HYDROGEN EMBRITTLEMENT OF FERROUS MATERIALS · The stepwise repeated slow strain rate test (SW...
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Université Libre de Bruxelles Faculty of Applied Sciences Department of Matter and Materials Materials Science and Electrochemistry Group
Supervisor Jean – Luc Delplancke Co Supervisor Antoine Pourbaix
Academic year 2005 – 2006
HYDROGEN EMBRITTLEMENT OF
FERROUS MATERIALS
Mioara Elvira Stroe
Supervisor Dr. Jean Luc Delplancke
Co – supervisor Antoine Pourbaix
Local Members of the Jury Dr. Luc Segers
Dr. Marie–Paule Delplancke
Dr. Marc Degrez
Invited Members of the Jury Dr. Patrick Toussaint Industeel Belgium, Group Arcelor
Dr. Mihai Popa Institute of Physical Chemistry “I.G. Murgulescu”, Romania
Belgium, January 2006
To Luiza, Cris, Anastasis and Anouka
Preface
This thesis is submitted to the Faculty of Applied Sciences at the Université Libre
de Bruxelles, Belgium, in order to fulfil the requirements for obtaining the Ph.D. degree in
Applied Sciences.
This study was financed by Industeel Belgium, in the frame of a broader research
program between Industeel Belgium and CEBELCOR
Acknowledgements
I am deeply indebt to Antoine Pourbaix, co – supervisor of this thesis, for guiding
me during all these years. His clarity of spirit and enthusiasm continuously amazed me and
inspired me. I thank him for constantly encouraging me and for the extensive discussions that
helped me to find the way.
By his support I could visit some laboratories abroad (NPL in UK, Statoil Norway,
ECP France) and to participate to several conferences.
I would like to thank Jean Luc Delplancke, the head of Department of Materials
Science and Electrochemistry for hosting me in his Department and for all support he granted
me in the past four years.
I like to acknowledge Industeel Belgium, and particularly Patrick Toussaint and
Jean Jacques Dufrane for financial and scientific support.
I am very glad that I found in Renée Scherer, Jacques Kissel and Suzanne de
Kegel not only very kind colleagues but also friends. My work and my stay here was more
pleasant due to their presence.
I enjoyed collaborating with Jean Dille, Roger D’Haens, Lionel Canet, Olivier van
de Vyver and Victor Wertz from the Department of Materials Science and Electrochemistry.
I would like to thank to Catherine Dagbert from Ecole Centrale Paris. Part of
fractional thermal degassing tests presented in Section 7.2. were performed with her
assistance.
I am pleased to mention the good collaboration with Vincent Ligier to whom I thank
for helping me with measurements by fractional thermal degassing at CRMC Industeel Creusot
and also with many useful advices.
I thank to Liane Smith (Intetech Ltd. UK) and Stein Olsen (Statoil Norway) for the
insights on the industrial aspects of the problem of hydrogen embrittlement.
I like to thank to my sister and my parents for encouraging me all this time. The
holydays and their phone calls cheered me up whenever was needed.
My gratitude goes to my friend Tarik Bouali whose determined character and keen
sense of detail were an example for me.
ABSTRACT
This work deals with the damage due to the simultaneous presence of hydrogen in
atomic form and stress – straining.
The aim of this work is twofold: to better understand the hydrogen embrittlement
mechanisms and to translate the acquired knowledge into a more appropriate qualification test.
The phenomena of hydrogen entry and transport inside the metals, together with
the different types of damages due to the presence of hydrogen, are presented.
The analysis of the most important models proposed up to now for hydrogen
embrittlement (HE) indicated that the slow dynamic plastic straining is a key factor for the
embritteling process. There is a synergistic effect of hydrogen – dislocations interactions: on
one hand hydrogen facilitates the dislocations movement (according to the HELP mechanism)
and on the other hand dislocations transport hydrogen during their movement when their
velocity is lower than a critical value.
This work is focused on supermartensitic stainless steels, base and welded
materials. The interest on these materials is due to their broad use in offshore oil production.
First, the material’s characterisation with regards to hydrogen content and
localisation was performed. This was conducted in charging conditions that are representative
of industrial applications.
Because of previous industrial experience it was necessary to find a more
appropriate qualification test method to asses the risk of HE.
In this work we proposed the stepwise repeated slow strain rate test (SW R –
SSRT) as a qualification test method for supermartensitic stainless steels.
This test method combines hydrogen charging, test duration, plastic, dynamic and
slow strains. Thus, this test method is coherent with both the model HELP proposed for
hydrogen embrittlement and the observations of industrial failures.
The stepwise repeated slow strain rate test (SW RSSRT) is interesting not only as
a qualification test of martensitic stainless steels, but also as a qualification test of conditions for
using these materials (type of straining, range of strain and stress, strain rate, hydrogen
charging conditions, etc.).
RESUME
Ce travail se rapporte à l’endommagement provoqué par la présence simultanée
de l’hydrogène sous forme atomique et une contrainte (appliquée où résiduelle).
Ce travail a comme but une meilleure compréhension du mécanisme de la
fragilisation par l’hydrogène (FPH) et la recherche d’un essai de qualification qui soit cohérent
avec ce mécanisme.
Les phénomènes liés à l’entrée et au transport de l’hydrogène au sein des métaux,
ensemble avec les différents types d’endommagements dus à la présence de l’hydrogène, sont
présentés.
L’analyse des modèles proposés jusqu’au présent pour la fragilisation par
l’hydrogène (FPH) suggère que la déformation lente plastique dynamique est le facteur clé pour
le processus de la fragilisation. Il y a un effet synergétique des interactions entre l’hydrogène et
les dislocations: d’un coté l’hydrogène facilite le mouvement des dislocations (d’après le modèle
HELP) et d’un autre coté les dislocations transportent l’hydrogène pendant leur mouvement,
pourvu que leur vitesse soit en dessous d’une valeur critique.
Le travail a été conduit sur des aciers supermartensitiques, matériau de base et
soudé. L’intérêt pour ces matériaux réside de leur large utilisation dans la production du pétrole
en offshore.
D’abord, le matériau a été caractérisé du point de vu de la teneur et de la
localisation de l’hydrogène. Les essais ont été conduits dans des conditions représentatives
pour les cas industriels.
L’expérience industrielle d’auparavant indique qu’il est nécessaire de trouver un
test de qualification plus approprié pour estimer la susceptibilité à la fragilisation par
l’hydrogène.
Dans ce travail on propose un essai de traction lente incrémentée (SW R – SSRT)
comme méthode de qualification pour les aciers supermartensitiques.
L’essai combine le chargement en hydrogène, la durée d’essai, la déformation
lente, plastique et dynamique. Donc, cette méthode d’essai est cohérente avec le modèle HELP
proposé pour FPH et les observations des accidents industriels.
Cet essai est intéressant pas seulement comme essai de qualification pour les
aciers supermartensitiques, mais aussi comme essai de qualification pour les conditions
d’utilisation des ces matériaux (type de déformation, niveau de déformation et contrainte,
vitesse de déformation, conditions de chargement en hydrogène, etc.).
TABLE OF CONTENT NOTATION 1. INTRODUCTION …………………………………………………………..
1.1. ORIGIN AND AIMS OF THE WORK 1.2. STRUCTURE OF THE WORK
2. HYDROGEN ENTRY AND TRANSPORT IN METALS ………………
2.1. HYDROGEN ADSORPTION 2.1.1. ELECTROCHEMICAL CHARGING
2.1.2. CHARGING FROM GASEOUS HYDROGEN ATMOSPHERE
2.1.3. THE INFLUENCE OF SURFACE STATE ON ADSORPTION
2.2. HYDROGEN ABSORPTION 2.2.1. ATOMIC HYDROGEN TRANSFER (CLASSICAL
MECHANISM)
2.2.2. DIRECT TRANSFER OF H+ THROUGH THE INTERFACE
(MODEL PROPOSED BY CROLET ET AL.)
2.3. HYDROGEN TRANSPORT IN MATERIAL 2.3.1. DIFFUSION
2.3.1.1. IDEAL DIFFUSION, FICK’S LAW
2.3.1.2. TEMPERATURE EFFECTS
2.3.1.3. DIFFUSION UNDER STRESS GRADIENT
2.3.2. TRAPPING
2.3.3. TRANSPORT OF HYDROGEN BY MOVING DISLOCATIONS
2.4. SUMMARY OF HYDROGEN IN METALS
3. TYPES OF DAMAGES DUE TO HYDROGEN ………………………..
3.1. HYDROGEN INDUCED CRACKING (HIC) AND STEPWISE CRACKING (SWC)
1.
3.5.
7.
10.10.
15.
18.
18.
19.
22.
23.23.
23.
25.
26.
26.
28.
30.
33.
36.
3.2. STRESS ORIENTED HYDROGEN INDUCED CRACKING (SOHIC) 3.3. HYDROGEN REACTION WITH THE METAL MATRIX (HYDRIDE
FORMATION) 3.4. HYDROGEN REACTIONS WITH NON METALLIC PHASES 3.5. HYDROGEN EMBRITTLEMENT (HE ) OR HYDROGEN STRESS
CRACKING (HSC) 3.6. SULPHIDE STRESS CRACKING (SSC)
4. HYDROGEN EMBRITTLEMENT ………………………………………..
4.1. DECOHESION MECHANISM 4.1.1. THERMODYNAMIC ASPECTS OF INTERFACIAL
DECOHESION
4.1.2. ELECTRONIC DISTRIBUTION IN H – METAL SYSTEMS
4.1.3. EXPERIMENTAL OBSERVATIONS
4.1.4. CONCLUSIONS FOR THE DECOHESION MECHANISM
4.2. PLASTICITY MODEL: HYDROGEN ENHANCED LOCALISED
PLASTICITY “HELP” 4.2.1. HYDROGEN SHIELDING EFFECT
4.2.1.1. HYDROGEN EFFECT ON THE INTERACTIONS
BETWEEN DISLOCATIONS
4.2.1.2. INTERACTIONS BETWEEN DISLOCATIONS AND
AN IMPURITY ATOM IN THE PRESENCE OF
HYDROGEN
4.2.2. MICROSCOPIC OBSERVATIONS
4.2.3. MACROSCOPIC OBSERVATIONS
4.2.4. CONCLUSIONS FOR THE HELP MECHANISM
4.3. CONCLUSIONS ON THE PARAMETERS AND ON THE MODELS PROPOSED FOR HYDROGEN EMBRITTLEMENT
5. INDUSTRIAL ASPECTS AND NEED FOR A HE TEST METHOD ...
5.1. HISTORIC OF SUPERMARTENSITIC STAINLESS STEEL USE IN OFF SHORE
37. 38.
39. 39.
40.
41.
44.
44.
48.
48.
49.
50.
51.
52.
55.
55.
60.
61.
61.
65.
67.
5.2. FAILURES DUE TO HYDROGEN EMBRITTLEMENT 5.3. NEED FOR A HE TEST METHOD
6. MATERIALS AND EXPERIMENTAL TECHNIQUES …………………
6.1. MATERIAL DESCRIPTION 6.1.1. OVERVIEW OF GENERAL MECHANICAL PROPERTIES
6.1.2. CHEMICAL COMPOSITION AND MICROSTRUCTURE
6.1.3. WELD DESCRIPTION
6.2. EXPERIMENTAL METHODS 6.2.1. PERMEATION METHOD
6.2.2. THERMAL DEGASSING
6.2.2.1. FRACTIONAL THERMAL DEGASSING
6.2.2.2. TOTAL DEGASSING
6.2.3. NANOINDENTATION METHOD
6.2.4. MECHANICAL TESTS
6.2.4.1. CONSTANT LOAD TEST
6.2.4.2. SLOW STRAIN RATE TEST (SSRT)
6.2.4.3. REPEATED SLOW STRAIN RATE TEST (RSSRT)
6.2.4.4. STEPWISE REPEATED SLOW STRAIN RATE TEST
(SW RSSRT)
7. EXPERIMENTAL RESULTS …………………………………………….
7.1. PERMEATION TESTS RESULTS 7.2. RESULTS FOR THERMAL DEGASSING TESTS
7.2.1. FRACTIONAL THERMAL DEGASSING
7.2.2. TOTAL DEGASSING
7.2.3. CONCLUSIONS OF THERMAL DEGASSING TESTS
7.3. RESULTS OF NANOINDENTATION TESTS 7.4. RESULTS OF MECHANICAL TESTS
7.4.1. RESULTS FOR CONSTANT LOAD TESTS
69.71.
73.
75.75.
77.
78.
81.81.
88.
88.
89.
91.
94.
94.
96.
99.
100.
103.
105.
118.118.
121.
121.
122.
127.127.
7.4.2. RESULTS OF SLOW STRAIN RATE TESTS
7.4.3. REPEATED SLOW TRAIN RATE TESTS RESULTS
7.4.4. STEPWISE REPEATED SLOW STRAIN RATE TESTS
RESULTS
8. DISCUSSION ………………………………………………………………
8.1. HYDROGEN DISLOCATIONS INTERACTIONS 8.2. THE EMBRITTLING PHENOMENON: FROM HELP TO
EMBRITTLEMENT 8.3. BEHAVIOUR OF VARIOUS FERROUS MATERIALS IN THE
PRESENCE OF HYDROGEN 8.4. PROPOSAL FOR SPECIFIC HE TESTS FOR MARTENSITIC
MATERIALS 8.5. RESULTS OF HE TESTS USED IN THIS WORK 8.6. SW RSSRT AS A QUALIFICATION TEST FOR MARTENSITIC STEELS
AND FOR OPERATING CONDITIONS
9. CONCLUSIONS …………………………………………………………... 10. REFERENCES ……………………………………………………………. 11. APPENDICES ……………………………………………………………..
APPENDIX 1. HYDROGEN EVOLUTION REACTIONS …………………………. APPENDIX 2. THERMODYNAMIC AND KINETIC ASPECTS OF THE
INTERFACIAL DECOHESION …………………………………….. APPENDIX 3. ATOM SUPERPOSITION AND ELECTRON DELOCALISATION
MOLECULAR ORBITAL METHOD (ASED – MO) ……………… APPENDIX 4. HYDROGEN SHIELDING EFFECT ………………………………..
128.
148.
161.
171.
173. 175.
175.
177.
178.
181.
183.
189.
201.
203.
213.
227. 229.
NOTATION
Roman letters
A
A.R.
AFM
b
C0
CE
CL
D
Dok
E
Ea
Er
F
2Fk*
G
GTAW
h
Hnano
[H]
[H+]
HAZ
HE
HELP
HIC
HID
i
i0
J
Jabs
Jads
Jdes
Jdsb
Jss
Surface
Area reduction
Atomic force microscopy
Burgers vector
Subsurface concentration
Counter electrode
Constant load test
Diffusion coefficient
Preexponential term for kink diffusion
Potential
Activation energy
Reduced elastic modulus
Faraday constant
Free energy of formation of a double – kink on a dislocation
Shear modulus
Gas tungsten arc welding
Depth
Nanohardness
Concentration of hydrogen atoms on the metallic surface
Concentration of hydrogen cations in solution
Heat affected zone
Hydrogen embrittlement
Hydrogen enhanced localised plasticity
Hydrogen induced cracking
Hydrogen induced decohesion
Current density
Exchange current density
Flux
Flux of absorbed hydrogen atoms
Flux of adsorbed hydrogen atoms
Flux of desorbed hydrogen atoms
Flux of hydrogen atoms diffusing out from the bulk of material
Steady state flux
k
ki
l
l
L
m
ni
Ni
No
Nr
Ns
P
Pnano
PGMAW
Qk
r
R
RE
R SSRT
S
Snano
SCE
SCC
SEM
SOHIC
SSC
SSRT
SW M SSRT
SW R SSRT
t
T
TEM
TTF
UTS
vcr
V
VH
Boltzmann’s constant
Rate constant for reaction i
Dislocation length
Strain increment
Membrane thickness
Mass
Stoichiometric coefficient of species i
Density of irreversible traps
Number of interstitial sites occupied by hydrogen
Density of reversible traps
Number of interstitial sites in the matrix
Hydrogen partial pressure
Indentation load
Pulse gas metal arc welding
Activation energy for kink diffusion
Distance in polar coordinates
Gas constant
Reference electrode
Repeated slow strain rate test
Sieverts constant
Stiffness
Saturated calomel electrode
Stress corrosion cracking
Scanning electron microscopy
Stress oriented hydrogen induced cracking
Sulphide stress cracking
Slow strain rate test
Stepwise monotonic slow strain rate test
Stepwise repeated slow strain rate test
Time
Temperature
Transmission electron microscopy
Time to failure
Ultimate tensile strength
Critical velocity of dislocation
Mean molar volume
Molar volume of hydrogen
Greek letters
x
W
WB
WE
YS
YS0.2%
Distance
Activation energy
Bonding energy between hydrogen and trap
Working electrode
Yield strength
Offset yield strength
αi Transfer coefficient of reaction i β Proportionality constant γ Proportionality constant δ Separation distance between two layers of the interface δc Critical separation distance
∆l Strain to failure ε Strain η Overpotential θ Coverage degree θ0 Equilibrium coverage degree
θL Occupancy of the interstitial sites
θr Occupancy of the reversible sites
µ Bulk modulus ν Poisson’s coefficient σ Stress σh Hydrostatic stress τ Shear stress ϕ (χ, δ) Cohesive function
φ Angle in polar coordinates
1. INTRODUCTION
1. INTRODUCTION
2
1. INTRODUCTION
3
1.1. ORIGIN AND AIMS OF THE WORK Several cracking accidents occurred recently in offshore exploitations that were
attributed to hydrogen embrittlement (HE).
The structures involved are flowlines and equipments installed on the bottom of the
sea.
These flowlines are protected against corrosion by cathodic protection with
aluminium – indium (AlIn) or aluminium – zinc – indium (AlZnIn) sacrificial anodes and by heavy
duty coatings.
The flowlines are subjected to elastic and plastic deformations during laying and
during operation: reeling and dereeling, laying, movements on the sea bed due to marine
streams, thermal expansion, pressure tests, or accidental interference with fishing activities.
The materials of the pipelines that experienced failure are martensitic and
supermartensitic stainless steels (SMSS) and duplex stainless steels (DSS).
Of course, these materials are known to be sensitive to hydrogen embrittlement.
However, extensive design analysis and qualification testing [1] indicate that they are
appropriate for this application. In particular extensive long-term testing showed no cracking
under constant load and under constant plastic deformation (four point bend tests) at – 1050
mV to – 1200 mV versus saturated calomel electrode (SCE).
As these materials are much more cost effective than carbon steel, their use has
markedly increased in the recent past [2] and is planned to increase further in the future.
These cracking accidents came as a surprise to many operators, because the
materials passed all the qualification tests and because, currently, there are about 2000 km of
such SMSS and DSS pipelines in operation and only few accidents occurred.
This work has two main purposes:
a better understanding of the hydrogen embrittlement mechanisms
involved in the failures,
1. INTRODUCTION
4
in case the HE tests used appear non appropriate, find better qualification
tests that better reflect the mechanisms and parameters involved in HE.
This study is focused on martensitic stainless steels, due notably to a marked trend
for a broader use of this material.
In principle two approaches can be considered:
a detailed fundamental analysis of the HE phenomena, to see the factors
that may cause failures,
a comprehensive analysis of the accidents.
Since a comprehensive analysis of the industrial accidents is not currently
available, this study was conducted mostly on the basis of an analysis of the fundamental
aspects of hydrogen embrittlement.
Extensive work was conducted and several models were proposed for hydrogen
embrittlement. But, none of the models proposed up to now can explain all the observed
phenomena or the role of all factors.
For example, the hydrogen content was often considered as the main factor (as in
the decohesion and the adsorption models, see section 4). The stress level is also considered
in most studies. But the loading mode, the local H accumulation and the local stress
concentration in the bulk of the material were not always given due consideration.
It was thus felt necessary to revisit the existing models with the aim of identifying
and analysing the influencing parameters.
Hydrogen embrittlement is a loss of mechanical properties due to the presence of
hydrogen in atomic form and stress. A significant decrease of ductility and /or fracture strength,
delayed fracture and absence of metal loss are typical features of HE.
In fact, this work showed that the fundamental approach combined with the real life
test parameters and with the analysis of the actual failures proved to be interestingly coherent.
1. INTRODUCTION
5
1.2. STRUCTURE OF THE WORK
After the presentation of the origin and the aims of this work (Section 1.1.), the
most important aspects of the hydrogen entry and behaviour inside the materials are presented
in Section 2.
In Section 3. a summary of different damages due to hydrogen is presented. This
chapter aims to identify the characteristics of Hydrogen Embrittlement (HE) in comparison with
other types of hydrogen damages. HE is the consequence of simultaneous presence of
hydrogen in atomic form and stress.
Several models were proposed up to now for hydrogen embrittlement. An analysis of
the most important is presented in Section 4. The factors involved in these models and that
must be considered for testing materials, were identified.
The industrial context at the origin of this work and the need for specific tests are
described in Section 5.
This study is focused on supermartensitic stainless steels. The description of the
materials and the experimental methods selected and used to characterise the materials for HE
is given in Section 6.
The results are presented in Section 7.
The discussion (Section 8) addresses the test methods that are coherent with the
mechanisms for hydrogen embrittlement and analyses the results, with a comparison with the
real conditions of failures.
Section 9 (Conclusions) summarises the important factors for hydrogen embrittlement
that are derived from the HELP model, how these factors can be included in a specific test
procedure for HE, how the results of a test proposed here are coherent with the models and
with the industrial experience.
1. INTRODUCTION
6
2. HYDROGEN ENTRY AND
TRANSPORT IN METALS
2. HYDROGEN IN METALS
8
2. HYDROGEN IN METALS
9
In this section the different steps involved in hydrogen entry and transport through
the material are presented.
The first step is hydrogen adsorption on the material surface. As source of hydrogen, electrochemical evolution of hydrogen by cathodic
polarisation, corrosion reaction or gaseous hydrogen atmosphere can be mentioned.
In this work two cases are analysed: cathodic protection in aqueous solution
(Section 2.1.1.) and adsorption from gaseous hydrogen atmosphere (Section 2.1.2.).
The influence of metallic surface state on the hydrogen adsorption is analysed in
Section 2.1.3.
The adsorbed atoms could then undergo absorption, passing through the metallic interface. This step leads to accumulation of a subsurface hydrogen concentration, C0. The C0
dependency on applied potential or current (for electrochemical charging) and pressure (for
charging from gaseous hydrogen atmosphere) is presented in Section 2.2.
The next process is the transport of hydrogen through the material. The different aspects, like diffusion, trapping and the hydrogen transport by moving dislocations are
presented in Section 2.3.
2. HYDROGEN IN METALS
10
2.1. HYDROGEN ADSORPTION
The adsorbed hydrogen atoms can be formed by different paths, according to the
source of hydrogen.
By cathodic polarisation or corrosion reaction, electroadsorbed species are formed
on the metallic surface whereas in the presence of a gaseous atmosphere the molecular
hydrogen can undergo physisorption or chemisorption.
2.1.1. ELECTROCHEMICAL CHARGING
In solution under cathodic polarisation, the hydrated hydrogen cations, H3O+, are
transported by diffusion / migration towards the cathode. There, the cation undergoes reduction
and becomes atomic hydrogen, H.. The atomic hydrogen can recombine to form molecular
hydrogen, H2 that leaves the metallic surface.
For the reduction of hydrogen ions two different reaction mechanisms are possible,
depending on the nature of the metal:
A. Volmer – Tafel mechanism (electrochemical reduction followed by chemical recombination)
adsorbed
k
khydrated HeH ↔
−
−+ +
1
1
Volmer reaction .)1.2(
2
2
2
HHHk
kadsorbedadsorbed ↔
−
+ Tafel reaction .)2.2(
B. Volmer – Heyrovsky mechanism (electrochemical reduction followed by electrochemical recombination)
adsorbed
k
khydrated HeH ↔
−
−+ +
1
1
Volmer reaction .)1.2(
2
3
3
HeHHk
kadsorbedhydrated ↔
−
−+ ++ Heyrovsky reaction .)3.2(
2. HYDROGEN IN METALS
11
Depending on the nature of the metal, the different mechanisms of hydrogen
reduction could take place. The paths followed by hydrogen reduction reaction on different
metals are given in Table 2.1.
For iron and steels the most probable mechanisms are coupled reduction –
chemical combination or slow reduction – fast electrochemical as noted in Table 2.1.
Table 2.1. Mechanisms followed by hydrogen reduction on different metals [3]
Metal Mechanism
Fe A : Coupled reduction, recombination
or
B :Slow reduction, fast electrochemical
Ti B: Fast reduction, slow electrochemical
Pd A : Fast reduction, slow recombination
Pt A : Fast reduction, slow recombination
Ni A : Slow reduction, fast recombination
For each of the two mechanisms, the reactions and the dependency of the degree
of coverage, θ, on the current or potential will be described.
θ is necessary to calculate the subsurface concentration C0.
The subsurface concentration, C0, is an important factor as it determines the
hydrogen content in the material (see Section 2.2. and 2.3.). It also determines the filling of
reversible traps, as will be presented in Section 2.3.
A. Volmer – Tafel mechanism The first reaction (Volmer reaction) is the cathodic reduction of hydrated cations to
form atomic hydrogen that remains adsorbed on the metallic surface.
The second reaction is the recombination of atomic hydrogen to form molecular
hydrogen and is a purely chemical reaction.
2. HYDROGEN IN METALS
12
The general expression for the rate of an electrochemical reaction is:
RT
FrevEE
einiC
RTW
kerate
))( −−
Π−
=
α
.)4.2(
Assuming that the Volmer reaction is the rate determining reaction, the expression
for the potential – current density dependency can be written as:
[ ]
−−
+−
= − η
αη
α
RT
FVHkRT
FVHki)1(
expexp 111 .)5.2(
The concentration of atomic hydrogen adsorbed on the surface, [H], is proportional
to the degree of coverage, θ. The reduction of hydrogen cation H+ occurs only on the sites that
are not covered by adsorbed hydrogen atoms. This part is equal to (1 – θ), so the second term
on the right side of equation (2.5.) is directly proportional to (1 – θ).
The current – potential relationship becomes:
−−−−
= − η
αθη
αθ
RT
FVkRT
FVki)1(
exp)1(exp 111 .)6.2(
By introducing the exchange current density for Volmer reaction, i0,V, and the
overvoltage expressions, η, the equation (2.6.) becomes:
−−
−−
−
= ηα
θθηα
θθ
RTF
RTFii VVV
)1(exp11exp
00,01 .)7.2(
2. HYDROGEN IN METALS
13
The equation (2.7.) expresses the dependence of the degree of coverage on the
current density i1 .
The Tafel reaction is a pure chemical reaction, so its rate constant does not depend on the potential. The reaction rate is given by:
[ ] ²)1( 2222 θθ −−−=−= kkdtHdFi .)8.2(
At equilibrium, i.e. when the overall rate is zero, the degree of coverage reaches
the equilibrium value, θ0, given by:
²)1( 022
022,0 θθ −=−= kki .)9.2(
For the Volmer – Tafel mechanism when the rate is determined by the Volmer
reaction, the degree of coverage is (See Appendix 1 ):
2,0
10 1 i
i−= θθ .)10.2(
where i0,2 is the reaction exchange current density for the equilibrium value of the
potential.
B. Volmer – Heyrovsky mechanism (electrochemical reduction followed by electrochemical recombination (Figure 2.2.)
adsorbed
k
khydrated HeH ↔
−
−+ +
1
1
Volmer reaction .)1.2(
2
3
3
HeHHk
kadsorbedhydrated ↔
−
−+ ++ Heyrovsky reaction .)3.2(
2. HYDROGEN IN METALS
14
The Heyrovsky reaction (2.3.) consists of the reduction of a hydrated hydrogen
cation with a hydrogen atom that is adsorbed on the metallic surface, with the formation of
molecular hydrogen. This equation is also an electrochemical reaction, as well as the Volmer
reaction (2.1.). The rate of the reaction is potential dependent.
The rate of the cathodic partial reaction is proportional to the degree of coverage,
θ, and the hydrogen cations concentration, [H+]. The reversal reaction is proportional to the
molecular hydrogen concentration, [H2], and the free part of the surface (1 – θ). The rate of
reaction (2.3.) is given by:
[ ] [ ]
−−−
−= +− η
αθη
αθ
RT
FHHkRT
FHHki)1(
expexp)1( 3233 .)11.2(
For the Volmer – Heyrovsky mechanism, θ depends on the current density of each
partial reaction involved, as both of them are charge transfer reactions.
Considering the equations (2.5.) and (2.11.) and for large overvoltage, the degree
of coverage becomes independent of the potential. E.g. for high cathodic overvoltage, θ is
expressed as:
H
V
ii
,0
,0
0
0
11
1
θθ
θ
−+
= .)12.2(
where i0,V and i0,H are the exchange current densities for the Volmer and
Heyrovsky reactions respectively.
The hydrogen coverage on the metal substrate depends both on the mechanism of
hydrogen evolution on the metal (A or B) and on the charging conditions (current density or
potential).
2. HYDROGEN IN METALS
15
2.1.2. CHARGING FROM GASEOUS HYDROGEN ATMOSPHERE
The model proposed by Wang in 1936 [4] and then improved by other authors [5 –
10] for the dissociative chemisorption of gaseous hydrogen is presented in Figure 2.1.
The process involves several steps:
a. The gas molecule strikes the material surface and splits into atoms that adhere
there.
adsorbedHH 22 ↔ .)13.2(
The flux of adsorbing atoms is second order in (1 – θ) and could be expressed by:
PkJ adsads )²1( θ−= .)14.2(
b. There is a reversal reaction of recombination of adsorbed atoms with the
formation of molecular hydrogen, which leaves the metallic surface. The desorbing flux is
second order in θ, since two adjacent atoms are needed to recombine:
²θdesdes kJ = .)15.2(
c. The adsorbed atoms could traverse the metallic interface and become absorbed
atoms. The corresponding flux is:
γθ=absJ .)16.2(
2. HYDROGEN IN METALS
16
d. The atoms inside the material could diffuse out to the surface and the flux is
proportional to the subsurface hydrogen concentration, C0, and the fraction of unoccupied
surface sites, through which hydrogen can diffuse out:
0)1( CJdsb θβ −= .)17.2(
The net flux has the following form:
²)²1( θθ desads kPkJ −−= .)18.2(
0)1( CJ θβγθ −−= .)19.2(
At equilibrium, there is no net flux. The degree of coverage, θ0, and subsurface
hydrogen concentration, C0, can be deduced as:
Pkk
des
ads=− 0
0
1 θθ
.)20.2(
PkkCdes
adseq β
γ=,0 .)21.2(
The expression for the concentration is known as the Sieverts’ law:
PSC eq =,0 .)22.2(
where S is Sieverts’ constant that depends on the kinetics of adsorption and
desorption processes:
βγ
des
ads
kkS = .)23.2(
2. HYDROGEN IN METALS
17
This model explains quantitatively how the net flux changes with the external gas
pressure.
The Sieverts’ law shows that the subsurface hydrogen concentration is
proportional to the square root of the hydrogen atmosphere pressure.
In Figure 2.2. an example of this dependency is presented for carbon steel at
different temperatures [11]. On the ordinate the flux units are presented, as the flux is
proportional to the subsurface concentration (see section 6. 1. Permeation test method).
J ads =kads(1–θ )²P
J dsb = β(1–θ )C0
J des = kdesθ²
J abs = γ θ
gas interface metal bulk
Figure 2.1. Fluxes involved in the hydrogen adsorption and absorption from gaseous atmosphere
0
5
10
15
20
25
0 50 100 150 200 250 300
square root of hydrogen pressure (Pa1/2)
Flux
(in
arbi
trar
y un
its)
Figure 2.2. Hydrogen flux – hydrogen pressure dependency at different temperatures for carbon steel [11]
413 K 483 K
533 K
633 K
698 K
2. HYDROGEN IN METALS
18
This type of charging can take place in the same time with electrochemical
charging: (for instance: pipelines at great depths, cathodically protected, with simultaneous
electrochemical charging and charging from gaseous H2 from bubbles at high hydrostatic
pressure).
2.1.3. THE INFLUENCE OF SURFACE STATE ON THE ADSORPTION
Presence of promoters for hydrogen entry An important aspect of hydrogen behaviour is the substantial enhancement of
absorption in the presence of specific compounds. These compounds such as S2-, HS –, H2S,
As etc., hinder the recombination of hydrogen atoms on the metallic surface and therefore
enhance the absorption reaction.
These compounds are usually referred to as poisons.
Even small quantities of poison strongly increase the hydrogen uptake. In Table
2.2. the hydrogen amount penetrating the material for constant charging current, when the
amount of sulphide in solution increases, is presented [12].
Table 2.2. Hydrogen uptake function of sulphide content in solution [12]
[S2–], ppm Hydrogen penetrating the steel (%)
3.5 x 10 – 3 1.6
1.3 x 10 – 2 2.4
2.75 x 10 – 2 5.8
3.6 x 10 – 1 25.6
Oxide films formed on the metallic surface are barriers for H absorption and are
hindering the hydrogen passage through the interface [13 – 17].
2.2. HYDROGEN ABSORPTION
With regard to the passage of hydrogen through the metallic interface, with the
accumulation of a subsurface concentration, C0, two mechanisms were proposed up to now:
2. HYDROGEN IN METALS
19
one mechanism considers that the same species (atomic H) adsorbed on
the surface lead to molecular and absorbed hydrogen (classical mechanism
presented in Section 2.2.1.)
Crolet et al. recently suggested that hydrogen is passing in ionic form (H+)
directly through the metallic interface to form a solid solution (Section 2.2.2.)
2.2.1. ATOMIC H TRANSFER (CLASSICAL MECHANISM)
After the reduction of hydrogen cations, a part of the hydrogen atoms that are
adsorbed on the metallic surface will recombine to form molecular hydrogen that leaves the
surface.
Another part of adsorbed hydrogen atoms will undergo an absorption reaction inside the material, according to the equilibrium:
absorbedadsorbed HH ↔ .)24.2(
The direct reaction, of passage of atomic hydrogen through the interface, depends
on the surface coverage (θ) and on the number of available sites in the subsurface that
hydrogen can occupy.
The consequence is the accumulation of hydrogen under the metallic surface,
leading to a concentration C0.
The reversal reaction, of hydrogen passage form the subsurface towards the
surface can take place.
The rate for the reversal reaction is proportional to the subsurface concentration
and to the concentration of empty sites on the surface through which hydrogen could be
desorbed (1 – θ ).
The rate of the overall reaction is:
)1(1 00 θθ −−
−= CkNN
ki dess
absabs .)25.2(
2. HYDROGEN IN METALS
20
At equilibrium (i abs = 0) and for small coverage degree θ and small degree of
saturation, the subsurface concentration of hydrogen C0 is proportional to the degree of
coverage:
0Ckk desabs =θ .)26.2(
or:
θKC =0 .)27.2(
where K is the ratio of the rate constants for the direct and reversal reaction of the
hydrogen passage through the interface (2.24.).
The equation (2.27.) shows that the subsurface concentration of hydrogen, C0, is a
function of the degree of coverage, θ.
We remind here that in the previous section we saw that θ depends on the
charging conditions (current density and potential) and also on the temperature.
Thus, the concentration of hydrogen in the material will also be depending on these
parameters.
Assuming that the passage of hydrogen through the interface (2.24.) is the slowest
step, then, for the Volmer - Tafel mechanism the relationship between the subsurface
concentration and the charging current can be found considering that reactions (2.1.) and (2.2.)
are at equilibrium, thus:
[ ] ²exp)1( 21 θηαθ kRTFHki =
−= + .)28.2(
Replacing θ from (2.28.) into (2.27.) leads to the value of C0 :
ik
KC2
01
= .)29.2(
2. HYDROGEN IN METALS
21
The subsurface concentration C0 depends not only on the charging current, but
also on the kinetics of hydrogen evolution (through k2).
The square root dependence on the charging current is followed up to certain value
of the current density. Above a limiting value, the subsurface concentration of hydrogen
becomes independent of the charging current (Figure 2.3.). This corresponds to the saturation
of the surface ( θ = 1).
In the presence of promoters (or poisons) this square root dependency is followed
up to high values of charging current density as presented in Figure 2.3 [18].
Thus, the subsurface concentration, C0, depends on the charging conditions
(applied current or potential), on temperature, pH, state of the surface (presence of poisons,
presence of oxides, other species than hydrogen adsorbed on the surface).
1,0E+00
1,0E+01
1,0E+02
1,0E+03
1,0E+00 1,0E+01 1,0E+02 1,0E+03 1,0E+04i1/2 (µA/cm²)
Ct (
ppm
wt)
1,0E-05
1,0E-04
1,0E-03
1,0E-02
C0
(ppm
wt)
Figure 2.3. Example of experimental hydrogen content – charging current density dependency. Tests were conducted on 22Cr duplex stainless steel in a chloride solution without H2S (1) and
saturated with H2S (2) [18].
(1)
(2)
2. HYDROGEN IN METALS
22
2.2.2. DIRECT TRANSFER OF H+ THROUGH THE INTERFACE (MODEL
PROPOSED BY CROLET ET AL.)
In the classical mechanism presented above, it is considered that the same
adsorbed atoms lead either to molecular hydrogen evolution or to atomic hydrogen absorbed in
the material.
Crolet [19 – 21] considers that a hydrated hydrogen cation looses its water
atmosphere and will proceed directly through the interface. Thus, the subsurface concentration
is given by the passage of H+ (in ionic form) through the interface.
In this new model for hydrogen absorption the species that are leading to
molecular hydrogen (atomic hydrogen adsorbed on the surface) are different from the ones that
are undergoing absorption.
The equilibrium (2.24.) is written as:
++ ↔ metalhydrated HH .)30.2(
The direct transfer of the proton H+ could take place not only from H+ from water,
but also by deprotonation of other complexes adsorbed on the surface: H2S becomes HS- ,and
similarly for H3As, H3P, HSCN, HF.
The severity of these species with regard to cracking increases with decreasing
stability of these complexes. Thus, the adsorbed HS-ads, is not an inhibitor for recombination
reaction (2.2.) or (2.3.) but a catalyst for the direct transfer of H+ through the interface (reaction
2.30.):
+−
−+
+→
→+
metaladsorbedadsorbed
adsorbedadsorbedhydrated
HHSSH
SHHSH
2
2
.)31.2(
2. HYDROGEN IN METALS
23
This mechanism gives a new explanation of the damaging effects of H2S and other
poisons: these species favour the direct transfer of H+ in the metal without decreasing the
recombination of atomic H.
This new direct transfer mechanism does not necessarily exclude the classical
mechanism, where atomic hydrogen is passing through the interface.
Apparently more studies are still conducted on these interesting questions.
2.3. HYDROGEN TRANSPORT WITHIN THE MATERIAL
In the following, the diffusion laws are presented for the ideal case of diffusion
without trapping. Then the different types of traps that can be encountered in a real material are
presented, with the expression for diffusion in the presence of traps. In the last subsection
hydrogen diffusion inside the material under other gradients than composition gradient is
presented.
2.3.1. DIFFUSION
2.3.1.1. Ideal diffusion, Fick’s laws
Due to its small volume, a hydrogen atom can diffuse and occupy the interstitial
sites inside the material (Figure 2.4.).
(a) (b) Figure 2.4. Octahedric interstitial sites of face centred cubic (a) and body
centred cubic (b) matrix [22]
2. HYDROGEN IN METALS
24
The face-centred cubic (f.c.c.) lattice has one octahedral interstitial site per metal
atom and two tetrahedral interstitial sites per metal atom in the unit cell.
The body-centred cubic (b.c.c.) lattice has three octahedral interstitial sites per
metal atom and six tetrahedral interstitial sites per metal atom in the unit cell. In the f.c.c. lattice
the octahedral positions (O) have the largest free volume, whereas in the b.c.c. lattice the
tetrahedral sites (T) are the largest. In Table 2.3. several metals with crystallographic structure
and preferred occupied sites are presented [22].
Table 2.3. Interstitial sites occupied by hydrogen in different metals [22]
Host lattice Crystallographic structure Occupied sites
α – Fe b.c.c. T
γ – Fe f.c.c. O
Pd f.c.c. O
Ta b.c.c. T
V b.c.c. T
Nb Rhomb. T
where T are tetrahedral sites and O octahedral sites .
The subsurface concentration, C0, determines a concentration gradient that is the
driving force for the diffusion.
The diffusion obeys the Fick’s laws:
Fick’s first law for diffusion: xCDJ∂∂
−= .)32.2(
and
Fick’s second law for diffusion: ²
²xCD
tC
∂∂
=∂∂
.)33.2(
where D is the diffusion coefficient for the ideal case , where diffusion takes place
without trapping.
2. HYDROGEN IN METALS
25
For a given material the diffusion coefficient is constant. Some values of the
diffusion coefficient for different materials are presented in Table 2.4.
Table 2.4. Diffusion coefficient of hydrogen in different materials at room temperature
Material D (cm²/s) Ref.
Carbon steel 2.5 x 10 – 6 [11]
Ferritic stainless steel 10 – 7 [23]
Austenitic stainless steel 2.15 x 10 – 12 [33]
Martensitic stainless steel 2 x 10 – 9 [24 – 28]
Duplex stainless steel 10 –9 – 10 – 10 (depending on
the ferrite / austenite ratio)
[23, 29 – 32 ]
2.3.1.2. Temperature effect
The diffusion coefficient has an exponential expression dependence with the
temperature:
−=kTEDD aexp0 .)34.2(
In Figure 2.5. the diffusion coefficient – temperature dependency for different steels
is presented [33].
1,00E-14
1,00E-10
1,00E-06
1,00E-02
0 100 200 300 400
temperature (°C)
D (m
²/s)
C steelduplexaustenitic
Figure 2.5. Evolution of diffusion coefficient (D) with the
temperature for different steels [33]
2. HYDROGEN IN METALS
26
The interstitial hydrogen is reversible, therefore at room temperature it can diffuse
out from the metal.
The diffusion coefficients (apparent and real) and the subsurface concentration, C0,
can be easily measured and calculated from permeation experiments (See Section 6.).
2.3.1.3. Diffusion under stress gradient
When a stress is applied, hydrogen diffuses under stress gradient toward the
places of high stress. The diffusion flux depends not only on the concentration gradient, but also
on the stress gradient according to equation:
−−=
−
hgradRTVcgradcDJ σ .)35.2(
Stress – induced hydrogen diffusion takes place whether the inhomogeneous
stress is caused by applied forces or residual stresses.
Due tot the stress gradient, the diffusion of hydrogen can take place even when
hydrogen distribution is uniform inside the material (grad c = 0).
2.3.2. TRAPPING
In real cases, the hydrogen atoms are not located only in the interstitial positions,
but they are trapped by the different defects inside the material.
Any metallurgical defect inside the material can act as a trap for hydrogen.
According to their energy, traps are divided into reversible, for which the energy is low and
hydrogen can leave easily the trap, and irreversible (or deep traps) where more energy has to
be provided for hydrogen release.
Examples of traps are presented in Table 2.5.
2. HYDROGEN IN METALS
27
The presence of traps in the material will hinder the hydrogen diffusion. Therefore,
the diffusion will be apparently slower than for an ideal crystal.
Table 2.5. Types of traps existing in ferrous materials
Traps Binding energy
(kJ / mol)
Degassing temperature
(°C) Material Ref.
Matrix 6.9 Room
temperature Fe [34]
Grain boundaries 17.15 112 Fe [35]
215 Fe [35]
200 Fe [36]
Dislocations 20 – 26
272
AISI 4340
(carbon steel
0.39%C)
[37]
338 AISI 4340 [37]
305 Fe [35] Microvoids 35 – 48
480 Carbon steel
(0.47%C) [38]
MnS inclusions 72 495 AISI 4340 [37]
Carbides
interfaces 96.6 723 Fe [36]
The diffusion laws have to take into account the presence of reversible and
irreversible traps.
The energy of reversible traps is low and comparable to the energy of interstitial
sites.
According to Oriani’s theory [39], the amount of hydrogen trapped into the
reversible traps is always in equilibrium with the lattice hydrogen.
2. HYDROGEN IN METALS
28
−=
− RTWB
L
L
r
r exp11 θθ
θθ
.)36.2(
The diffusion law is expressed by the equations:
tN
tN
xCD
tC i
ir
r ∂∂
−∂∂
−∂∂
=∂∂ θθ
²²
.)37.2(
where :
rrrr pCkt
θθθ −−=∂∂ )1( .)38.2(
)1( irii Cktθθ −=
∂∂
.)39.2(
The Fick’s law can be written as:
²²xCD
tC
eff ∂∂
=∂∂
.)40.2(
where Deff is the effective diffusion coefficient including the effect of traps.
2.3.3. TRANSPORT OF HYDROGEN BY MOVING DISLOCATIONS
The plasticity model proposed for HE suggests that hydrogen enhances
dislocations mobility (See Section 4.2. Plasticity model). In the same time, moving dislocations
could transport hydrogen during their movement.
Therefore, the transport of hydrogen by dislocation is an important aspect in
understanding the hydrogen effects on the mechanical properties of the material.
2. HYDROGEN IN METALS
29
Under plastic deformation the number of dislocations is increased and, as
dislocations offer more space for hydrogen, there is more hydrogen in the metal. Also, as
plastic deformation imposes a movement of dislocations, the transport of hydrogen is facilitated
[40].
There are indeed experiments that show an increased solubility and a decreased
apparent diffusivity of hydrogen for samples that have been cold worked prior to permeation
experiment. The latter is due to the trapping effect of dislocations.
Considerable controversy has arisen with respect to the exact role that dislocation
transport plays in the embrittlement process.
Experiments conducted on Ni [41] and Ni – Cr alloys [42] showed that the
diffusivity increases very much under plastic deformation during hydrogen charging. The
diffusivity appears to increase by approximately 5 orders of magnitude, from about 10-10cm²/sec
to 10-5 cm²/sec.
Bastien and Azou suggested that moving dislocations could carry hydrogen [43]
and that a local high hydrogen concentration can develop when dislocations annihilate or
intersect a void.
Franck [44] observed that deformation enhances hydrogen outgassing of mild
steel.
Two types of transport behaviour are generally discussed:
a. All the hydrogen is introduced into the material prior to plastic deformation.
Initially, the hydrogen is uniformly distributed and the total hydrogen content remains constant.
When the system is mechanically loaded, new dislocations are formed. A
redistribution of the hydrogen from the lattice and old traps towards the newly formed
dislocations occurs.
At the same time, the dislocation motion starts. According to their velocity, the
moving dislocations transport or loose the trapped hydrogen. Authors generally consider that if
the velocity is sufficiently high, all the hydrogen will be left behind as dispersed through the
lattice and perhaps partially absorbed by static traps.
For steels, this dumping process may double the lattice hydrogen concentration if
the deformation rate is very high.
2. HYDROGEN IN METALS
30
Dislocations will act as hydrogen source inside the material.
For velocities near or less than a critical value (case of slow strain rate tests) the
hydrogen is transported by moving dislocations.
If the dislocation slows down, e.g. after intersection with an obstacle, its hydrogen
concentration may increase again to a level higher than that of fast moving dislocations.
Hence, dislocations which are stopped or slowed down are sinks for hydrogen.
b. The second case is the case where hydrogen charging and plastic deformation
occur simultaneously. The dislocations moving from the surface can be assumed to transport
hydrogen at a concentration equal to that of the external charging medium. In this case
dislocations will be sources of hydrogen inside the material because:
– fast moving dislocations loose their hydrogen, as in a.
– slow moving dislocations may loose hydrogen when their initial concentration is
higher than inside the material
The critical velocity of dislocation to transport or loose hydrogen was calculated as
[45]:
−
−=
RTF
RTQ
RTblDv kkokcr
*2expexpσ .)41.2(
For iron all these parameters are known [45] : l = 1 µm, b = 0.248 nm, ν = 1013 s–1 ,
G = 86 GPa (shear modulus), Qk = 3.4 kJ / mol and 2Fk* = 28.4 kJ / mol, and the critical velocity
equals:
vcr = 8.33 x 103 (σ / G), in m/s (2.42.)
For material testing, the most severe conditions will be those where hydrogen is
transported more easily by dislocations, thus at a strain rate below the critical value given by
equation (2.42.).
2. HYDROGEN IN METALS
31
2.4. SUMMARY OF HYDROGEN IN THE METAL
The hydrogen entry and transport through the material is influenced by the
charging conditions (through C0), the material structure, the level of stress and the strain.
The charging conditions (potential or current density, hydrogen pressure,
temperature, solution pH) lead to a given subsurface concentration, C0.
The subsurface concentration, C0, was for a long time considered as the main
factor for the susceptibility to hydrogen embrittlement (See Section 3. and Section 4.)
The subsurface concentration, C0, is the driving force for diffusion of hydrogen
inside the material.
It is pointed out that there is a limit value for C0 corresponding to saturation in given
charging conditions. This limit value is very much increased in the presence of promoters for
hydrogen entry.
The total hydrogen content is given by the reticular hydrogen (hydrogen located in
interstitial positions of the matrix) and by the hydrogen trapped in metallurgical defects
(hydrogen reversibly or irreversibly trapped).
Thus the total hydrogen content depends not only on the charging conditions but
also on the history of the material: for instance, a previous plastic deformation increases the
density of dislocations, thus there are more available hydrogen trapping sites in the material.
The transport by diffusion takes place under concentration gradient established by
C0 and also by stress gradient, due to externally applied forces or residual stresses. As a
consequence, the total content of hydrogen inside the material is increased when C0 increases,
but also when a stress is applied to the sample.
Under dynamic plastic deformation, dislocations can transport hydrogen during
their movement. For certain materials, like Ni [41, 42], this type of transport is more rapid than
by simple diffusion.
2. HYDROGEN IN METALS
32
3. TYPES OF DAMAGES DUE TO
HYDROGEN
3. TYPES OF DAMAGES DUE TO HYDROGEN
34
3. TYPES OF DAMAGES DUE TO HYDROGEN
35
In this chapter a summary of the most important damages caused by the presence
of hydrogen in the material is presented.
The purpose is to identify where the problem studied in this work is situated among
the series of hydrogen damages.
These damages are generally classified according to various factors:
- the form of hydrogen that produces the damage: atomic hydrogen, gaseous
hydrogen, other gases (CH4, H2O), metal hydrides ;
- the source of hydrogen: electrochemical hydrogen (cathodic protection,
electroplating, corrosion, pickling), gaseous hydrogen atmosphere, H2S and other poisons;
- presence or absence of applied stress.
There are inevitable interferences between these three classification modes.
It is possible that a better understanding of the mechanisms of hydrogen damages
might in the future suggest a more logical classification.
The problem studied in this work is related to damages due to the presence of hydrogen in atomic form, under applied stresses.
3. TYPES OF DAMAGES DUE TO HYDROGEN
36
3.1. HYDROGEN INDUCED CRACKING (HIC) AND STEPWISE
CRACKING (SWC)
Atomic hydrogen H diffuses inside the material and recombines as molecular
hydrogen, H2, at specific sites. This H2 can develop high pressure at these sites.
In more or less ductile materials (yield strength below about 540 MPa [46]), these
high pressures deform the material and produce blisters of gaseous molecular hydrogen H2.
HIC blisters are typical of low strength steels in environments containing H2S.
For less ductile material cracking can occur once the pressure exceeds a critical
value.
Atomic hydrogen is usually produced by a corrosion reaction in H2S containing
environments.
This type of failure is typical for medium or high strength carbon steel pipe
transporting H2S containing products.
Figure 3.1. Hydrogen induced cracking (HIC) of carbon steel in H2S environment [47]: blisters are associated
to MnS inclusions
3. TYPES OF DAMAGES DUE TO HYDROGEN
37
The recombination of H into H2 generally occurs on elongated MnS inclusions [47]
(Figure 3.1.). Counter measures are reducing the S content in steel to very low levels (0.001 %)
or adding calcium (Ca) or rare earth elements (Cerium for example) to build spherical
inclusions.
This type of damage occurs in the absence of applied stress. The stress is
produced by the internal hydrogen pressure.
HIC may propagate in a stepwise manner (stepwise cracking SWC), which is
shown in Figure 3.2.
3.2. STRESS ORIENTED HYDROGEN INDUCED CRACKING
(SOHIC)
SOHIC is a combination of HIC and sulphide stress cracking SSC or hydrogen
embrittlement (see below). It involves blisters formed by H2, as in HIC, but it occurs in the
Figure 3.2. Typical aspect for cracking by stepwise cracking (SWC) [46]
3. TYPES OF DAMAGES DUE TO HYDROGEN
38
presence of an applied or residual stress. The joint presence of atomic H and stress produces
thin cracks than can interconnect HIC cracks (see arrow on Figure 3.3.).
.
These cracks develop perpendicular to the applied stress direction [47]. Figure 3.3.
presents a typical aspect of cracking by stress oriented hydrogen induced cracking (SOHIC).
3.3. HYDROGEN REACTION WITH THE METAL MATRIX (HYDRIDE FORMATION)
Hydrogen can form brittle hydrides with a number of metals: Ti, Zr, V, Nb, Ta, Mg,
U, Th and their alloys.
Failures of Ti tubes were observed in condensers near tube plates that were
cathodically protected.
Hydride formation occurs above a critical hydrogen concentration. Pre-existing
cracks may be the initiation site, since H tends to diffuse towards the region of high stress at the
Figure 3.3. Stress Oriented Hydrogen Induced Cracking (SOHIC) [47]
stress direction stress direction
3. TYPES OF DAMAGES DUE TO HYDROGEN
39
crack tip. The hydride phase has a higher volume than the parent metal and this creates local
elastic or plastic deformation.
This type of failure does not occur on ferrous based materials.
3.4. HYDROGEN REACTIONS WITH NON METALLIC PHASES Hydrogen can react with iron carbides in the steel to form methane CH44. The
reaction occurs at temperature of 200 to 300°C.
These decarburising damages affect the material in two ways: by reduction of
carbon content (and a reduction of the strength of the material) and by high internal pressures
produced by methane that may lead to cracking.
Also, hydrogen can react at high temperature with certain non-metallic inclusions. One example is the reaction of hydrogen with copper oxide inclusions during annealing of copper in hydrogen atmosphere.
The reaction is
)(222 2 gOHCuHOCu +→+
with a weakening of the copper matrix.
3.5. HYDROGEN EMBRITTLEMENT (HE) (OR HYDROGEN
STRESS CRACKING HSC)
This type of failure occurs in the presence of atomic hydrogen and under residual or applied stress.
This phenomenon is of concern for high strength steels (yield stress YS > 600 N /
mm²). In the presence of hydrogen, their mechanical resistance can decrease considerably,
below the yield strength.
For many steels, there is a threshold stress below which HE does not occur.
However, this threshold stress is a function of the strength of the material and of the
3. TYPES OF DAMAGES DUE TO HYDROGEN
40
environment. Generally, the higher the yield or tensile strength, the lower the threshold stress.
HE is definitely linked to absorption of H, and there is often an incubation time for charging and
transport of H, resulting in delayed fracture.
Hydrogen embrittlement (or hydrogen stress cracking, as stress is a prerequisite)
generally produces clear single cracks (intergranular or transgranular), as opposed to often
branching cracks for stress corrosion cracking SCC.
An interesting manner to differentiate HE (or HSC) and SCC was presented by
Brown [48] who showed a decreasing time to failure when the electrochemical potential is either
increased or decreased: shorter time to failures at higher potentials are attributed to SCC, with
anodic dissolution, while early cracking at lower potentials are attributed to hydrogen effects,
possibly in the absence of any corrosion.
The sources of atomic hydrogen can be cathodic protection, electroplating, pickling
or just corrosion.
This work is focused on this type of damage; the source of hydrogen is cathodic protection, there is no corrosion and stress and strain are present.
3.6. SULPHIDE STRESS CRACKING SSC
Sulphide stress cracking, SSC, is a special case of HE or HSC where sulphide
compounds (or other poisons) increase the entry of atomic hydrogen in the metal lattice. The
name was given in relation with this type of environment.
Sulphide stress cracking may be particularly rapid and catastrophic.
Hard microstructures are more sensitive to sulphide stress cracking. Improper heat
treatments or heat affected zone of low heat input welds are frequent causes of sulphide stress
cracking.
The occurrence of this type of damage in sour environment is often prevented by
limiting the hardness of the material.
The problem dealt with in this work, does not consider H2S or other
“poisons”.
4. HYDROGEN EMBRITTLEMENT
4. HYDROGEN EMBRITTLEMENT
42
4. HYDROGEN EMBRITTLEMENT
43
From a fundamental point of view, HE is not completely understood, despite the
large amount of studies conducted on this topic.
Several models were proposed for hydrogen embrittlement and a brief description
of them is presented in the following.
Adsorption model One of the first mechanisms proposed for HE is the one proposed by Petch [49].
This model considers that hydrogen adsorbed on the surface decreases the surface energy.
The reduction of surface energy is proportional to the concentration of adsorbed hydrogen.
When hydrogen is adsorbed on the internal surfaces of cracks or voids the surface energy
decreases, reaching values below a critical stress and thus leading to fracture.
This model does not explain why other gases, like O2 or N2, with higher adsorption
energies, have not the same embritteling effects.
Decohesion model [50] (see Section 4.1.)
According to this model, hydrogen inside the material decreases the cohesion
forces that exist between atoms.
This model is applicable to brittle fracture (cleavage or intergranular) but it cannot
explain the fractures accompanied by plasticity.
This model also considers that there is a critical hydrogen concentration for the
occurrence of brittle fracture.
Plasticity models
Regarding the effect of hydrogen on the plasticity of the materials, two contradictory theories are developed:
Stroh [51] considers that hydrogen blocks dislocations and thus increases the flow
stress.
This theory is contradicted by the observations of Beachem [52] who proposes that
hydrogen facilitates the dislocations movement, favouring the plasticity of the material.
4. HYDROGEN EMBRITTLEMENT
44
These latter observations are the basis for the HELP model (Hydrogen Enhanced Localised Plasticity) that will be detailed in Section 4.2.
Another mechanism that considers the effects of hydrogen on the plasticity of
material is proposed by Lynch [53 – 55]. According to this mechanism, hydrogen adsorbed on
crack tip facilitates the dislocations injection and crack advancement. This mechanism is similar
to the mechanism for embrittlement by liquid metals and is taking into account only the effects
of hydrogen on the surface of the material.
Among all these models, the most elaborated and well established models are the
decohesion mechanism and the plasticity model HELP.
A detailed analysis of these two models is presented in the following sections.
4.1. DECOHESION MECHANISM
The decohesion mechanism is one of the earliest mechanisms proposed for HE. It
was initiated by Troiano [50], and improved by Oriani [56 – 58].
This mechanism is based on the postulate that solute hydrogen decreases the forces required to separate the crystal along a crystallographic plane, i.e. the cohesive force and correspondingly the energy to form cleavage surface (Figure 4.1.).
Decohesion is supported by the fact that HE seems to occur in the absence of
significant local deformation, by thermodynamic arguments and by theoretical calculations of
electronic distribution of systems in the presence of hydrogen.
4.1.1. THERMODYNAMIC ASPECTS OF INTERFACIAL DECOHESION [59] The interfacial layer was modelled in order to obtain a relationship between the
hydrogen content and the cohesive strength and the work of decohesion.
The thermodynamic of decohering interface was well established [59 – 62] with the
emphasis of two limiting cases: infinitely fast separation and infinitely slow separation.
4. HYDROGEN EMBRITTLEMENT
45
Figure 4.1. Hydrogen effect on the cohesive energy (U) and on the cohesive
stress (σ) of a material. U°cohesion is the cohesive energy (the energy
required to separate the two half solids along the cleavage plane to a separation larger than the critical distance (r) in the absence of hydrogen; UHcohesion is the cohesive energy in the presence of
hydrogen in solid solution, σ°cohesion is the cohesive stress (the
stress to disrupt the atomic bonds) in the absence of hydrogen;
σHcohesion is the cohesive stress in the presence of hydrogen in solid
solution; a is the lattice parameter; εH is the strain induced by
hydrogen in solid solution [50, 56 – 58].
Ucohesion , σcohesion
U°cohesion
UHcohesion
σ°cohesion
σHcohesion r
HH
H HH
HH
HHH H
a = a0 + εH a0
a = a0 + εH a0
rH
(a) (b)
4. HYDROGEN EMBRITTLEMENT
46
For slow separation, the diffusion of impurity towards the interface is much faster than the separation; the chemical potential of impurity remains constant while its interfacial
concentration varies.
In the case of fast separation, where the diffusion is slow compared to the separation time, the interface remains isolated from the impurity source, the concentration in the
interface remains constant, and the chemical potential changes during the separation process.
Recently, the intermediate situation, where the two processes (separation and
diffusion) are comparable to each other, was modelled [57, 62]. This situation is closely related
to the diffusion – controlled brittle fracture taking place in many materials.
The three regimes can be represented in concentration – separation distance
coordinates, (c, δ), as in Figure 4.2. There is a critical state for which the separation reaches the
critical value, δ = δc. On the right of the critical separation line the fracture occurs, whereas on
the left side the interface is subjected to stress but the fracture does not occur yet.
For fast separation, the H concentration remains constant during the evolution of
system up to fracture and this regime is represented by a horizontal line.
For slow separation, the evolution of system is represented by a curve µ(c, δ) =µ0.
The intermediate regime lies between these two curves.
The cohesive strength and work of decohesion, that are concentration dependent,
where calculated.
The mathematical development of the model is presented in Appendix 2.
The cohesion of the interface is described by a function that depends on the
concentration of hydrogen (c) and the separation δ between the layers that form the interface.
This function is called the cohesive function, ϕ (c, δ). The cohesive function depends linearly on
hydrogen concentration and by a more complex function (cubic polynomials) on the separation
δ. For the critical separation δc, the cohesive function becomes zero.
The interfacial stress depends on c and δ through ϕ.
The calculations conducted by this model (see Appendix 2) show that the
cohesive stress of the interface decreases with an increase of the hydrogen concentration (Figure 4.3.)
4. HYDROGEN EMBRITTLEMENT
47
critical separation line
slow
fast
Figure 4.2. Schematic trajectories of interfacial separation in coordinates
hydrogen concentration c versus separation distance δ. The
initial state is characterised by c0 and δ0. The interface fails
when the trajectory crosses the critical separation (δc) line
[59]
Normalised separation, δ/δc
Nor
mal
ised
coh
esiv
e st
ress
σ∗
Figure 4.3. Normalised cohesive stress for different values of hydrogen concentration [59]
4. HYDROGEN EMBRITTLEMENT
48
4.1.2. ELECTRONIC DISTRIBUTION IN H – METAL SYSTEMS
The decohesion mechanism is supported by calculation of the electronic
distribution of the metal – hydrogen systems.
There is an increasing amount of studies on to the hydrogen effects on metallic
bonds [62 – 71].
The atom superposition and electron delocalisation molecular orbital method
(ASED – MO) (see Appendix 3.) is a semi – empirical method that can predict the molecular
structure from atomic data (atomic wave functions and ionisation potentials).
The calculations conducted using this method show that hydrogen inside the
transition metals determines an electronic delocalisation of the surrounding metals atoms.
The bond between hydrogen atom and the metallic atoms is formed at the expense
of metal – metal bond of neighbouring atoms.
The calculations conducted for H – Fe system show that hydrogen diminishes the
strength of Fe – Fe bond for the first neighbour atoms by more than 40% of the initial value.
4.1.3. EXPERIMENTAL OBSERVATIONS
Intergranular fracture consistent with decohesion has been observed in some particular systems where other embritteling species are segregated at the boundaries: Ni – S
system with low levels of S [72] and the systems Ni3Al containing B, where solute H did appear
to decrease the grain boundary cohesion [73].
The decohesion mechanism seems to be operative in the case of β – Ti – H
system [62], where the strain to failure and the nature of the fracture surfaces depend on the
hydrogen content (Figure 4.4.). The strain to failure depends on the hydrogen concentration and
it has a sharp transition in ductility for a hydrogen concentration (expressed as atomic ratio) H /
M = 0.28. For H / M < 0.21 the fracture surfaces are characterised by ductile microvoid
coalescence with decreasing microvoid sizes as the H concentration increases. At H / M > 0.27
the fracture surfaces is cleavage in nature.
For systems with low solubility of hydrogen, such as steels, the hydrogen
distribution at the crack tip is dominated by the trapped hydrogen and the concentration at the
crack tip exceeds that of the bulk by a factor of 102. Since hydrogen embrittlement occurs in
4. HYDROGEN EMBRITTLEMENT
49
steels at an average concentration of about 10 atomic ppm, the enhanced concentration is of
the order of 103 atomic ppm. This is a low concentration to account for low macroscopic strain
fracture on the basis of decohesion.
4.1.4. CONCLUSIONS FOR DECOHESION MECHANISM
The decohesion mechanism considers that there is a critical concentration of
hydrogen atoms for which brittle fracture occurs.
This mechanism could be applied for intergranular fracture, where high
concentration of hydrogen accumulates at grain boundaries (and thus reaching the critical
concentration for brittle fracture)
The plasticity associated with the fracture is not compatible with the decohesion
mechanism.
Figure 4.4. Strain to failure dependency on the hydrogen concentration
of β – Ti alloys. A sharp transition on ductility is observed
for hydrogen concentration of about 0.28 [62]
4. HYDROGEN EMBRITTLEMENT
50
There is little definitive evidence of the hydrogen decohesion in systems with low
solubility of hydrogen, such as steels.
The available evidence suggests that solute hydrogen does not weaken atomic
bond. The elastic constant measurements [74 – 76] and phonon dispersion curves [77] show a
stiffening of the lattice bonds, rather than a softening.
4.2. PLASTICITY MODEL: HYDROGEN ENHANCED LOCALISED PLASTICITY – HELP
The basis of this model was established by Beachem [52], who was the first to
propose that in the case of hydrogen embrittlement the failure occurs by locally ductile
processes.
The HELP (Hydrogen Enhanced Localised Plasticity) mechanism is based on consistent observations that the presence of hydrogen in solid solution increases the mobility of
dislocations (Figure 4.5.) and creates localised high deformation regions [78 – 88].
The reason of this increased mobility is attributed to reduction of interactions
between dislocations and between dislocations and other obstacles (such as C atoms, grain
boundaries) when hydrogen is present in system.
Dislocations thus move closer to each other, and closer to obstacles, and produce
denser or more compact pile-ups when H is present.
The result of this is that microscopic regions of high deformation (where H
increases the mobility of dislocations) are surrounding less ductile zones where dislocations are
closely packed. The applied stress is then concentrated on these hard zones that represent only
a small portion of the cross section. When the tensile stress in these small portions is higher
than the ultimate tensile strength, failure occurs.
Even if, at very localised (microscopic) level, plasticity is enhanced by hydrogen, at
macroscopic level the material exhibits a brittle behaviour (reduced strain to failure, lower
fracture strength) [78].
4. HYDROGEN EMBRITTLEMENT
51
The assumption for the HELP mechanism is that hydrogen creates an atmosphere
around dislocations that shields the elastic interactions between dislocations, and between
dislocations and other obstacles.
This model is well established with respect to the influence of hydrogen on the
dislocations behaviour.
This model is supported by calculations of elastic shielding due to hydrogen
atmosphere (see 4.2.1) and by in situ transmission electron microscopy (T.E.M.) observations
of the influence of hydrogen on the dislocation behaviour (see 4.2.2, ).
4.2.1. HYDROGEN SHIELDING EFFECT
The hydrogen shielding effect was modelled [89 – 95]. Analytical and finite element
Figure 4.5. Hydrogen effect on dislocations velocity: dislocations velocity increases when hydrogen pressure increases. In the figure the ratio dislocation velocity in hydrogen atmosphere to velocity in vacuum is represented. Curve 1 shows the effect of introducing hydrogen for the first time, and curve 2 the effect after hydrogen was removed and reintroduced. Tests conducted on alfa -Titanium
4. HYDROGEN EMBRITTLEMENT
52
calculations were conducted to estimate the effects of the presence of hydrogen on the
interactions between two edge dislocations and between a dislocation and an impurity atom
(like interstitial C atoms).
When hydrogen diffuses into the lattice, despite its small volume, it introduces an
elastic strain in the matrix.
In this model, first the distribution of hydrogen in equilibrium with an applied stress
is calculated.
The stress varies with the position inside the material, thus, the hydrogen
distribution evolves similarly.
Then the stress exerted by the hydrogen atmosphere on a dislocation is calculated.
The total shear stress exerted on a dislocation is the sum of the shear stress due
to the hydrogen stress field and the shear stress due to the other dislocations.
4.2.1.1. Hydrogen effect on the interactions between dislocations The hydrogen shielding effect was modelled taking into account the strain induced
by the presence of hydrogen inside the matrix, the hydrogen segregation around dislocations
and the interactions between parallel dislocations with the same sign and Burgers vectors.
(a) Analytical calculation
The entire mathematical development is presented in Appendix 4.
The shear stress exerted by the H atmosphere is calculated and is determined as a
function of hydrogen concentration, CH, and of material characteristic through µ (bulk modulus):
φφφνπ
τπ
drdr
rCNVµ R
rH
A
HH
2sin),()1(2
2
0 2∫ ∫−−= .)1.4(
The interaction between two parallel dislocations of the same sign , in the absence
of hydrogen, is calculated and is established as being function of the material (through the bulk
modulus µ and Poison’s coefficients v), of the Burgers vector b and the separation distance l ;
4. HYDROGEN EMBRITTLEMENT
53
lµb
Dωω
νπτ 2coscos
)1(21
−−= .)2.4(
The total stress exerted on dislocation is the sum τH + τD.
(b) Numerical integration results
Numerical integration was calculated for the niobium system [96].
(For iron and steels the available data are still dispersed.)
According to this model, the hydrogen atmosphere in equilibrium with a stress field
of a single dislocation is symmetric with respect to the dislocation plane (Figure 4.6.).
When two dislocations approach one another, the symmetry of hydrogen
atmosphere changes, due to the superposition of the stress fields of the two dislocations.
For dislocations of the same sign (Figure 4.7.), the hydrostatic stress field is
reinforced positively below the slip plane and negatively above the slip plane. This
reinforcement increases as the dislocations approach each other. Consequently, the hydrogen
concentration increases in the regions of positive stress enhancement and its value becomes
larger than the concentration of the corresponding region in the atmosphere of a single
dislocation.
For dislocations of opposite sign (Figure 4.8.), that attract each other, the positive
hydrostatic stress field of each dislocation is weakened and the hydrogen concentration is lower
than that of a single dislocation.
The shear stress is diminished in the presence of hydrogen and this reduction
depends on the separation distance between the dislocations. The effect of hydrogen shielding
is higher when the distance between the dislocations is smaller. For high dislocations
separation (> 10 Burgers vectors) the magnitude of the effect is almost independent of the
distance between dislocations.
4. HYDROGEN EMBRITTLEMENT
54
Figure 4.6. Symmetrical contours of normalised hydrogen concentration C/C0 around a single edge dislocation at a normal hydrogen concentration C0 = 0.1 and temperature of 300K [96]
Figure 4.7. Contours of normalised hydrogen concentration C/C0 around two parallel edge dislocations of equal Burgers vectors b, on the same slip plane, at a normal hydrogen concentration C0 = 0.1 and temperature of 300K [96]
Figure 4.8. Contours of normalised hydrogen concentration C/C0 around two parallel edge dislocations of opposite and equal Burgers vectors b, on the same slip plane, at a normal hydrogen concentration C0 = 0.1 and temperature of 300K [96]
4. HYDROGEN EMBRITTLEMENT
55
A direct consequence of the shielding effect of hydrogen on the dislocation behaviour is that in the presence of hydrogen the spacing between dislocations in a pile – up decreases. This effect is higher for the dislocations at the tip of the pile – up, where the separation distance between dislocations is smaller.
The result of this is that microscopic regions of high deformation (where H
increases the mobility of dislocations) are surrounded by hard zones, where more compact pile-
ups are formed. The stress distribution is not uniform through the whole section of the
specimen and spots of stress concentration occur.
Maybe, for high hydrogen concentration, dislocations of same sign can join causing
fracture by coalescence.
4.2.1.2. Interaction between dislocations and an impurity atom in the
presence of hydrogen
A model similar to the one presented above was used to calculate the interactions
between dislocations and a defect and the influence of hydrogen on these interactions [89].
Interstitial atoms (like carbon) are barriers