Related Experiment Video
Updated: Jan 25, 2026

07:50
Hydrogen Charging of Aluminum using Friction in Water
Published on: January 28, 2020
6.5K
Hydrogen embrittlement in metallic nanowires
Sheng Yin1, Guangming Cheng2, Tzu-Hsuan Chang2
1School of Engineering, Brown University, Providence, Rhode Island, 02912, USA.
Nature Communications
|May 3, 2019
Summary
Hydrogen embrittlement in metallic nanowires (NWs) is poorly understood. Surface hydrogen enhances yield strength by suppressing dislocation nucleation, altering failure mechanisms in silver NWs.
Area of Science:
- Materials Science
- Nanotechnology
- Mechanical Engineering
Background:
- Hydrogen embrittlement is a known phenomenon in bulk metals, but its mechanisms in nanostructures remain unclear.
- Deformation and failure in nanostructures are often governed by dislocation nucleation processes.
Purpose of the Study:
- To investigate the fundamental mechanisms of hydrogen embrittlement in metallic nanostructures.
- To utilize metallic nanowires (NWs) as a model system for studying hydrogen effects at the nanoscale.
Main Methods:
- Quantitative in-situ transmission electron microscopy (TEM) nanomechanical testing.
- Molecular dynamics (MD) simulations.
- In-situ stress relaxation experiments.
Main Results:
- Penta-twinned silver (Ag) nanowires (NWs) exhibited enhanced yield strength in the presence of surface-adsorbed hydrogen.
- A transition in failure mechanism from distributed plasticity to localized necking was observed.
- Hydrogen-induced suppression of dislocation nucleation at the NW free surface was identified as the governing mechanism.
Conclusions:
- Surface-adsorbed hydrogen significantly influences the mechanical behavior and failure modes of metallic nanowires.
- Dislocation nucleation suppression is a key factor in hydrogen embrittlement at the nanoscale.
- Metallic NWs provide a valuable platform for understanding fundamental hydrogen-metal interactions.
Related Concept Videos
Hydrogen Bonds
131.9K
Hydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, and has a partial negative charge. The other is a hydrogen atom that has bonded with another electronegative atom and has a partial positive charge.
Hydrogen Bonds Control the World!
Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are unequally shared....
Hydrogen Bonds Control the World!
Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are unequally shared....
131.9K
Hydrogen Bonds
13.6K
A hydrogen bond is formed when a weakly positive hydrogen atom already bonded to one electronegative atom (for example, the oxygen in the water molecule) is attracted to another electronegative atom from another polar molecule, such as water (H2O), hydrogen fluoride (HF), or ammonia (NH3). The huge electronegativity difference between the H atom (2.1) and the atom to which it is bonded (4.0 for an F atom, 3.5 for an O atom, or 3.0 for an N atom), combined with the very small size of an H atom...
13.6K
Alkali Metals
24.3K
Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the alkali metals are unusually low for metals and decrease going down the group, while the density increases going down the group with the exception of potassium (Table 1).
Table 1: Properties of the alkali metals
Table 1: Properties of the alkali metals
24.3K
Bonding in Metals
52.2K
Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Drüde called the “Electron Sea Model”.
52.2K
Metallic Solids
20.5K
Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
20.5K
Metal-Ligand Bonds
24.1K
The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
24.1K

