Question 1 :
In a non stoichiometric sample of ferrous oxide with NaCl structure, the ratio of $Fe^{+3}$ to $Fe^{2+}$ was found to be 0.15. The fraction of octahedral sites occupied by vacancies is :<br/>
Question 2 :
Iron crystallizes in several modifications, At about $910^o$C, the body centred $\alpha$-form undergoes transition to the face centred cubic $\gamma$-form. Assuming that the distance between nearest neighbours is same in the two forms at the transition temperature. Calculate the ratio of density of $\gamma$-iron to that of $\alpha$-iron at the transition temperature.
Question 3 :
Radii of $A^+$ and that of $X^-$ and $Y^-$ have been given as<br/>$A^+=1.00$ pm<br/>$X^-=1.00$ pm<br/>$Y^-=2.00$ pm<br/>Determine the volume of unit cells of AX and AY crystals.<br/>
Question 4 :
$Na$ and $Mg$ crystallize in $BCC$ and $FCC$ type crystals respectively, then the number of atoms of $Na$ and $Mg$ present in the unit cell of their respective crystal is<br>
Question 5 :
An alloy of copper and gold crystallizes in a cubic lattice in which the gold atoms occupy the lattice points at the corners of cube and copper atoms occupy the centre of each face. The formula of this compound is :
Question 6 :
A crystalline solid between A and B has the following arrangement of atoms: <br/>(i) Atoms A are arranged in a CCP array.<br/>(ii) Atoms B occupy all the octahedral voids and half of the tetrahedral voids.<br/>What is the formula of the compound?<br/>
Question 7 :
A solid has a structure in which $W$ atoms are located at the corners of a cubic lattice, $O$ atoms at the centre of the edges and $Na$ atoms at the centre of the cubic. The formula for the compound is:
Question 8 :
In a solid $AB$ having $NaCl$ structure atoms, occupy the corners of the unit cell. If all the face centred atoms along one of the axis are removed, then the resultant stoichiometry of the solid is:<br>
Question 9 : An element crystalline in body centered cubic lattice has an edge of 500 pm. If its density is 4 g $cm^{-3}$, the atomic mass of the element (in g $mol^{-1}$) is: <div>(consider $N_A=6\times10^{23}$) <br/></div>
Question 10 :
$Al$(at.wt.$27$) crystallizes in the cubic system with a cell edge of $4.05\mathring { A } $. Its density is $2.7g/{ cm }^{ 3 }$. Determine the unit cell type and calculate the radius of the $Al$ atom.
Question 11 :
A solid is formed and it has three types of atoms X, Y, Z. X forms an FCC lattice with Y atoms occupying one-forth of tetrahedral viods and Z atoms occupying half of the octahedral voids. The formula of the solid is?
Question 12 :
A crystal is made up of particles A, B, and C, A forms fcc packing, B occupies all octahedral voids and C occupies all tetrahedral voids. If all the particles along one body diagonal are removed, then the formula of the crystal would be:
Question 13 :
In a cubic structure of compounds which is made from $X$ and $Y$, where $X$ atoms are at the corners of the cube and $Y$ at the face centres of the cube. The molecular formula of the compound is
Question 14 :
An alloy of $Cu, Ag$ and $Au$ is found to have copper constituting fcc lattice. If silver atoms occupy the edge-centers and gold is present at body-center, the alloy has the formula _______.
Question 15 :
If in a cubic cell, atoms $A$ present at all corners and atoms $B$ at the center of each face. What will be the molecular formula of the compound, if all the atoms present in one body diagonal are replaced by atom $C$?<br>
Question 16 :
The pattern of successive layers of ccp arrangement can be designated as:
Question 17 :
An ionic solid has ${C_5}Cl$ structure. The length of body diagonal is $7.0\,\mathop {\text{A}}\limits^{\text{o}} .$ The edge length of the cube and inter-ionic distance respectively are:
Question 18 :
The density of argon (face centered cubic cell) is $1.83\, g/cm^3$ at $20^oC$. What is the length of an edge a unit cell?
Question 19 :
$CsCl$ crystallizes in a cubic lattice that has a $Cl^-$ at each corner and $Cs^+$ at the centre of the unit cell. If $(r_{Cs^+})=1.69\overset{o}{A}$ and $(r_{Cl^-})=1.81\overset{o}{A}$, what is the value of edge length a of the cube?<br>
Question 20 :
In a unit cell, atoms $A, B, C$ and $D$ are present at corners, face-centres, body-centre and edge-centres respectively. If atoms touching one of the plane passing through two diagonally opposite edges are removed, then formula of compound is:
Question 21 :
The density and edge length values for a crystallise elemens with $fcc$ lattice are $10 g$ $cm^{-3}$ and 400 pm, respectively. The number of unit cell in $32 g$ of this crystal is:
Question 22 :
Statement 1: In a crystal of $Ca$, the separation of $(1,1,1)$ planes is twice as great as that of $(2,2,2)$ planes.<br/>Statement 2: The length of the side of crystal lattice is $0.556$ nm $(\sqrt{12}=3.46)$.
Question 23 :
Gold is plated with rhodium to give a base for mounting diamonds in modern jewellery. The rhodium-gold alloy consists of gold atoms in fcc structure with half the face centers being replaced by rhodium atoms. Formula of this alloy is :<br/>
Question 24 :
Aluminium crystallizes in a cubic close packed structure. Its metallic radius is $125$ pm. The edge length (in pm) of the unit cell and number of unit cells per cc of aluminium, respectively, are :
Question 26 :
A binary solid $(A^+B^-)$ has a zinc blende structure with $B^-$ ions constituting the lattice and $A^+$ ions occupying $25\%$ tetrahedral holes. The formula of solid is:
Question 27 :
A binary solid has a primitive cubical structure with $B^-$ ions constituting the lattice points and $A^+$ ions occupying 25% of its tetrahedral holes. The molecular formula of the crystal is:<br/>
Question 28 :
$AB$ crystallises in a bcc lattice with edge length an equal to 387 pm. The distance between two oppositely charged ions in the lattice is:<br/>
Question 29 :
A solid has three types of atoms $X,\ Y$ and $Z$. $X$ forms an $FCC$ lattice with $Y$ atoms occupying all the tetrahedral voids and $Z$ atoms occupying half of the octahedral voids. The formula of the solid is
Question 31 :
An element crystallizes in FCC lattice of edge length $400$pm. Calculate the maximum diameter which can be placed in interstitial sites without distorting the structure.
Question 32 :
In a crystalline solid, anions $B$ are arranged in ccp lattice and cations $A$ occupy $50$% of the octahedral voids and $50$% of the tetrahedral voids. What is the formula of the solid?
Question 33 : The ratio of the volume of a tetragonal lattice unit cell to that of a hexagonal lattice unit cell is: <div>(both having same respective lengths)</div>
Question 34 :
Assertion: It occupies certain holes of this type but not the other holes of the same type?
Reason: The proximity of two cations $(A^{2+ }\,\,and \,\,B^{4+})$ would be electrostatically unfavourable.
Question 35 :
In a cubic arrangement of atoms of A, B and C, atoms of A are present at the corners of the unit cell, B atoms are at face centers and C at tetrahedral voids. If one of the atom from one corner is missing in the unit cell, then the simplest formula of the compound will be:
Question 36 :
A compound is formed by cation $C$ and anion $A$. The anions form hexagonal close packed (hcp) lattice and the cations occupy $75\%$ of octahedral voids. The formula of the compound is :
Question 37 :
A crystal of sodium hydride has an fcc unit cell of $\text{H}^-$ ions with $\text{Na}^+$ ions at the body centres of a unit cell and in the centre of edges. The number of $\text{H}^-$ that touch each $\text{Na}^+$ is:
Question 38 :
Aluminium crystallizes in a cubic close packed structure. Its metallic radius is $125pm$.<br>i) Calculate the edge length of unit cell<br>ii) How many unit cells are there in $1.00cm^3$ of aluminium?
Question 39 :
A compound formed by elements $X$ and $Y$ crystallizes in a cubic structure, where $X$ is at the corners of the cube and $Y$ is at six face centers. What is the formula of the compound?
Question 40 :
An element $X$ (At. wt. = 80g/mol) having fcc structure, calculate no. of unit cell in $8\ gm$ of $X$.
Question 41 :
Aluminium (atomic mass = 27) crystallises in a cubic system with edge length of 4A. Its density is $2.7\, g\, cm^{-3}$. The number of aluminium atoms present per unit cell is:
Question 42 :
In metal oxide, the oxide ions are arranged in corners as well as on faces and metal cation occupy $\dfrac{2}{3}$ of octahedral voids, the formula of oxide is:
Question 44 :
In a close-packed structure of mixed oxides, the lattice is composed of oxide ions, one-eighth of tetrahedral voids are occupied by divalent cations $A$ while one-half of octahedral voids are occupied by trivalent cations $B$. The formula of the oxide is:
