Carbon group
The name carbon group (also carbon-silicon group ) refers to the 4th main group ( " Tetrels " ) ( according to the new numbering of IUPAC group 14) of the periodic table. It comprises the elements carbon (C ), silicon (Si), germanium (Ge), tin (Sn) and lead (Pb). Also, a radioactive element that Flerovium (Fl) is represented.
Diamonds
C60 fullerene
High-purity silicon
Silicon powder
Germanium
α and β tin
Lead
Properties
The elements of the group of carbon have very different chemical and physical properties, because the group is divided by the dividing line between metals and non-metals in two parts. The first element of the group carbon, is a non-metal, the two following ( silicon and germanium) are semi-metals and any additional ( tin, lead and Flerovium ) are metals.
Physical Properties
With increasing atomic number atomic mass grow, atomic radius and ionic radius. The density of graphite (C) and silicon are close together ( about 2.3 kg/dm.sup.3 ), it rises within the main group to lead on 11.34 kg/dm.sup.3. In the Mohs hardness there is also a large wingspan, up to 1.5 minimum ranges from a maximum of 10 for diamond in tin. The highest electrical conductivity tin with 9.17 MS / m, the smallest has silicon to 25.2 mS / m. The first ionization energy decreases with increasing atomic number of 11.26 eV for carbon to 7.34 eV for tin from. Lead has 7.42 eV again a slightly higher value. The electronegativity decreases with increasing atomic number of 2.5 (C ) to 1.6 (Pb) tends to decline, outliers with 1.7 is the silicon.
Electron configuration
The electronic configuration is [ X] ys2yp2. The X indicates the period are used, in which the element is found for the electron configuration of a period of higher standing noble gas, and for the y must. Germanium from a (y -1) d10 orbital is present; and lead from there is also a (y -2) f14 orbital.
For the individual elements are the electron configurations:
- Carbon: [ He] 2s22p2
- Silicon: [ Ne ] 3s23p2
- Germanium: [ Ar] 3d104s24p2
- Zinn: [ Kr ] 4d105s25p2
- Lead: [ Xe] 4f145d106s26p2
- Flerovium (calculated): [ Rn] 5f146d107s27p2
The oxidation states are 4 and -4, with increasing atomic number but also gains the 2 oxidation state in importance.
Chemical reactions
Due to the large differences within the group it is difficult to specify a general reaction behavior, as this will vary from item to item. In the following equations, the E stands for an element of the carbon group.
- Reaction with oxygen:
- Reaction with hydrogen ( without chain formation, not spontaneous):
- Reaction with water:
- Reaction with halogens ( chlorine on the example ):
Chain formation
A special feature of the group 14 elements is their ability to form long-chain hydrogen compounds of the structure XH3 ( XH2 ) n- XH3. All hydrogen atoms are covalently bonded, but the stability of these compounds increases with increasing atomic number of the element from.
- Hydrocarbons: The group of hydrocarbons is the most extensive, as the number of carbon atoms and thus the chain length are virtually no limits. A further specific feature of the carbon material is the ability to form stable double and triple bonds. With the hydrocarbons and their derivatives deals organic chemistry.
- Silanes: the case of silicon, the ability to chain formation is already limited to a maximum of 15 Si - Si bonds. Double or even triple bonds are unstable at silicon and the following elements, but also the silanes are not among the most stable compounds.
- Germane Germanium is capable only to a maximum of nine Ge-Ge bonds. This limits the possibilities of course, a strong.
- Zinnwasserstoffe: In tin only a single Sn - Sn bond is possible. There are therefore only two compounds of this class: SnH4 and SnH3 - SnH3.
- Lead hydrogen: Lead does not have the ability to chain formation. Only pBH4 is known, but also this link is almost unstable.
Also ring formations are possible, the molecular formula is then ( XH2 ) n
Compounds
- Oxide (IV) hydroxides and acids Carbon dioxide ( CO2) is a triatomic linear built and, therefore, non-polar molecule, due to the stability of the C = O double bond, and is present in a gaseous aggregate state. In water it forms the fickle, weak carbonic acid ( H2CO3 ).
- In silica (SiO2) exist exclusively single bonds. It is a solid and is composed of SiO4 tetrahedra which are linked to each other, all the vertices. In nature SiO2 occurs as quartz. Amorphous SiO2 ( silica ) is the essential component of the glass.
- Germanium dioxide ( GeO 2 ) substantially corresponds to the silicon dioxide, but may also crystallize in the rutile structure. The latter reacts with water to the germanic acid ( H4GeO4 ).
- Tin ( IV ) oxide ( SnO2 ) is a solid and insoluble in water.
- Lead (IV ) oxide ( PbO2 ) is also an insoluble in water solid.
- Carbon monoxide ( CO) is a toxic gas.
- Silicon monoxide ( SiO) is a dark brown, amorphous solid of polymer ( SiO) x chains.
- Silicones consist of three-dimensional networks of alternating silicon and oxygen, which are mostly located on the silicon atoms organic radicals ( eg, methyl groups (- CH3) ).
- Lead (II ) oxide
- Lead (II, IV) -oxide
Occurrence
The earth's crust consists of 27.7 % from elements of the carbon group. Of this amount, 99.8 % silicon, the second most abundant element in the earth's crust (after oxygen).
The remaining 0.2 % are broken down as follows:
- 99.1 % carbon
- 0.94 % lead
- 0.02 % tin
- 0.01 % germanium.
With the exception of germanium they occur under natural conditions in some native deposits.