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The density of chromium metal is 7.2 g c...

The density of chromium metal is 7.2 g `cm^(-3)`. If the unit cell has edge length of 289 pm, determine the type of unit cell. Also, calculate the radius of an atom of chromium. (Atomic mass of chromium = 52 a.m.u.)

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To solve the problem, we will follow these steps: ### Step 1: Understand the given data - Density of chromium (D) = 7.2 g/cm³ - Edge length of the unit cell (a) = 289 pm = 289 x 10⁻¹² m = 289 x 10⁻¹⁰ cm - Atomic mass of chromium (M) = 52 g/mol - Avogadro's number (Nₐ) = 6.022 x 10²³ atoms/mol ...
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Knowledge Check

  • An element occurs in bcc structure. It has a cell edge length of 250 pm. Calculate the molar mass if its density is 8.0 g cm^(-3) . Also calculate the radius of an atom of this element.

    A
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    B
    108. 27 pm
    C
    208.24pm
    D
    108.25 pm

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