Rubidium is chemical element 37 on the periodic table. Its symbol is Rb. Its atomic mass is 85.47. It has 37 protons and 37 electrons. It is a soft silver colored metal. It was first discovered in 1861 by Robert Wilhelm Bunsen and G. Kirchoff in Heidelberg, Germany.
Properties[change | change source]
Physical properties[change | change source]
Chemical properties[change | change source]
Rubidium is very reactive. It will ignite in air because it reacts with many other elements in the air like oxygen and nitrogen. Rubidium reacts very violently with water to make hydrogen and rubidium hydroxide, a strong corrosive base. The reaction is normally very hot so the hydrogen ignites.
Chemical compounds[change | change source]
Rubidium forms chemical compounds in only one oxidation state: +1. Some rubidium compounds have a mixed oxidation state, though. Rubidium chloride is the most common rubidium compound. Rubidium hydroxide and rubidium carbonate are also used commonly. Rubidium compounds makes a red-violet color in a flame. Most rubidium compounds are colorless. Rubidium compounds are not as common as other alkali metal compounds, such get sodium compounds. Otherwise, they are similar.
- Rubidium chloride, similar to sodium chloride
- Rubidium hydride, strong reducing agent
- Rubidium hydroxide, powerful base
- Rubidium nitrate, strong oxidizing agent
- Rubidium oxide, yellow, strong base when dissolved in water
Occurrence and preparation[change | change source]
Rubidium is about as common as zinc. It is the 23rd most common element in the Earth's crust. Most minerals only have a small amount of rubidium in them. It normally comes in small quantities in other minerals. It is made by reduction of rubidium ores with calcium. It is expensive because calcium is difficult to make and the rubidium needs to be kept in argon and away from water or air.
Uses[change | change source]
There are not many common uses for rubidium. Rubidium compounds are sometimes used in purple fireworks. It and its compounds are used mainly in science research though. It is also used to make superoxide ions. It is used in some special types of glass.
Safety[change | change source]
Rubidium compounds are not very dangerous in the human body; however, if a person gets too much from eating, they could get sick because it acts like other alkali metal ions such as sodium ions in sodium chloride. Rats can live with up to half of their potassium replaced with rubidium, though it is not likely for that to happen.
Rubidium is very dangerous. It reacts with air and water and makes corrosive substances.
References[change | change source]
- "Visual Elements: Rubidium". rsc.org. 2011 [last update]. http://www.rsc.org/chemsoc/visualelements/pages/data/rubidium_data.html. Retrieved 26 June 2011.