318731
In an FCC unit cell, atoms are numbered as shown below. The atoms not touching each other are (atom numbered 3 is centre of front face).
1 2 and 4
2 3 and 4
3 1 and 3
4 1 and 2
Explanation:
Atoms along one edge or at corners do not touch each other in fcc cell.
CHXII01:THE SOLID STATE
318732
How many nearest neighbours does potassium have in BCC lattice?
1 6
2 8
3 4
4 12
Explanation:
No. of nearest neighbour \(=8\) (All body centre atom w.r.t. corner atom).
CHXII01:THE SOLID STATE
318733
Right option of the number of tetrahedral and octahedral voids in hexagonal primitive unit cell are:
1 6,12
2 2,1
3 12,6
4 8,4
Explanation:
For hexagonal primitive unit cell Number of effective atoms per unit cell, \(Z=6\) \(\therefore\) Total no. of tetrahedral voids \(=2 \mathrm{Z}\) \[ \begin{aligned} & =2 \times 6 \\ & =12 \end{aligned} \] Total no. of octahedral voids \(=\mathrm{Z}\) \[ =6 \]
NEET - 2021
CHXII01:THE SOLID STATE
318734
In mineral \(\mathrm{MX}_{2}, \mathrm{M}^{2+}\) does \(\mathrm{CCP}\) and \(\mathrm{X}^{-}\)occupy the tetrahedral voids. The number of cations and anions per unit cell, the coordination number of cation and percent of tetrahedral voids occupied are
1 \(8,4,8,100 \%\)
2 \(8,4,8,50 \%\)
3 \(4,8,8,50 \%\)
4 \(4,8,8,100 \%\)
Explanation:
The number of formula units in ccp(rank) \(=4\) \[ \therefore 4 \mathrm{MX}_{2} \] Hence, number of cations \(\left(\mathrm{M}^{2+}\right)=4\), \(\operatorname{Anions}\left(\mathrm{X}^{-}\right)=8\) C.N. of cation \(=8\); All tetrahedral voids are occupied.
318731
In an FCC unit cell, atoms are numbered as shown below. The atoms not touching each other are (atom numbered 3 is centre of front face).
1 2 and 4
2 3 and 4
3 1 and 3
4 1 and 2
Explanation:
Atoms along one edge or at corners do not touch each other in fcc cell.
CHXII01:THE SOLID STATE
318732
How many nearest neighbours does potassium have in BCC lattice?
1 6
2 8
3 4
4 12
Explanation:
No. of nearest neighbour \(=8\) (All body centre atom w.r.t. corner atom).
CHXII01:THE SOLID STATE
318733
Right option of the number of tetrahedral and octahedral voids in hexagonal primitive unit cell are:
1 6,12
2 2,1
3 12,6
4 8,4
Explanation:
For hexagonal primitive unit cell Number of effective atoms per unit cell, \(Z=6\) \(\therefore\) Total no. of tetrahedral voids \(=2 \mathrm{Z}\) \[ \begin{aligned} & =2 \times 6 \\ & =12 \end{aligned} \] Total no. of octahedral voids \(=\mathrm{Z}\) \[ =6 \]
NEET - 2021
CHXII01:THE SOLID STATE
318734
In mineral \(\mathrm{MX}_{2}, \mathrm{M}^{2+}\) does \(\mathrm{CCP}\) and \(\mathrm{X}^{-}\)occupy the tetrahedral voids. The number of cations and anions per unit cell, the coordination number of cation and percent of tetrahedral voids occupied are
1 \(8,4,8,100 \%\)
2 \(8,4,8,50 \%\)
3 \(4,8,8,50 \%\)
4 \(4,8,8,100 \%\)
Explanation:
The number of formula units in ccp(rank) \(=4\) \[ \therefore 4 \mathrm{MX}_{2} \] Hence, number of cations \(\left(\mathrm{M}^{2+}\right)=4\), \(\operatorname{Anions}\left(\mathrm{X}^{-}\right)=8\) C.N. of cation \(=8\); All tetrahedral voids are occupied.
318731
In an FCC unit cell, atoms are numbered as shown below. The atoms not touching each other are (atom numbered 3 is centre of front face).
1 2 and 4
2 3 and 4
3 1 and 3
4 1 and 2
Explanation:
Atoms along one edge or at corners do not touch each other in fcc cell.
CHXII01:THE SOLID STATE
318732
How many nearest neighbours does potassium have in BCC lattice?
1 6
2 8
3 4
4 12
Explanation:
No. of nearest neighbour \(=8\) (All body centre atom w.r.t. corner atom).
CHXII01:THE SOLID STATE
318733
Right option of the number of tetrahedral and octahedral voids in hexagonal primitive unit cell are:
1 6,12
2 2,1
3 12,6
4 8,4
Explanation:
For hexagonal primitive unit cell Number of effective atoms per unit cell, \(Z=6\) \(\therefore\) Total no. of tetrahedral voids \(=2 \mathrm{Z}\) \[ \begin{aligned} & =2 \times 6 \\ & =12 \end{aligned} \] Total no. of octahedral voids \(=\mathrm{Z}\) \[ =6 \]
NEET - 2021
CHXII01:THE SOLID STATE
318734
In mineral \(\mathrm{MX}_{2}, \mathrm{M}^{2+}\) does \(\mathrm{CCP}\) and \(\mathrm{X}^{-}\)occupy the tetrahedral voids. The number of cations and anions per unit cell, the coordination number of cation and percent of tetrahedral voids occupied are
1 \(8,4,8,100 \%\)
2 \(8,4,8,50 \%\)
3 \(4,8,8,50 \%\)
4 \(4,8,8,100 \%\)
Explanation:
The number of formula units in ccp(rank) \(=4\) \[ \therefore 4 \mathrm{MX}_{2} \] Hence, number of cations \(\left(\mathrm{M}^{2+}\right)=4\), \(\operatorname{Anions}\left(\mathrm{X}^{-}\right)=8\) C.N. of cation \(=8\); All tetrahedral voids are occupied.
318731
In an FCC unit cell, atoms are numbered as shown below. The atoms not touching each other are (atom numbered 3 is centre of front face).
1 2 and 4
2 3 and 4
3 1 and 3
4 1 and 2
Explanation:
Atoms along one edge or at corners do not touch each other in fcc cell.
CHXII01:THE SOLID STATE
318732
How many nearest neighbours does potassium have in BCC lattice?
1 6
2 8
3 4
4 12
Explanation:
No. of nearest neighbour \(=8\) (All body centre atom w.r.t. corner atom).
CHXII01:THE SOLID STATE
318733
Right option of the number of tetrahedral and octahedral voids in hexagonal primitive unit cell are:
1 6,12
2 2,1
3 12,6
4 8,4
Explanation:
For hexagonal primitive unit cell Number of effective atoms per unit cell, \(Z=6\) \(\therefore\) Total no. of tetrahedral voids \(=2 \mathrm{Z}\) \[ \begin{aligned} & =2 \times 6 \\ & =12 \end{aligned} \] Total no. of octahedral voids \(=\mathrm{Z}\) \[ =6 \]
NEET - 2021
CHXII01:THE SOLID STATE
318734
In mineral \(\mathrm{MX}_{2}, \mathrm{M}^{2+}\) does \(\mathrm{CCP}\) and \(\mathrm{X}^{-}\)occupy the tetrahedral voids. The number of cations and anions per unit cell, the coordination number of cation and percent of tetrahedral voids occupied are
1 \(8,4,8,100 \%\)
2 \(8,4,8,50 \%\)
3 \(4,8,8,50 \%\)
4 \(4,8,8,100 \%\)
Explanation:
The number of formula units in ccp(rank) \(=4\) \[ \therefore 4 \mathrm{MX}_{2} \] Hence, number of cations \(\left(\mathrm{M}^{2+}\right)=4\), \(\operatorname{Anions}\left(\mathrm{X}^{-}\right)=8\) C.N. of cation \(=8\); All tetrahedral voids are occupied.
