Types of Crystalline Solids

Q. In a solid, oxide ions are arranged in ccp. One-sixth of tetrahedral voids are occupied by cation A while one-third of octahedral voids are occupied by cation B. What is the formula of compound?

Q. A solid has a structure in which W atoms are located at the corners of the cubic lattice, O atoms at the center of the edges and Na atom at the centre of the cube. The formula of the compound is

1. $NaW{O}_4$
2. $NaW{O}_2$
3. $N{a}_{2}W{O}_3$
4. $NaW{O}_3$

Q.

Why does a diamond have a high melting point?

Q.

Why liquids do not fill their container completely?

Q. $N{H}_{4}Cl$ crystallizes in a body centred cubic lattice , with a unit cell distance of $387pm$. Calculate the radius of the $N{H}_4^{+}$ ion if the radius of the $C{l}^{-}$ ion is $181pm$.

1. $608.67pm$
2. $52.67pm$
3. $335.15pm$
4. $154.15pm$

Q.

Match the following:

$\begin{array}{cc}ColumnI& ColumnII\\ \left(1\right)I^2& \left(i\right)Ionicsolid\\ \left(2\right)Cu& b\left(ii\right)Covalentsolid\\ \left(3\right)Diamond& \left(iii\right)Molecularsolid\\ \left(4\right)ZnS& \left(iv\right)Metallicsolid\end{array}$

1. (1)-(iii), (2)-(iv), (3)-(ii), (4)-(i)

2. (1)-(iii), (2)-(ii), (3)-(iv), (4)-(i)

3. (1)-(ii), (2)-(iv), (3)-(i), (4)-(iii)

4. (1)-(iv), (2)-(iii), (3)-(ii), (4)-(i)

Q. how many gram atoms of H and S are contained in 0.40 mole of H2S?give me complete solution

Q.

Explain

(i) The basis of similarities and differences between metallic and ionic crystals.

(ii) Ionic solids are hard and brittle.

Q.

Is ${\mathrm{Fe}}_2{\mathrm{O}}_3$ it a covalent or ionic bond?

Q.

Match the following:

(1) I${}_2$ (i) Ionic solid

(2) Cu (ii) Covalent solid

(3) Diamond (iii) Molecular solid

(4) ZnS (iv) Metallic solid

1. (1)-(ii), (2)-(iv), (3)-(i), (4)-(iii)

2. (1)-(iii), (2)-(ii), (3)-(iv), (4)-(i)

3. (1)-(iv), (2)-(iii), (3)-(ii), (4)-(i)

4. (1)-(iii), (2)-(iv), (3)-(ii), (4)-(i)

Q.

Graphite is used as a lubricant because it is

1. a good conductor of heat

2. a good conductor of electricity

3. soft and slippery

4. soluble in organic solvents

Q. What is meant by Polar molecules?
and what are non polar molecules?

Q. Which of the following statement about graphite and diamond is true?

1. They have the same crystal lattice structure
2. They have the same degree of hardness
3. They have the same electric conductivity
4. The melting points of both are very high

Q.

Amongst the following, the form of water with lowest ionic conductance at $298\mathrm{K}$ is

1. distill water

2. sea water

3. saline water used for intra venous injection

4. water from a well

Q. Which of the following statement(s) is/are incorrect regarding the defects in solids?

1. $AgBr$ crystal show both Schottky and Frenkel defect
   
2. Solids containing F-centers are paramagnetic
   
3. Doping in crystal introduces dislocation defect
   
4. Metal deficient defect can occur with extra cation present in the interstitial voids

Q. Copper crystallises in a structure of face centered cubic unit cell. The atomic radius of copper is $1.28$$A^{\circ }$. What is edge length of the unit cell?

1. $2.16A^{\circ }$
2. $3.62A^{\circ }$
3. $3.94A^{\circ }$
4. $4.15A^{\circ }$

Q. total number of atoms in 44 g of Carbon dioxide is ?

Q.

5. Why are germanium and silicon referred to as semiconductors?

Q.

Which of the following is not the characteristic of ionic solids ?

(a) Very low value of electrical conductivity in the molten state

(b) Brittle nature

(c) Very strong forces of interactions

(d) Anisotropic nature

Q.

Which of the following is/are molecular solid(s)?

1. Iron (Fe)

2. Solid SO₂

3. CaF₂

4. Diamond

Q.

Which of the following cannot be regarded as molecular solid ?

(a)SIC (silicon carbide) (b) AIN

(c) Diamond (d) $I_2$

Q.

Dry ice is an example of molecular solid.

1. True
2. False

Q. What are triangular voids?Is these voids are formed 1D?formula for finding these voids

Q.

What is hydrated radius

Q. Which of the following crystal system will exhibit the geometry of a match box?

1. Cubic
2. Orthorhombic
3. Triclinic
4. Monoclinic

Q.

Hydrogen is a poor conductor of heat as compared to other gases.

1. True
2. False

Q.

The ionization enthalpy of ${\mathrm{Na}}^{+}$formation from $\mathrm{Na}\left(\mathrm{g}\right)$ is $495.8\mathrm{kJ}{\mathrm{mol}}^{-1}$, while the electron gain enthalpy of $\mathrm{Br}$ is$-325.0\mathrm{kJ}{\mathrm{mol}}^{-1}$. Given the lattice enthalpy of $\mathrm{NaBr}$ is$-728.4\mathrm{kJ}{\mathrm{mol}}^{-1}$. The energy for the formation of $\mathrm{NaBr}$ ionic solid is$(-)$_______ $\times {10}^{-1}\mathrm{kJ}{\mathrm{mol}}^{-1}$

Q.

Classify each of the following solid as ionic, metallic, molecular, network (covalent) or amorphous.

Tetraphosphorus decoxide $\left(P_4{O}_{10}\right)$

Ammonium phosphate, $(N{H}_4{)}_{3}P{O}_4$

SiC

$I_2$

$P_4$

Plastic

Graphite

Brass

Rb

LiBr

Si

Q.

Match the following:

(1)HCl (i) Polar Molecular solid

(2)Ice (ii) Non-polar Molecular solid

(3)CCl${}_4$ (iii) H-bonded Molecular solid

1. (1)-(iii), (2)-(ii), (3)-(i)

2. (1)-(i), (2)-(ii), (3)-(iii)

3. (1)-(ii), (2)-(iii), (3)-(i)

4. (1)-(i), (2)-(iii), (3)-(ii)

Q.

Match the following:

$\begin{array}{cc}ColumnI& ColumnII\\ \left(1\right).Non-polarMolecularsolids& \left(i\right)Coulombicorelectrostaticforces\\ \left(2\right).H-BondedMolecularsolids& \left(ii\right).H-bonding\\ \left(3\right).Ionicsolids& \left(iii\right).Metallicbonding\\ \left(4\right).Weakdispersionforces& \left(iv\right).Weakdispersionforces\\ \left(5\right).Metallicsolids& \left(v\right).dipole–dipoleinteraction.\\ & \left(vi\right).covalentBonding.\end{array}$

1. (1)-(iv), (2)-(ii), (3)-(iv), (4)-(vi), (5)-(iii)

2. (1)-(iv), (2)-(ii), (3)-(i), (4)-(vi), (5)-(iii)

3. (1)-(iv), (2)-(ii), (3)-(iv), (4)-(vi), (5)-(iii)

4. (1)-(v), (2)-(i), (3)-(iv), (4)-(vi), (5)-(ii)