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MSE 2001 > Test 1: Ch 1-3 > Flashcards

Test 1: Ch 1-3 Flashcards

1
Q

Scope of MSE

A

chemistry, physics, engineering

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2
Q

Metals

A
  • atoms are located in repeating positions (crystal)
  • free electrons making metals good conductors
  • strong but dense
  • moderate temp resistance
  • ductile
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3
Q

Ceramics

A
  • metallic and non-metallic atoms
  • many, but not all, are crystalline
  • no free electrons
  • very strong, moderate density, high temp stability
  • brittle
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4
Q

Polymers

A
  • long chain molecules with repeating groups
  • low strength, temp sensitive
  • easy to form into complex shapes
  • low density, ductile or brittle
  • covalently bonded
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5
Q

Semiconductors

A
  • bonding similar to ceramics, require high purity
  • mechanical properties similar to ceramics
  • covalently bonded
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6
Q

Composites

A
  • two or more materials combined

- structural applications where rigidity strength and low density are critical

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7
Q

Atomic Scale

A

pm

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8
Q

Unit Cell Scale

A

sub nm

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9
Q

Grain size scale

A

nm, µm

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10
Q

Life size scale

A

nm, µm, mm, m, km

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11
Q

Primary atomic bonding

A

ionic, covalent, metallic

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12
Q

Secondary atomic bonding

A

Van der Waals, Hydrogen

-arises from interaction b/w dipoles

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13
Q

ionic bonding

A
  • charge transfer
  • from the extremes of the periodic table, large difference in electronegativity
  • metals and nonmetals
  • transfer of an electron from the electropositive atom to the electronegative atom
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14
Q

covalent bonding

A

-sharing electrons in an attempt to make a complete shell

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15
Q

metallic bonding

A

-electrons shared by all the atoms in the substance

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16
Q

Force curves

A

-the steeper the slope of a force curve at the equilibrium distance, the higher the elasticity

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17
Q

Characteristics of Ionic Bonding

A
  • bonding energy 150-370 Kcal/mol
  • non-directional bond (strength of bond equal in all directions)
  • low electrical conductivity
  • brittle and high melting temp
18
Q

Coordination number and Geometry

A

2-linear
3-triangular
4-tetrahedral, square planar

19
Q

coordination number

A

how many atoms are in contact with another

20
Q

Characteristics of covalent bonding

A
  • electrons are shared to form a bond
  • bonding energy is less than ionic (75-300)
  • directional bonding (bond not of equal strength in all directions
21
Q

covalent crystalline solids

A
  • high melting temperatures
  • low conductivity
  • very hard and brittle
22
Q

Characteristics of metallic bonding

A
  • electrons are shared to form a bond
  • medium strength bonds
  • bonding energy weakest (25-200)
  • non-directional bond (strength of bond equal in all directions)
  • conductors
  • ductile
23
Q

Van der Waals bonding

A
  • weak bonding

- often bonding force between molecules

24
Q

Hydrogen bonding

A

-special type of secondary bond between some molecules containing Hydrogen (Cl, N, O, F)

25
Q

Bravais Lattices (4)

A
  • cubic
  • tetragonal
  • orthorhombic
  • rhombahedral
26
Q

Types of cubic crystal structures

A
  • face centered cubic
  • body centered cubic
  • simple cubic
27
Q

FCC

A
  • face centered cubic
  • 4 lattice points ((1/8 x 8)+ 1/2 x 6)
  • CN = 12
  • APF = 4r/sqrt(2)=.740
28
Q

BCC

A
  • body centered cubic
  • 2 lattice points
  • CN = 8
  • APF = 4r/sqrt(3) = .680
29
Q

SC

A
  • simple cubic
  • 1 lattice point
  • CN = 6
  • APF = .52
30
Q

Atomic Packing Factor (APF)

A

volume of atoms in unit cell/ volume of unit cell

31
Q

ceramic bonding

A

mostly ionic, some covalent

-ionic character increases with difference in electronegativity

32
Q

polymorphism

A

the same atoms can have more than one crystal structure

33
Q

FCC stacking sequence

A

ABCABC…

34
Q

BCC stacking sequence

A

ABABAB…

35
Q

alloys

A

atomic-sale mixtures of atoms

36
Q

electropositive

A

gives up an electron more easily than gaining one (3 or less valence electrons)

37
Q

electronegative

A

gains an electron more easily than it loses one (5 or more valence electrons)

38
Q

When is a bond half ionic and half covalent?

A

when the difference of electronegativity is 1.7

-when lower, more covalent. when higher, more ionic

39
Q

Long range order (LRO)

A

Materials that exhibit order over distances much greater than the bond length

40
Q

Short range order

A

the local arrangement of nearest-neighbor atoms about a central atom

41
Q

Lattice Points

A

the vertices of the unit cell

42
Q

Lattice Parameter

A

the length of the unit cell edges

MSE 2001 (2 decks)

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