Class XII Chemistry Chapter 1 The Solid State NCERT Solution is given below.
Question 1.16:
A compound is formed by two elements M and N. The element N forms ccp and atoms of M occupy 1/3rd of tetrahedral voids. What is the formula of the compound?
Answer
The ccp lattice is formed by the atoms of the element N.
Here, the number of tetrahedral voids generated is equal to twice the number of atoms of the element N.
According to the question, the atoms of element M occupy 1/3rd of the tetrahedral voids.
Therefore, the number of atoms of M is equal to 2 x 1/3 = 2/3rd of the number of atoms of N.
Therefore, ratio of the number of atoms of M to that of N is M: N = (2/3) : 1 = 2:3
Thus, the formula of the compound is M2 N3.
Question
1.15:
A compound forms hexagonal close-packed structure. What is the total number of voids in 0.5 mol of it? How many of these are tetrahedral voids?
Answer
A compound forms hexagonal close-packed structure. What is the total number of voids in 0.5 mol of it? How many of these are tetrahedral voids?
Answer
Question 1.16:
A compound is formed by two elements M and N. The element N forms ccp and atoms of M occupy 1/3rd of tetrahedral voids. What is the formula of the compound?
Answer
The ccp lattice is formed by the atoms of the element N.
Here, the number of tetrahedral voids generated is equal to twice the number of atoms of the element N.
According to the question, the atoms of element M occupy 1/3rd of the tetrahedral voids.
Therefore, the number of atoms of M is equal to 2 x 1/3 = 2/3rd of the number of atoms of N.
Therefore, ratio of the number of atoms of M to that of N is M: N = (2/3) : 1 = 2:3
Thus, the formula of the compound is M2 N3.
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