Material Science MCQs (Multiple-Choice Questions)

1. Which of the following is true about material science?

1. Materials science studies the interaction between a material's atomic and molecular structure.
2. Materials science studies the characteristics of materials.
3. Materials science studies how the material is transformed into an object.
4. All of the above

Answer: D) All of the above

Explanation:

All the above statements are correct.

• Materials science is the study of the interactions between a material's atomic and molecular structure, as well as how these interactions affect the material's qualities and behavior.
• Materials science is the study of material properties, which include thermal, mechanical, electrical, and magnetic, among others.
• Materials science investigates how a material is converted into an item, including techniques such as casting, forging, and machining, and how these transformations affect the material's qualities and performance.

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2. How many classifications are there for materials?

1. 5
2. 6
3. 2
4. 4

Answer: D) 4

Explanation:

Metals, polymers, ceramics, and composites are the four major types of materials.

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3. Which of the following types of material has a large number of nonlocalized electrons?

1. Metallic materials
2. Polymers
3. Ceramics
4. Composites

Answer: A) Metallic materials

Explanation:

Metallic materials have a high range of nonlocalized electrons. Metal electrons are nonlocalized, which means they are not linked to individual atoms and can move freely across the crystal structure, providing a "floor" of mobile electrons capable of carrying electricity.

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4. Cast iron belongs to which of the following categories?

1. Metals
2. Polymers
3. Ceramics
4. Composites

Answer: A) Metals

Explanation:

Cast iron falls within the category of metals. Cast iron is well-known for its great castability, outstanding mechanical qualities, and high wear resistance, making it a popular material for engine blocks, pipelines, cookware, and other uses.

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5. Which of the following types of metal is known as steel metal?

1. Non-Ferrous metals
2. Ferrous
3. Alloys
4. All of the above

Answer: B) Ferrous

Explanation:

Steel is a type of metal that belongs to the ferrous metal group. Steel is mostly made of iron with a small percentage of carbon and other components. Ferrous metals are those that have iron as a major component, and steel consists mainly of iron with a tiny amount of carbon and other elements.

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6. Which of the following is true about ceramic structure?

1. Ceramics have a crystalline structure.
2. Ceramics have a highly repetitive pattern structure.
3. The atoms of ceramics are highly ordered.
4. All of the above

Answer: D) All of the above

Explanation:

All three statements (A, B, and C) about the structure of ceramics are correct. Ceramics have a crystalline structure, which means that their atoms are arranged in a repeating pattern.

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7. Which of the following is not a type of biomaterial?

1. Composite
2. Alloys
3. Metals
4. Ceramics

Answer: B) Alloys

Explanation:

Alloys are not generally considered a unique form of biomaterial. Biomaterials are often classified into three types: Metals, polymers, and ceramics.

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8. Which of the following is true about isotopes?

1. In chemistry, an isotope is an atom with the same number of protons but with a different number of neutrons.
2. In chemistry, an isotope is an atom with the same number of neutrons but with a different number of protons.
3. None
4. Both A and B

Answer: A) In chemistry, an isotope is an atom with the same number of protons but with a different number of neutrons.

Explanation:

Isotopes are elements that have the same number of protons but differ in the number of neutrons in their atomic nuclei. Carbon-12 (12C) and carbon-14 (14C) are two isotopes of carbon, for example. Both have six protons, but they differ in the number of neutrons.

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9. An ion with a net negative charge is known as ____

1. Cation
2. Electron
3. Neutron
4. Anion

Answer: D) Anion

Explanation:

An ion with a net negative charge is referred to as an "anion." Anions are generated when an atom obtains one or more electrons, resulting in an excess of negatively charged electrons in the nucleus relative to protons that are charged positively.

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10. Atoms with the same number of neutrons but a different number of protons are called _____.

1. Isotones
2. Isotopes
3. Isomers
4. Isobars

Answer: A) Isotones

Explanation:

Isotones are atoms of various chemical elements that have the same neutron number but different atomic numbers (which indicate different numbers of protons).

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11. What do you mean by Ion?

1. The amount of energy required to extract an electron from an atom
2. Any atom or molecule that carries a net charge
3. It is the energy change that occurs in an atom when it obtains an electron
4. None

Answer: B) Any atom or molecule that carries a net charge

Explanation:

An ion is a molecule or atom with an uneven number of protons and electrons, resulting in a net electrical charge.

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12. The amount of energy required to extract an electron from an atom is known as ____.

1. Isothermal energy
2. Orbital energy
3. Atomic orbital energy
4. Ionization energy

Answer: D) Ionization energy

Explanation:

The amount of energy required to remove an electron from an atom is referred to as ionization energy. This energy is commonly measured in electronvolts (eV) or kilojoules per mole (kJ/mol).

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13. Which of the following is true about the nucleus?

1. The nucleus is made up of neutrons
2. The nucleus is made up of protons
3. The nucleus is made up of protons and neutrons
4. The nucleus is made up of shells and subshells

Answer: C) The nucleus is made up of protons and neutrons

Explanation:

An atom's nucleus is made up of protons and neutrons that are bound together by a strong nuclear force. Neutrons are neutrally charged particles, whereas protons are positively charged particles.

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14. How many types of chemical bonds are there based on strength?

1. 6
2. 7
3. 2
4. 5

Answer: C) 2

Explanation:

Chemical bonds are divided into primary and secondary bonds based on their strength.

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15. Which of the following types of bonds is an interatomic bond?

1. Primary bond
2. Secondary bond
3. Both A and B
4. None of the above

Answer: A) Primary bond

Explanation:

Interatomic bonds, or primary bonds, are strong chemical bonds that involve the sharing of electrons between atoms and are responsible for binding atoms together in molecules and compounds.

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16. How many types of bonds are there?

1. 5
2. 6
3. 4
4. 2

Answer: C) 4

Explanation:

There are four types of bonds:

• Ionic Bonding
• covalent bonding
• metallic bonding
• Hydrogen bonding

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17. Which of the following bonds is classified as a secondary bond?

1. Ionic Bonding
2. Covalent bonding
3. Metallic bonding
4. Hydrogen bonding

Answer: D) Hydrogen bonding

Explanation:

Primary (or strong) chemical bonds such as ionic, covalent, and metallic bonds are stronger than secondary bonds. Hydrogen bonds are a sort of secondary bond that is comparatively weaker than the primary bonds.

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18. In which of the following types of bonding do all positively charged atoms attract all negatively charged atoms?

1. Ionic Bonding
2. Covalent bonding
3. Metallic bonding
4. Hydrogen bonding

Answer: A) Ionic Bonding

Explanation:

In ionic bonding, all positively charged atoms (cations) attract all negatively charged atoms (anions). These bonds are produced by electrostatic attraction between oppositely charged ions, where electrons are transported from one atom to another, resulting in positively charged cations and negatively charged anions.

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19. Which of the following types of atomic models in material science says that atoms have a high density of positively charged nuclei in the center and negatively charged electrons revolving around them?

1. Bohr model
2. Rutherford model
3. Wave mechanical model
4. Band theory model

Answer: D) Band theory model

Explanation:

The Rutherford model was offered by Ernest Rutherford in 1911, which states that atoms have a high density of positively charged nuclei in the center with negatively charged electrons revolving around them.

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20. Which of the following theories explains the bonding and anti-bonding interactions between atoms in a molecule?

1. Wave mechanical model
2. Band theory model
3. Molecular orbital theory
4. Band theory model

Answer: C) Molecular orbital theory

Explanation:

The molecular orbital theory describes the bonding and anti-bonding interactions between atoms in a molecule.

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21. Which of the following mathematical formulas is used to find the radius of the nucleus?

1. R = R₀ (A) ^1/3 cm
2. R = R₀ (A) cm
3. R = R₀ (A) ^1/2 cm
4. R = R₀ (A) ³ cm

Answer: A) R = R₀ (A) ^1/3 cm

Explanation:

R = R₀ (A) ^1/3 cm. This formula is used to find the radius of the nucleus, where R is the radius of the nucleus, R0 is a constant, and A is the mass number of the nucleus.

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22. Number of orbitals in a subshell?

1. L
2. L+1/3
3. L+10
4. L+1

Answer: D) L+1

Explanation:

The azimuthal quantum number (denoted by L) in an atom denotes the number of orbitals in a subshell. As a result, the number of orbitals in a subshell equals L + 1.

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23. In which of the following conditions is a photon emitted?

1. When an atom or molecule moves from a lower energy state to a higher energy level
2. When an atom or molecule moves from a higher energy state to a lower energy level
3. When an atom or molecule stays in a higher energy state
4. When an atom or molecule moves, it stays at a lower energy level

Answer: B) When an atom or molecule moves from a higher energy state to a lower energy level

Explanation:

A photon is emitted when an atom or molecule moves from a higher energy state to a lower energy state, releasing excess energy in the form of a photon.

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24. Which of the following statements is not true according to Bohr's models?

1. When an electron moves from a higher to a lower energy level, it emits a photon
2. Electrons do not radiate energy
3. Electrons can absorb or emit energy
4. Electrons can exist in every orbit, irrespective of their discrete energy levels

Answer: D) Electrons can exist in every orbit, irrespective of their discrete energy levels

Explanation:

According to Bohr's theory, electrons can only exist in certain, defined orbits with quantized energy levels.

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25. Horizontal rows in the periodic table are called ____.

1. Periods
2. Groups
3. Family
4. Block

Answer: A) Periods

Explanation:

Periods are horizontal rows in the periodic table. Each period indicates a different energy level.

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26. Which of the following statements is true about the periodic table?

1. Elements in the same group have different valence electron configurations but the same chemical properties
2. Elements in the same group have the same valence electron configuration but different chemical properties
3. Elements in the same group have different valence electron configurations and different chemical properties
4. Elements in the same group have the same valence electron configuration and the same chemical properties

Answer: D) Elements in the same group have the same valence electron configuration and the same chemical properties

Explanation:

Elements in the same group have the same valence electron configuration and the same chemical properties because their outermost energy level has the same number of electrons.

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27. Who is the father of the periodic table?

1. Dimitri Mendeleev
2. Niels Bohr
3. Ernest Rutherford
4. None of the above

Answer: A) Dimitri Mendeleev

Explanation:

Russian chemist Dmitri Mendeleev is generally credited with developing the first widely accepted periodic table of elements. He presented his version of the periodic table in 1869, which arranged the known elements according to their properties and atomic weights.

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28. What are the SI units for measuring atomic radii?

1. Nanometer
2. Picometer
3. Both A and B
4. None of the above

Answer: C) Both A and B

Explanation:

Atomic radii are usually measured in nanometers (nm) and picometers (pm). 1nm=1×10⁻⁹m and 1pm=1×10⁻¹²m.

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29. What is the relationship between the atomic number and effective nuclear charge in the periodic table?

1. As the atomic number increases, the effective nuclear charge also increases
2. As the atomic number decreases, the effective nuclear charge also decreases
3. As the atomic number increases, the effective nuclear charge decreases
4. As the atomic number decreases, the effective nuclear charge increases

Answer: A) As the atomic number increases, the effective nuclear charge also increases

Explanation:

As we go from left to right in the periodic table, the atomic number increases, increasing the number of protons in the nucleus. As a result, the nucleus has a larger positive charge, which increases the effective nuclear charge.

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30. Which of the following has the highest ionization energies in the periodic table?

1. Non-metals
2. Metals
3. Noble gases
4. Halogens

Answer: C) Noble gases

Explanation:

Noble gases have the highest ionization energies because they have stable electron configurations.

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31. What is the effect on ionization energy when we move from left to right across periods in the periodic table?

1. Ionization energy increases
2. Ionization energy decreases
3. Remain same
4. None of the above

Answer: A) Ionization energy increases

Explanation:

Because the effective nuclear charge increases, ionization energies increase from left to right.

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32. Fill in the blank: The metallic character ____ as we move across the table from left to right.

1. Increases
2. Decreases
3. Same
4. losses

Answer: B) Decreases

Explanation:

The metallic character decreases as we move across the table from left to right.

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33. In the periodic table, Fluorine, Chlorine, and Bromine is considered as ____.

1. Noble gases
2. Alkali metals
3. Alkali earth metals
4. Halogens

Answer: D) Halogens

Explanation:

Fluorine, chlorine, bromine, iodine, and stanol are the five nonmetal elements that makeup halogens. When they react with metals, they generate salts.

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34. Which of the following halogens is a known liquid in the periodic table?

1. Fluorine
2. Chlorine
3. Bromine
4. Iodine

Answer: C) Bromine

Explanation:

Bromine is a known liquid at normal temperature; it exists as a brown-red liquid.

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35. Which of the following has higher ionization energy?

1. Nitrogen
2. Oxygen
3. Carbon
4. Hydrogen

Answer: A) Nitrogen

Explanation:

The highest ionization energy is found in nitrogen. Nitrogen is found in the periodic table's p-block.

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36. Which of the following has the highest degree of symmetry among all the crystal systems?

1. Monoclinic system
2. Cubic system
3. Hexagonal system
4. Tetragonal system

Answer: B) Cubic system

Explanation:

The cubic system has the maximum degree of symmetry due to the equal length of its three mutually perpendicular axes and the regularity of its lattice structure.

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37. The hexagonal system shows which of the following types of Bravais lattices?

1. Primitive
2. Non-primitive
3. Body-centered
4. Face centered

Answer: A) Primitive

Explanation:

The arrangement of points that creates the structure in the hexagonal system is known as a primitive Bravais lattice.

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38. Which of the following is not an example of FCC (face-centered cubic)?

1. Aluminium
2. Copper
3. Lead
4. Zinc

Answer: D) Zinc

Explanation:

Aluminium, copper, and lead are examples of FCC, and zinc is an example of a hexagonal close-packed.

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39. Among FCC structures and HCP structures, which have the highest packing efficiency?

1. FCC
2. HCP
3. Both
4. None

Answer: B) HCP

Explanation:

When compared to the face-centered cubic (FCC) structure, the hexagonal close-packed (HCP) structure has higher packing efficiency.

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40. Which of the following is true about amorphous solids?

1. Amorphous solids have a non-crystalline atomic structure
2. Amorphous solids have a crystalline atomic structure
3. Amorphous solids have a semi-crystalline atomic structure
4. None of the above

Answer: A) Amorphous solids have a non-crystalline atomic structure

Explanation:

Amorphous solids have a non-crystalline atomic structure, which means their atoms are not placed in a regular, repeating pattern, as they are in crystals. Instead, the atoms in amorphous solids are randomly organized.

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41. What is the formula for Bragg's Law?

1. d sin θ = nλ
2. 2d sin θ = 2n^λ
3. 2d sin θ = nλ
4. 2d sin θ = n²λ

Answer: C) 2d sin θ = nλ

Explanation:

Bragg's law is expressed as: 2dsinθ=nλ

Where:

• d is the spacing between crystal lattice planes.
• θ is the angle of incidence of the X-ray beam.
• n is an integer representing the order of the diffraction, and
• λ is the wavelength of the x-ray.

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42. Which of the following types of defects is known as a dislocation defect?

1. Point defect
2. Volume defect
3. Line defect
4. Bulk defect

Answer: C) Line defect

Explanation:

Line defects, also known as dislocation defects, are irregularities in the regular arrangement of atoms in a crystal along lines or planes.

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43. Which of the following types of point defects occupy the spaces between the lattice points?

1. Vacancy defect
2. Substitute defect
3. Interstitials defect
4. None of the above

Answer: C) Interstitials defect

Explanation:

Interstitials are atoms or molecules that occupy the spaces between the lattice points.

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44. Among Schottky and Frenkel defects, which reduces the crystal's density?

1. Schottky defects
2. Frenkel defects
3. Both
4. None

Answer: A) Schottky defects

Explanation:

The Schottky defect decreases the density of the crystal by creating vacancies.

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45. Which of the following linear defects are created by shear stress?

1. Edge dislocation
2. Mixed dislocation
3. Interfacial dislocation
4. Screw dislocation

Answer: D) Screw dislocation

Explanation:

Screw dislocations are linear defects created by shear stress.

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46. Fill in the blank: The Burgers vector for an edge dislocation is ____ to the dislocation line.

1. Parallel
2. Straight line
3. Perpendicular
4. None of the above

Answer: C) Perpendicular

Explanation:

The Burgers vector for an edge dislocation is perpendicular to the dislocation line.

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47. How does pressure affect the diffusion process?

1. Reduces the process
2. Increases the process
3. Shows no reaction
4. None of the above

Answer: B) Increases the process

Explanation:

Pressure accelerates diffusion. This is because the pressure increases the density of the diffusing particles, which increases the frequency of collisions, which in turn speeds their diffusion.

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48. Which Fick's law is used for steady-state diffusion?

1. Fick's First Law
2. Fick's second law
3. Both A and B
4. None of the above

Answer: A) Fick's First Law

Explanation:

According to this law, the diffusion flux, J, is exactly proportional to the concentration gradient (C) and the diffusion coefficient (D) of the substance.

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49. Which of the following properties remains constant during steady-state diffusion?

1. Flux
2. Equilibrium conditions
3. Linear concentration gradient
4. Kinetic energy

Answer: A) Flux

Explanation:

The flux is constant during steady-state diffusion. Flux is the amount of material that diffuses through a unit area per unit of time.

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50. Fill in the blanks: The term 'steady state diffusion' refers to a situation in which the rate of diffusion within a material remains constant across ____.

1. Temperature
2. Time and speed
3. Speed
4. Time

Answer: D) Time

Explanation:

The term "steady state diffusion" refers to the situation in which the rate of diffusion within a material remains constant across time.

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