An Introduction
Platinum is a precious metal and is represented with the platinum symbol, Pt. The word Platinum comes from the Spanish word "Platina." Platina means Silver. It is one of the rarest elements found in the earth's crust with an estimated abundance of 5 μg/kg. Platinum can conduct electricity. Platinum, along with rhodium, palladium, ruthenium, iridium, and osmium, forms a group of elements called platinum group metals (PGM). If you are wondering Who discovered Platinum, it was discovered by Antonio de Ulloa in 1735.
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This article contains the uses of platinum, its electronic configuration, atomic number, and properties of platinum. The frequently asked questions at the end of this article will help you if you incur any doubts while going through the same.
Platinum is a dense highly unreactive malleable silverish white chemical element with the symbol Pt. The atomic number of platinum is 78. The plant's name is derived from the Spanish Platina which is a root word of Plata "silver". Platinum is one of the rarest elements but a highly desired and valuable metal. The shell structure of platinum is 2.8. 18.32. 17.1.
Platinum Atomic Number
Platinum element belongs to group 10 of the periodic table of elements. Platinum is one of the transition metals. The atomic number of Platinum is 78, and the atomic mass of Platinum is 195.094 g/mol. The platinum melting point is 1768.3° C, and the Boiling point is 3825 ° C. It is solid at room temperature. Platinum also has some health effects. If spilled on the skin, they can cause rashes and irritation. If inhaled, it can cause Shortness of breath, sneezing, and irritation in the nose. Platinum as a metal won't cause major health issues, but Platinum salt is very dangerous. It may cause cancer, hearing problems, organ damage like intestine and kidney, etc.
Electronic Configuration of Platinum
If we follow the Aufbau principle the electronic configuration of Pt will be \[1s^{2} 2s^{2} p^{6} 3s^{2} p^{6} d^{10} 4s^{2} p^{6} d^{10} f^{14} 5s^{2} p^{6} d^{8} 6s^{2}\] but Pt has an exception. But a rule of thumb says, half filled shells are more stable. So in that case Pt will have an electronic configuration of \[1s^{2} 2s^{2} p^{6} 3s^{2} p^{6} d^{10} 4s^{2} p^{6} d^{10} f^{14} 5s^{2} p^{6} d^{9} 6s^{1}\]. Most common oxidation states of the Platinum are +2 and +4. +1 and +3 are very less common.
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Properties of Platinum
Following are the properties of Platinum:-
Atomic number: 78
Atomic symbol: Pt
Atomic weight: 195.1
Density: 12.4 ounces per cubic inch
Phase at room temperature: solid
Melting point: 3,215.1 degrees, Fahrenheit (1,768.4°C)
Boiling point: 6,917 F (3,825°C)
Van Der Waals radius: 0.138 nm
Ionic radius: 0.096 nm (+2)
Isotopes: 13
Electronic shell: \[ [Xe] 4f^{14} 5d^{9} 6s^{1}\]
The energy of first ionization: \[867 kJ.mol^{-1}\]
The energy of second ionization: \[1788 kJ.mol^{-1}\]
Discovered by: Julius Scaliger in 1735
The electronic configuration of PT :
\[ [Xe] 4f^{14} 5d^{9} 6s^{1}\]
Or
\[1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{10} 4s^{2} 4p^{6} 4d^{10} 5s^{2} 5p^{6} 4f^{14} 5d^{9} 6s^{1}\]
Physical Properties:
Platinum is heavy, soft, malleable, and ductile.
It is stable at high temperatures and has excellent resistance against corrosion.
Platinum is the second most ductile metal after gold.
Platinum is one of the densest metals with a density of 21.45 grams per cubic centimeter.
Chemical Properties:
Platinum is regarded as a noble metal, which makes it chemically stable.
It doesn't get tarnished in the air because it doesn't react with the oxygen present in the air.
It is also resistant to acid attacks.
It is corroded by halogens, cyanides, sulfur, and alkalis.
Platinum absorbs high quantities of Hydrogen gas at high temperatures, just like a sponge soaks water, which is an unusual property of Platinum.
Platinum shows a strong tendency to form complex ions. The most common one is Pt(I), which has a planar structure and is diamagnetic.
Uses of Platinum
Platinum is used for jewelry because it is chemically unreactive and soft.
It is used in dental fillings and surgical tools because of its unreactivity.
Platinum is used in lasers and in the making of photographic materials.
The metal is used as catalysts for improving the efficiency of fuel cells.
Platinum is used in coatings of razors.
An alloy of Platinum, along with Cobalt, is used for making strong permanent magnets.
It is used as a catalyst in the production of Nitric acid, Benzene, and Silicone.
Platinum is extensively used especially in the petroleum industry as it is an excellent catalyst that plays an important role in extracting gasoline for making high octane fuels.
Platinum is highly valued for its purity and beauty. The strength, hardness, resistance, and color of this metal are the reason for it being highly in demand for jewelry making. The flexibility of this metal is an important characteristic for jewelry designers.
Platinum is also used in fiber optic cables and hard disk drive coating.
Platinum is also used in explosives and fertilizers as gauze for converting ammonia to nitric acid.
Platinum is also used in glassmaking equipment and any manufacturing of fiberglass.
Platinum is used in applications such as pacemakers, hard disks, and fertilizer manufacture.
Through Platinum future equities investors also gain exposure. They can also buy coins, bars, Exchange Traded Funds(ETFs).
Production of Platinum Metal
Platinum Ores:
Platinum is usually extracted from Sperrylite and Cooperite, the two Platinum-containing ores. It is also found in the native state as well.
How is It Extracted?
The ore is crushed, and the Froth-Flotation process is done. During Flotation, the air is passed through the ore-water mixture, also called Slurry. The Platinum particle is chemically attached to the oxygen rise up to the surface in a froth, and then it is skimmed off for refining it further.
In the next step, it is dried up and then heated up to 1500° C in an electric furnace, and then air is blown through it to remove iron and Sulfur impurities.
Aqua regia is then used to dissolve platinum metal from the mineral concentrate by creating chlorine that attaches to Platinum to form chloroplatinic acid.
Finally, the ammonium chloride is used to change the chloroplatinic acid to ammonium hexachloroplatinate, which can then be burned to develop the pure platinum metal.
Fun Facts About Platinum
The extraction of Platinum is a very intensive process in terms of capital and labor. For the production of barely 31 g of Pure Platinum, we need 7 to 11 tons of Platinum ore and a time of around six months.
Platinum and Platinum alloys were used to make Platinum hunk, which is used as an international standard for measuring a Kilogram. This cylinder weighs about 1 Kg (2.2 lbs).
Platinum is the least reactive metal known to humankind.
Even a 1 g of Platinum can stretch into a 2000 meter long wire.
Platinum is widely used as a catalyst in chemical reactions.
There are 6 naturally occurring isotopes of Platinum, 190Pt (0.01%), 192Pt (0.78%), 194Pt (33.0%), 195Pt (33.8%), 196Pt (25.2%) and 198Pt (7.2%).
FAQs on Platinum
1. What is platinum and where is it placed on the periodic table as per CBSE Class 12 Chemistry syllabus?
Platinum is a precious, dense, silverish-white transition metal with the symbol Pt and atomic number 78. It is located in Group 10 of the periodic table and is classified as a transition element due to its d-block position, as outlined in the CBSE Class 12 Chemistry syllabus for 2025-26.
2. What is the electronic configuration of platinum and why does it show exceptions from the Aufbau principle?
Platinum has the electronic configuration [Xe] 4f14 5d9 6s1. This configuration is an exception to the Aufbau principle because a half-filled or fully filled d-subshell provides extra stability. Electrons from the 6s orbital are promoted to the 5d orbital to achieve this stable arrangement, which is typical for many transition metals.
3. What are the key physical and chemical properties of platinum relevant for board exam questions?
Key properties of platinum include:
- Malleable and ductile (second most ductile after gold)
- Densest metal: 21.45 g/cm3
- High melting point: 1768°C
- Chemically inert: does not tarnish in air or react with most acids
- Good conductor of electricity
- Acts as a catalyst in various chemical reactions
4. How is platinum extracted from its ores according to the CBSE Chemistry syllabus?
Platinum is extracted from ores like Sperrylite and Cooperite using a series of steps:
- Ore is crushed and subjected to the froth-flotation process
- Impurities like iron and sulphur are removed by heating and air blowing
- The concentrate is dissolved in aqua regia to form chloroplatinic acid
- Ammonium chloride converts this to ammonium hexachloroplatinate
- This compound is then decomposed by heat to yield pure platinum metal
5. What are the industrial and real-world uses of platinum in line with board exam expectations?
Platinum is used in:
- Jewelry due to its lustre, durability, and non-reactivity
- Catalysts in chemical industries, especially in fuel cells and in catalytic converters for vehicles
- Medical tools and dental fillings due to hypoallergenic properties
- Electronic components and hard disk coatings
- Glass manufacturing equipment and fiberglass production
6. What is the significance of platinum as a catalyst in chemical reactions, and why is it preferred over other metals?
Platinum is highly effective as a catalyst because of its ability to adsorb reactants on its surface, increasing reaction rates without being consumed. Its chemical inertia and high resistance to corrosion allow it to function in harsh environments, making it valuable for industrial-scale reactions like the formation of nitric acid and petroleum refining.
7. How do platinum, white gold, and other platinum group metals differ in composition and properties for exam comparison type questions?
Platinum is a pure element (Pt), while white gold is an alloy made from gold mixed with metals like nickel and silver.
- Platinum is denser, rarer, and hypoallergenic
- White gold is lighter and may cause allergies due to nickel
- The platinum group also includes ruthenium, rhodium, palladium, osmium, and iridium, which share some physical and chemical properties such as resistance to corrosion, but differ in crystal structure and applications.
8. Why is platinum more expensive than gold and many other metals?
Platinum is more expensive because it is about 30 times rarer than gold, is denser and heavier, and requires intensive mining and extraction processes. Its price is also influenced by its high demand in jewelry, industrial applications, and investment products.
9. What happens when platinum is exposed to aqua regia, and why does this mixture dissolve platinum but not most acids?
Aqua regia, a mixture of concentrated nitric acid and hydrochloric acid, dissolves platinum by creating highly reactive chlorine species that oxidize and dissolve the otherwise inert metal to form chloroplatinic acid. Platinum is generally resistant to single acids due to its noble character, but aqua regia can attack it due to its potent oxidizing and complexing effects.
10. What health and safety aspects are associated with platinum and its compounds, as per the current syllabus?
Metallic platinum is considered non-toxic and safe for use in medical and dental devices. However, platinum salts are toxic and can cause health issues such as skin rashes, respiratory problems, and even damage to internal organs. Careful handling is necessary in industrial contexts where platinum compounds are used.
11. What are some unique chemical properties of platinum that set it apart from other transition metals?
Platinum displays a strong tendency to form complex ions, is highly resistant to corrosion and oxidation, and can absorb large amounts of hydrogen gas. Unlike most other transition metals, it remains untarnished in air and is not attacked by most acids, but only by specific chemicals like aqua regia and certain halogens or cyanides.
12. How does the stability of platinum isotopes affect its industrial and scientific applications?
Platinum exists naturally as a mixture of six isotopes, most of which are stable. This stability contributes to its suitability in precise scientific instruments and standard weights, as well as its reliability in industrial processes involving high temperatures and corrosive environments.
13. What are the misconceptions students often have about platinum's reactivity and toxicity?
Students may mistakenly believe all forms of platinum are toxic or that it reacts readily with acids. In reality, pure platinum metal is very inert and safe to handle, but some platinum compounds (salts) are hazardous. Only specially formulated mixtures like aqua regia can dissolve platinum effectively.
14. Why does platinum command strategic importance in industrial chemistry and technological innovation?
Platinum's unique combination of high melting point, corrosion resistance, and exceptional catalytic activity make it essential in key industries such as automotive (catalytic converters), energy (fuel cells), and chemical manufacturing (production of fertilizers, acids, and polymers). Its role enables more efficient, environmentally friendly, and sustainable technologies.
