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Midterms

Pamela Rose Llanes Material Science and Engineering Reviewer Engineering English 200 cards

Cards in this deck (200)

  1. 1What are the three methods to test materials?Mechanical Testing, Chemical Testing and Optical Testing
  2. 2A type of material that is electrically conductive.Metal
  3. 3Have electrical conductivities intermediate between conductors and insulators.Semiconductor
  4. 4A mixture of two different materials to create a new material with combined properties.Composite
  5. 5Length scale that pertains to clusters of atoms that make up small particles or material features.Nano Structure, 10^-9 m
  6. 6What are the three reasons why studying Materials Science and Engineering is important?1. To be able to select a material for a given use based on considerations of cost and performance.
    2. To understand the limits of materials and the change of their properties with use.
    3. To be able to create a new material that will have some desirable properties.
  7. 7What are the three types of polymers in engineering materials?Thermoplastics, Thermosets and Elastomers
  8. 8The defect forms when an atom leaves its place in the lattice, creating a vacancy, and becomes an interstitial by lodging in a nearby location.Frenkel Defect
  9. 9It is a special type of grain boundary across which there is a specific mirror lattice symmetry.Twin Boundary
  10. 10What is the other term for linear defect?Dislocation
  11. 11A half row of atoms is inserted in the crystal.Linear Defect
  12. 12It is a homogeneous mixture of two crystalline solids with similar crystal lattices.Solid Solution
  13. 13It is a type of defect where an atom is not present at their lattice sitesVacancy defect
  14. 14What are the three types of interfacial defects?Surface, Grain Boundary and Twin Boundary
  15. 15What are the two types of solid solution?Substitutional Solid Solution, Interstitial Solid Solution
  16. 16It is the ability of a solid material to exist in more than one form or crystal structure.Polymorphism
  17. 17It is a consequence of phase relationships between two or more waves scattered by obstacles.Diffraction
  18. 18Composed of a collection of small solids called "grains."Polycrystalline Materials
  19. 19It has a cubic unit cell with atoms are located at all eight corners and a single atom at the cube center.Body-Centered Cubic Crystal Structure
  20. 20A building block of the crystal structure. by virtue of its geometry and the position of atoms within.Unit Cells
  21. 21A bonding through an electrostatic force between delocalized electrons and positively charged metal atoms.Metallic Bonding
  22. 22What are the seven crystal lattice systems?Cubic, Tetragonal, Hexagonal, Orthorhombic, Rhombohedral, Monoclinic and Triclinic
  23. 23A type of subshell which consists of 7 orbitals that can holds up 14 electrons.f subshell
  24. 24Group of non-reactive, inert gases that are located in the far right column of the periodic table.Noble gases, Group 18 (VIII or 0)
  25. 25Elements can be characterized by their reactivity and valence electron configuration.Chemically
  26. 26Elements with low electronegativity value.Electropositive
  27. 27Position of the electron is described by the electron cloud or a probability distribution.Wave Mechanical Model
  28. 28The electrons are now defined by their “quantum numbers”.Wave Mechanical Model
  29. 29Each shell is composed of subshells.Wave Mechanical Model
  30. 30A bond that only exist in between the atom and the atom it is bonded with.Covalent Bond
  31. 31Sharing of the electrons between the two atoms will then bind the structure together.Covalent Bond
  32. 32What are the four common applications for Permanent Dipole Bonds a.k.a. Hydrogen Bonds?Adhesives, Surfactants, Emulsifiers and Desiccants
  33. 33What are the two ways to determine the number of valence electrons in an element?1. Using the group number in the periodic table.
    2.. Using the electron configuration of the element.
  34. 34The ability to buffer acids.Alkalinity
  35. 35Corrode many different kinds of metals or wear them away through chemical processes.Acidity
  36. 36The characteristic of metals.Acidity
  37. 37The characteristic that neutralizes acidity.Alkaline
  38. 38Chemical composition of the elements present in the metals and alloys.Composition
  39. 39Surface deterioration caused by the chemical reaction.Corrosion
  40. 40All metals are extracted from their ores.Corrosion
  41. 41Wide range of physical processes where moving particles or radiation of some form.Scattering
  42. 42How matter bound takes up a photon's energy — and so transforms electromagnetic energy into internal energy of the absorbed.Absorption
  43. 43Phenomenon in which the phase velocity of a wave depends on its frequency.Dispersion
  44. 44How far a beam of light can go through the material before getting absorbed.Absorption Coefficient
  45. 45How fast light rays travel through a given medium.Index of Refraction
  46. 46Ratio of the charge flowing across the conductor to the potential applied.Capacitance
  47. 47The reciprocal of resistivity.Electrical Conductivity
  48. 48A conductor's resistance increases as its length increases.Electrical Resistivity
  49. 49The relationship between voltage, current, and resistance.Ohm's Law
  50. 50Two other related electrical property of metal.Ductile and Corrosion Resistance
  51. 51They can be drawn into thin wires without breaking.Ductile
  52. 52Many metals are highly resistant to corrosion.Corrosion Resistance
  53. 53Ability of material to withstand high voltagesDielectric Strength
  54. 54It is used in the selection of insulating materials.Dielectric Strength
  55. 55The electrical conductivity and resistivity of metals can change with temperature.Temperature Coefficient of Resistance
  56. 56Exhibit ____ at very low temperatures.Superconductivity
  57. 57Transferring heat quickly and efficiently.Thermal Conductivity
  58. 58It impedes or resists the flow of electric current.Resistivity
  59. 59It is defined as the reciprocal of conductivity.Resistivity
  60. 60It increases linearly with an increase in temperature.Resistivity
  61. 61The material which is a bad conductor.Insulator
  62. 62Pure metals have good ____ at room temperature.Conductivity
  63. 63It allows the flow of electric current.Conductivity
  64. 64A parameter that indicates how easily an electric current can flow through a material.Conductivity
  65. 65It is defined as the reciprocal of resistance.Conductivity
  66. 66This two metals is considered as good electrical conductors.Copper and Aluminum
  67. 67The characteristic of a metal that enables the flow of electric current through it.Electrical Properties
  68. 68____ can move easily throughout the metal, making them excellent conductors of electricity.Free electrons
  69. 69When an external magnetic field is introduced to a ferromagnet substance, the atomic dipoles align themselves with it.Magnetic Hysteresis
  70. 70When a ferromagnetic material is subjected to a gradually increasing magnetic field, simultaneously there will be a corresponding increase in the intensity of magnetization.Hysteresis
  71. 71Capacity of a magnetic field to stay in a substance after the external source has been removed is called retentivity.Retention
  72. 72It provides information on the magnetic strength of such a substance.Retention
  73. 73The force which opposes the magnetizing force.Coercive Force
  74. 74It is applied to remove previous magnetization or residual magnetism.Coercive Force
  75. 75Measure that indicates the ease with which magnetism may be developed in the materials.Permeability
  76. 76Can be easily magnetized or demagnetized and they retain actually no magnetism when the magnetizing force is removed.Soft Magnetic Materials
  77. 77It is used in a large variety of electrical and electronic components.Magnetic Materials
  78. 78The quantity of heat required to raise the temperature of a unit mass of a substance through 1 Degree Celsius.Specific Heat
  79. 79The temperature at which it begins to melt when heat is added to it.Melting Point
  80. 80The tendency of some materials to expand when they heat up.Thermal Expansion
  81. 81What are the two components of Thermal Conductivity?Electronic Contribution and Phonon Contribution
  82. 82The relationship between the electrical conductivity and the electrical component of the thermal conductivity of a metal.Electronic Contribution
  83. 83A quantized lattice vibration, as we heat the lattice up the atoms are going to start vibrating.Phonon Contribution
  84. 84Transport heat from hotter regions to cooler regions.Phonon
  85. 85The ability of the metal to transmit heat energy through it.Thermal conductivity
  86. 86Resistance of the material to penetrate.Hardness
  87. 87Measurement of the amount of energy a material can absorb before failure takes place.Toughness
  88. 88The ability of a metal to withstand deformation under compression without rupture..Malleability
  89. 89Property of a material by virtue of which a material can regain its original shape and size after the removal of load.Elasticity
  90. 90Property of a material by virtue of the material cannot regain its original shape and size after the removal of the load.Plasticity
  91. 91Ability of a metal to withstand elongation under tension without rupture.Ductility
  92. 92Property of breaking without permanent distortion.Brittleness
  93. 93The point at which the failure of the material takes place.Fracture or Breaking Point
  94. 94The point at which a material endures maximum stress before failure.Ultimate Stress Point
  95. 95The point at which the material starts showing to deform plastically.Yield Point
  96. 96The maximum stress that a substance can endure before permanently being deformed.Elastic Limit
  97. 97The ratio of stress and strain provides us with the proportionality constant known as young's modulus.Proportional Limit
  98. 98The relationship between stress and strain for materials.The Stress-Strain Graph
  99. 99The elastic restoring force acts parallel to the surface area.Tangential Stress
  100. 100The restoring force per unit area perpendicular to the body surface.Normal Stress
  101. 101What are the two types of stress?Normal Stress and Tangential Stress
  102. 102What are the five limit/point of Stress-Strain Graph?Proportional Limit, Elastic Limit, Yield Point, Ultimate Stress Point and Fracture or Breaking Point
  103. 103It is the physical quantity that describes the magnitude of forces that cause deformation.Stress
  104. 104The force applied per unit area in mechanics.Stress
  105. 105What are the five types of Strain?Tensile Strain, Compressive Strain, Shear Strain, Longitudinal Strain and Volumetric Strain
  106. 106This is the strain produced on the body due to the deforming force, which leads to only the change in volume of the object.Volumetric Strain.
  107. 107The strain produced on the body due to the deforming force, which leads to a change in only the length of the object.Longitudinal Strain
  108. 108Due to the tangential stress, an angle tilt is caused in the body.Shear Strain
  109. 109The change in length (or area) of a body caused by compressive strain.Compressive Strain
  110. 110Defined as a change in the length (or area) of a body caused by tensile tension.Tensile Strain
  111. 111The ratio of change of shape or size to the original shape or sizeStrain
  112. 112The ratio of the amount of deformation experienced by the body in the direction of force applied to the initial sizes of the body.Stress
  113. 113Defined a linear zone in which the force required to stretch material was proportionate to the extension of the material.Hooke’s Law
  114. 114States that the flux is directly proportional to the concentration gradient.Fick’s First Law
  115. 115What are the two types of Diffusion Mechanisms?Vacancy Diffusion and Interstitial Diffusion
  116. 116Involves atoms that migrate from an interstitial position to a neighboring one that is empty.Interstitial Diffusion
  117. 117Involves the interchange of an atom from a normal lattice position to an adjacent vacant lattice site or vacancy.Vacancy Diffusion
  118. 118A process of mass transfer of individual molecules of a substance as a result of random molecular motion.Diffusion
  119. 119Does not possess the long-range order of its crystalline counterpart.Amorphous Solids
  120. 120The ultimate imperfection in a solid is total disorder.Amorphous Solids
  121. 121The driving force for diffusion.Concentration
  122. 122Occur by having blocks of atoms moving in a coordinated manner along a given direction (twinning direction) and boundary (twinning plane).Twin Boundaries
  123. 123Consist of single-crystal grains separated from one another through transition regions.Grain Boundaries
  124. 124The properties of polycrystalline and single-phase materials are under consideration.Grain Size Determination
  125. 125The advent of the digital age, grain size determination was performed.Photomicrographs
  126. 126It is a planar defect/interfacial defect that can occur in crystalline materials. Crystalline materials form repeating patterns of layers of atoms. Errors can occur in the sequence of these layers.Stacking fault
  127. 127The junction of two crystals which differ in lattice structure and composition. In coherent phase boundaries the atomic configuration of the two crystals is the same at the boundary plane and the lattices are continuous across the boundary.Phase boundary
  128. 128What are the two other defects?Phase Boundary and Stacking Fault
  129. 129The boundaries or planes that separate a material into regions, with each region having the same crystalline structure but a different orientation.Surface
  130. 130Boundaries separating two small grains or crystal having different crystallographic orientation in polycrystalline materials.Grain Boundary
  131. 131What are the two types of grain boundary?Low-angle Boundary and High-angle Boundary
  132. 132Dislocation core – maximum strain on the dislocation Burgers vector - the vector of the lattice dislocation Dislocation core is parallel to the burgers vector.Screw Dislocation Burgers Circuit
  133. 133Half of the crystal structure have shifted downwards, and lattices forms new bonds with the layer below them.Screw Dislocation
  134. 134The process in which the dislocation moves one step at the time in the crystal.Dislocation Glide
  135. 135Takes less force than moving the whole crystal structure at once.Gliding
  136. 136Dislocation core – maximum strain on the dislocation Burgers vector - The vector of the lattice dislocation Dislocation core is perpendicular to the burgers vector.Edge Dislocation Burgers Circuit
  137. 137The size of the solute atom is much smaller than that of the solvent atom, the solute atom can occupy an interstitial position.Interstitial Solid Solution
  138. 138The size of the solute atom is similar to that of the solvent atom, the solute atoms can replace solvent atom.• Substitutional Solid Solution
  139. 139Refer to a tiny concentration of an element or compound.Solute
  140. 140The most abundant element or compound.Solvent
  141. 141A mixture of metals formed by adding a certain amount of metals.Alloy
  142. 142In non-ionic crystals it means a lattice vacancy defect.Schottky Defect
  143. 143In ionic crystals, the defect forms when oppositely charged ions leave their lattice sites, creating vacancies.Schottky Defect
  144. 144It is a defect in which an atom or molecule occupies the intermolecular spaces in crystals.Interstitial defect
  145. 145What are the two extrinsic defects?Substitutional impurities and Impurity interstitial
  146. 146What are the two intrinsic defects?Vacancies and Self-interstitials
  147. 147missing atomsVacancies
  148. 148extra atomsSelf-interstitials
  149. 149What are the three types of Imperfections in Crystals?Point (1D), Line (2D) and Interfacial (3D)
  150. 150Defects that occur only at or around a single lattice point. They are not extended in space in any dimension.Point Defect
  151. 151What are the three types of Imperfections in Solids?Point Defects, Line Defects and Surface Defects
  152. 152Any deviation from the perfectly arranged arrangement of constituent particles in a crystal.Disorder/Defect
  153. 153Any abnormality in the pattern of crystal arrangement in solids.Imperfections in Solid
  154. 154"Without form." Their structure resembles a liquid.Amorphous
  155. 155Lacks systematic and regular arrangements of atoms.Non-Crystalline Solids
  156. 156An apparatus used to determine the angles at which diffraction occurs for powdered specimens; its features are represented schematically.Diffractometer
  157. 157High energy electromagnetic radiation.X-rays
  158. 158Physical properties of single crystals depend on the crystallographic direction.Anisotropy
  159. 159Perfect periodic and repeated arrangement of atoms.Single Crystals
  160. 160The crystal assumes a regular geometric shape with flat faces.Single Crystals
  161. 161Small crystals form at various positions which have random crystallographic orientations.Polycrystalline Materials
  162. 162What are the two types of crystals?Single Crystals and Polycrystalline Materials
  163. 163The most unsymmetrical crystal system. None of the three axes are equal in length, none are perpendicular. The inclined angles make it that the crystal forms in the paired faces. Example: TurquoiseTriclinic
  164. 164All three axes are different in length. Two of them are perpendicular to each other. Example: VivianiteMonoclinic
  165. 165All three axes are equal in length. None of them are perpendicular to each other. Trigonal System Example: Aragonite, RubyRhombohedral
  166. 166All three axes are unequal in length. All angles intersect each other at right angles. Example: TopazOrthorhombic
  167. 167Four axes are present. Three lies on the same plane, equal in length, and separated by equal angles. They are all perpendicular to the last axis. Example: ApatiteHexagonal
  168. 168The main axis varies in length, while the other two lie in the same plane and are equal in length. All three angles intersect at right angles. Example: ZirconTetragonal
  169. 169All three axes are equal in length and perpendicular to each other. The three angles intersect at right angles. Most Symmetrical Example: HaliteCubic
  170. 170What are the three lengths?a, b, and c
  171. 171What are the three interaxial angles?α, β, and γ
  172. 172A response to change in temperature, pressure, or both.Polymorphism and Allotropy
  173. 173The existence of two or more forms of a chemical element.Allotropy
  174. 174Occurs in elemental solids.Allotropy
  175. 175The difference in atomic arrangement of compounds with the atoms of the same element.Allotropy
  176. 176The difference in crystal structure of chemical compounds.Polymorphism
  177. 177Occurs in Chemical Compounds.Polymorphism
  178. 1786 atoms are assigned to each unit cell.Hexagonal Close-Packed Crystal Structure
  179. 179More complex than FCC and BCC.Hexagonal Close-Packed Crystal Structure
  180. 180A total of 2 atoms may be assigned to a given unit cell.Body-Centered Cubic Crystal Structure
  181. 181Typically has less strength than metals with FCC and HCP structure.Body-Centered Cubic Crystal Structure
  182. 182Another common metallic crystal structure.Body-Centered Cubic Crystal Structure
  183. 183A total of 4 atoms may be assigned to a given unit cell.Face-Centered Cubic Crystal Structure
  184. 184One of the most common crystalline structures.Face-Centered Cubic Crystal Structure
  185. 185Found among many metals.Face-Centered Cubic Crystal Structure
  186. 186Atoms located at each of the corners and center of each face.Face-Centered Cubic Crystal Structure
  187. 187Eight atoms distributed at the eight corners, each of the eight atoms are part of other adjacent cubic structures as well.Face-Centered Cubic Crystal Structure
  188. 188What are the three Main Crystalline Structure of Metals?Face-Centered Cubic Crystal Structure, Body-Centered Cubic Crystal Structure and Hexagonal Close-Packed Crystal Structure
  189. 189Structures made entirely of metal elements bonded through metallic bonding.Metallic Structures
  190. 190(8 corners / unit cell) (1/8 lattice points / corner) + (6 face center / unit cell) x (1/2 lattice point / face center) = 4 lattice point / unit cellFace Centered
  191. 191(8 corners / unit cell) (1/8 lattice points / corner) + (1 body center / unit cell) x (1 lattice points / body center) = 2 lattice point / unit cellBody Centered
  192. 192(8 corners / unit cell) (1/8 lattice points / corner) = 1 lattice point / unit cellSimple Cubic
  193. 193between b and cα (alpha)
  194. 194between a and cβ (beta)
  195. 195between a and bγ (gamma)
  196. 196The axial length or dimensions denoted as 'a', 'b', and 'c'.Lattice Parameters
  197. 197The angles in between the lattice parameters.Lattice Parameters
  198. 198What are the 14 types of Lattices?Simple Cubic, Body-Centered Cubic, Face-Centered Cubic, Simple Tetragonal, Body-Centered Tetragonal, Simple Monoclinic, End-centered Monoclinic, Simple Orthorhombic, Body-centered Orthorhombic, Face-centered Orthorhombic, End-centered Orthorhombic, Rhombohedral, Hexagonal and Triclinic
  199. 199What year did Auguste Bravais showed that crystals could be divided into 14 distinct lattices?1850
  200. 200What are the two types of Unit cell?Primitive Unit Cell and Non-Primitive Unit Cell

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Engineering Material Science and Engineering Reviewer Flashcards on Midterms, created by Pamela Rose Llanes on 15/03/2023.
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