Carbon group

The carbon group is a periodic table group consisting of carbon (C), silicon (Si), germanium (Ge), tin (Sn), lead (Pb), and flerovium (Fl).Carbon C Atomic Number: 6 Atomic Weight: 12.0107 Melting Point: 3948.15 KBoiling Point: 4300 KSpecific mass: 2.267 g/cm3 Electronegativity: 2.55Silicon Si Atomic Number: 14 Atomic Weight: 28.0855 Melting Point: 1638.15 K Boiling Point: 3538 KSpecific mass: 2.3296 g/cm3 Electronegativity: 1.9Germanium Ge Atomic Number: 32 Atomic Weight: 72.64 Melting Point: 1211.45 K Boiling Point: 3106 KSpecific mass: 5.323 g/cm3 Electronegativity: 2.01Tin Sn Atomic Number: 50 Atomic Weight: 118.710 Melting Point: 505.21 K Boiling Point: 2875 KSpecific mass: 7.287 g/cm3 Electronegativity: 1.96Lead Pb Atomic Number: 82 Atomic Weight: 207.2 Melting Point: 600.75 K Boiling Point: 2022 KSpecific mass: 11.342 g/cm3 Electronegativity: 2.33Flerovium Fl Atomic Number: 114 Atomic Weight: Melting Point: ? 340 K Boiling Point: ? 420 K Specific mass: ? 22 g/cm3 Electronegativity: ? The carbon group is a periodic table group consisting of carbon (C), silicon (Si), germanium (Ge), tin (Sn), lead (Pb), and flerovium (Fl). In modern IUPAC notation, it is called Group 14. In the field of semiconductor physics, it is still universally called Group IV. The group was once also known as the tetrels (from the Greek word tetra, which means four), stemming from the Roman numeral IV in the group names, or (not coincidentally) from the fact that these elements have four valence electrons (see below). Like other groups, the members of this family show patterns in electron configuration, especially in the outermost shells, resulting in trends in chemical behavior: Each of the elements in this group has 4 electrons in its outer orbital (the atom's top energy level). The last orbital of all these elements is the p2 orbital. In most cases, the elements share their electrons. The tendency to lose electrons increases as the size of the atom increases, as it does with increasing atomic number.Carbon alone forms negative ions, in the form of carbide (C4−) ions.Silicon and germanium, both metalloids, each can form +4 ions.Tin and lead both are metals while flerovium is a synthetic, radioactive (its half life is very short), element that may have a few noble gas-like properties, though it is still most likely a post-transition metal. Tin and lead are both capable of forming +2 ions. Carbon forms tetrahalides with all the halogens. Carbon also forms three oxides: carbon monoxide, carbon suboxide (C3O2), and carbon dioxide. Carbon forms disulfides and diselenides. Silicon forms two hydrides: SiH4 and Si2H6. Silicon forms tetrahalides with fluorine, chlorine, and iodine. Silicon also forms a dioxide and a disulfide. Silicon nitride has the formula Si3N4. Germanium forms two hydrides: GeH4 and Ge2H6. Germanium forms tetrahalides with all halogens except astatine and forms dihalides with all halogens except bromine and astatine. Germanium bonds to all natural single chalcogens except polonium, and forms dioxides, disulfides, and diselenides. Germanium nitride has the formula Ge3N4. Tin forms two hydrides: SnH4 and Sn2H6. Tin forms dihalides and tetrahalides with all halogens except astatine. Tin forms chalcogenides with one of each naturally occurring chalcogen except polonium, and forms chalcogenides with two of each naturally occurring chalcogen except polonium and tellurium. Lead forms one hydride, which has the formula PbH4. Lead forms dihalides and tetrahalides with fluorine and chlorine, and forms a tetrabromide and a lead diiodide, although the tetrabromide and tetraiodide of lead are unstable. Lead forms four oxides, a sulfide, a selenide, and a telluride.