Methane is the hydrocarbon that belongs to the simplest group of alkanes, its chemical formula is CH4. Each of the hydrogen atoms is bonded to the carbon by a bond covalent. Methane is a nonpolar substance that occurs as a gas at ordinary temperatures and pressures. It is colorless, and has no odor, and is insoluble in water. In nature it is produced as a final product of anaerobic putrefaction that occurs in plants. This natural process can be beneficial if you want to produce biogas. It is important to note that a large part of anaerobic microorganisms produce it using CO2 as the final electron acceptor.
If what you want is to understand this compound as a molecule, it must be taken into account that carbon is the most important atom of organic molecules and its atomic number is 6, since it is located in sixth place in the periodic table of the elements. The fact that carbon has 6 as an atomic number means that it has 6 protons in the nucleus and 6 electrons in the periphery. On the other hand, it is important to bear in mind that electrons are arranged in shells and orbitals and that electrons are a fundamental element to give way to the formation of molecules.
Along the same lines, if four hydrogens are attached to carbon, each hydrogen contributes one electron and with the help of the valence electrons of carbon, a two-electron bond is produced. Thus, a total of four bonds are formed and each one will have two electrons, so the carbon will end up surrounded by eight electrons in its outermost shell. When the methane molecule is formed, carbon achieves great stability.
The main characteristics of methane is that it is colorless, odorless and tasteless; it is insoluble in water and its liquefaction is difficult. Methane can react with the following halogens: fluorine, chlorine and bromine, giving way to a mixture of halomethanes and a hydrogen halide. If it fuses with fluorine it can cause a violent explosion. In return it binds with chlorine and bromine required in the initial phase to provide energy as light or heat, and the reaction is less potent, particularly in the case of bromine.
