3 55 points previous answers ncsugenchem102labv1

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3.5/5 points |Previous AnswersNCSUGenChem102LabV1 6.POST.03.Many metals pack in cubic unit cells. The density of a metal and length of the unit cell can be used to determine thetype for packing. For example,ironhas a density of7.87g/cm3and a unit cell side lengthaof2.87. (11.10-8cm.)(a) How manyironatoms are in exactly 1 cm3=?
(b) How many unit cells are in exactly 1 cm3?
(c) How manyironatoms are there per unit cell?
(d) The atoms/unit cell suggests thatironpacks as abody-centeredbody-centeredunit cell.Knowledge of the type of packing and side lengthaof the unit cell will allow calculation of the atomic radius, usingone of the equations below. You may need to draw the unit cell to determine which formula to use to calculate theatomic radius.(e) What is the atomic radius ofiron?1.241.24Additional Materials
Solid State Modeling4.5/5 points |Previous AnswersNCSUGenChem102LabV1 6.POST.04.Green checksandred X'sare not displayed for this question.Use what you learned in lab about atoms in cubic structures to answer the following questions about a solid whosecrystal structure was found to have atoms "A" incorner and center sitesand "B" in theface sitesof a cubic unit cell.How many "A"s are there in a unit cell?22"A"(s)How many "B"s are there in a unit cell?33"B"(s)

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Term
Fall
Professor
CHRIS
Tags
Cubic crystal system, Diamond cubic, Crystal system, Atomic packing factor

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