What is Holmium Definition Atomic Number Electron Configuration and Uses
With an Atomic Mass of 164.9303, the chemical element Ho (Holmium) is one of the rarest compounds on earth. Holmium proves excellences in terms of malleability and ductility. This is a white-coloured, silvery textured soft material that possesses unusual magnetic characteristics. From nuclear control reaction procedures to medical treatment options that are non-invasive to a patient, Holmium plays a key role in many real-time applications. Known for its high significance, let us learn about this element Ho, by understanding its properties, chemical nature, examples, and a few important applications.
Important Details about What Holmium is
‘Per Teodor Cleve’ (1840-1905) was the 1st Swedish chemist, who discovered Holmium spectroscopically in 1879 when working with another earth metal ‘Erbium’. The name was assigned for his place of birth named Uppsala in Stockholm, Sweden.
Holmium is one of the rarest elements found on earth and is categorized as lanthanides. The element Ho is located in the 67th position in the periodic table. This is a silver, shiny material but turns yellowish oxide (Ho2O3), during the process of oxidation or when heated directly. Being completely soluble in acids, Holmium gets affected due to the presence of oxygen and water.
As we noted before, the element Holmium has unusual magnetic potential and it also records the highest magnetic moment ever, which is 10.6 µB for a naturally-derived chemical substance.
Let us now quickly understand the physical and chemical properties of Holmium from the following.
Physical and Chemical Properties of the Element Ho
Firstly, here are the physical properties of Holmium.
A key rarest element found on earth. But it is more common than silver and gold.
Soft and silvery in texture and appearance.
Is both malleable and ductile.
Amount of Ho available inside the crust of the earth is approximated to be 0.7 to 1.2 parts per million. But mined in a few countries such as India, the United States of America, Sri Lanka, China, Australia and Brazil, in reserves estimated to be around 400,000 tonnes.
Hexagonal close-packed (hcp) is the crystal structure of Ho.
Forms an alloy when combined with other metals.
High temperature is proportional to its high reactivity.
HOL-me-um is the pronunciation.
Holmium possesses unusual attractive properties along with electrical conductivity, and majorly seen at times of low-temperature conditions.
Gadolinite and Monazite are the rarest isotopes of Ho.
Now, we have Some Important Chemical Properties.
[Xe] 4f11 6s2 is the Electronic Configuration of Ho.
The atomic number is 67 and the atomic mass is 164.9303.
Noted in the periodic table at Row 6.
Present in the section of Lanthanides in the f-block of the periodic table.
Solid structure at 20°C celsius.
Somewhat electropositive.
Stability in room temperature.
Trivalently bonded.
1.23 is the Electronegativity as per the Pauling scale.
2,720°C (4,930°F) is the Boiling Point and Melting Point is 1,470°C (2,680°F).
8.803 grams is the Density of Ho per 1 Cubic Centimetre.
Good desolvation in other acids, similar to other metals.
A gist about the Isotopes and Extraction of Holmium
An isotope is defined to be the more than 2 forms of a chemical element. For the element Ho, there is only 1 naturally-existing isotope which is holmium-165. Holmium-163 is a synthetic isotope with a half-life of 4570 years.
There is a minimum count of 20 isotopes of Holmium that are found to be radioactive. However, there is no proven cases or enough scientific evidence about the health issues or safety measures for using Holmium to date.
When there is a chemical ration between Holmium Fluoride (HoF3) and the Calcium metal, then this process gives rise to Holmium (Ho).
The Significant Applications of Holmium
Even though the element is radioactive and there is no proven record for its toxicity (generally stated to be Low) there are enough applications for using Ho in industries and other research fields. Given below are some important applications of Holmium in real-life.
Holmium acts as a Flux concentrator to many high magnetic fields and also, this is used as an alloy in the production and manufacturing of magnets.
The rods of nuclear control reactors make use of Holmium considering its good neutron absorption capacity. Moreover, the same absorption power of Ho makes it suitable for use as a burnable poison.
For Cubic Zirconia and Glass production, the Holmia also called the holmium oxide, is preferred for giving a natural yellow and red colouration.
To calibrate things, optical spectrophotometers prefer Holmium.
The pole pieces of several static magnets make use of this powerful element Ho, owing to its high permeability.
For non-invasive medical processes, the element Ho is used in the case of solid-state specialized lasers for programs such as cancer treatment, fibre-optics, dental operations, and even for kidney stones.
Holmium is majorly used in the treatment procedures of the eye disorder glaucoma, and even to correct failed or wrong glaucoma surgeries. Holmium lasers come handy for reducing the abnormal range of pressure in human eyes.
In the future, with enough research for its quantum property, one can utilize Holmium for quantum computers and other classical control methods.
Conclusion
Holmium (Ho) is a silver, rare earth metal, with the atomic number 67 and present in the 6th row, f-block of the periodic table. The element is categorized under the lanthanides. It has unusual electrical and magnetic properties and is used in nuclear reactors for its good absorption power. The reactivity of Ho is high at increased temperatures but usually stable at room temperature. Holmium-165 is the only naturally-occurring isotope but there are 20 radioactive isotopes noted for Ho. The toxicity of this element is still not known completely but there is a good number of applications for Holmium in the fields of medicine and dental procedures.
FAQs on Holmium Element Overview Properties and Applications
1. What is holmium and what type of element is it?
Holmium is a chemical element with the symbol Ho and atomic number 67, classified as a lanthanide (rare earth metal) in the f-block of the periodic table. It is a soft, silvery metal that belongs to the inner transition elements. Key facts about holmium include:
- Group: Lanthanide series
- Period: 6
- Block: f-block
- Standard state at 25°C: Solid (s)
Holmium is known for its strong magnetic properties and is used in lasers and magnetic applications.
2. What is the electron configuration of holmium?
The ground-state electron configuration of holmium (Ho, Z = 67) is [Xe] 4f11 6s2. This means:
- [Xe] represents the xenon core (54 electrons)
- 4f11 indicates 11 electrons in the 4f subshell
- 6s2 indicates 2 electrons in the 6s subshell
As a lanthanide, holmium fills the 4f orbitals, which are responsible for many of its magnetic and spectral properties.
3. What are the common oxidation states of holmium?
The most common and stable oxidation state of holmium is +3. In chemical compounds, holmium typically forms the ion Ho3+. For example:
- Holmium(III) oxide: Ho2O3
- Holmium(III) chloride: HoCl3
The +3 oxidation state is characteristic of lanthanides due to the loss of two 6s electrons and one 4f electron.
4. Where is holmium found in nature?
Holmium is found in nature in rare earth minerals such as monazite and bastnäsite. It does not occur as a free element but is present in trace amounts within these minerals. Key points:
- Occurs combined with other lanthanides
- Extracted by ion-exchange and solvent extraction methods
- Primarily obtained from monazite sand deposits
Holmium is relatively rare in the Earth’s crust but more abundant than precious metals like gold.
5. What are the physical properties of holmium?
Holmium is a soft, silvery-yellow metal with one of the highest magnetic moments of any element. Important physical properties include:
- Atomic mass: 164.93 u
- Melting point: 1474°C
- Boiling point: 2695°C
- Density: 8.79 g/cm3
Holmium exhibits strong paramagnetism due to its unpaired 4f electrons, making it significant in magnetic applications.
6. How does holmium react with oxygen?
Holmium reacts with oxygen when heated to form holmium(III) oxide, Ho2O3. The balanced chemical equation is:
4Ho(s) + 3O2(g) → 2Ho2O3(s)
- The oxide formed is stable and pale yellow.
- This reaction shows holmium’s typical +3 oxidation state.
Like other lanthanides, holmium slowly oxidizes in air at room temperature.
7. What are the uses of holmium in chemistry and industry?
Holmium is used mainly in lasers, magnetic materials, and nuclear control rods due to its unique magnetic and spectral properties. Major uses include:
- Holmium:YAG lasers in medical and dental procedures
- Magnetic flux concentrators in high-strength magnets
- Neutron absorber in nuclear reactors (due to high neutron absorption cross-section)
Holmium’s sharp optical absorption lines also make it useful for spectrophotometer calibration.
8. Why is holmium considered a rare earth element?
Holmium is considered a rare earth element because it belongs to the lanthanide series and occurs dispersed in minerals rather than in concentrated deposits. Although not extremely scarce, it is:
- Difficult to separate from other lanthanides
- Found in low concentrations in ores
- Extracted through complex chemical separation techniques
The term “rare earth” refers more to extraction difficulty than actual crustal abundance.
9. What is the atomic number and atomic mass of holmium?
Holmium has an atomic number of 67 and a standard atomic mass of approximately 164.93 u. This means:
- It has 67 protons in its nucleus.
- A neutral holmium atom has 67 electrons.
- Its most stable naturally occurring isotope is Ho-165.
The atomic number determines its position in the periodic table and its chemical behavior.
10. Is holmium reactive with water or acids?
Holmium reacts slowly with cold water and more rapidly with dilute acids to form Ho3+ salts and hydrogen gas. For example, with hydrochloric acid:
2Ho(s) + 6HCl(aq) → 2HoCl3(aq) + 3H2(g)
- Holmium is relatively stable in dry air.
- It forms protective oxide layers on its surface.
This behavior is typical of lanthanide metals, which readily form +3 oxidation state compounds.
