Q. Which of the following describes the term 'lattice energy'? (2023)
A.
Energy required to vaporize a solid
B.
Energy released when ions form a solid
C.
Energy required to melt a solid
D.
Energy required to break a solid into its constituent atoms
Show solution
Solution
Lattice energy is defined as the energy released when gaseous ions combine to form a solid ionic compound.
Correct Answer:
B
— Energy released when ions form a solid
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Q. Which of the following has the highest density? (2019)
A.
Sodium chloride
B.
Copper
C.
Graphite
D.
Silicon dioxide
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Solution
Copper has a higher density compared to the other listed materials due to its closely packed atomic structure.
Correct Answer:
B
— Copper
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Q. Which of the following is a characteristic of ionic solids? (2020)
A.
High electrical conductivity in solid state
B.
High melting point
C.
Low density
D.
Malleable
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Solution
Ionic solids are characterized by high melting points due to the strong electrostatic forces between the ions.
Correct Answer:
B
— High melting point
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Q. Which of the following is a property of amorphous solids? (2023)
A.
Anisotropic
B.
Isotropic
C.
Definite melting point
D.
Ordered structure
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Solution
Amorphous solids are isotropic, meaning their properties are the same in all directions, unlike crystalline solids.
Correct Answer:
B
— Isotropic
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Q. Which of the following is a property of covalent network solids? (2023)
A.
Good electrical conductors
B.
High melting points
C.
Malleable
D.
Soluble in water
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Solution
Covalent network solids, such as diamond, have very high melting points due to the strong covalent bonds throughout the structure.
Correct Answer:
B
— High melting points
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Q. Which of the following is an example of a metallic solid? (2023)
A.
NaCl
B.
SiO2
C.
Fe
D.
C12H22O11
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Solution
Iron (Fe) is an example of a metallic solid, characterized by its metallic bonding and properties.
Correct Answer:
C
— Fe
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Q. Which of the following is an example of a molecular solid? (2023)
A.
NaCl
B.
Diamond
C.
Iodine (I2)
D.
Iron (Fe)
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Solution
Iodine (I2) is an example of a molecular solid, where molecules are held together by van der Waals forces.
Correct Answer:
C
— Iodine (I2)
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Q. Which of the following is an example of a non-stoichiometric solid? (2023)
A.
NaCl
B.
FeO
C.
MgO
D.
KCl
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Solution
FeO is an example of a non-stoichiometric solid because it can have varying ratios of iron and oxygen.
Correct Answer:
B
— FeO
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Q. Which of the following is NOT a characteristic of crystalline solids? (2019)
A.
Anisotropy
B.
Definite melting point
C.
Isotropy
D.
Long-range order
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Solution
Crystalline solids exhibit anisotropy, meaning their properties vary with direction, while isotropy refers to uniform properties in all directions.
Correct Answer:
C
— Isotropy
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Q. Which of the following is NOT a characteristic of ionic solids? (2021)
A.
High melting point
B.
Electrical conductivity in solid state
C.
Brittleness
D.
Solubility in water
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Solution
Ionic solids do not conduct electricity in the solid state; they conduct when melted or dissolved in water.
Correct Answer:
B
— Electrical conductivity in solid state
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Q. Which of the following is NOT a property of crystalline solids? (2021)
A.
Anisotropy
B.
Definite melting point
C.
Isotropy
D.
Long-range order
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Solution
Crystalline solids exhibit anisotropy, meaning their properties vary with direction. Isotropy is a property of amorphous solids.
Correct Answer:
C
— Isotropy
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Q. Which of the following is NOT a property of metals? (2021)
A.
Good electrical conductivity
B.
Brittleness
C.
Malleability
D.
Ductility
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Solution
Brittleness is not a property of metals; they are typically malleable and ductile.
Correct Answer:
B
— Brittleness
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Q. Which of the following is NOT a type of crystal system? (2021)
A.
Cubic
B.
Tetragonal
C.
Hexagonal
D.
Quadratic
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Solution
Quadratic is not a recognized type of crystal system; the correct systems include cubic, tetragonal, hexagonal, orthorhombic, and others.
Correct Answer:
D
— Quadratic
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Q. Which of the following is NOT a type of crystalline solid? (2021)
A.
Ionic
B.
Molecular
C.
Amorphous
D.
Metallic
Show solution
Solution
Amorphous solids do not have a long-range order and are not classified as crystalline solids.
Correct Answer:
C
— Amorphous
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Q. Which of the following properties is characteristic of covalent network solids? (2019)
A.
High electrical conductivity
B.
Brittleness
C.
Low melting points
D.
Solubility in water
Show solution
Solution
Covalent network solids are typically brittle due to the strong covalent bonds that do not allow for easy deformation.
Correct Answer:
B
— Brittleness
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Q. Which of the following properties is characteristic of ionic solids? (2021)
A.
High electrical conductivity
B.
Low melting point
C.
Brittleness
D.
Malleability
Show solution
Solution
Ionic solids are typically brittle due to the strong electrostatic forces between the ions, which cause them to shatter when force is applied.
Correct Answer:
C
— Brittleness
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Q. Which of the following properties is typical of metallic solids? (2019)
A.
Brittleness
B.
Electrical conductivity
C.
Low melting point
D.
Insulating nature
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Solution
Metallic solids are known for their high electrical conductivity due to the presence of free-moving electrons.
Correct Answer:
B
— Electrical conductivity
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Q. Which of the following solids has a high degree of anisotropy? (2019)
A.
Ionic solids
B.
Covalent solids
C.
Metallic solids
D.
Molecular solids
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Solution
Covalent solids exhibit a high degree of anisotropy due to their directional bonding.
Correct Answer:
B
— Covalent solids
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Q. Which of the following solids has a high thermal conductivity? (2019)
A.
Ionic solids
B.
Covalent solids
C.
Metallic solids
D.
Molecular solids
Show solution
Solution
Metallic solids have high thermal conductivity due to the presence of free-moving electrons.
Correct Answer:
C
— Metallic solids
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Q. Which of the following structures has the highest packing efficiency? (2019)
A.
Simple cubic
B.
Body-centered cubic
C.
Face-centered cubic
D.
Hexagonal close-packed
Show solution
Solution
The face-centered cubic (FCC) structure has the highest packing efficiency of approximately 74%.
Correct Answer:
C
— Face-centered cubic
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Q. Which of the following types of solids has the highest melting point? (2019)
A.
Ionic solids
B.
Covalent network solids
C.
Molecular solids
D.
Metallic solids
Show solution
Solution
Covalent network solids, such as diamond, have the highest melting points due to the strong covalent bonds throughout the structure.
Correct Answer:
B
— Covalent network solids
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Q. Which type of crystal system has the highest symmetry? (2022)
A.
Cubic
B.
Tetragonal
C.
Orthorhombic
D.
Monoclinic
Show solution
Solution
The cubic crystal system has the highest symmetry among all crystal systems.
Correct Answer:
A
— Cubic
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Q. Which type of solid has a definite melting point and is composed of molecules held together by van der Waals forces? (2022)
A.
Ionic solid
B.
Metallic solid
C.
Molecular solid
D.
Covalent solid
Show solution
Solution
Molecular solids are composed of molecules held together by van der Waals forces and have a definite melting point.
Correct Answer:
C
— Molecular solid
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Q. Which type of solid has a definite melting point and is usually hard and brittle? (2022)
A.
Molecular solids
B.
Ionic solids
C.
Metallic solids
D.
Amorphous solids
Show solution
Solution
Ionic solids have a definite melting point and are typically hard and brittle due to the strong ionic bonds between the ions.
Correct Answer:
B
— Ionic solids
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Q. Which type of solid has a definite melting point? (2022)
A.
Amorphous solid
B.
Crystalline solid
C.
Polymeric solid
D.
Metallic solid
Show solution
Solution
Crystalline solids have a definite melting point due to their ordered structure, unlike amorphous solids which melt over a range of temperatures.
Correct Answer:
B
— Crystalline solid
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Showing 31 to 55 of 55 (2 Pages)
Physical Chemistry - Solid State MCQ & Objective Questions
Understanding "Physical Chemistry - Solid State" is crucial for students aiming to excel in their exams. This topic not only forms a significant part of the syllabus but also helps in developing a strong conceptual foundation. Practicing MCQs and objective questions related to solid-state chemistry can greatly enhance your exam preparation and boost your scores. By regularly solving practice questions, you can identify important questions and improve your problem-solving skills.
What You Will Practise Here
Crystal structures and types of lattices
Unit cell dimensions and calculations
Types of solids: ionic, covalent, metallic, and molecular
Defects in solids: point defects, line defects, and surface defects
Electrical and thermal properties of solids
Band theory of solids and its applications
Phase diagrams and phase transitions
Exam Relevance
The topic of "Physical Chemistry - Solid State" is frequently featured in various examinations such as CBSE, State Boards, NEET, and JEE. Students can expect questions that test their understanding of crystal structures, properties of solids, and calculations related to unit cells. Common question patterns include multiple-choice questions that require conceptual clarity and application of formulas, making it essential to practice regularly.
Common Mistakes Students Make
Confusing different types of crystal lattices and their properties
Miscalculating unit cell dimensions and relationships
Overlooking the significance of defects in solids
Failing to apply band theory correctly in problem-solving
Neglecting the importance of phase diagrams in understanding material behavior
FAQs
Question: What are the key properties of ionic solids?Answer: Ionic solids are characterized by high melting points, electrical conductivity in molten state, and brittleness due to strong ionic bonds.
Question: How do defects in solids affect their properties?Answer: Defects can influence electrical conductivity, mechanical strength, and diffusion rates in solids, making them crucial for material performance.
Start your journey towards mastering "Physical Chemistry - Solid State" by solving practice MCQs today! Testing your understanding with objective questions will not only prepare you for exams but also enhance your confidence in tackling complex problems.
