Further, in AFD, as per Pythagoras theorem. For every circle, there is one pointing towards the left and the other one pointing towards the right. 6.11B: Structure - Caesium Chloride (CsCl) - Chemistry LibreTexts This colorless salt is an important source of caesium ions in a variety of niche applications. One of our favourite carry on suitcases, Antler's Clifton case makes for a wonderfully useful gift to give the frequent flyer in your life.The four-wheeled hardcase is made from durable yet lightweight polycarbonate, and features a twist-grip handle, making it very easy to zip it around the airport at speed. Click 'Start Quiz' to begin! Now correlating the radius and its edge of the cube, we continue with the following. directions. Though each of it is touched by 4 numbers of circles, the interstitial sites are considered as 4 coordinates. Advertisement Remove all ads. The determination of the mass of a single atom gives an accurate nitrate, carbonate, azide) All atoms are identical. Example 2: Calculate Packing Efficiency of Face-centered cubic lattice. Solution Verified Create an account to view solutions Recommended textbook solutions Fundamentals of Electric Circuits 6th Edition ISBN: 9780078028229 (11 more) Charles Alexander, Matthew Sadiku 2,120 solutions Particles include atoms, molecules or ions. So, if the r is the radius of each atom and a is the edge length of the cube, then the correlation between them is given as: a simple cubic unit cell is having 1 atom only, unit cells volume is occupied with 1 atom which is: And, the volume of the unit cell will be: the packing efficiency of a simple unit cell = 52.4%, Eg. The Attempt at a Solution I have obtained the correct answer for but I am not sure how to explain why but I have some calculations. It is the entire area that each of these particles takes up in three dimensions. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. As per our knowledge, component particles including ion, molecule, or atom are arranged in unit cells having different patterns. Density of Different Unit Cells with Solved Examples. - Testbook Learn Since a simple cubic unit cell contains only 1 atom. There is no concern for the arrangement of the particles in the lattice as there are always some empty spaces inside which are called void spaces. The fraction of void space = 1 - Packing Fraction % Void space = 100 - Packing efficiency. Also, 3a=4r, where a is the edge length and r is the radius of atom. I think it may be helpful for others also!! See Answer See Answer See Answer done loading No Board Exams for Class 12: Students Safety First! Use Coupon: CART20 and get 20% off on all online Study Material, Complete Your Registration (Step 2 of 2 ), Sit and relax as our customer representative will contact you within 1 business day, Calculation Involving Unit Cell Dimensions. We convert meters into centimeters by dividing the edge length by 1 cm/10-2m to the third power. There is one atom in CsCl. Simple cubic unit cell has least packing efficiency that is 52.4%. , . Therefore body diagonalc = 4r, Volume of the unit cell = a3= (4r / 3)3= 64r3 / 33, Let r be the radius of sphere and a be the edge length of the cube, In fcc, the corner spheres are in touch with the face centred sphere. The steps below are used to achieve Face-centered Cubic Lattices Packing Efficiency of Metal Crystal: The corner particles are expected to touch the face ABCDs central particle, as indicated in the figure below. Packing efficiency is the fraction of a solids total volume that is occupied by spherical atoms. Many thanks! as illustrated in the following numerical. To read more,Buy study materials of Solid Statecomprising study notes, revision notes, video lectures, previous year solved questions etc. If any atom recrystalizes, it will eventually become the original lattice. Packing Efficiency: Structure, Types & Diagram - Collegedunia Coordination number, also called Ligancy, the number of atoms, ions, or molecules that a central atom or ion holds as its nearest neighbours in a complex or coordination compound or in a crystal. Since the edges of each unit cell are equidistant, each unit cell is identical. unit cell dimensions, it is possible to calculate the volume of the unit cell. Packing Efficiency of Face CentredCubic Question 3: How effective are SCC, BCC, and FCC at packing? Put your understanding of this concept to test by answering a few MCQs. Thus 26 % volume is empty space (void space). Atomic coordination geometry is hexagonal. in the lattice, generally of different sizes. Concepts of crystalline and amorphous solids should be studied for short answer type questions. Simple cubic unit cells only contain one particle. Required fields are marked *, Numerical Problems on Kinetic Theory of Gases. Question no 2 = Ans (b) is correct by increasing temperature This video (CsCl crystal structure and it's numericals ) helpful for entrances exams( JEE m. CsCl is more stable than NaCl, for it produces a more stable crystal and more energy is released. Which unit cell has the highest packing efficiency? We can calculate the mass of the atoms in the unit cell. And so, the packing efficiency reduces time, usage of materials and the cost of generating the products. They have two options for doing so: cubic close packing (CCP) and hexagonal close packing (HCP). Simple, plain and precise language and content. Polonium is a Simple Cubic unit cell, so the equation for the edge length is. The constituent particles i.e. The cubic closed packing is CCP, FCC is cubic structures entered for the face. The centre sphere of the first layer lies exactly over the void of 2ndlayer B. Select the correct answer and click on the Finish buttonCheck your score and answers at the end of the quiz, Visit BYJUS for all Chemistry related queries and study materials, Your Mobile number and Email id will not be published. To determine this, the following equation is given: 8 Corners of a given atom x 1/8 of the given atom's unit cell = 1 atom. What is the packing efficiency in SCC? The packing efficiency of simple cubic lattice is 52.4%. Lattice(BCC): In a body-centred cubic lattice, the eight atoms are located on the eight corners of the cube and one at the centre of the cube. Sodium (Na) is a metallic element soluble in water, where it is mostly counterbalanced by chloride (Cl) to form sodium chloride (NaCl), or common table salt. The packing efficiency is the fraction of space that is taken up by atoms. P.E = ( area of circle) ( area of unit cell) Common Structures of Binary Compounds. Find many great new & used options and get the best deals for TEKNA ProLite Air Cap TE10 DEV-PRO-103-TE10 High Efficiency TransTech aircap new at the best online prices at eBay! So, 7.167 x 10-22 grams/9.265 x 10-23 cubic centimeters = 7.74 g/cm3. Question 3:Which of the following cubic unit cell has packing efficiency of 64%? Its packing efficiency is about 52%. The packing Although it is not hazardous, one should not prolong their exposure to CsCl. For determining the packing efficiency, we consider a cube with the length of the edge, a face diagonal of length b and diagonal of cube represented as c. In the triangle EFD, apply according to the theorem of Pythagoras. It is stated that we can see the particles are in touch only at the edges. It shows the different properties of solids like density, consistency, and isotropy. Both hcp & ccp though different in form are equally efficient. !..lots of thanks for the creator The volume of the unit cell will be a3 or 2a3 that gives the result of 8a3. NCERT Solutions Class 12 Business Studies, NCERT Solutions Class 12 Accountancy Part 1, NCERT Solutions Class 12 Accountancy Part 2, NCERT Solutions Class 11 Business Studies, NCERT Solutions for Class 10 Social Science, NCERT Solutions for Class 10 Maths Chapter 1, NCERT Solutions for Class 10 Maths Chapter 2, NCERT Solutions for Class 10 Maths Chapter 3, NCERT Solutions for Class 10 Maths Chapter 4, NCERT Solutions for Class 10 Maths Chapter 5, NCERT Solutions for Class 10 Maths Chapter 6, NCERT Solutions for Class 10 Maths Chapter 7, NCERT Solutions for Class 10 Maths Chapter 8, NCERT Solutions for Class 10 Maths Chapter 9, NCERT Solutions for Class 10 Maths Chapter 10, NCERT Solutions for Class 10 Maths Chapter 11, NCERT Solutions for Class 10 Maths Chapter 12, NCERT Solutions for Class 10 Maths Chapter 13, NCERT Solutions for Class 10 Maths Chapter 14, NCERT Solutions for Class 10 Maths Chapter 15, NCERT Solutions for Class 10 Science Chapter 1, NCERT Solutions for Class 10 Science Chapter 2, NCERT Solutions for Class 10 Science Chapter 3, NCERT Solutions for Class 10 Science Chapter 4, NCERT Solutions for Class 10 Science Chapter 5, NCERT Solutions for Class 10 Science Chapter 6, NCERT Solutions for Class 10 Science Chapter 7, NCERT Solutions for Class 10 Science Chapter 8, NCERT Solutions for Class 10 Science Chapter 9, NCERT Solutions for Class 10 Science Chapter 10, NCERT Solutions for Class 10 Science Chapter 11, NCERT Solutions for Class 10 Science Chapter 12, NCERT Solutions for Class 10 Science Chapter 13, NCERT Solutions for Class 10 Science Chapter 14, NCERT Solutions for Class 10 Science Chapter 15, NCERT Solutions for Class 10 Science Chapter 16, NCERT Solutions For Class 9 Social Science, NCERT Solutions For Class 9 Maths Chapter 1, NCERT Solutions For Class 9 Maths Chapter 2, NCERT Solutions For Class 9 Maths Chapter 3, NCERT Solutions For Class 9 Maths Chapter 4, NCERT Solutions For Class 9 Maths Chapter 5, NCERT Solutions For Class 9 Maths Chapter 6, NCERT Solutions For Class 9 Maths Chapter 7, NCERT Solutions For Class 9 Maths Chapter 8, NCERT Solutions For Class 9 Maths Chapter 9, NCERT Solutions For Class 9 Maths Chapter 10, NCERT Solutions For Class 9 Maths Chapter 11, NCERT Solutions For Class 9 Maths Chapter 12, NCERT Solutions For Class 9 Maths Chapter 13, NCERT Solutions For Class 9 Maths Chapter 14, NCERT Solutions For Class 9 Maths Chapter 15, NCERT Solutions for Class 9 Science Chapter 1, NCERT Solutions for Class 9 Science Chapter 2, NCERT Solutions for Class 9 Science Chapter 3, NCERT Solutions for Class 9 Science Chapter 4, NCERT Solutions for Class 9 Science Chapter 5, NCERT Solutions for Class 9 Science Chapter 6, NCERT Solutions for Class 9 Science Chapter 7, NCERT Solutions for Class 9 Science Chapter 8, NCERT Solutions for Class 9 Science Chapter 9, NCERT Solutions for Class 9 Science Chapter 10, NCERT Solutions for Class 9 Science Chapter 11, NCERT Solutions for Class 9 Science Chapter 12, NCERT Solutions for Class 9 Science Chapter 13, NCERT Solutions for Class 9 Science Chapter 14, NCERT Solutions for Class 9 Science Chapter 15, NCERT Solutions for Class 8 Social Science, NCERT Solutions for Class 7 Social Science, NCERT Solutions For Class 6 Social Science, CBSE Previous Year Question Papers Class 10, CBSE Previous Year Question Papers Class 12, Important Questions For Class 12 Chemistry, Important Questions For Class 11 Chemistry, Important Questions For Class 10 Chemistry, Important Questions For Class 9 Chemistry, Important Questions For Class 8 Chemistry, Important Questions For Class 7 Chemistry, Important Questions For Class 6 Chemistry, Class 12 Chemistry Viva Questions With Answers, Class 11 Chemistry Viva Questions With Answers, Class 10 Chemistry Viva Questions With Answers, Class 9 Chemistry Viva Questions With Answers, Packing efficiency in face centered cubic unit cell, Packing efficiency in body centered cubic unit cell, Packing efficiency in simple cubic unit cell, CBSE Previous Year Question Papers Class 10 Science, CBSE Previous Year Question Papers Class 12 Physics, CBSE Previous Year Question Papers Class 12 Chemistry, CBSE Previous Year Question Papers Class 12 Biology, ICSE Previous Year Question Papers Class 10 Physics, ICSE Previous Year Question Papers Class 10 Chemistry, ICSE Previous Year Question Papers Class 10 Maths, ISC Previous Year Question Papers Class 12 Physics, ISC Previous Year Question Papers Class 12 Chemistry, ISC Previous Year Question Papers Class 12 Biology, JEE Main 2023 Question Papers with Answers, JEE Main 2022 Question Papers with Answers, JEE Advanced 2022 Question Paper with Answers. It is a salt because it decreases the concentration of metallic ions. r k + =1.33 , r Cs + =1.74 , r Cl-=1.81 Mathematically. Packing fraction in ionic structure | Physics Forums Radioactive CsCl is used in some types of radiation therapy for cancer patients, although it is blamed for some deaths. To determine its packing efficiency, we should be considering a cube having the edge length of a, the cube diagonal as c, and the face diagonal length as b. Crystallization refers the purification processes of molecular or structures;. Crystalline Lattices - Department of Chemistry This misconception is easy to make, since there is a center atom in the unit cell, but CsCl is really a non-closed packed structure type. Questions are asked from almost all sections of the chapter including topics like introduction, crystal lattice, classification of solids, unit cells, closed packing of spheres, cubic and hexagonal lattice structure, common cubic crystal structure, void and radius ratios, point defects in solids and nearest-neighbor atoms. The fraction of the total space in the unit cell occupied by the constituent particles is called packing fraction. In crystallography, atomic packing factor (APF), packing efficiency, or packing fractionis the fraction of volumein a crystal structurethat is occupied by constituent particles. If you want to calculate the packing efficiency in ccp structure i.e. The fraction of void space = 1 Packing Fraction Where, r is the radius of atom and a is the length of unit cell edge. Therefore, it generates higher packing efficiency. Try visualizing the 3D shapes so that you don't have a problem understanding them. corners of its cube. We have grown leaps and bounds to be the best Online Tuition Website in India with immensely talented Vedantu Master Teachers, from the most reputed institutions. Your email address will not be published. The interstitial coordination number is 3 and the interstitial coordination geometry is triangular. The higher are the coordination numbers, the more are the bonds and the higher is the value of packing efficiency. The percentage of packing efficiency of in cscl crystal lattice is a) 68% b) 74% c)52.31% d) 54.26% Advertisement Answer 6 people found it helpful sanyamrewar Answer: Answer is 68% Explanation: See attachment for explanation Find Chemistry textbook solutions? Dan suka aja liatnya very simple . Find the number of particles (atoms or molecules) in that type of cubic cell. Considering only the Cs+, they form a simple cubic (Cs+ is teal, Cl- is gold). The packing efficiency of body-centred cubic unit cell (BCC) is 68%. These unit cells are given types and titles of symmetries, but we will be focusing on cubic unit cells. The formula is written as the ratio of the volume of one, Number of Atoms volume obtained by 1 share / Total volume of, Body - Centered Structures of Cubic Structures. \[\frac{\frac{6\times 4}{3\pi r^3}}{(2r)^3}\times 100%=74.05%\]. CsCl is an ionic compound that can be prepared by the reaction: \[\ce{Cs2CO3 + 2HCl -> 2 CsCl + H2O + CO2}\]. The numerator should be 16 not 8. CrystalLattice(SCC): In a simple cubic lattice, the atoms are located only on the corners of the cube. status page at https://status.libretexts.org, Carter, C. The atomic coordination number is 6. In the crystal lattice, the constituent particles, such as atoms, ions, or molecules, are tightly packed. Face-centered Cubic (FCC) unit cells indicate where the lattice points are at both corners and on each face of the cell. And the packing efficiency of body centered cubic lattice (bcc) is 68%. Cesium Chloride is a type of unit cell that is commonly mistaken as Body-Centered Cubic. We always observe some void spaces in the unit cell irrespective of the type of packing. 1.1: The Unit Cell - Chemistry LibreTexts Thus, packing efficiency will be written as follows. These unit cells are imperative for quite a few metals and ionic solids crystallize into these cubic structures. They are the simplest (hence the title) repetitive unit cell. Study classification of solids on the basis of arrangement of constituent particles and intermolecular forces. Simple cubic unit cell: a. In a simple cubic lattice structure, the atoms are located only on the corners of the cube. Click Start Quiz to begin! To determine this, we multiply the previous eight corners by one-eighth and add one for the additional lattice point in the center. Find molar mass of one particle (atoms or molecules) using formula, Find the length of the side of the unit cell. As a result, particles occupy 74% of the entire volume in the FCC, CCP, and HCP crystal lattice, whereas void volume, or empty space, makes up 26% of the total volume. space. { "1.01:_The_Unit_Cell" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "6.2A:_Cubic_and_Hexagonal_Closed_Packing" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.2B:_The_Unit_Cell_of_HPC_and_CCP" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.2C:_Interstitial_Holes_in_HCP_and_CCP" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.2D:_Non-closed_Packing-_Simple_Cubic_and_Body_Centered_Cubic" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "showtoc:no", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FInorganic_Chemistry%2FMap%253A_Inorganic_Chemistry_(Housecroft)%2F06%253A_Structures_and_Energetics_of_Metallic_and_Ionic_solids%2F6.02%253A_Packing_of_Spheres%2F6.2B%253A_The_Unit_Cell_of_HPC_and_CCP%2F1.01%253A_The_Unit_Cell, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), http://en.Wikipedia.org/wiki/File:Lample_cubic.svg, http://en.Wikipedia.org/wiki/File:Laered_cubic.svg, http://upload.wikimedia.org/wikipediCl_crystal.png, status page at https://status.libretexts.org. Face-centered, edge-centered, and body-centered are important concepts that you must study thoroughly. Unit Cells - Purdue University Unit cell bcc contains 4 particles. 6: Structures and Energetics of Metallic and Ionic solids, { "6.11A:_Structure_-_Rock_Salt_(NaCl)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.11B:_Structure_-_Caesium_Chloride_(CsCl)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.11C:_Structure_-_Fluorite_(CaF)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.11D:_Structure_-_Antifluorite" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.11E:_Structure_-_Zinc_Blende_(ZnS)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.11F:_Structure_-_-Cristobalite_(SiO)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.11H:_Structure_-_Rutile_(TiO)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.11I:_Structure_-_Layers_((CdI_2)_and_(CdCl_2))" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.11J:_Structure_-_Perovskite_((CaTiO_3))" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "6.01:_Introduction" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.02:_Packing_of_Spheres" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.03:_The_Packing_of_Spheres_Model_Applied_to_the_Structures_of_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.04:_Polymorphism_in_Metals" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.05:_Metallic_Radii" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.06:_Melting_Points_and_Standard_Enthalpies_of_Atomization_of_Metals" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.07:_Alloys_and_Intermetallic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.08:_Bonding_in_Metals_and_Semicondoctors" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.09:_Semiconductors" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.10:_Size_of_Ions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.11:_Ionic_Lattices" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.12:_Crystal_Structure_of_Semiconductors" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.13:_Lattice_Energy_-_Estimates_from_an_Electrostatic_Model" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.14:_Lattice_Energy_-_The_Born-Haber_Cycle" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.15:_Lattice_Energy_-_Calculated_vs._Experimental_Values" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.16:_Application_of_Lattice_Energies" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.17:_Defects_in_Solid_State_Lattices" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, 6.11B: Structure - Caesium Chloride (CsCl), [ "article:topic", "showtoc:no", "license:ccbyncsa", "non-closed packed structure", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FInorganic_Chemistry%2FMap%253A_Inorganic_Chemistry_(Housecroft)%2F06%253A_Structures_and_Energetics_of_Metallic_and_Ionic_solids%2F6.11%253A_Ionic_Lattices%2F6.11B%253A_Structure_-_Caesium_Chloride_(CsCl), \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), tice which means the cubic unit cell has nodes only at its corners.