* Low Ionization Energy: It readily loses its outermost electron, becoming a positively charged ion (Rb+). This ease of ionization makes it highly reactive, especially with nonmetals.
* Large Atomic Radius: Rubidium's large atomic radius means its outermost electron is far from the nucleus and is held less tightly, making it easily lost.
* Electropositive Nature: Rubidium is highly electropositive, meaning it has a strong tendency to lose electrons and form positive ions.
Here's what its reactivity looks like:
* Reaction with Air: Rubidium reacts explosively with air, igniting spontaneously and forming rubidium oxide.
* Reaction with Water: It reacts violently with water, releasing hydrogen gas and generating heat that can ignite the hydrogen, causing an explosion.
* Reaction with Halogens: Rubidium reacts vigorously with halogens (like chlorine, bromine, and iodine) to form rubidium halides.
* Reaction with Acids: Rubidium reacts explosively with acids, generating hydrogen gas.
Handling and Storage:
Due to its extreme reactivity, rubidium is stored under inert atmospheres like argon or in mineral oil to prevent contact with air and moisture. It requires careful handling in a laboratory setting to avoid accidents.
Applications:
Despite its reactivity, rubidium has niche applications:
* Atomic Clocks: Rubidium's spectral properties are used in atomic clocks, known for their high precision.
* Photocells: Rubidium is used in some types of photocells.
* Research: Used in various research fields, including chemistry and physics.
In summary: Rubidium is a highly reactive alkali metal, reacting explosively with air, water, and many other substances. Its reactivity stems from its low ionization energy, large atomic radius, and electropositive nature. While dangerous to handle, it finds applications in specific fields due to its unique properties.
