Preparing for the Joint Entrance Exam (JEE) can be a daunting task. With so many subjects to cover and so many topics to study, it can be challenging to know where to start. One essential topic in the JEE Mains syllabus is the The Solid State. In this article, we will provide 50+ MCQ questions on the The Solid State, along with detailed solutions to help you prepare for the JEE Mains exam.
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These 50+ MCQ questions are selected by the experts of studyrate.in and these are more difficult questions, which will help you to better understand The Solid State JEE Mains MCQ Questions with Answers.
The Solid State JEE Mains MCQ
Which of the following compounds exhibits both ionic and covalent bonding? a) NaCl b) SiO2 c) MgO d) FeS
Answer: b) SiO2
Explanation: SiO2, also known as silicon dioxide or silica, exhibits both ionic and covalent bonding. It has a three-dimensional network structure where silicon atoms are covalently bonded to oxygen atoms. However, there is no transfer of electrons between silicon and oxygen, making it a covalent compound.
Which of the following statements is true regarding amorphous solids? a) They have a definite geometric shape. b) They have long-range order. c) They are anisotropic in nature. d) They have sharp melting points.
Answer: d) They have sharp melting points.
Explanation: Amorphous solids lack long-range order, meaning their constituent particles are not arranged in a regular pattern. They do not have a definite geometric shape, as they tend to be irregular in nature. They are isotropic, meaning their properties do not depend on the direction of measurement. Unlike crystalline solids, amorphous solids do not have sharp melting points and instead soften over a range of temperatures.
The number of octahedral voids per atom in a close-packed structure is: a) 2 b) 4 c) 6 d) 8
Answer: b) 4
Explanation: In a close-packed structure, such as a face-centered cubic (FCC) or hexagonal close-packed (HCP) arrangement, each atom is in contact with 12 nearest neighbors. Out of these 12 nearest neighbors, 6 are in the same layer, occupying octahedral voids. Therefore, the number of octahedral voids per atom in a close-packed structure is 4.
Which of the following represents a Schottky defect? a) Anions missing from lattice sites b) Cations missing from lattice sites c) Anions occupying interstitial sites d) Cations occupying interstitial sites
Answer: b) Cations missing from lattice sites
Explanation: A Schottky defect is a type of point defect in ionic solids where both cations and anions are missing from their regular lattice sites. This defect occurs to maintain electrical neutrality in the crystal lattice. Therefore, cations missing from lattice sites represent a Schottky defect.
Which of the following statements is true for p-type semiconductors? a) They are doped with a pentavalent impurity. b) They have an excess of electrons. c) They are formed by doping a semiconductor with a trivalent impurity. d) They have an excess of holes.
Answer: c) They are formed by doping a semiconductor with a trivalent impurity.
Explanation: P-type semiconductors are formed by doping a pure semiconductor with a trivalent impurity, such as boron or aluminum. These impurities create electron deficiency or “holes” in the crystal lattice, resulting in a net positive charge. Therefore, p-type semiconductors have an excess of holes.
The coordination number of a metal ion in a body-centered cubic (BCC) structure is: a) 4 b) 6 c) 8 d) 12
Answer: c) 8
Explanation: In a body-centered cubic (BCC) structure, each metal ion is in contact with eight nearest neighbors. Therefore, the coordination number of a metal ion in a BCC structure is 8.
Which of the following substances exhibits Frenkel defect? a) AgCl b) NaCl c) CaO d) ZnS
Answer: a) AgCl
Explanation: Frenkel defect is a type of point defect where a cation is dislocated from its regular lattice site and occupies an interstitial position within the crystal lattice. AgCl exhibits Frenkel defect because silver cations (Ag+) can occupy interstitial sites in the crystal lattice of AgCl.
The density of a solid is 5.0 g/cm³ and its unit cell edge length is 2.5 Å. The molar mass of the solid is approximately: a) 100 g/mol b) 200 g/mol c) 400 g/mol d) 800 g/mol
Answer: b) 200 g/mol
Explanation: The density of a solid can be calculated using the formula:
Density = (Mass of unit cell) / (Volume of unit cell)
The volume of a unit cell can be calculated as (Edge length)³. Therefore, the mass of the unit cell is (Density) × (Volume of unit cell). Since the given density is in g/cm³, the volume of the unit cell should be converted to cm³. Finally, the molar mass can be calculated by dividing the mass of the unit cell by Avogadro’s number.
Which of the following oxides is considered an amphoteric oxide? a) Na2O b) Al2O3 c) CO2 d) CaO
Answer: b) Al2O3
Explanation: Amphoteric oxides can act as both acidic and basic oxides, depending on the reaction conditions. Al2O3, also known as aluminum oxide or alumina, is an amphoteric oxide. It can react with both acids and bases to form salts.
The process of conversion of a solid directly into a vapor is called: a) Sublimation b) Evaporation c) Condensation d) Fusion
Answer: a) Sublimation
Explanation: Sublimation is the process where a solid directly converts into a vapor without passing through the liquid state. Examples of substances that undergo sublimation include dry ice (solid carbon dioxide) and iodine crystals.
The energy required to remove an electron from a solid to infinity is called: a) Ionization energy b) Electron affinity c) Lattice energy d) Work function
Answer: a) Ionization energy
Explanation: Ionization energy is the energy required to remove an electron from an atom or ion in the gas phase to infinity. In the context of solids, ionization energy refers to the energy required to remove an electron from a solid to an infinitely separated state.
The electrical conductivity of a semiconductor: a) Increases with an increase in temperature b) Decreases with an increase in temperature c) Remains constant with temperature d) First increases and then decreases with temperature
Answer: d) First increases and then decreases with temperature
Explanation: The electrical conductivity of a semiconductor initially increases with an increase in temperature due to the increased thermal energy, which allows more charge carriers to move. However, at higher temperatures, intrinsic carriers may be thermally ionized, leading to a decrease in conductivity.
Which of the following compounds shows Frenkel defect? a) MgO b) NaCl c) ZnO d) CsCl
Answer: a) MgO
Explanation: Frenkel defect occurs when a cation leaves its lattice site and occupies an interstitial site in the crystal lattice. MgO exhibits Frenkel defect because magnesium cations (Mg2+) can occupy interstitial sites in the crystal structure of MgO.
The efficiency of close packing in a crystal lattice is approximately: a) 26% b) 52% c) 68% d) 74%
Answer: d) 74%
Explanation: The efficiency of close packing is defined as the ratio of the volume occupied by the spheres to the total volume of the unit cell. The maximum packing efficiency achievable in a crystal lattice is approximately 74%.
Which of the following properties is not shown by an ionic compound? a) High melting and boiling points b) Conductivity in the molten state c) Ability to form alloys d) Brittleness
Answer: c) Ability to form alloys
Explanation: Ionic compounds typically do not show the ability to form alloys. Alloys are formed by the mixing of two or more metallic elements, where the metallic bonds play a crucial role. Ionic compounds consist of positively and negatively charged ions held together by strong electrostatic forces, which makes them less likely to form alloys.
Which of the following represents a substitutional solid solution? a) Heterogeneous mixture b) Interstitial alloy c) Alloys with different crystal structures d) Alloys with similar atomic sizes
Answer: d) Alloys with similar atomic sizes
Explanation: A substitutional solid solution is formed when atoms of different elements replace each other in the crystal lattice. For this to occur, the elements should have similar atomic sizes to maintain the crystal structure. Therefore, alloys with similar atomic sizes represent a substitutional solid solution.
The geometry of a unit cell in a face-centered cubic (FCC) crystal lattice is: a) Tetrahedral b) Octahedral c) Cubic d) Dodecahedral
Answer: c) Cubic
Explanation: The unit cell in a face-centered cubic (FCC) crystal lattice has a cubic geometry. It consists of atoms at each corner of the cube and one atom at the center of each face.
The edge length of a unit cell of a simple cubic lattice is 3.5 Å. The volume of the unit cell in cm³ is approximately: a) 4.375 b) 42.875 c) 43.75 d) 437.5
Answer: a) 4.375
Explanation: The volume of a unit cell in a simple cubic lattice can be calculated as (Edge length)³. Therefore, substituting the given edge length of 3.5 Å (convertible to cm), the volume of the unit cell is approximately 4.375 cm³.
The intermolecular forces responsible for the adsorption of gases on solids are: a) Covalent bonds b) Ionic bonds c) Vander Waals forces d) Hydrogen bonding
Answer: c) Vander Waals forces
Explanation: The intermolecular forces responsible for the adsorption of gases on solids are mainly Vander Waals forces. Vander Waals forces include London dispersion forces and dipole-dipole interactions, which arise due to temporary fluctuations in electron distribution and the presence of dipoles in molecules.
The compound formed by cationic and anionic vacancies in a crystal lattice is known as: a) Frenkel defect b) Schottky defect c) Interstitial defect d) Stoichiometric defect
Answer: b) Schottky defect
Explanation: Schottky defect refers to the formation of cationic and anionic vacancies in a crystal lattice, leading to the maintenance of electrical neutrality. It is a type of point defect commonly observed in ionic compounds.
Which of the following substances is an example of an n-type semiconductor? a) Pure silicon b) Boron-doped silicon c) Phosphorus-doped silicon d) Aluminum-doped silicon
Answer: c) Phosphorus-doped silicon
Explanation: An n-type semiconductor is formed by doping a pure semiconductor with a pentavalent impurity. Phosphorus is a pentavalent impurity, and when doped into silicon, it introduces excess electrons, making the material an n-type semiconductor.
The process of conversion of a gas directly into a solid is called: a) Vaporization b) Deposition c) Condensation d) Sublimation
Answer: b) Deposition
Explanation: Deposition is the process where a gas directly converts into a solid without going through the liquid state. This occurs when the temperature of the gas decreases, causing the gas molecules to lose energy and form a solid.
The property of a substance to absorb moisture from the atmosphere is called: a) Hygroscopy b) Deliquescence c) Efflorescence d) Sublimation
Answer: a) Hygroscopy
Explanation: Hygroscopy refers to the property of a substance to absorb moisture from the atmosphere. Substances that are hygroscopic tend to be capable of attracting and retaining water molecules.
Which of the following oxides is an example of an acidic oxide? a) Na2O b) MgO c) SO2 d) CaO
Answer: c) SO2
Explanation: Acidic oxides are oxides that react with water to form acids. SO2, sulfur dioxide, is an example of an acidic oxide as it can dissolve in water to form sulfurous acid (H2SO3).
The ability of a solid to be drawn into wires is called: a) Ductility b) Malleability c) Conductivity d) Luster
Answer: a) Ductility
Explanation: Ductility is the property of a substance that allows it to be drawn into thin wires. It is a characteristic commonly observed in metals.
The coordination number of an atom in a body-centered cubic (BCC) lattice is: a) 4 b) 6 c) 8 d) 12
Answer: b) 6
Explanation: In a body-centered cubic (BCC) lattice, each atom is in contact with 8 nearest neighbors. The coordination number represents the number of nearest neighbors surrounding an atom, and in the case of BCC, it is 6.
The formula unit of sodium chloride (NaCl) represents: a) One sodium ion and one chloride ion b) One sodium atom and one chlorine atom c) One sodium atom and two chlorine atoms d) One sodium ion and two chloride ions
Answer: a) One sodium ion and one chloride ion
Explanation: The formula unit of sodium chloride (NaCl) represents one sodium ion (Na+) and one chloride ion (Cl-) in the crystal lattice. It does not indicate the individual atoms present.
Which of the following statements is true regarding the arrangement of particles in a crystalline solid? a) Particles are randomly arranged. b) Particles are arranged in a regular and repeating pattern. c) Particles are arranged in a disordered manner. d) Particles are arranged with long-range order.
Answer: d) Particles are arranged with long-range order.
Explanation: In a crystalline solid, particles are arranged in a regular and repeating pattern, which exhibits long-range order. This means that the arrangement of particles extends throughout the entire crystal lattice.
The type of solid that exhibits a sharp melting point is: a) Amorphous solid b) Crystalline solid c) Molecular solid d) Metallic solid
Answer: b) Crystalline solid
Explanation: Crystalline solids have a well-defined and regular arrangement of particles, which leads to a sharp melting point. In contrast, amorphous solids do not have a regular arrangement and soften over a range of temperatures.
The process of conversion of a solid directly into a gas is called: a) Sublimation b) Evaporation c) Condensation d) Fusion
Answer: a) Sublimation
Explanation: Sublimation is the process where a solid directly converts into a gas without passing through the liquid state. This occurs when the temperature and pressure conditions allow the solid to vaporize without melting.
We hope there JEE MCQ of Class 12 : The Solid State will help you to score an excellent rank in JEE Mains and Advanced. If you have any queries feel free to write in the comments section. We at Study Rate are always ready to serve our students.