Related Experiment Video
Updated: Apr 24, 2026
09:38
Fabrication Procedures and Birefringence Measurements for Designing Magnetically Responsive Lanthanide Ion Chelating Phospholipid Assemblies
Published on: January 3, 2018
6.9K
Phase equilibria in the neodymium-cadmium binary system.
Barbara Skołyszewska-Kühberger1, Thomas L Reichmann1, Herbert Ipser1
1Department of Inorganic Chemistry (Materials Chemistry), University of Vienna, A-1090 Wien, Austria.
Journal of Alloys and Compounds
|September 9, 2014
Summary
This study establishes the neodymium-cadmium phase diagram, identifying key intermetallic compounds and reactions. Findings detail the system's thermal behavior and solid solubility for neodymium-cadmium alloys.
Area of Science:
- Materials Science
- Metallurgy
- Physical Chemistry
Background:
- Understanding binary alloy phase diagrams is crucial for materials development.
- The neodymium-cadmium system's phase equilibria were previously not fully characterized.
Purpose of the Study:
- To establish the equilibrium phase diagram of the neodymium-cadmium system.
- To identify and characterize intermetallic compounds and phase transition reactions.
Main Methods:
- Thermal analysis
- Metallographic analysis
- X-ray analysis
- Dilatometric analysis
Main Results:
- Established the neodymium-cadmium phase diagram based on 70 alloys.
- Identified seven intermetallic compounds (three congruent, four incongruent melting).
- Determined four eutectic and one eutectoid reaction points.
- Found negligible solid solubility of neodymium in cadmium.
Conclusions:
- The study provides a comprehensive phase diagram for the neodymium-cadmium system.
- Detailed characterization of intermetallic compounds and reactions offers valuable data for alloy design.
- Phase transition data aids in understanding solid solutions in neodymium-cadmium alloys.
Related Concept Videos
01:07Ladder Diagrams: Complexation Equilibria
735
Ladder diagrams are useful for evaluating equilibria involving metal-ligand complexes. The vertical scale of the ladder diagram represents the concentration of unreacted or free ligand, pL. The horizontal lines on the scale depict the log of stepwise formation constants for metal-ligand complexes and indicate the dominant species in all the regions.
The formation constant, K1, for the formation of Cd(NH3)2+ complex from cadmium and ammonia is 3.55 × 102. Log K1 (i.e. pNH3) is 2.55, and...
The formation constant, K1, for the formation of Cd(NH3)2+ complex from cadmium and ammonia is 3.55 × 102. Log K1 (i.e. pNH3) is 2.55, and...
735
01:21Chemical Equilibria: Systematic Approach to Equilibrium Calculations
1.8K
Equilibrium calculations for systems involving multiple equilibria are often complex. For example, to calculate the solubility of a sparingly soluble salt in an aqueous solution in the presence of a common ion, one must consider all the equilibria in this solution. Calculations for these systems can be complicated and tedious, so a systematic approach with a series of steps is often helpful. The process is detailed below.
The first step is to identify all the chemical reactions involved, The...
The first step is to identify all the chemical reactions involved, The...
1.8K
02:59The Nernst Equation
33.2K
Nonstandard Reaction Conditions
The interconnection between standard cell potentials and various thermodynamic parameters such as the standard free energy change ΔG° and equilibrium constant K has been previously explored. For example, a redox reaction involving zinc(II) and tin(II) ions at 1 M concentration with Eºcell = +0.291 V and ΔG° = −56.2 kJ is spontaneous.
The interconnection between standard cell potentials and various thermodynamic parameters such as the standard free energy change ΔG° and equilibrium constant K has been previously explored. For example, a redox reaction involving zinc(II) and tin(II) ions at 1 M concentration with Eºcell = +0.291 V and ΔG° = −56.2 kJ is spontaneous.
33.2K
01:24Electrochemical Systems
169
Electrochemical systems provide a fascinating insight into the dynamic interplay of charged species within various phases. One notable example is the interaction between a membrane permeable to K⁺ ions but not to Cl⁻ ions, separating an aqueous KCl solution from pure water. As K⁺ ions diffuse through the membrane, they generate net charges on each phase, leading to a potential difference between them.Similarly, when a piece of Zn is immersed in an aqueous ZnSO₄ solution,...
169
01:30Ladder Diagrams: Redox Equilibria
917
Ladder diagrams are useful tools for understanding redox equilibrium reactions, especially the effects of concentration changes on the electrochemical potential of the reaction. The vertical axis in the redox ladder diagrams represents the electrochemical potential, E. The area of predominance is demarcated using the Nernst equation.
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...
917
02:20Dynamic Equilibrium
63.1K
A reversible chemical reaction represents a chemical process that proceeds in both forward (left to right) and reverse (right to left) directions. When the rates of the forward and reverse reactions are equal, the concentrations of the reactant and product species remain constant over time and the system is at equilibrium. A special double arrow is used to emphasize the reversible nature of the reaction. The relative concentrations of reactants and products in equilibrium systems vary greatly;...
63.1K