Carbon is a chemical element with the symbol C and atomic number 6. It is a member of the group 14 elements in the periodic table, and is the basis of all known life on Earth. It is a non-metal, and is the fourth most common element in the universe, after hydrogen.
Carbon is the element with the largest number of chemical compounds, with more than 10 million known to date. Each carbon atom can bond to four other carbon atoms, allowing them to form chains and rings. Pure carbon exists in three forms (allotropes) on Earth: graphite, diamond and buckminsterfullerene (spherical structure with 60 carbon atoms bonded together to form 12 pentagons and 20 hexagons).
It has many important uses, including in the production of steel and other metals, as a component of many polymers, and as a source of energy in the form of fossil fuels.
Diamond is the hardest substance in nature, and used in jewelry. Also, the blades of some saws are coated with diamonds and can cut any material except another diamond. Graphite is much softer, which is why it is used in pencils, and is also used in some batteries. Coal is currently the largest source of fuel for electricity generation. Crude oil, natural gas and coal are naturally occurring hydrocarbons.
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 (C)
| Atomic weight | [12.0096, 12.0106] |
| Discoverer (year) | unknown (~ 1694) |
| Natural form | non-metallic solid (hexagonal) |
| Electron configuration | [He] 2s2 2p2 |
| M.p. (ºC) | 3500 |
| B.p. (ºC) | 4827 |
| Earth's crust abundance (ppm) | 200 |
| Isotope (abundance %) | 12C (98.93), 13C (1.07) |
| Density (g/cm3) | 2.26 |
| vdW radius (pm) | 170 |
| Covalent radius (pm) | 75 |
| Electronegativity (Pauling) | 2.55 |
| Vaporisation enthalpy (Kj/mol) | 771.00 |
| Fusion enthalpy (kJ/mol) | 117.00 |
| Specific heat capacity (J/g·K) at 25ºC and 1 at | 0.71 |
| Thermal conductivity (W/cm·K) at 25 ºC and 1 at | 1.960 |
| Oxidation number | +4, +2, -4 |
| Electronic affinity (eV) | 1.26 |
| 1st Ionization energy (eV) | 11.2603 |
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.
