Sodium is a chemical element with the symbol Na and atomic number 11. It is a soft, silvery-white, highly reactive metal that belongs to the alkali metals group in the periodic table. Sodium is the sixth most abundant element on Earth, and is a component of many minerals, including feldspars, sodalite, and rock salt.
The salt we eat every day contains a lot of sodium. Although very abundant on Earth, sodium is never found in its pure form naturally. Thus, it forms compounds with other elements. Sodium chloride, NaCl, which also contains chlorine, is the most common sodium compound. It is also known as the mineral halite, and is what makes seawater salty. Other sodium minerals include sodalite, a soft blue stone that can be shaped and polished. Pure sodium is soft enough to cut with a knife.
It reacts with oxygen in the air, forming a compound called sodium oxide, and bursts into flames when it comes into contact with water. Sodium compounds in fireworks burn with an orange-yellow color.
Sodium also reacts with water to form sodium hydroxide and hydrogen gas. it presents many important uses, including in the production of sodium hydroxide, as a component of certain medications, and in the production of soaps and detergents.
In ancient Egypt, crystals of sodium compounds were used for the momification process. Another useful compound is sodium bicarbonate, NaHCO3, which when mixed with water releases bubbles of carbon dioxide, CO2. When purified, sodium chloride, or common salt, has several uses. It causes ice to melt, so it is used mixed with sand to keep roads from freezing in winter. This helps thaw them and make them safer. It is also an important seasoning for foods.
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 (Na)
| Atomic weight | 22.98976928(2) |
| Discoverer (year) | Davy, Humphry (1807) |
| Natural form | metallic solid (cubic centred) |
| Electron configuration | [Ne] 3s1 |
| M.p. (ºC) | 98 |
| B.p. (ºC) | 883 |
| Earth's crust abundance (ppm) | 23600 |
| Isotope (abundance %) | 23Na (100)) |
| Density (g/cm3) | 0.97 |
| vdW radius (pm) | 227 |
| Covalent radius (pm) | 160 |
| Electronegativity (Pauling) | 0.93 |
| Vaporisation enthalpy (Kj/mol) | 89.04 |
| Fusion enthalpy (kJ/mol) | 2.60 |
| Specific heat capacity (J/g·K) at 25ºC and 1 at | 1.23 |
| Thermal conductivity (W/cm·K) at 25 ºC and 1 at | 1.410 |
| Oxidation number | 1 |
| Electronic affinity (eV) | 0.55 |
| 1st Ionization energy (eV) | 5.1391 |
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.
