Deuterium - Detailly Explained
Heavy hydrogen, often known as deuterium, is one of the stable isotopes of hydrogen. Deuterium gets its name from the Greek word deuterons, which means "second."
The stable isotopic variation of hydrogen gas has only one proton and one neutron. Protium, which does not have a neutron, makes up 99.9% of naturally occurring marine hydrogen, while Deuterium makes up only 0.02 percent.
Harold C. Urey, an American scientist, and his coworkers Ferdinand G. Brickwedde and George M. Murphy discovered deuterium in 1931. Urey anticipated that the vapor pressures of molecular hydrogen (H2) and a corresponding molecule with one hydrogen atom substituted by deuterium (HD) would differ, allowing them to be separated by liquid hydrogen distillation.
What is Deuterium?
Deuterium, also known as heavy hydrogen, is one of the isotopes of hydrogens that is stable. The name deuterium is derived from the Greek word deuterons, which means 'second'. The nucleus of the hydrogen-deuterium atom is known as a deuteron, containing one proton and one neutron. Protium does not have a neutron. Deuterium has a natural abundance of about one atom in between 6420 hydrogens in the oceans. Thus, deuterium takes account for approximately 0.02% (0.03% by mass) of all the hydrogens that occur naturally in the oceans, and protium takes account for the rest of 99.98%.
Deuterium Oxide
Deuterium oxide is an isotopic form of water which is always stable and non-radioactive. This element contains two atoms of deuterium (D) and one atom of oxygen, with DNA-labelling activity. It is also known as heavy water. It is called heavy water due to the presence of deuterium in it, which is a heavier hydrogen isotope as compared to the hydrogen isotope (protium), which is present in normal water.
The heavier hydrogen isotope brings out the nuclear properties of water. The increase in the mass of the water due to deuterium makes the water slightly different from normal water in terms of physical and chemical properties.
Facts, Properties and Uses
Properties
Deuterium has several properties as listed below:
Deuterium forms chemical bonds that are stronger than regular hydrogen.The triple point, boiling point, vapor pressure, heat of fusion, and heat of evaporation of deuterium are all much higher than those of common hydrogen.
The gas deuterium is colorless. When ionized, however, it gives off a distinctive pink hue.
Because of the stronger connections, heavy water has a density of 10.6 times that of conventional water (1.624 g/cm3). In standard water, heavy water ice sinks, but it floats in heavy water.
Heavy water has a higher viscosity than regular water. (12.6 μPa·s at 300 K).
Uses
Deuterated water is used in Magnetic Resonance Spectroscopy.
It is used as a moderator in nuclear reactors.
The metabolic rate of the human body can be determined by using it.
For tracking the process of Photosynthesis in plants, it is used as the primary tracer element.
By using Deuterium in Nuclear Magnetic Resonance Spectroscopy, magnetic field stabilization is being maintained.
It is used in the determination of the isotopologue of various organic compounds.
In heavy water form, it is used in Infrared Spectroscopy.
There is an important aspect of Nuclear fusion reaction known as Tritium. It is controlled by using Deuterium.
Facts
Atomic weight = 2.014
Molecular weight = 4.0282 g/mol
Symbolic representation = 2H
Boiling point = (-)249o C
Melting point = (-)254o C
Delton or Deuteron is the name for a single Deuterium nucleus. Deuterium has no radioactive effects due to its minute presence among the naturally occurring Hydrogen form.
It is naturally flammable and emits a pale blue flame.
It is non-toxic, however, it can deplete oxygen levels in the atmosphere, resulting in asphyxiation.
It is also referred to as Hydrogen 2 and Deuterons.
It has no color and odor.
By nature it is non-corrosive.
When the temperature is low, it is slightly soluble in water (cold water)
FAQs on Deuterium
1. What is deuterium, and how does it differ from regular hydrogen?
Deuterium, also known as heavy hydrogen, is a stable isotope of hydrogen. The key difference lies in its atomic nucleus. While a standard hydrogen atom (protium) has only one proton, a deuterium atom's nucleus contains one proton and one neutron. This extra neutron makes deuterium approximately twice as heavy as protium.
2. What are the key physical properties of deuterium?
Deuterium exhibits distinct physical properties due to its higher mass compared to protium. Key properties include:
- Symbol: ²H or D
- Atomic Weight: 2.014 u
- Melting Point: -254°C
- Boiling Point: -249°C
- Appearance: It is a colorless and odorless gas.
- Bonds: It forms stronger chemical bonds than protium.
3. What are the most important uses of deuterium in science and industry?
Deuterium has several significant applications, primarily in its form as heavy water (D₂O). Its main uses include:
- Nuclear Reactors: It is used as a moderator to slow down neutrons and sustain nuclear fission reactions.
- NMR Spectroscopy: Deuterated solvents are used in Nuclear Magnetic Resonance (NMR) to avoid interference from hydrogen signals.
- Scientific Tracers: It is used to label compounds and track their pathways in biological and chemical processes, such as studying metabolism or photosynthesis.
- Infrared (IR) Spectroscopy: Heavy water is used as a solvent in IR spectroscopy in place of normal water, as its absorption bands do not overlap with many organic compounds.
4. How does the single extra neutron in deuterium affect the properties of its compounds, like heavy water?
The extra neutron significantly increases the mass of the deuterium atom. This increased mass leads to stronger chemical bonds in its compounds. For example, in heavy water (D₂O), this results in:
- Higher Density: Heavy water is about 10.6% denser than regular water (H₂O), causing heavy water ice to sink in regular water.
- Different Physical Constants: It has a higher boiling point, melting point, and viscosity than H₂O.
- Slower Reaction Rates: Chemical reactions involving the breaking of a bond to deuterium are typically slower than those involving hydrogen. This can disrupt sensitive biological processes if ingested in large amounts.
5. Why is deuterium a stable isotope, while tritium (another hydrogen isotope) is not?
Deuterium's stability comes from its nuclear composition of one proton and one neutron. This combination forms a stable, low-energy state for a nucleus of two nucleons. In contrast, tritium has one proton and two neutrons. This proton-to-neutron ratio makes the tritium nucleus unstable, causing it to undergo radioactive decay to achieve a more stable configuration. Deuterium, being stable, is not radioactive.
6. What is the specific role of heavy water (D₂O) as a moderator in nuclear reactors?
In a nuclear reactor, the fission of uranium atoms releases high-energy, fast-moving neutrons. For a chain reaction to be sustained efficiently, these neutrons must be slowed down. Heavy water serves as an excellent neutron moderator because the deuterium nuclei can slow down fast neutrons through collisions without absorbing them as readily as the protium in regular water. This efficiency allows the reactor to operate with natural (unenriched) uranium as fuel.
7. Is it safe for humans to drink heavy water (deuterium oxide)?
Drinking a small amount of heavy water is generally considered safe and not harmful. It is not radioactive. However, consuming large quantities over a prolonged period can be dangerous. Because deuterium forms stronger bonds and reacts more slowly than hydrogen, high concentrations of D₂O in the body can disrupt delicate biochemical processes, such as cell division and enzyme function, leading to symptoms of poisoning.
