Test 3. Chapter 12 Flashcards

1
Q

ceramic bonding?

A
  • mostly ionic, some covalent

- % ionic character increase with difference in electronegativity

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2
Q

ceramic bonding depends on what?

A

bonding

large vs small ionic bond character

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3
Q

define coordination number

A

maximize the number of nearest oppositely charged neighbors

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4
Q

what is charge neutrality

A

net charge in the structure should be zero

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5
Q

coordination number increases with ???

A

rcation/ranion

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6
Q

AX-type crystal structures include, _____________-

A

NaCl, Cs,Cl, and zinc blende

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7
Q

AX2 crystal structure includes

A

UO2, ThO2, ZrO2, CeO2, fluorite

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8
Q

why are ceramics more brittle than metals?

A

slippage along planes

  • in ionic solids this slippage is very difficult
  • too much energy needed to move one anion past another anion
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9
Q

How can you measure elastic modulus

A

Room T behavior is usually elastic, with brittle failure.

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10
Q

why is 3 point bend testing often used?

A

tensile tests are difficult for brittle materials

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11
Q

most common elements on earth are _____________?

A

Si, O

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12
Q

silicate ceramics

A

crystobalite

They are so small that the they have unusually unit structure. They share oxygen atoms

Crystalline SiO2 (silica) structures are quartz,
crystobalite, & tridymite

• The strong Si-O bond leads to a strong, high melting
material (1710ºC)

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13
Q

armorphous silica

A

done have organized patter for the way we assemble the basic structure together

not enough atoms to cancel out the charge of the oxygen atoms so now you have HYDROGEN atoms added

Silica gels - amorphous SiO2

– Si4+ and O2- not in well-ordered
lattice

– Charge balanced by H+
(to form
OH-
) at “dangling” bonds
• very high surface area > 200 m2
/g

– SiO2
is quite stable, therefore
unreactive
• makes good catalyst support

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14
Q

define silica glass

A

a dense form of amorphous silica

  • has Na+ ions to correct charge inbalance. “counter cations”

– Borosilicate glass is the pyrex glass used
in labs
• better temperature stability & less brittle than sodium
glass

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15
Q

silicates

A

Combine SiO4
4- tetrahedra by having them share
corners, edges, or faces

Cations such as Ca2+, Mg2+, & Al3+ act to
neutralize & provide ionic bonding

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16
Q

layered silicates

A

– SiO4 tetrahedra connected
together to form 2-D plane

  • (Si2O5)2-
  • So need cations to balance charge
17
Q

carbon forms

A

amorphous/olycrystalline-surface area ca 1000m^2/g

18
Q

what are different forms for diamond? and describe?

A

– tetrahedral carbon
• hard – no good slip planes
• brittle – can cut it

– large diamonds – jewelry

– small diamonds
• often man made - used for
cutting tools and polishing
– diamond films (artificial)
• hard surface coat 

– tools,
medical devices, etc.

19
Q

carbon forms - graphite

A
  • layer structure-aromatic layers
  • weak van der waals forcer between layers
  • planes slip easily, good lubricant
20
Q

carbon forms- fullerenes and nanotubes

A
  • fullerenes or carbon nanotubes
  • wrap the graphite sheet by curving into ball or tube
  • buckminister fullerness
21
Q

what are some defects in ceramic structures?

A

frenkel defect- a cation is out of place ( a pair of cation vacancy +cation interstitial_

shottky defect- a pair set of cations and anion vacancy

22
Q

impurities must also satisfy __________= electroneutrailty

A

charge valance

23
Q

ceramic materials have _________ and __________ bonding

A

covalent and ionic bonding

24
Q

structures based on :

A

CHARGE NEUTRALITY

maximizing # of nearest oppositely charged neighbors

25
Q

structures may be predicted based on:

A

ratio of the cation and anion radi

26
Q

defects ?????//

A

must have preserved charge neutrality

have a concentration that varies exponentially w/T

27
Q

room T mechanical response is elastic, but fracture is brittle negligible deformation

-elevated T creep properties are generally superior to those of metals (and polymers)

A

general