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MSE 2001 > Midterm 1 (ch.1-3) > Flashcards

Midterm 1 (ch.1-3) Flashcards

1
Q

What are the types of material properties?

A
  • mechanical
  • physical (electric, magnetic, optical, thermal, elastic, chemical)
  • transport
  • radiation response
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2
Q

What is a structure-insensitive property?

A

one that does not depend on the mass of the substance or system

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3
Q

What are examples of structure-intensive properties?

A
  • temperature, pressure, density
  • elastic modulus
  • thermal coefficient of expansion (TCE) - (may change depending on porosity and texturing)
  • specific gravity
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4
Q

What is a structure-sensitive property?

A
  • a property that depends on impurities and the imperfection of the crystal structure of a material
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5
Q

What are some examples of structure-sensitive properties?

A
  • yield strength
  • thermal conductivity
    electrical resistivity
  • fracture toughness
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6
Q

What do material sciences and engineering study?

A
  • different types of materials
  • the structure-property-process relationships
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7
Q

What are the different types of materials?

A
  • metals
  • ceramics/ glasses
  • polymers
  • composites
  • semiconductors
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8
Q

What are examples of metals?

A
  • iron
  • copper
  • aluminum
  • silver
  • gold
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9
Q

Metals description

A

atoms located in regularly defined, repeating positions (crystal), have free electrons

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10
Q

Metals strengths (pros)

A
  • good electrical conductors
  • strong
  • ductile
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11
Q

Define Ductile

A
  • term for materials that can absorb energy by “bending” rather than by fracture when subject to external loads
  • (able to be drawn out into a thin wire/ plasticity)
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12
Q

Metals weaknesses

A
  • dense
  • moderate temperature resistance
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13
Q

Ceramics/glasses examples

A
  • sand
  • dinnerware
  • window glass
  • graphite
  • sanitary ware (toilets, bathtubs, etc)
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14
Q

Ceramics/ glasses description

A
  • combination of metallic and non-metallic atoms
  • some ceramics are crystalline
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15
Q

Ceramics/ glasses strengths (pros)

A
  • very strong and moderate density
  • high temperature stability
  • chemically resistant
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16
Q

Ceramics glasses weaknesses

A
  • no free electrons (not conductive)
  • brittle
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17
Q

Polymers examples

A
  • nylon
  • cellulose
  • Teflon
  • kevlar
  • polystyrene
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18
Q

Polymers description

A
  • long chain molecules with repeating groups
  • can be ductile or brittle
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19
Q

Polymers strengths (pros)

A
  • low density
  • easy to form into complex shapes
  • inexpensive
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20
Q

Polymers weaknesses

A
  • low strength
  • temperature sensitive
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21
Q

Composites examples

A
  • Carbon/carbon
  • Carbon/epoxy
  • plywood
  • steel belted tires
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22
Q

Composites description

A
  • 2+ materials combined
23
Q

Composites strengths (pros)

A
  • strong and rigid
  • low density
24
Q

Semi-conductors examples

A
  • silicon
  • germanium
  • GaAs
  • CdTe
  • InP
25
Q

Semi-conductors description

A
  • bonding and mechanical properties similar to ceramics
  • conductive
26
Q

Semi-conductors strengths (pros)

A

used in electronic and optical devices

27
Q

Define brittle

A
  • unable to absorb energy from external loads by bending
  • fracture easily
28
Q

Define conductivity

A

the ease with which electric charge is transported through a material in response to an external electric field

29
Q

Define stiff

A

an object is rigid as it resists bending

30
Q

Define crystalline

A

having atoms or ions arranged on a 3D lattice having long-range order

31
Q

Define amorphous

A

lacks the long-range order that is characteristic of crystalline solid
- either rubbers or glasses

32
Q

what are the main components of an atom?

A

protons, neutrons, and electrons

33
Q

What are the properties of an atom determined by?

A
  • the atomic mass number (Z)
  • mass of the atom
  • spatial distribution of electrons in orbits
  • energy of the electrons
  • ease of adding or removing an electron to make a charged atom
34
Q

What atomic properties can be changed by an external field?

A
  • spatial distribution of electrons in orbits
  • energy of the electrons
  • ease of adding or removing an electron to form an ion
35
Q

What kind of characteristics do electrons exhibit?

A

characteristics of particles and waves

36
Q

What is the principle quantum number?

A
  • n
  • integer number (1,2,3…)
  • refers to shell/ energy level
  • K: n=1; L: n=2; M: n=3
37
Q

What is the Azimuthal quantum number?

A
  • l
  • assigned numbers from l=0 (n-1)
  • refers to sub-shell
  • s: l=0; p: l=1; d: l=2; f: l=3
38
Q

What is the magnetic quantum number?

A
  • m
  • assigned numbers between positive and negative l
  • total number = (2l+1)
39
Q

What is the spin quantum number?

A
  • M s (M sub s)
  • either +1/2 or -1/2
  • reflects the different electronic spins of an electron
40
Q

Which quantum numbers are the energy of a shell primarily dependent on?

A
  • n and l
41
Q

What is the periodic table trend of electronegativity?

A

it increases from left to right and upwards in the periodic table

42
Q

What does electronegative describe; what kind of elements?

A

elements with high electronegativity (non-metals)

43
Q

What does electropositive describe; what kind of elements?

A

elements with low electronegativity (metals)

44
Q

What is electronegativity difference? What does it determine?

A
  • the difference between 2 elements’ electronegativities
  • determines bond type between those elements
45
Q

What change in electronegativity values correspond with different bonds?

A

> 1.7 = ionic bond
0.6-1.7 = polar covalent bond
<0.6 = nonpolar covalent bond

46
Q

What does primary bonding determine?

A

physical, mechanical, and chemical properties

47
Q

What does primary bonding involve in terms of electrons?

A

a transfer or sharing of outer electrons

48
Q

Are atoms shared or transferred with ionic bonding?

A

transferred

49
Q

What are some properties of ionic bonds?

A
  • non-directional bond
  • low electrical conductivity
  • brittle
  • high melting temperature
  • happens when ions of opposite charge attract as a result of coulombic attraction
50
Q

Are electrons transferred or shared in covalent bonds?

A

shared

51
Q

What are some properties of covalent bonds?

A
  • directional bonds
  • low electrical conductivity
  • very hard/strong
  • high melting temperature
  • > or equal to 4 valence electrons
52
Q

Are electrons shared or transferred in metallic bonds

A

shared

53
Q

What are some properties of metallic bonds?

A
  • non-directional bonds
  • good electrical conductivity (free electrons)
  • ductile and opaque
  • <3 valence electrons

MSE 2001 (4 decks)

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