The name rubidium comes from the Latin word rubidium, meaning “deepest red“. This refers to the red flame it produces when burned. This element is highly reactive, and ignites on contact with air. In contact with water, it reacts vigorously, producing hydrogen gas and much heat.
Rubidium is not only found in a few minerals, but is widespread in small quantities in a wide range of minerals, such as leucite and polucite. The pure metal is obtained mainly from the mineral lepidolite. Another mineral called rubicline has even more rubidium, but it is very rare. Rubidium atoms are sensitive to light and can be used in photoelectric cells and night vision equipment.
This element has radioactive forms, which can be used to date the age of rocks. When injected into a patient’s body, rubidium targets tumors, which show up clearly on PET (positron emission tomography) scans. Rubidium is also used by light-sensitive electronics called photomultipliers, and in the manufacture of insulators for high-voltage cables and some special types of glass.
Electron configuration
The electron configuration of an element describes the arrangement of electrons in the atoms of that element, and be used to predict its chemical properties and reactivity.
In the electron configuration notation, the letters "s", "p", "d", and "f" represent the different types of atomic orbitals, and the superscripts indicate the number of electrons in each orbital. The orbitals are filled in a specific order, starting with the lowest energy orbital and working up.
Emission spectra
Each element in the periodic table presents its own unique emission spectra, which is determined by the energy levels of its electrons. When an electron in an atom is excited to a higher energy level, it can de-excite by emitting a photon of light with an energy equal to the difference between the two levels. This results in a characteristic emission line in the spectra (which corresponds to specific wavelengths of light). These spectra are usefull to identify the elements present in a sample.
Symmary of properties (Rb)
| Atomic weight | 85.4678(3) |
| Discoverer (year) | Bunsen, Robert Wilhelm & Kirchhoff, Gustav Robert (1861) |
| Natural form | metallic solid (centred cubic) |
| Electron configuration | [Kr] 5s1 |
| M.p. (ºC) | 39 |
| B.p. (ºC) | 688 |
| Earth's crust abundance (ppm) | 90 |
| Isotope (abundance %) | 85Rb (72.17), 87Rb (27.83) |
| Density (g/cm3) | 1.63 |
| vdW radius (pm) | 303 |
| Covalent radius (pm) | 215 |
| Electronegativity (Pauling) | 0.82 |
| Vaporisation enthalpy (Kj/mol) | 69.20 |
| Fusion enthalpy (kJ/mol) | 2.19 |
| Specific heat capacity (J/g·K) at 25ºC and 1 at | 0.36 |
| Thermal conductivity (W/cm·K) at 25 ºC and 1 at | 0.580 |
| Oxidation number | 1 |
| Electronic affinity (eV) | 0.49 |
| 1st Ionization energy (eV) | 4.1771 |
Definition of terms in the previous table
- Atomic weight: The average mass of an element's atoms, typically given in atomic mass units (amu).
- Natural form: The most stable and abundant form of an element that occurs naturally in the environment.
- Electron configuration: The arrangement of electrons in an atom or molecule.
- Melting point: The temperature at which a solid substance turns into a liquid.
- Boiling point: The temperature at which a liquid substance turns into a gas.
- Earth's crust abundance (ppm): The concentration of an element in the Earth's crust, typically given in parts per million (ppm).
- Isotope (abundance %): A variant of an element that has the same number of protons in the nucleus, but a different number of neutrons. The abundance of an isotope is the percentage of the isotope in a sample of the element.
- Density (g/cm3): The mass of a substance per unit volume.
- vdW radius (pm): The radius of an atom or molecule as predicted by the van der Waals model, typically given in picometers (pm).
- Covalent radius (pm): The distance from the center of an atom to the center of another atom with which it is bonded covalently, typically given in picometers (pm).
- Electronegativity (Pauling): A measure of an atom's ability to attract electrons in a chemical bond, based on the Pauling scale.
- Vaporisation enthalpy (kJ/mol): The amount of energy required to convert a substance from a liquid to a gas at a constant temperature.
- Fusion enthalpy (kJ/mol): The amount of energy required to convert a substance from a solid to a liquid at a constant temperature.
- Specific heat capacity (J/g·K) at 25ºC and 1 at: The amount of heat required to raise the temperature of 1 gram of a substance by 1 degree Celsius at a constant pressure.
- Thermal conductivity (W/cm·K) at 25 ºC and 1 at: The ability of a substance to conduct heat, typically given in watts per centimeter per kelvin.
- Oxidation number: A positive or negative integer that represents the number of electrons that an atom has gained or lost in a chemical compound.
- Electronic affinity: The energy change associated with adding an electron to a neutral atom to form a negative ion.
- 1st Ionization energy: The energy required to remove the most loosely bound electron from a neutral atom.
