Metals and Alloys W3 Flashcards

1
Q

Where are metals used in dentistry?

A

Metal prostheses: inlay, onlay, partial crowns, full crowns, bridges, endodontic posts
Cast metal substrcutures: metal-resin protheses

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2
Q

What forms are metals generally used in for dentistry

A

Alloy form - We want strong metals in the oral cavity, need compressive and tensile material and control of the phases formed for corrosion resistance…
therefore we alloy a pure metal = STRONG

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3
Q

What form do metals take in their solid state?

A

Crystaline - highly ordered 3D arrangement of atoms

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4
Q

What are the different types of Unit cells for crystal structures**

A
  • *FCC** (face centred cubic) - 4 atoms per lattice point (box)
  • *BCC** (body centred cubic) - 2 atoms per lattice point (box)
  • *HCP** (hexagonal close packed) ex. Ti
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5
Q

What is the difference between single crystal and polycrystalline material - what would be the prefered material in dentistry and why?

A

Single crystal: repeated arrangement of atoms = Flat regular faced crystalline material

Polycrystalline: Made of crystals of different size, orientation, shape ie. GRAINS

Dentistry = polycrystalline because grain boundaries and point defects stop cracking propagation and increase the strength of the material.

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6
Q

What two things strengthen a material (metal)?*

A
  • Point defects
  • Grain boundries
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7
Q

What size grains provide strength*

A

Smaller grains = High strength material
- Strengthen the material due to localised point defects that impede dislocation propagation.

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8
Q

How do you identify if a metal will be readily oxidised or reduced

A

The ‘activity series’ which is based on standard reducion potentials (order of what is easily oxidised (more -ve reduction potential) and what isnt as easily oxidised (more +ve reduction potential) ie. measure of ease of oxidation.

Active = easily oxidised, Inactive = oxidation difficult

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9
Q

What does the term ‘active metals’ refer to

A

Metals that are inclined towards rapid oxidation

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10
Q

Patient has Amalgam fillings. What happens when they bite on a piece of alfoil?

A

Due to Al (anode) reacting with the filling/Hg (cathode) in the presence of saliva (electrolyte)
= reaction circuit creates current sensed by nerve
= pain/buzzing sensation

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11
Q

What is the definition of corrosion*

A

Chemical or electrochemical reactions between a metal based material and its environment that produces a deterioration of the material and its properties
- Redox process where electrons are lost (oxidised) by one chemical species and gained by another (reduced)

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12
Q

What is the predominant form of corrosion for the oral cavity and how does this differ from the other type of corrosion

A

Electrochemical corrosion - requires presence of fluid electrolyte (saliva)

Chemical corrosion- forms through oxidation reactions. Also called dry corrosion as doesn’t require fluid for electrical current.

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13
Q

What happens when ion rusts and what speeds up this process?

A
  • oxidation of Fe to Fe2+
  • reduction of O2 to O2-
  • oxidation of Fe2+ to Fe3+

Fe acts as both the anode (where pitting occurs) and a catode (elsewear).

Electrolyte solutions such as salt water. These enhance electrical circuit allowing passage of a current.

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14
Q

What are dissimilar metals

A

Metals at close proximity (in salvia - electrolyte) which have a difference in electrode potential
= voltaic cell established

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15
Q

Explain what happens in the mouth when gold crowns and amalgam fillings are in close proximity*

A
Amalgam oxidised (corrosion) and gold reduced 
with saliva acts as electrolyte allowing set up of voltaic cell = creates current
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16
Q

What is stress corrosion cracking and what 3 things are required for this to occur?

A

corrosion forms pits -> crack initiation -> crack propagation

Requires: susceptible material, corrosive environment and tensile stress- compressive stress is common in mouth.

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17
Q

What are phase equilibrium diagrams**

A

A map of the phases and phase equilibria of a system against variables such as temp, pressure, composition ect.

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18
Q

Define sublimation

A

From solid to gas (vapour) - without liquid intermediate

Opposite = deposition (gas to solid)

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19
Q

How do you freeze bone long term so that it is useable?**

A

Freeze drying is a example of an application of phase diagrams

This is how bone allografts are prepared for storage at room temp.
Sublimation: Ice is removed from frozen bone without melting to liquid. Goes from solid to Gas by lowering temp, then pressure, then rasing temp.
Example of exploiting phase diagrams

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20
Q

Where does equilibria exist on phase diagrams?

AND

What is the Equilibrium Boundary and where is it found?

A

Equilibria exists on phase boundary lines.

Equilibrium boundary- the conditions where two phases exist in equilibrium/where its changing between 2 phases

Found on sublimation curve, boiling curve and freezing point curve.

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21
Q

Difference between Triple Point and Critical Point

A
  • *Critical Point::** Temperature above which higher pressure (applied pressure) does not liquify
    ie. On gas to liquid phase boundry (vapour pressure line), usually pressure applied to gas causes a liquid.

Triple Point: where all three phases are at equilibrium, used for calibrating thermometers

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22
Q

Draw and label a phase diagram for H20. What are the triple point, critical point and sublimate pressure?

A

Triple point = 0.01 degrees, 0.006 atms

Critical point = 374 degrees, 218 atms

Sublimates at pressures above 0.006 atm

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23
Q

What is the eutectic point?**

A

Mixture of substances (in fixed proportions) which melt at a temp that is lower than the melting points of each of the seperate components
Ex. lidocaine + prilocaine

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24
Q

What are polymorphs

A

compounds with different crystalline forms that are in the same state/phase

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25
Q

What are drug polymorphs*

A

Solid-state drugs in different crystalline conformations, due to intermolecular forces = different physical properties (solubility, bioavailability)

26
Q

What is a clinical example of phase diagrams, specifically exploiting the eutectic point**

A
  • *Lidocaine and prilocaine**
  • normally solid at room temp, need liquid to apply
  • once the eutectic point is found the emulsion (at that proportion) will be liquid at room temp
27
Q

Define a metal*

A

A class of solid substances characterised by high electrical and thermal conductivity as well as by malleability, ductility, and high reflectivity of light.

28
Q

Define an alloy*

A

A material with metallic properties resulting from the combination of > 1 element (2 or more)

29
Q

Homogenous solutions (solution alloys) include, substitutional and interstitial alloys, compare*

A

Substitutional: crystal structure of solvent retained, solute atoms enter the lattice and substitute for some solvent atoms
- atoms are similar size and have similar chemical bonding
Example: Form binary metal alloys ex.
Cu+Zn (brass)

Interstitial: One atom type is smaller and fits into the interstices of the structure. E.g. Fe+C (stainless steel - small carbon atoms fit into interstices of the iron matrix.

30
Q

What properties can alloying change*

A

Physical properties: Lustre, malleability, ductility, hardness, melting point, corrosion

31
Q

What is a solid solution?*

A

Both metals are completely soluble in each other in all combining proportions

32
Q

What are noble metals and why are they used in dental alloys*

A

Like noble gases
- relatively chemically inert, resistant to oxidation
Therefore good for dental alloys!
ex. gold, platinum

33
Q

What are base metals

A
  • *Non-noble, more easily oxidised**
    ex. Fe, Ti, Co
34
Q

Compare and give an example of homogeneous and heterogeneous alloys*

A
  • *Heterogeneous**: components not dispersed uniformly ie. 2 distinct phases/microstructures/products
    ex. in pearlite steel - ferrite (phase 1) cementite (phase 2)
  • *Homogenous**: components dispersed uniformly but randomly at ALL proportions. Same crystal type (BCC ect.)
    ex. stainless steel (interstitial)
35
Q

What are intermetallics and why are they special*

A

Components have discrete compositions ie. repeating unit cell

Gamma phase in dental amalgam
ex. Ag3Sn - y (gamma) phase dental amalgam

36
Q

What is amalgam

A

Substance formed by mixing Hg with another metal = alloy

37
Q

What elements are in dental amalgam

A

Ag, Sn, Cu, Zn, Hg

38
Q

What is the process of amalgamation (generally)

A

Mixing liquid mercury with the powedered intermetallic solid alloy (silver tin) to form amalgam

39
Q

What is the setting reaction for a low Cu alloy (Amalgamation)**

A

Ag3Sn + Hg —> Ag3Sn + Ag2Hg3 + Sn8Hg

Copper increases strength and reduces corrosion
All products in gamma phase (y, y1 and y2 respectively) - These are all solid phases but are structurally different to each other, hence the use of the word microstructure.

40
Q

Why do we add copper in amalgamation*

A

Copper added to the alloy > 5% removes the Sn8Hg (y2) phase and you get a secondary reaction (another reaction) forming Copper-tin.
Ie. favourable as y2 phase was the weakest and least corrosion resistant
= increases strength, reduces corrosion

41
Q

What is the Pd-Ag (paladium silver alloy) used for?

A

Homogeneous alloy at all proportions

Used for cast metal prosthesis
Noble metal alloy & similar size atoms = solution alloy

42
Q

What is the best cooling rate to achieve homogeneous alloys

A

Slow cooling = grains become homogeneous

43
Q

What happens when we cool things to quickly

A

heterogenous composition = layered grains of differing compositon ie. coring = more susceptible to corrosion

44
Q

Whats special about titanium (Ti)*

A
  • corrosion resistant due to surface of TiO2 film!
  • offers strength/weight advantages
  • physical properties easily modified by alloying
  • is used for biocompatible implant materials (osseointegration of live bone and implant)
45
Q

What is osseointegration, give an example of a metal used**

A

A direct structural and functional interface between the live bone and Ti impact surface (without any intervening fibrous C.T)

46
Q

What phases can Ti exist in*

A
  • *a (alpha) phase** - commercially ‘pure’ form - HCP structural form
  • *B (beta) phase** - BCC structural form

Adding oxygen to Ti makes a significant difference to the strength*

47
Q

What happens when you alloy Ti and Aluminium and Vanadium*

A
  • *Aluminium** promotes the alpha phase (decreases density, increases strength)
  • *Vanadium** promotes the beta phase

Together/both phases exist at the same time = substitutional alloy

= Ti 6Al 4V

48
Q

What is the benefit of alloying Ti with Aluminium and Vanadium (substitutional alloy)*

A

Combination of alpha and beta phase enable heat treatment and precipitate hardening which strengthens the structure…
= Heat resistant, low density, strong, resistant to corrosion and fatigue, good elasticity and biocompatible

49
Q

Binary metal alloys can be defined as?

What does their formation depend on?

A

Substitutional solution alloys- Homogenous and random

  1. proportion of elements
  2. rates of cooling from liquid state
50
Q

What is an example of an inter metallic compound and what does it mean?

A

components have discrete concentrations- every unit cell is the same

Ag3Sn gamma phase dental amalgam

51
Q

What is coring and when does it occur?

A

Layered grains of differing compositions. Occurs in fast cooling, results in higher grain boundaries, high corrosion chance.

52
Q

What is osseointegration and what metal does it relate to?

A

Titanium fuses directly to bone:

Direct structural and functional interface between live bone and Ti implants surface

Doesn’t intervene with connective tissue.

53
Q

What is the allotropic phase change Ti undergoes and at what temp does this occur?

A

alpha HCP → Beta BCC

For pure titanium above 882 degrees undergoes this phase change ie, when you heat

54
Q

What does formation of a homogenous solution alloy depend on and how might coring be avoided?

A
  • The formation of a homogenous binary metal solution alloy depends on the proportions of the combining metal elements and rates of cooling from liquid state.
  • For slow cooling, diffusion of atoms in solid grains at temperature allows grains to become homogenous.
  • If fast cooling, we can end up with layered grains of differing composition (coring)
55
Q

What 4 conditions in the oral cavity contribute to corrosion?

A

Conditions: moisture, electrolytes, temp variance and pH changes.

56
Q

What is an electrode potential?

Why are effective electrode potentials altered?

A

measurement of potential for equlibrium- differences between electrode and electrolyte

Differences in materials, deformations in homegeneties across structures. Electrolyte concentration variances.

57
Q

What is the negative effect of cold working metal alloys in relation to stress?*

A

Causes stress corrosion - oxide layer is removed = deformed (stressed) regions

= anodic regions where oxidation can occur. Less stressed regions- cathode.

58
Q

What enables corrosion of grain boundaries?

A

heat treatment

59
Q

Describe what is happening on the left and right of this diagram.

Ie. describe the difference in cooling with regard to grain size, corrosion and grain boundries*

A

Left: Fast cooling- small grains = coring = less corrosion resistant = more grain boundaries

Right: Slow cooling - larger grain = homogeneous = more corrosion resistant = less grain boundaries

60
Q

Which is the reduction and which is the oxidation in this diagram?

A

Reduction = O2 + 4H + 4e- → 2H2O (GOLD)

Oxidation = Sn8Hg → Sn2+ (dental filling)

61
Q

What is metallic bonding and what are the forces involved?*

A

Metallic bonding: Metal + Metal

Electron sea model: delocalised ‘sea’ of mobile valence electrons around metal ions