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The Solid State Chemistry - The Solid State

Gujarat Board (GSEB) - STD 12 Science - Chemistry (GSEB - English Medium). 444 questions in this chapter.

Question types

The Solid State question types

444 questions across 7 question groups — pick any mix to generate a Chemistry paper with step-by-step answer keys.

444
Questions
7
Question groups
5
Question types
Sample Questions

The Solid State questions

One sample from each question group in this chapter. Select any group above to see the full set with answer keys.

Q 1M.C.Q (1 Marks)1 Mark
Silicon doped with electron-rich impurity forms ________.
  • A
    p-type semiconductor.
  • ✓
    n-type semiconductor.
  • C
    Intrinsic semiconductor.
  • D
    Insulator.

Answer: B.

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Q 3M.C.Q (1 Marks)1 Mark
Which of the following arrangements correctly represents hexagonal and cubic close packed structure respectively?
  • ✓
    $\text{ABAB}.....$ and $\text{ABCABCABC}.....$
  • B
    $\text{ABCABC}.....$ and $\text{ABAB}....$
  • C
    Both have $\text{ABCABC}......$ arrangement
  • D
    Both have $\text{ABAB}...$ arrangement

Answer: A.

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Q 5M.C.Q (1 Marks)1 Mark
A solid can be irreversibly deformed. The stamping of sheets of steel into 'fins' of motor cars is a case of :
  • A
    Vaccum deformation
  • ✓
    Plastic deformation
  • C
    Elastic deformation
  • D
    Flexible shaping

Answer: B.

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Q 6Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
 Assertion: ln any ionic solid with Schottky defect, the number of positive and negative ions is same.
Reason: Equal number of cationic and anionic vacancies are present.
  • ✓
    Assertion and reason both are correct statements, and reason is correct explanation for assertion.
  • B
    Assertion and reason both are correct statements, but reason is not correct explanation for assertion.
  • C
    Assertion is correct statement, but reason is wrong statement.
  • D
    Assertion is wrong statement, but reason is correct statement.

Answer: A.

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Q 7Assertion (A) & Reason (B) MCQ1 Mark
Directions: In the following questions, the Assertions $(A)$ and Reason$(s)\ (R)$ have been put forward. Read both the statements carefully and choose the correct alternative from the following:
Assertion: No compound has both Schottky and Frenkel defects.
Reason: Both defects change the density of the solid.
  • A
    If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.
  • B
    If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.
  • C
    If the Assertion is correct but Reason is incorrect.
  • ✓
    If both the Assertion and Reason are incorrect.

Answer: D.

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Q 8Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
Assertion: In $\text{NaCl}$ crystal, each $Na^+$ ion is touching six $Cl^-$ ions but these $Cl^-$ ions do not touch each other.
Reason: The radius ratio $\frac{\text{r}_\text{Na}}{\text{r}_\text{Cl-}}$ is greater than $0.414$ required for exact fitting.
  • ✓
    Assertion and reason both are correct statements, and reason is correct explanation for assertion.
  • B
    Assertion and reason both are correct statements, but reason is not correct explanation for assertion.
  • C
    Assertion is correct statement, but reason is wrong statement.
  • D
    Assertion is wrong statement, but reason is correct statement.

Answer: A.

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Q 9Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
Assertion: The total number of atoms present in simple cubic unit cell in one.
Reason: Simple cubic unit cell has atoms at its corners, each of which is shared between four adjacent unit cells.
  • A
    Assertion and reason both are correct statements, and reason is correct explanation for assertion.
  • B
    Assertion and reason both are correct statements, but reason is not correct explanation for assertion.
  • ✓
    Assertion is correct statement, but reason is wrong statement.
  • D
    Assertion is wrong statement, but reason is correct statement.

Answer: C.

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Q 10Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
Assertion: Molecular solids are characterized by low melting point.
Reason: Molecular solids are made up of covalent molecules.
  • A
    Assertion and reason both are correct statements, and reason is correct explanation for assertion.
  • ✓
    Assertion and reason both are correct statements, but reason is not correct explanation for assertion.
  • C
    Assertion is correct statement, but reason is wrong statement.
  • D
    Assertion is wrong statement, but reason is correct statement.

Answer: B.

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Q 213 Marks Question3 Marks
Calculate the distance between $Na^+$ and $Cl^-$ ions in $NaCl$ crystal if its density is $2.165\ g\ cm^{-3}. [$Molar mass of $NaCl=58.5\ g\ mol^{-1};\ N_A=6.02 x 10^{-23}\ mol^{-1}].$
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Q 26Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions:In contrast to the disorders of gases and liquids, there is translational order in crystals. However, disordered or amorphous solids also exist which lack such order, they are really highly viscous liquids. In translational order entire structure or lattice, can be generated by repeated replication of a small regular figure, termed as unit cell. The planes of any crystalline structure can be specified using Miller indices, which is also serve to identify single crystal faces.The ordered structure, or lattice, of a solid can be determined by X-ray or neutron diffraction studies, in which a beam of X-rays of neutrons is scattered from the sample to produce a diffraction pattern which can be analyzed to reveal the crystal structure of the sample. All crystal lattices can be classified into 14 Bravais lattices belonging to 7 systems. For example, the simple cubic, face-centred cubic and body-centred cubic lattices are the 3 lattices of the cubic system. Cubic and hexagonal close-packed structures have the structure of tightly packed spheres, where each sphere touches 12 neighbours, 6 in the same plane and 3 above and 3 below. These two dose-packed structures differ in the placement of successive planes or layers. For the hexagonal close packing, a third layer is laid down to reproduce the first layer, so that the structure could be represented by ABABAB …. For cubic close packing, third layer is again displaced, corresponding to ABCABC.
The following questions are multiple choice questions. Choose the most appropriate answer:
  1. In hexagonal close packing, a sphere has coordination number of.
  1. 4
  2. 6
  3. 8
  4. 12
  1. Which of the following arrangements correctly represents hexagonal and cubic close packed structure respectively?
  1. ABCABC...and ABAB...
  2. ABAB...and ABCABC...
  3. Both have ABAB ... arrangement.
  4. Both have ABCABC... Arrangement.
  1. The arrangement of the first two layers, one above the other, in hep and ccp arrangements is.
  1. Exactly same in both cases
  2. Partly same and partly different
  3. Different from each other
  4. Nothing definite.
  1. Which of the following statements is not correct?
  1. The amorphous solids have a random, disordered arrangement of constituents.
  2. The simple cubic, face-centred and body-centred are the three lattices of the cubic system.
  3. The number of Bravais lattice in which a crystal can be categorized is 7.
  4. A metal that crystallizes in hep structure has coordination number 12.
  1. Which of the following statements about amorphous solids is incorrect?
  1. They melt over a range of temperature.
  2. There is no orderly arrangement of particles.
  3. They are anisotropic.
  4. They are rigid and incompressible.
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Q 27Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions:
Most important crystal lattices are the simple cubic, body centred cubic and face centred cubic. In simple cubic lattice, all the atoms are present at all the corners of the cube. In body-centred cubic lattice, atoms are present at all the corners and at the body-centre. In face-centred cubic lattice, atoms are present at the corners and at the centers of all six faces. In the formation of crystals, the constituent particles get closely packed together. The closely packed arrangement is that in which maximum available space is occupied, leaving minimum vacant space. The most efficient close packing, can be achieved in two ways, one which is called hexagonal close packing.(hcp) and the other, cubic close packing (ccp or fcc)
In these questions (Q. No. i-iv) a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
  1. Assertion and reason both are correct statements, and reason is correct explanation for assertion.
  2. Assertion and reason both are correct statements, but reason is not correct explanation for assertion.
  3. Assertion is correct statement, but reason is wrong statement.
  4. Assertion is wrong statement, but reason is correct statement.
  1. Assertion: Face centred cubic cell has $4$ atoms per unit cell.
Reason: ln fee unit cell, there are $8$ atoms at the corners and $ 6$ atoms at face centres
  1. Assertion: CsCl has body-centred cubic arrangement.
Reason: CsCl has one $Cs^+$ ion and $8$ $CI^-$ ions in its unit cell.
  1. Assertion: fcc and hcp have same packing efficiency.
Reason: bcc and fcc both have same number of atoms per unit cell and same arrangement.
  1. Assertion: The total number of atoms present in a simple cubic unit cell is one.
Reason: Simple cubic unit cell has atoms at its corners, each of which is shared between eight adjacent unit cells.
  1. Assertion: The packing efficiency is maximum for the fee structure.
Reason: The coordination number is $12$ in fcc structures.
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Q 28Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions:
In ideally ionic structures, the coordination numbers of the ions are determined by electrostatic considerations. Cations surround themselves with as many anions as possible, and vice versa. This maximizes the attractions between neighbouring ions of opposite charge and hence maximizes the lattice energy of the crystal. This requirement led to the formulation of the radius ratio rule for ionic structures, in which the ions and the structure adopted for a particular compound depend on the relative sizes of the ions. Thus, for the stable ionic crystalline structures, there is definite radius ratio limit for a cation to fit perfectly in the lattice of anions, called radius ratio rule. This depends upon the ratio of radii of two types of ions $\frac{\text{r}_+}{r}$This ratio for coordination numbers $3, 4, 6$ and $8$ are respectively $0.155 - 0.225, 0.225 - 0.414, 0.414 - 0.732$ and $0.732 - 1.000$. The coordination number of ionic solids also depends upon temperature and pressure. On applying high pressure, coordination number increases. On the other hand, on applying high temperature, it decreases.
The following questions are multiple choice questions. Choose the most appropriate answer:
  1. The ionic radii of $K^+,Rb^+$ and $Br-$ are $137, 148$ and $195$pm. The coordination number of cation in RbBr and KBr structures are respectively.
  1. $8, 6$
  2. $6, 4$
  3. $6, 8$
  4. $4, 6$
  1. For a coordination number $4,$ the maximum limiting radius ratio is.
  1. $0.414$
  2. $0.732$
  3. $0.225$
  4. $0.155$
  1. If the radius of $Na^+$ ion is 95 pm and that of $Cl^-$ ion is $181$  pm, the coordination number of $Na^+$ ion is.
  1. $6$
  2. $4$
  3. $8$
  4. $12$
  1. Which is not the correct statement for ionic solids, in which positive and negative ions are held by strong electrostatic attractive forces?
  1. The radius ratio $\frac{\text{r}_+}{r}$ increases as coordination number increases.
  2. As the difference in size of ions increases, coordination number increases.
  3. When coordination number is eight, $\frac{\text{r}_+}{r}$ ratio lies between $0.225$ to $0.414.$
  4. In ionic solid of the type AX (ZnS, wurtzite), the coordination number of $Zn^2$ and $S^2$- respectively are $4 $and $4.$
  1. If the pressure of CsCl is increased, then its coordination number will.
  1. Increase
  2. Remain the same
  3. Decrease
  4. None of these.
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Q 29Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions:
The idealized ionic solid consists of two interpenetrating lattices of oppositely-charged point charges that are held in place by a balance of coulombic force of long range. But real ions occupy space, no such "perfect" ionic solid exists in nature. Chemists usually apply the term "ionic solid" to binary compounds of the metallic elements of groups $1 - 2$ with one of the halogen elements or oxygen. The most well known ionic solid is sodium chloride, also known by its geological names as rock-salt or halite. Structurally, each ion in sodium chloride is surrounded and held in tension by six neighbouring ions of opposite charge; this is known as $(6, 6)$ coordination. The resulting crystal lattice is of a type known as simple cubic. There are many other fundamental ionic structures (not all cubic) and these are: Zinc blende structure $(ZnS) $: having ccp arrangement of $S^2-$ and $Zn^{2+}$ in alternate tetrahedral voids; Wurtzite structure $(ZnS)$ having hcp arrangement of $S^2-$ and $Zn^{2+}$ in alternate tetrahedral voids; Fluorite structure $(CaF2)$ having ccp arrangement of $Ca^{2+}$ and$ F^-$ in all tetrahedral voids Antifluorite structure $(Na_2O)$ having ccp arrangement of $O^{2-}$ and $Na^+$ in all tetrahedral voids. These solids tend to be quite hard and have high melting points.
The following questions are multiple choice questions. Choose the most appropriate answer.
  1. In $NaCl$ crystal, each $Cl^-$ ion is surrounded by.
  1. $4\ Na^+$ ions
  2. $6\ Na^+$ ions
  3. $1\ Na^+$ ion
  4. $2\ Na^+$ ions
  1. In an antifluorite structure, cations occupy.
  1. Tetrahedral voids.
  2. Centre of cube
  3. Octahedral voids
  4. Corners of cube.
  1. Anti fluorite structure is derived from fluorite structure by.
  1. Heating fluorite crystal lattice.
  2. Subjecting fluorite structure to high pressure.
  3. Interchanging the positions of positive and negative ions in the lattice.
  4. None of these.
  1. In crystal structure of sodium chloride, the arrangement of $Cl^-$ion is.
  1. fcc
  2. both fcc and bcc
  3. bcc
  4. None of these
  1. Ionic solid $BaF_2$ has which kind of structure?
  1. Fluorite
  2. Antifluorite
  3. Wurtzite
  4. Rock-salt
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Q 30Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions:
In an assembly of atoms or molecules, a solid phase is formed whenever the interatomic attractive forces significantly exceed the disruptive thermal forces and thus restrict the mobility of atoms, forcing them into more or less fixed positions. From energy considerations, it is evident that in such solids the atoms or molecules will always attempt to assume highly ordered structures which are characterised by symmetry. Depending on the nature of the active interatomic forces, all solids may be subdivided into the following categories :
Ionic solids: These solids consist of positively and negatively charged ions arranged in a regular fashion throughout the solid. These solids are very hard and brittle, have very high melting points and have high enthalpies of vaporisation, e.g., NaCl, MgO, KCl, LiCl etc.
Covalent solids: In these solids, the constituent particles are atoms which are linked together by a continuous system of covalent bonds. These bonds are strong and directional in nature. The covalent crystals are hard, have high melting points, are poor conductors of electricity. Diamond is a typical example of covalent solids.
Metallic solids: ln these solids, the constituent particles are positive ions immersed in a sea of mobile electrons. Metallic solids may be hard as well as soft. They are good conductors of heat and electricity, e.g., common metals such as nickel, copper and alloys.
Molecular solids: ln these the constituent particles are molecules. The molecules are held together by dispersion forces or London forces, dipole-dipole forces or hydrogen bonds.
In these questions (Q. No. i-iv), a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
  1. Assertion and reason both are correct statements, and reason is correct explanation for assertion.
  2. Assertion and reason both are correct statements, but reason is not correct explanation for assertion.
  3. Assertion is correct statement, but reason is wrong statement.
  4. Assertion is wrong statement, but reason is correct statement.
  1. Assertion: Molecular solids are characterized by low melting point.
Reason: Molecular solids are made up of covalent molecules.
  1. Assertion: Ionic solids are characterized by high melting and boiling point.
Reason: Ionic solids have coulombic forces of attraction between their ions.
  1. Assertion: Covalent solids are insulators of electricity.
Reason: Covalent solids are constituted by ions.
  1. Assertion: Diamond and graphite do not have the same covalent structure.
Reason: Silicon carbide is typical example of network solid.
  1. Assertion: Covalent solids have high melting points.
Reason: Covalent solids have strong electrostatic forces of attraction.
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Q 325 Marks Questions5 Marks
How will you distinguish between the following pairs of terms:
  1. Hexagonal close-packing and cubic close-packing?
  2. Crystal lattice and unit cell?
  3. Tetrahedral void and octahedral void?
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Q 335 Marks Questions5 Marks
The edge length of unit cell of a metal having molecular weight $75g/ mol$ is $5\mathring{\text{A}}$ which crystallises in cubic lattice. If the density is $2g/ cm^3$ then find the radius of metal atom. $(N_A = 6.022 \times 10^{23}​​​​​​​)$
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Q 355 Marks Questions5 Marks
Chromium crystallises in bcc structure. If its atomic diameter is $245\ pm$, find its density. Atomic mass of $Cr = 52$ amu and $N_A = 6.02 \times 10^{23}\ mol^{–1}.$
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