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Mat Sci > Exam 1 Vocab > Flashcards

Exam 1 Vocab Flashcards

1
Q

Metals

A

Strong and ductile
High thermal and electrical conductivites
Opaque and reflective

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2
Q

Polymers and plastics

A

Compounds of nonmetallic elements
Soft ductile low strength and low densities
Low thermal and electrical conductivities
Opaque translucent or transparent

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3
Q

Ceramics

A

Compounds of metallic and nonmetallic elements
Oxides carbides nitrides and csulfides
Low thermal and electrical conductivities
Opaque translucent or transparent

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4
Q

Procedure of material selection

A

Determine desirable prop
List properties of different materials to id candidate materials
Determine best candidate material

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5
Q

Mechanical properties

A

Different treatment methods get different levels of hardness

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6
Q

Electrical properties

A

Factors that affect electrical resistivoty:
Inc temp-> inc rest
Inc impurity -> inc res
Deformation increases resistivity

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7
Q

Thermal conductivity

A

Measure of materials ability to conduct heat

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8
Q

Thermal properties

A

Inc impurity-> decreases conductivity

High porosity -> poor heat conductors

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9
Q

Magnetic properties

A

Magnetic storage

Magnetic permeability

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10
Q

Optical properties

A

Light transmitance
Single crystal-> transparent
Poly crystal-> translucent
Porosity poly-> opaque

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11
Q

Deteriorative properties

A

Form stress corrosion properties

Can b improved by minimizing imperfections and treatments

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12
Q

Lecture 1 summary

A

Appropriate materials and processing decisions are engineers to understand materials in the properties

Materials properties depend on their structures structures are determined by how materials are processed

In terms of chemistry the three classifications of materials are metals ceramics and polymers

Most properties of materials font to the following six categories:
Mechanical electrical thermal magnetic optical and deteriorative

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13
Q

Atomic number

A

Number of protons in a nucleus of atom

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14
Q

Atomic weight

A

6.022e23 atoms/mol

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15
Q

Electron structure

A

Wavelike and particle like characteristics

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16
Q

Electron wave like characteristics

A

Electron position in terms of probability density

Shape size and orientation of probability density determined by quantum numbers

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17
Q

Quantum numbers

A

N-> principal shell, 1,2,3,4
L -> azimuthal -> S,p,d,f
mi -> magnetic num of orbitals
ms -> spin +- .5

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18
Q

Valence electrons

A

Electrons residing in the other orbital of an Adam they are available for bonding

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19
Q

Cation

A

Metal Adam that donates an electron left

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20
Q

Anion

A

Nonmetal atom that accepts electron right

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21
Q

Coulombic attraction

A

The force of attraction between positive and negative charges

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22
Q

Ionic bonding

A

Common in ceramics

Full transfer of electrons

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23
Q

Covalent bonding

A

SP orbital sharing

Find hybridization SP three energy level

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24
Q

Metallic bonding

A

Electrons delicalized to form electron cloud

25
Q

Mixed bonding

A

Lids 2% ionic character

26
Q

Secondary bonding

A

Occurs in Palmer’s

Dipoles interact weekly between chains

27
Q

Properties relating to bonding

A

Bond length r
Bond energy Eo
Greater Eo for higher melting temp

28
Q

Ceramics

A

Ionic and covalent bonding

High melting temperature large E small alpha

29
Q

Metals

A

Metallic bonding
Moderat melting temperature moderately e
Moderate alpha

30
Q

Polymers

A

Covalent and secondary bonding
Weak bond energy between chains
Secondary bonding responsible for most physical properties
Low melting temperature small E large alpha

31
Q

Amorphous

A

Noncrystalline materials nonuniform bagging happens in more complex structures

32
Q

Metallic crystal structures

A

Bonds between metals or nondirectional
Nearest neighbor distance is tend to be small
High degree of shielding of ion Cors provided by free electron cloud
Simple structure

33
Q

Coordination number

A

A number of nearest neighbor or touching Adams

34
Q

Atomic packing factor

A

Volume of Adams in unit cell per unit cell volume

35
Q

Anistrophy

A

Property value depends on Chris Sullivan graphic direction of measurement observed in single crystals

36
Q

Isotrophy

A

Properties may or may not very with direction of measurement grains are randomly oriented

37
Q

Polymorphism/allotropic

A

Two or more distinct crystal structure for the same material

38
Q

Polymer

A

Many repeating units
Most are hydrocarbons
Sat or unsat

39
Q

Saturated hydrocarbon

A

Bonded to four other Adams no double bonds

More units equals higher boiling point

40
Q

Unsaturated hydrocarbon’s

A

Have double and triple bonds somewhat unstable

41
Q

Isomerism

A

Two compounds with the same formula in different structures

42
Q

Polymer chemistry

A

Free radical polymerization

43
Q

Palmer molecular shape or confirmation

A

Chain bending and twisting or possible by rotation of carbon Adams around the chain bonds

44
Q

Stereoisomerism

A

Mirror images of same bind structure

45
Q

Tacticity

A

Stereo irregularity or spacing arrangement of r units along chain

46
Q

Isotactic

A

All r groups on same side of chain

47
Q

Syndiotactic

A

R groups alternate sides

48
Q

Atactic

A

R groups randomly positioned

49
Q

Cis isomerism

A

R in same side of chain

50
Q

Trans isomerism

A

R on opposite sides

51
Q

Polymer crystallinity

A

Almost never complete
Chain folded structure
Spirulites form the crystals

52
Q

Spirulites

A

Growth starts from central nucleation site and then split growing out word in branching there is a Maltese cross in each

53
Q

Point defects

A

Vacancy

Interstitial atoms

54
Q

Dislocations

A

Linear defect

55
Q

Grain boundary

A

2d interfacial defect

56
Q

Frankel defect

A

A cation is displaced from its lattice position to an interstitial spot, makes vacancy at lattice and interstitial defect at point of relocation

57
Q

Schottky defect

A

Oppositely charged ions leave their sites creating vacancies

58
Q

Rothery rules

A

Conditions for formation of substitutional solid solutions:

Difference in radius is the less than 15%
Similar electronegativities
Same crystal structure for pure metals
Valances all else being equal a metal will have a greater tendency to dissolve in the metal of higher valance been one of the lower valence

Mat Sci (1 decks)

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