What is Antimony Definition Atomic Number Electronic Configuration Oxidation States Compounds and Uses
Antimony, an SB element is described as a chemical element. A lustrous gray metalloid is found mainly in nature as the sulfide mineral stibnite (Sb2S3). Antimony compounds are known since ancient times and were powdered to use in cosmetics and medicines, often known by the Arabic name kohl. Also, the metallic Antimony was known, but it was identified erroneously as lead upon its discovery.
China has been the most abundant Antimony and its compound producer for some time, where most of the production comes from a mine in Hunan.
It is naturally found in Earth’s crust layer in the ores of stibnite and valentinite.
The Antimony symbol is, Sb, and the antimony atomic number is 51.
Environmental Effects of Antimony
Antimony, an SB element, and chemical element found in soils, air, and water in minimal amounts. It mainly pollutes soils. It can travel through groundwater with greater distances towards other surface waters and locations. Few laboratory tests conducted on rats, guinea pigs, rabbits have shown that a high amount of Antimony may relatively kill small animals. Rats may experience heart, liver, lung, and kidney failures before death. On the other side, animals that breathe in fewer Antimony volumes for a stipulated time may experience eye irritations, lung damage, and hair loss. Even dogs may experience heart problems when they are exposed to lower levels of Antimony. Animals that breathe Antimony continually for a couple of months may experience severe fertility problems. It has not been specified fully that using Antimony can cause cancer.
Health Effects of Antimony
Especially the people who work with Antimony may suffer the effects of exposure by continual breathing in antimony dust. For Humans, the exposure to Antimony can take place by drinking water, breathing air, and eating foods that contain it. Moreover, by skin contact with water, soil, and other substances that contain Antimony. Breathing in Antimony bound to hydrogen in the gaseous phase mainly causes health effects.
Relatively high exposure to antimony concentrations (9 mg/m3 of air) for a certain period can irritate skin, eyes, and lungs.
As the exposure often continues, more serious health effects may occur, including heart problems, lung diseases, severe vomiting, diarrhea, and stomach ulcers.
It is yet to be known whether Antimony can cause reproductive failure cancer.
Antimony is used as a medicine for parasitic infections, but people who have a high intake of those medicines become sensitive to it have experienced health effects in the past. Health effects like these have made us more aware of the dangers when exposed to Antimony. All these significant effects are highly seen in HIV and the visceral leishmaniasis coinfections.
Biological and Physiological Significance
Various compounds like Antimony are highly toxic. The antimony compounds usage for medicinal purposes was temporarily outlawed many centuries ago because of the numerous fatalities they had caused. A hydrated potassium antimonyl tartrate, known as “tartar emetic,” is currently added in medicine as a diaphoretic, expectorant, and emetic. The maximum concentration of antimony dust which can be tolerable in the air is about the same as for arsenic, 0.5 milligrams per cubic meter.
Properties of Antimony
Physical Properties of Antimony
Antimony is an SB element and a silvery-white colour; a shiny element looks like a metal. It is hard and brittle like a nonmetal, and it has a scaly surface. Also, it can be prepared as a black powder because of having a shiny brilliance to it.
The melting point of Antimony is about 630°C (1,170°F), whereas the boiling point is of 1,635°C (2,980°F). Relatively it is a soft material that can be scratched by the glass. It has a density of 6.68 grams per cubic centimeter. Its Relative atomic mass is 121Sb, and ChemSpider (a free chemical structure database) ID is 4510681.
A metalloid is an element having characteristics of both metals and nonmetals.
Chemical Properties of Antimony
Antimony is a moderately active element. It does not associate with oxygen in the air at room temperature. Also, it does not react with either coldest acids or with cold water. However, it can dissolve in some hot acids in aqua regia. Aqua regia is formed by a mixture of hydrochloric acid and nitric acid. Also, it often reacts with materials that do not react with either acid separately.
Future of Antimony
Although large amounts of Antimony have been used for the manufacture of alloys and flame retardants and is expected to remain the fact in the immediate future. As science develops more or developing markets or the improved uses are getting developed, the demand for Antimony may also result in increasing.
Antimony Uses
A few of the Antimony uses are listed below.
Pure Antimony is used when manufacturing certain semiconductors such as infrared detectors and diodes
It is used to increase its durability and harden lead
Batteries use Antimony for its smooth functioning
Also, it is used to make small arms & bullets
In addition, antimony, as an SB element, is an excellent flame retardant.
FAQs on Antimony Element Structure Properties and Applications
1. What is antimony?
Antimony is a metalloid element with the chemical symbol Sb and atomic number 51. It is located in Group 15 of the periodic table and shows properties intermediate between metals and nonmetals.
- Atomic mass: approximately 121.76 u
- Common oxidation states: +3 and +5
- Appearance: silvery-gray, brittle solid
2. What is the electron configuration of antimony?
The electron configuration of antimony (Sb) is [Kr] 4d10 5s2 5p3. This configuration shows that antimony has five valence electrons in the 5s and 5p orbitals.
- Period: 5
- Group: 15 (pnictogens)
- Valence shell configuration: 5s2 5p3
3. What are the common oxidation states of antimony?
The most common oxidation states of antimony are +3 and +5. The +3 state is more stable due to the inert pair effect.
- SbCl3 (antimony(III) chloride) – oxidation state +3
- SbCl5 (antimony(V) chloride) – oxidation state +5
4. What is antimony trioxide used for?
Antimony trioxide (Sb2O3) is mainly used as a flame retardant synergist in plastics and textiles. It enhances the effectiveness of halogen-containing flame retardants.
- Prepared by roasting stibnite: 2Sb2S3(s) + 9O2(g) → 2Sb2O3(s) + 6SO2(g)
- Used in glass, ceramics, and pigments
5. Is antimony a metal or nonmetal?
Antimony is classified as a metalloid, meaning it has properties of both metals and nonmetals. It shows moderate electrical conductivity and brittle behavior.
- Metal-like: conducts electricity slightly
- Nonmetal-like: brittle and not malleable
- Forms covalent compounds such as SbCl3
6. How is antimony extracted from stibnite?
Antimony is extracted from stibnite (Sb2S3) by roasting followed by reduction with carbon. The process occurs in two main steps:
- Roasting: 2Sb2S3(s) + 9O2(g) → 2Sb2O3(s) + 6SO2(g)
- Reduction: Sb2O3(s) + 3C(s) → 2Sb(l) + 3CO(g)
7. What are the physical properties of antimony?
Antimony is a silvery-gray, brittle solid with moderate electrical conductivity. Its key physical properties include:
- Melting point: about 630.6°C
- Boiling point: about 1587°C
- Density: approximately 6.68 g/cm3
8. What is the difference between antimony(III) chloride and antimony(V) chloride?
Antimony(III) chloride (SbCl3) contains antimony in the +3 oxidation state, while antimony(V) chloride (SbCl5) contains antimony in the +5 oxidation state. The key differences are:
- SbCl3: trigonal pyramidal shape, more stable
- SbCl5: trigonal bipyramidal shape, stronger Lewis acid
9. Why is antimony considered toxic?
Antimony is considered toxic because many of its compounds can interfere with biological processes and cause health effects when inhaled or ingested.
- Sb2O3 dust may irritate lungs and skin
- Soluble antimony compounds can affect the liver and heart
- Long-term exposure is regulated in workplaces
10. What are the main uses of antimony in industry?
Antimony is mainly used in flame retardants, alloys, and semiconductors. Its industrial applications include:
- Sb2O3 in flame-retardant plastics
- Alloys with lead to increase hardness in batteries and bearings
- Semiconductor materials such as InSb (indium antimonide)
