Element Project Kayli Yip

Name: Radium

Symbol: Ra

Atomic Number: 88

Atomic Mass: 226.0 amu

Number of Protons: 88

Number of Electrons: 88

Number of Neutrons: 138

Physical Properties

Color: Silvery White

Molar Volume: 41.09 cm3/mol

Density: 5.5 g/cm3

Boiling Point: 1737 °C

Melting Point: 700 °C

Specific Heat: 0.120 J/g/°C

Chemical Properties

Oxidation States: 2

Enthalpy of Formation: 7.15 kJ/mol

Coordination Number: 12

Concentration: 1 - 100 Bq/m3

Substances It Reacts With: When exposed to air, it reacts with nitrogen to quickly form a black coating of radium nitrite. Radium combines with most non-metals, including oxygen, fluorine, chlorine, and nitrogen. It also reacts with acids with the formation of hydrogen gas.

Who Discovered: Marie and Pierre Curie

Date: December 21st, 1898

Location: France

The Curies succeeded in isolating element 84, polonium, and then element 88, radium. Marie devised a method for separating radium from its radioactive residues, making possible the closer study of its therapeutic properties.

Industrial Uses: nuclear panels, aircraft switches, and radon gas in cancer treatment

Areas in the World: extracted from uranium ores mainly in Belgium, Canada, the Czech Republic, Slovakia, the United Kingdom, and Russia.

Environmental Concerns: Mining, processing, and reclamation in Virginia have the potential to affect surface water quality and quantity groundwater quality and quantity, soils, air quality, and biota.

1. Radium is the heaviest of the alkaline earth metals.

2. It is highly radioactive and can be extremely dangerous.

3. Due to its oxidation, it changes from a silvery white color to black when exposed to air.

4. Radium-226 has a half-life of 1602 years, the longest of all radium isotopes.

5. Radium exposure, which could result from inhaling or swallowing, could cause cancer, anemia, cataracts, and even death.

6. Radium is in the same group as calcium and is therefore sometimes used to treat bone cancer through emitting alpha particles that kill cancerous cells.

7. Radium was used to paint the numbers and hands in clocks to be visible in the dark. However, this was stopped after many factory workers died from exposure.

8. We are constantly exposed to small amounts of radiation as it is naturally occurring in our environment.

9. Marie and Pierre Curie's laboratory notebooks are still too radioactive to be handled today, due to their work with radium.

10. Radium can be found in everyday products, including wristwatches and toothpaste.

11. It has an abundance of roughly one part per trillion in the Earth's crust. This makes it the 84th most abundant element in the crust.

12. Radium is created from the decay of the uranium atom, which then turns into several other unstable elements before finally ending in the element lead.

13. The name of this element comes from the Latin world "radius", which means ray.

14. Radium has no known biological role because it is toxic due to its radioactivity.

15. An equivalent amount of radium would be three million times more radioactive than uranium.

16. Radium was the first radioactive element to be made synthetically.

17. It is a solid state at room temperature.

18. A sample of radium metal maintains itself at a higher temperature than its surroundings because of the radiation it emits.

19. At the time of the Manhattan Project in 1944, the "tolerance dose" for workers was set at 0.1 microgram of ingested radium.

20. Currently, other than its use in nuclear medicine, radium has no commercial applications. Formerly, it had other uses but since the toxicity is known now, less dangerous isotopes are used instead radioluminescent devices.

Made with Adobe Slate

Make your words and images move.

Get Slate

Report Abuse

If you feel that this video content violates the Adobe Terms of Use, you may report this content by filling out this quick form.

To report a Copyright Violation, please follow Section 17 in the Terms of Use.