Q4 TO BE SOLVED ANS IS 2.83 Leader Test Series/Joint Package Course/06-02-2022/Paper-2Paragraph for Questions 3 and 4प्रश्न 3 एवं 4 के लिये अनुच्छेदA cubic unit cell contains Manganese ions at all corners and Fluoride ions at all edge centres.(Given : Molar mass of : Mn = 55gm ; F = 19 gm) [Given : "NA = 6 × 103]एक घनीय इकाई सैल में मैग्नीज आयन सभी कोनो पर तथा फ्लोराइड आयन सभी किनारों के केन्द्रों पर उपस्थित है| a = 64 x 10-12.4.(दिया है : मोलर द्रव्यमान : Mn = 55gm ; F = 19gm) [दिया है : NA = 6 × 103]The density of solid (in gm/cm³) is :-ठोस का घनत्व (gm/cm3 में) है :-4.If radius of Manganese ion is 66 pm and of fluoride ion 134 pm, then what is the shortest distancebetween two fluoride ions.यदि मैग्नीज आयन की त्रिज्या 66 pm तथा फ्लोराइड आयन की त्रिज्या 134 pm है, तो दो फ्लोराइड आयनों के मध्य निकटतम दूरीक्या है ?Space for Rough Work/कच्चे कार्य के लिए स्थान

In this question, we have to find the shortest distance between two fluoride ions.

4. If radius of Manganese ion is 66 pm and of fluoride ion 134 pm, then what is the shortest distance between two fluoride ions. यदि मैग्नीज आयन की त्रिज्या 66 pm तथा फ्लोराइड आयन की त्रिज्या 134 pm है, तो दो फ्लोराइड आयनों के मध्य निकटतम दूरी क्या है ?

4. If radius of Manganese ion is 66 pm and of fluoride ion 134 pm, then what is the shortest distance between two fluoride ions. यदि मैग्नीज आयन की त्रिज्या 66 pm तथा फ्लोराइड आयन की त्रिज्या 134 pm है, तो दो फ्लोराइड आयनों के मध्य निकटतम दूरी क्या है ?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter9: Liquids, Solids, And Materials

Section: Chapter Questions

Problem 121QRT

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The edge length of the unit cell of tantalum metal, Ta, is 330.6 pm; the unit cell is body-centered cubic (one atom at each lattice point). Tantalum has a density of 16.69 g/cm3. What is the mass of a tantalum atom? Use Avogadros number to calculate the atomic mass of tantalum.
Consider the sodium chloride unit cell shown in Figure 9.21. Looking only at the front face (five large Cl- ions, four small Na+ ions), (a) how many cubes share each of the Na+ ions in this face? (b) how many cubes share each of the Cl- ions in this face?
Aluminum metal crystallizes with a face-centered cubic unit cell. The volume of the cell is 0.0662 nm3. (a) What is the atomic radius of aluminum in cm? (b) What is the volume of a single aluminum atom? (c) What is the density of a single aluminum atom? (d) In face-centered cubic cell packing, the fraction of empty space is 26.0%. When this is factored in, what is the calculated density of aluminum?
What is a lattice? What is a unit cell? Describe a simple cubic unit cell. How many net atoms are contained in a simple cubic unit cell? How is the radius of the atom related to the cube edge length for a simple cubic unit cell? Answer the same questions for the body-centered cubic unit cell and for the face-centered unit cell.
The CsCl structure is a simple cubic array of chloride ions with a cesium ion at the center of each cubic array (see Exercise 69). Given that the density of cesium chloride is 3.97 g/cm3, and assuming that the chloride and cesium ions touch along the body diagonal of the cubic unit cell, calculate the distance between the centers of adjacent Cs+ and Cl ions in the solid. Compare this value with the expected distance based on the sizes of the ions. The ionic radius of Cs+ is 169 pm, and the ionic radius of Cl is 181 pm.
In the LiCl structure shown in Figure 9.21, the chloride ions form a face-centered cubic unit cell 0.513 nm on an edge. The ionic radius of Cl- is 0.181 nm. (a) Along a cell edge, how much space is between the Cl- ions? (b) Would an Na+ ion (r=0.095nm) fit into this space? a K+ ion (r=0.133nm)?
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Shown below is the cubic unit cell of an ionic compound. Answer the questions by referring to this structure. Be careful to note that some atoms are hidden by those in front. a One of the spheres (red or green) represents a monatomic, metallic ion. The other color sphere represents a monatomic, nonmetal ion. Which spheres probably represent the metal ion? Explain. b How many red spheres are there in the unit cell? How many green ones? c From the information you have, deduce the general formula of the compound, using M for the metallic element and X for the nonmetallic element. What are the formulas of the ions? d Give an example of a compound that might have this structure. Explain why you think this compound might have this structure. Which ion of this compound would be represented by the red spheres?
A unit cell of cesium chloride is illustrated in Figure 12.8. The density of the solid is 3.99 g/cm3, and the radius of the Cl ion is 181 pm. Calculate the radius of the Cs+ ion in the center of the cell. (Assume that the Cs+ ion touches all of the comer Cl ions.)
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.
Consider the three types of cubic units cells. (a) Assuming that the spherical atoms or ions in a primitive cubic unit cell just touch along the cubes edges, calculate the percentage of occupied space within the unit cell. (Recall that the volume of a sphere is (4/3)r3, where r is the radius of the sphere.) (b) Compare the percentage of occupied space in the primitive cell (pc) with the bcc and fcc unit cells. Based on this, will a metal in these three forms have the same or different densities? If different, in which is it most dense? In which is it least dense?
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