Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution:  The structures of CsCl, NaCl, and ZnS. Each structure type can be generated by the combination of a two-atom motif and the appropriate lattice.CuI, CsI, and NaI each adopt a different type of structu

Problem


A diagram showing motif, crystal lattice and crystal structure for three different substances.


 The structures of CsCl, NaCl, and ZnS. Each structure type can be generated by the combination of a two-atom motif and the appropriate lattice.


CuI, CsI, and NaI each adopt a different type of structure. The three different structures are those shown in the following figure.


Write the coordination numbers of iodide in CuI, CsI, and NaI, respectively.

Solution

We're being asked to determine the coordination number of iodide in the given compounds.


The coordination number is the number of ions that immediately surround an ion of the opposite charge within a crystal lattice.


Crystalline solids represent structures with well-organized patterns and shapes. When examining the particles within a crystal you may observe them tightly packed in an organized pattern. The smallest portion of which is termed the unit cell.


  • The Simple Cubic Unit Cell is composed of cube with an atom at each corner. An atom in a simple cubic lattice structure contacts six other atoms, so its coordination number is six (6).
  • The body-centered cubic unit cell is composed of a cube with one atom at each of its corners and one atom at the center of the cube. Any atom in the structure touches four atoms in the layer above it and four atoms in the layer below it so its coordination number is eight (8).
  • The face-centered cubic unit cell is composed of a cube with one atom at each of its corners and one atom in the center of each cube face. Atoms in this structure contact six atoms in their layer, three atoms in the layer above it and three atoms in the layer below it so its coordination number is twelve (12).


Let’s analyze the problem using the information we have

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