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MAT SCI > QUIZ 1 > Flashcards

QUIZ 1 Flashcards

1
Q

Substances of which something is made from

A

Materials

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2
Q

Investigates the relationships that exists between STRUCTURE and PROPERTIES of materials

A

Materials Science

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3
Q

A scientific discipline concerned with the search for basic knowledge about the INTERNAL STRUCTURE, PROPERTIES AND PROCESSING of materials

A

Materials Science

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4
Q

Materials whose structures are designed to develop specific properties for a given application

A

Engineering materials

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5
Q

To continue to provide consumers with what they expect and need, designers must keep abreast with ______

A

new materials development

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6
Q

From teh structure property relationship, the material’s structure is ENGINEERED to produce a predetermined set of properties

A

materials engineering

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7
Q

An engineering discipline which is primarily concerned with the use of the fundamental and applied knowledge of materials so that they can be converted into products needed or desired by society

A

Materials science and engineering

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8
Q

Relates to the internal arrangement of a materials’ internal components

A

Structure

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9
Q

involves electrons and interactions within the nuclei

A

subatomic

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10
Q

arrangement of atoms or molecules relative to one another

A

atomic

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11
Q

large groups of atoms observed through a microscope

A

microscopic

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12
Q

structural elements visible through the naked eye

A

macroscopic

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13
Q

a material trait in terms of the kind and magnitude of response to a specified imposed stimulus

A

property

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14
Q

generally, definitions of properties are independent of the material’s shape and size

A

property

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15
Q

deformation to an applied load or force

A

mechanical property

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16
Q

the tendency of the object to be deformed elastically upon the application of forcee

A

elastic modulus

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17
Q 
the ability to
withstand an applied
stress without failure
(deformation that
cannot be reversed).
A

Strength

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18
Q

Response from an electric field

A

Electrical Property

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19
Q

the ability to conduct electric

current.

A

Electrical conductivity

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20
Q

Stimulus to a magnetic field

A

Magnetic Property

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21
Q

– is the measure of the resistance of a

ferromagnetic material to becoming demagnetized

A

Coercivity

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22
Q

Response to heat

A

Thermal Property

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23
Q

is the property of a
material that indicates
its ability to conduct
heat.

A

Thermal conductivity

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24
Q

Stimulus to electromagnetic or light radiation

A

Optical Property

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25
Q

the property of a material to

allow light to pass through

A

Optical Transmission

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26
Q

light passes through completely

A

Transparent

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27
Q

light passes through diffusely

A

Translucent

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28
Q

– does not allow light to pass through

A

Opaque

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29
Q

Reactivity of materials to

chemicals.

A

Deteriorative Property

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30
Q 
– the
disintegration of an
engineered material into
its constituent atoms due
to chemical reactions with
its surroundings,
commonly with oxygen
(oxidation).
A

Corrosion

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31
Q 
In the sense of materials science and
engineering, processing refers to the
altering of the structure of a material in
order to come out with a desired set of
properties
A

Processing

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32
Q

heating the metal to above the

recrystallization temperature and mainta

A

Annealing

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33
Q

– accomplished by a controlled
reheating of the work piece to a temperature
below its lower critical temperature

A

Tempering

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34
Q

heating the metal until the crystal

structure changes.

A

Austentizing

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35
Q

rapidly cooling the metal.

A

Quenching

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36
Q

The metal’s structure is not regular throughout.

A

Crystal grain

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37
Q

Metallic elements, e.g. iron, silver

A

Metals

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38
Q

Compounds of a metal and non-metal

A

Ceramics

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39
Q

Materials with long hydrocarbon chains, e.g.
plastics

A material composed of a combination of
metals, ceramics, and/or polymers

A

Polymers

Composites

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40
Q

Materials that are implanted into the human
body for replacement of diseased or damaged
parts

Materials whose properties lie between a
conductor and insulator, and find applications in
electronics

A

Biomaterials

Semiconductors

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41
Q 
The atom is composed of a
\_\_\_\_\_\_\_ composed of
protons and neutrons, with
the electrons circling around
the nucleus in \_\_\_\_\_\_
A

nucleus

shells.

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42
Q

Some elements have different number of
neutrons, thus having two or more atomic
masses. These are called ______

A

isotopes.

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43
Q

The _____ is the weighted average of
the atomic masses of the atom’s naturally
occurring isotopes.

A

atomic weight

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44
Q

1 amu is defined as ____ of the
atomic mass of the most common isotope of
_____

A

1/12

carbon

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45
Q

1 mole = _____atoms or molecules
The two schemes are related by
1 amu/atom (or molecule) = 1 g/mol
* This is known as ______where A =

A

6.023x10^23 atoms/mole

Avogadro’s Number,

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46
Q

has electrons revolving
around the nucleus in discrete
orbital shells.

A

 Bohr atomic model

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47
Q 
Each electron has a particular
value of energy (quantized) by
making a quantum jump to a
higher level by absorption of
energy, or to a lower energy
level by emission of energy.
These are termed as \_\_\_\_\_ or \_\_\_\_\_
A

energy

levels or states.

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48
Q

Makes up for the limitation of

the Bohr model.

A

Wave mechanical model

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49
Q

Considers the electron to

have wave-like and particle like characteristics.

A

Wave mechanical model

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50
Q 
The electron’s position is no
longer defined as a discrete
orbital, but as a probability of
an electron being at various
locations (probability
distribution or electron cloud).
A

Wave mechanical model

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51
Q

Specifies the size, shape, and spatial orientation

of the electron’s probability density.

A

Quantum Numbers

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52
Q

Dictates the number of states within each

electron subshell

A

Quantum Numbers

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53
Q

Shells are specified by a _____ having integral values (n = 1, 2, 3,…).
Sometimes they are designated by letters (K, L,
M,…). This relates the distance of the electron
from the nucleus.

A

principal quantum

number,

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54
Q

The number of states for each subshell is
defined by the ____, ml. s, p,
d, and f subshells have 1, 3, 5, and 7 states
respectively

A

third quantum number

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55
Q

The _______ l, signifies the
subshell denoted by a lower-case letter – an s,
p, d, or f, relates the shape of the subshell.

A

second quantum number

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56
Q

______ for an electron can either be up or
down, and is related by a fourth quantum
number ms, with two possible values (+½ or -½).

A

Spin moment

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57
Q

Elements are arranged according to electron

configuration.

A

Periodic Table of Elements

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58
Q

Elements with increasing atomic
numbers are arranged in seven horizontal rows
called____. Each column or _____ of
elements have similar valence electron
structures, as well as chemical and physical
properties.

A

periods

column or group

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59
Q

Consider two isolated atoms brought into close
proximity from infinity. At large distances, the
interactions are ______. As the atoms
approach, each exerts a force on the other,
repulsive and attractive.

A

negligible

60
Q

The net force FN between the two atoms is

_____ (give formula)

A

Fn = Fa + Fr

61
Q

The net force is a function of the ______ r.

A

interatomic

separation

62
Q

When FA and FR balance, there is a net force. true or false

A

false. no net force = 0

63
Q

For many atoms, r0 is

approximately _____.

A

0.3 nm (3Å)

64
Q

Force and energy are related mathematically by ____ (give formula)

A

E = integral of (Fdr)

65
Q

_______ is the minimum amount of
energy that would be required to separate the
two atoms

A

Bonding energy (E0)

66
Q

Found in compounds composed of metallic and
non-metallic elements, elements situated at the
horizontal extremities of the table.

A

Ionic Bonding

67
Q

Atoms of a metallic element _____ their

valence electron to the non-metallic element.

A

give up

68
Q

In the process of ionic bonding, they acquire a stable state or
________, and in addition, an
electrical charge (they become ions).

A

inert gas configuration

69
Q

example of ionic bonding

A

Table Salt (NaCl)

70
Q

 Attractive bonding forces are _____, i.e.,
positive & negative ions, by virtue of their
electrical charge, attract one another

A

coloumbic

71
Q

Ionic bonding is _______, magnitude of

bond is uniform in all directions around an ion.

A

non-directional

72
Q

Predominant bonding scheme in ceramics

A

ionic Bonding

73
Q

Ionic compounds have high bonding energies
(600-1500 kJ/mol), reflected in ____ melting
temperatures, hard and brittle, and electrically
and thermally insulative.

A

high

74
Q

Sharing of electrons between two adjacent

atoms

A

Covalent Bonding

75
Q

______atoms will contribute at least
one electron to the bond, with the shared
electron belonging to both atoms.

A

Covalently bonded

76
Q

example of covalent bonding

A

methane

77
Q

Covalent bond is _____, it is between
specific atoms and may exist only in the
direction between one atom and another that
participates in the electron sharing.

A

directional

78
Q

Number of covalent bonds that is possible for an

atom is determined from its ______

A

valence electrons,

79
Q

_____ materials typify covalent bond, being

composed of long carbon structures.

A

Polymeric

80
Q

It is _______ to have interatomic bonds that are
partially ionic and partially covalent, and, in fact,
very few compounds exhibit pure ionic or
covalent bonds. (possible or not possible)

A

possible

81
Q

For a compound, the degree of either bond type
depends on the relative position of the
constituent atoms in the periodic table
(electronegativity). The _____ the degree of
electronegativity (horizontally or vertically), the
____ ionic the bond. Conversely, the ____the
atoms are together, the _____ the covalency.

A

greater, more

closer , greater

82
Q

bonding found in metals and alloys

A

metallic bonding

83
Q

Valence electrons are not bound to any
particular atom and are more or less free to drift
throughout the entire metal. what bonding

A

metallic bonding

84
Q

Free electrons form an _______

A

electron cloud

85
Q

The non-valence electrons and nuclei form what
are called ______, which posses a positive
charge equal in magnitude to the total valence
electron charge per atom (due to the electron
not being attached to the atom).

A

ion cores

86
Q

example of metallic bonding

A

gold

87
Q

 Metallic bonds are

directional or non-directional?

A

non-directional

88
Q

A material in which the atoms are arranged in
periodic arrays over large distances (existence
of long-range order)

A

Crystalline Material

89
Q

 All metals, many ceramics, and certain polymers

form ______upon solidification.

A

crystalline structures

90
Q

Compounds which do not crystallize, or for
which long-range order is absent, are termed
non-crystalline or _______

A

amorphous

91
Q

Manner in which atoms, ions, or molecules are

spatially arranged.

A

Crystal Structure

92
Q

Crystalline structures are thought of as solid
spheres with well-defined diameters, termed as
_______, in which spheres
representing nearest neighbor atoms touch one
another.

A

atomic hard spheres

93
Q

Used in the context of crystal structures

A

Lattice

94
Q

A three-dimensional array of points, coinciding

with atom positions (or sphere centers).

A

Lattice

95
Q

Smallest repeating unit

within a crystal structure.

A

Unit Cell

96
Q 
 For most crystal
structures, unit cells are
\_\_\_\_ or \_\_\_\_\_,
having three sets of
parallel faces.
 Represents the
A

parallelipipeds, or prisms

97
Q

Atoms are located at each of the corners and

centers of the cube faces.

A

Face-centered Cubic (FCC)

98
Q

give examples of FCC elements

A

Copper
Silver
Aluminum
Gold

99
Q

Each corner atom is shared among eight unit
cells & the face centered atoms belong to two,
or, there are 8 1/8 atoms and 6 ½ atoms, a total
of 4 atoms per unit cell.

A

Face-centered Cubic (FCC)

100
Q

 Translation of the cube from a corner to a face

center will not alter the cell structure.

A

Face-centered Cubic (FCC)

101
Q

 Atoms are located at the eight corners and at the

center of the cube.

A

Body-centered Cubic (BCC)

102
Q

give examples of BCC elements

A

Chromium
Iron
Tungsten

103
Q

There are 8 1/8 atoms and 1 whole atom per unit

cell, a total of 2

A

Body-centered Cubic (BCC)

104
Q

Number of nearest neighbor or touching atoms

for a particular atom.

A

Coordination Number

105
Q

FCCs have a coordination number of ____.

BCCs have a coordination number of ____.

A

12

8

106
Q

Fraction of a solid sphere inside a unit cell

A

Atomic Packing Factor (APF)

107
Q

give the formula of Atomic Packing Factor (APF)

A

APF = total volume of atoms/volume of unit cell

108
Q

APF of fcc

A

0.74048

109
Q

APF of bcc

A

0.680175

110
Q

Length of side of cell, in fcc

A

s = 2r sqrt(2)

111
Q

Length of side of cell, in bcc

A

s = 4r/sqrt(3)

112
Q

The unit cell is a hexagonal

prism.

A

Hexagonal Close-packed (HCP)

113
Q

prism.
 Atoms are located at the
corners and the center of the
2 hexagonal planes.

A

Hexagonal Close-packed (HCP)

114
Q

Another plane in-between the
hexagonal planes contain ___
atoms

A

3

115
Q 
Contains 6 1/6 atoms and 1 ½
atom for each of the top and
bottom planes, a 3 atoms in
the middle plane; a total of 6
atoms per unit cell.
A

Hexagonal Close-packed (HCP)

116
Q

elements that have HCP structures

A

Cadmium
Zinc
Magnesium

117
Q

Some metals, as well as non-metals, may have
more than one crystal structure.
 This phenomenon is known as ______.

When formed in elemental solids, this condition
is often termed as _____

A

polymorphism

allotropy.

118
Q

The prevailing crystal structure depends on both

the _____ and _____

A

temperature

external pressure.

119
Q 
Unit cell geometry is
completely defined in
six parameters: edge
lengths a, b, c; and
three internal angles
, β, γ, sometimes
called \_\_\_\_\_
A

lattice

parameters.

120
Q

WHAT ARE THE seven crystal systems

A 
Cubic
Hexagonal
Tetragonal
Orthorhombic
Rhombohedral
Monoclinic
Triclinic
121
Q

When dealing with crystalline structures, it
becomes necessary to specify a particular
crystallographic plane of atoms or a
_______

A

crystallographic direction

122
Q

____ integers of indices are used to designate
directions and planes, based on a unit cell,
situated at one corner.

A

Three

123
Q

A line between two points, or a vector.

A

crystallographic direction

124
Q

In cubic crystals, several crystal directions are
equivalent and grouped in angle brackets is
called a ____. Furthermore, directions having
the same indices without regard to order or
sign are ______

A

family

equivalent.

125
Q

in hexagonal crystals, we will use a 4-axis, or______

coordinate system.

A

Miller-Bravais,

126
Q

in miller-bravais coordinate system, Axes a1, a2, and a3 are contained on a single
plane, called the ____, and are at 120° to
each other. The z-axis is perpendicular to the
basal plane

A

basal plane

127
Q

Crystallographic planes are represented by
three ______(except in hexagonal
crystals). Any two planes parallel to each other
are equivalent and have identical indices.

A

Miller indices hkl

128
Q

For cubic systems, planes and directions having
the same indices are _______ to one
another, but may not be the case for other
crystal systems.

A

perpendicular

129
Q

 Atomic arrangements for a particular plane of

interest depends on the ______

A

crystal structure.

130
Q

A _______contains all those planes that
are crystallographically equivalent – that is
having the same atomic packing.

A

family of planes

131
Q

the fraction of the line length in
a particular crystallographic direction that
passes through the atom centers.

A

Linear density

132
Q

– the fraction of the total
crystallographic plane area that is occupied by
atoms passing through the atom centers

A

Planar density

133
Q

which crystal structures have the most efficient packing of atoms? give the value of apf

A

FCC AND HCP

0.74048

134
Q

Single crystals exist in nature, but can also be artificially
grown.
Good examples are _______.

A

gemstones

135
Q

The atoms are arranged in perfect, periodic arrays and

extends throughout the specimen without interruption.

A

Single crystal

136
Q

Composed of many small crystals or grains

A

Polycrystalline material

137
Q

The region where two crystals meet is termed as the

_____________.

A

grain boundary

138
Q

The physical properties of single crystals of some

substances depend on the crystallographic direction

A

Anisotropy

139
Q

Properties like elastic modulus and electrical conductivity
may have different values in the [100] and [111]
directions.
 The directionality of these properties is termed as
_______.

A

anisotropy.

140
Q

_____________ lack a systematic and regular

arrangement of atoms over relatively large distances.

A

Noncrystalline solids

141
Q

other term for noncrystalline solids

A

amorphous.

142
Q

________ crystals are characterized by complex
molecular structures that can become ordered with some
difficulty

A

Amorphous

143
Q

give the formula of true density

A

rho = nA/VcNa

144
Q

For regular HCP crystals, the
ratio c/a should be _______
But some metals deviate from
this ratio.

A

1.63299.

145
Q

APF of HCP

A

0.74048.

MAT SCI (1 decks)

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