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Science Chemistry Chemistry: An Atoms-Focused Approach

One or more metallic elements that cannot form a rock salt structure with C l - ions, from among the highlighted elements. Solution: Blue: C s and Purple : S r do not form rock salt structure with C l - ions. Explanation: Concept: In the given figure, color and metal pairs are as follows: red: L i , yellow: N a , green: K , purple: S r , and blue: C s . The molecular formula of the compound of S r and C l is S r C l 2 . So, the metal to nonmetal ratio is 1:2. Therefore, Cl will occupy half of the octahedral holes in the crystal structure. Thus, S r cannot form a rock salt structure with C l - . A number of metal chlorides adopt the rock salt crystal structure, in which the metal ions occupy all the octahedral holes in a face centered cubic array of chloride ions. Face centered (close- packed) atoms in adjacent layers of a crystal lattice produce octahedral holes surrounded by six host atoms and tetrahedral holes surrounded by four host atoms. Octahedral holes are larger than tetrahedral holes and can accommodate larger non-host atoms in interstitial alloys. This can is determined by the ratio of atomic radius of non-host atom (Cl) to atomic radius of host atom (metal). This is shown in the following table (Table 18.4 from the book): L i N a K C s C l Atomic radius (pm) 152 186 227 265 99 ratio 0.65 0.53 0.44 0.37 - The standard range for the ratio of atomic radius of non-host atom to atomic radius of host atom for octahedral hole is 0.41 t o 0.73 . The ratio of atomic radius of non-host atom to atomic radius of host atom for C l a n d C s is 0.37 , which is not in the standard range of octahedral hole. Therefore, C s cannot form a rock salt structure with C l - . Conclusion: We can decide the metal that can form a crystal structure with non-host atom using the ratio of atomic radius of the non-host atom to atomic radius of the host atom for a particular type of hole.

One or more metallic elements that cannot form a rock salt structure with C l - ions, from among the highlighted elements. Solution: Blue: C s and Purple : S r do not form rock salt structure with C l - ions. Explanation: Concept: In the given figure, color and metal pairs are as follows: red: L i , yellow: N a , green: K , purple: S r , and blue: C s . The molecular formula of the compound of S r and C l is S r C l 2 . So, the metal to nonmetal ratio is 1:2. Therefore, Cl will occupy half of the octahedral holes in the crystal structure. Thus, S r cannot form a rock salt structure with C l - . A number of metal chlorides adopt the rock salt crystal structure, in which the metal ions occupy all the octahedral holes in a face centered cubic array of chloride ions. Face centered (close- packed) atoms in adjacent layers of a crystal lattice produce octahedral holes surrounded by six host atoms and tetrahedral holes surrounded by four host atoms. Octahedral holes are larger than tetrahedral holes and can accommodate larger non-host atoms in interstitial alloys. This can is determined by the ratio of atomic radius of non-host atom (Cl) to atomic radius of host atom (metal). This is shown in the following table (Table 18.4 from the book): L i N a K C s C l Atomic radius (pm) 152 186 227 265 99 ratio 0.65 0.53 0.44 0.37 - The standard range for the ratio of atomic radius of non-host atom to atomic radius of host atom for octahedral hole is 0.41 t o 0.73 . The ratio of atomic radius of non-host atom to atomic radius of host atom for C l a n d C s is 0.37 , which is not in the standard range of octahedral hole. Therefore, C s cannot form a rock salt structure with C l - . Conclusion: We can decide the metal that can form a crystal structure with non-host atom using the ratio of atomic radius of the non-host atom to atomic radius of the host atom for a particular type of hole.

Solution Summary: The author explains that metallic elements cannot form a rock salt structure with Cl- ions. The molecular formula of the compound of Sr and Cl is 1:2.

Chemistry: An Atoms-Focused Approach

Chemistry: An Atoms-Focused Approach

14th Edition

ISBN: 9780393912340

Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster

Publisher: W. W. Norton & Company

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Chapter 18, Problem 18.14VP

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Chapter 18 Solutions

Chemistry: An Atoms-Focused Approach

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