- •Electron configurations of carbon subgroup
- •Some physical properties of c subgroup elements
- •Physical properties
- •Occurrence
- •Silicon
- •Interaction with o2:
- •Interaction with chlorine:
- •Interaction with sulfur:
- •Compounds Carbon
- •Hydrogen compounds Carbon
- •Compounds Silicon
- •Si has no interaction with Zn, Al, Sn, Pb, Ag, Au and so it can be recrystallised from their melts. Hydrogen compounds Silicon
- •Chemical compounds
- •Oxygen containing compounds
- •Oxygen containing compounds
- •Chemical compounds
- •Compounds with halogens, sulfur, and nitrogen Carbon
Compounds Carbon
Carbides. They are binary compounds of carbon with more electropositive elements - metals, silicon, boron.
Carbides are formed only at high temperature interaction of carbon with elements (but technologically more frequent of carbon with oxides). All without exception they are very hard substances. Conventionally they can be divided into three large classes according the structure, character of bond and chemical properties:
ionic – are formed by active metals (they are easily decomposed by water or acids);
covalent – have an atomic crystalline lattice, are extraordinarily hard and chemically inert (SiC, B4C);
inclusion are metal-like, are conductors of electric current, they are very hard and refractory, extraordinarily chemically inert. The atoms of carbon in them are located between the knots of crystalline lattice of metals. Their composition often does not answer the ordinary valence states of atoms of elements (Mn4C, Mn3C, Mn8C3; Cr3C2, Cr7C3; MoC, Mo2X, WC, W2C; VC; NbC; Nb2C; TaC; Ta2C). Sometimes they have no definite stoichiometry and belong to bertollides, for example, TiC0,6-1,0, VC0,58-1,0.
Ionic carbides. This name is only conditional. They are divided on 1) acetylenides (the most widespread class), 2) methanides and 3) those which are decomposed by acids with formation of mixture of hydrocarbons and hydrogen.
Acetylenides. Are formed by most active metals (for example, Li2C2), have in composition bivalent ion C22-. They are easily decomposed by water with exothermic heat effect:
СаС2 + 2Н2О = Са(ОН)2 + С2Н2 Н298 = –125,5 kJ/mol
More frequently, worldwide is used and prepared CaC2 (~ 5 million of ton annually). It is used for preparation of C2H2 in gas welding and as reductant is in metallurgy. The carbide of calcium is preprec in electric furnaces at fusion of calcium oxide with coal:
СаО + 3С = СаС2 + СО Н298 = 464,4 kJ/mol
Methanides. Are known only for the beryllium and aluminium (Be2C and Al4C3). With hot water or diluted acids they are decomposed with the formation of methane:
Al4C3 + 12H2O = 4Al(OH)3 + 3CH4
Carbides of the third type. These are Fe3C, Co3C and some other. Are decomposed by acids:
Fe3C + 6HCl = 3FeCl3 + CH4 + H2.
At the same time are formed other gaseous hydrocarbons.
To the separate type belongs carbide Mg2C3, which is formed from MgC2 subject to the condition of breaking of carbon off at 500. At interaction with water, it gives pure propine:
Mg2C3 + H2O = 2Mg(OH)2 + CH3–CCH
The covalent carbides. Most widespread are SiC, V4C. They are inorganic polymers, and widely used in industry. A carborundum SiC has high hardness and wearproof, chemically is very inert. V4C is very hard (~diamond) and chemically stable.
Carbides of inclusion. NbC and TaC are melted at 3500 and 3900 and are most refractory from all known substances. Carbides of tungsten and tantalum are extraordinarily hard and are used for creation of superhard alloys.
Such carbides are decomposed by oxidizing alkaline melts only:
2WC + 5O2 + 8NaOH 2Na2WO4 + 2Na2CO3 + 4H2O
WC is oxidized in this reaction. In this case, it is possible conditionally to adopt the oxidation states of W and C equal to zero (0!). Then W gives 6 electrons, C - 4 electrons, and together WC gives 10 electrons to the molecule O2, which takes four electrons from WC. Basic coefficients are 2 before WC and 5 before O2.