Radium element periodic table

Radium is a chemical element with the symbol Ra and atomic number 88. It is a highly radioactive, silvery-white, metallic chemical element that was discovered in 1898 by Marie and Pierre Curie, who named it after the Latin word for “radiant.”

Radium is a naturally occurring element that is found in small amounts in the Earth’s crust, and it is produced by the radioactive decay of other elements, such as uranium and thorium. Radium atoms do not survive for long, and most of them quickly decay into radon, a radioactive noble gas.

Radium is the only radioactive element of the alkaline earth metals. It is also the rarest of this group.

It has been used in the past in medical treatments and as a luminous paint for watches and other instruments, but its use has largely been phased out due to its radioactivity and associated health risks. This element is highly dangerous and is rarely used today. However, in the early 20th century, radium compounds were in common use. Luminous paints, such as those used to make watch dials glow in the dark, were created with radium. People working with this paint often became ill, especially with cancer, because the radiation produced by radium damages DNA. However, until the 1940s, many people thought that the radioactivity of radium was not harmful, quite the contrary.

Radium element periodic table

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.

electron configuration of element Hg

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.

emmision spectra of element Hg

Symmary of properties (Ra)

Atomic weight[226]
Discoverer (year)Curie, Marie & Pierre (1898)
Natural formmetallic solid (centred cubic)
Electron configuration[Rn] 7s2
M.p. (ºC)700
B.p. (ºC)1737
Earth's crust abundance (ppm)<0.001
Isotope (abundance %)
Density (g/cm3)5.5
vdW radius (pm)283
Covalent radius (pm)211
Electronegativity (Pauling)0.89
Vaporisation enthalpy (Kj/mol)136.80
Fusion enthalpy (kJ/mol)7.15
Specific heat capacity (J/g·K) at 25ºC and 1 at-
Thermal conductivity (W/cm·K) at 25 ºC and 1 at-
Oxidation number2
Electronic affinity (eV)
1st Ionization energy (eV)5.2784

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.

Back to the Periodic Table of the Elements.