Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN: 9781305079243
Author: Steven S. Zumdahl, Susan A. Zumdahl
Publisher: Cengage Learning
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Chapter 9, Problem 80E

MnO has either the NaCI type structure or the CsCI type structure (see Exercise 69). The edge length of the MnO unit cell is 4.47 × 10-8 cm and the density of MnO is 5.28 g/cm3.

a. Does MnO crystallize in the NaCl or the CsCl type structure?

b. Assuming that the ionic radius of oxygen is 140. pm, estimate the ionic radius of manganese.

Expert Solution & Answer
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Interpretation Introduction

Interpretation:

  • The crystalline structure of MnO whether it is NaCl type or CsCl type has to be identified.
  • The ionic radius of Manganese in MnO has to be determined.

Concept Introduction:

In packing of atoms in a crystal structure, the atoms are imagined as spheres. The two major types of close packing of the spheres in the crystal are – hexagonal close packing and cubic close packing. Cubic close packing forms two types of lattices – body – centered lattice and face – centered lattice.

In body-centered cubic unit cell, each of the six corners is occupied by every single atom. Center of the cube is occupied by one atom. Each atom in the corner is shared by eight unit cells and a single atom in the center of the cube remains unshared. Thus the number of atoms per unit cell in BCC unit cell is,

                      8×18atomsincorners+1atomatthecenter=1+1=2atoms

                    The edge length of one unit cell is given bya=4R3where  a=edge length of unit cellR=radiusofatom.

In face-centered cubic unit cell, each of the six corners is occupied by every single atom. Each face of the cube is occupied by one atom. Each atom in the corner is shared by eight unit cells and each atom in the face is shared by two unit cells. Thus the number of atoms per unit cell in FCC unit cell is,

                8×18atomsincorners+6×12atomsinfaces=1+3=4atoms

                          The edge length of a unit cell is given byl=2R2where  a=edgelength of unit cellR=radius

The edge length of the unit cell containing anion and cation is related to ionic radii as,

l=2rC++2rA-whererC+andrA-areionicradiusofcationandanionrespectively.

Answer to Problem 80E

Answer

MnO has NaCl type structure.

Ionic radius of Manganese ion in MnO is calculated as 83.5 pm.

Explanation of Solution

Explanation

Record the given data.

Given data: edge length of MnO unit cell is 4.47×10-8cm

                     Density of MnO is 5.28 g/cm3

                     Ionic radius of Oxygen is 140pm

The edge length of a MnO unit cell ‘l’ is given. Density of MnO is given. The ionic radius of Oxygen is given.

Determine the mass of a unit cell of MnO crystalline solid.

      Density=massvolume5.28g/cm3=massl3mass=l3×5.28g/cm3=(4.47×10-8cm)3×5.28g/cm3=4.715×1022g

The edge length of the unit cell is known. Using that value the density of the unit cell is calculated using the equation Density=massvolume where cubic value of the edge length gives volume of the unit cell.

Determine the number of formula units per MnO unit cell.

Let ‘n’ be the number of formula units per MnO unit cell.

Then, massofaunitcell=Numberofformulaunits×averagemassofoneformulaunit......(1)

Average mass of one MnOunit=molarmassofMnOAvogadronumber=70.94g6.022×1023=1.18×10-22g......(2)

Substitute (2) in (1). Therefore,

                 4.715×1022g=n×11.8×10-23gn=4.715×1022g1.18×10-22g=3.994

The mass of a unit cell is calculated in the previous step. The average mass of one formula unit is determined using mass of a unit cell. The number of formula units per unit cell is calculated from this. The value obtained is 4. The crystalline structure of NaCl is face -centered cubic. It has 4 units of NaCl per unit cell. So the crystalline structure of MnO also NaCl type that is face – centered cubic.

Determine the ionic radius of Manganese ion in MnO

                 l=2rMn2++2rO2-rO2-=140pm=140×10-12m=1.40×10-8cml=4.47×10-8cm2rMn2+=l-2rO2-=4.47×10-8cm2(1.40×10-8cm)rMn2+=1.67×10-8cm2=0.835×10-8cm=83.5pm

The edge length of the unit cell is related to the ionic radius of ions of a ionic compound as l=2rC++2rA-whererC+andrA-areionicradiusofcationandanionrespectively.

Using the above formula the ionic radius of Manganese is calculated.

Conclusion

Conclusion

The crystalline structure of MnO is ascertained and the ionic radius of Manganese is calculated.

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Chapter 9 Solutions

Chemistry: An Atoms First Approach

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