 g cm^(-3) )

Zinc selenide, ZnSe, crystallizes in a face-centered cubic unit cell and has a density of 5.267 g/cc. Calculate the edge length of the unit cell.

An element with molar mass 2.7 xx 10^-2 kg mol^(-1) forms a cubic unit cell with edge length 405pm.If its density is 2.7 xx 10^(3) kg^(-3) , what is the nature of the cubic unit cell?

An element with molar mass 27 g mol^(-1) forms a cubic unit cell with edge length 4.05 xx 10^(-8) cm. If its density is 2.7g cm^(-3) , what is the nature of the cubic unit cell?

An element 'X' crystallises as face centred cubic lattice with edge length of 460 pm. The density of the element X, when molar mass of X atom is 60 g mol^(-1) is

Determine the type of cubic lattice to which the iron crystal belongs if its unit cell has an edge length of 286 pm and the density of iron crystals is 7.86g cm^(-3) .

A element crystallises in a bcc structure. The edge length of its unit cell is 288 pm. If the density of the crystal is 7.3 g cm^(-3) , what is the atomic mass of the element ?

A compound AB crystallises in the b.c.c lattice with unit cell edge length of 390 pm. Calculate (a) the distance between the oppsitely charged ions in the lattice. (b) the radius of A^(+) ion if radius of B^(-) ion is 175 pm.

VMC MODULES ENGLISH-THE SOLID STATE-ILLUSTRATIONS
  1. An ionic solid A^(o+)B^(Θ) crystallizes as an bcc structure. The dist...

    Text Solution

    |

  2. Potassium crystallizes in a body centered cubic lattice. What is the a...

    Text Solution

    |

  3. Calculate the packing fraction for the Ca unit cell, given that Ca cry...

    Text Solution

    |

  4. A compound formed by elements A and B crystallizes in cubic structure ...

    Text Solution

    |

  5. NH(4)Cl crystallises in a body centred cubic lattice with a unit cell ...

    Text Solution

    |

  6. A solid A^(+)B^(-) has NaCl type close packed structure. If the anion ...

    Text Solution

    |

  7. Calculate the void space in a primitive unit cell and also the fractio...

    Text Solution

    |

  8. Al crystallises in cubic shape unit cell and with edge length 405pm an...

    Text Solution

    |

  9. CdO has NaCl structures with density 8.27 g//c c .If the ionic radius...

    Text Solution

    |

  10. Gold has a close-packed structure which can be viewed as-spheres occup...

    Text Solution

    |

  11. An element has a bcc structure with a cell edge of 288 pm. The density...

    Text Solution

    |

  12. When heated above 916^(@)C, iron changes, its crystal structure from b...

    Text Solution

    |

  13. Iron occurs as BCC as well as FCC unit cell. If the effective radius o...

    Text Solution

    |

  14. Silver has a cubic unit cell with a cell edge of 408 pm. Its density i...

    Text Solution

    |

  15. The density of solid argon is 1.65g//mL at -233^(@)C . If the argon a...

    Text Solution

    |

  16. An element crystallizes as body - centred cubic lattic. Its density is...

    Text Solution

    |

  17. Calculate the value of Avogadro number from the internuclear distance...

    Text Solution

    |

  18. If all the atoms touching one face plane are removed in solid A^(o+)B^...

    Text Solution

    |

  19. The addition of CaCl(2) crystal to KCl crystal a. Lowers the density...

    Text Solution

    |

  20. If NaCl is dped with 10^(-3) mol % of SrCl(2). What is the concentrati...

    Text Solution

    |