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[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
RCH=CHR′ + ICl → RCH(I)–CH(Cl)R′ When such reactions are conducted in the presence of sodium azide, the iodo-azide RCH(I)–CH(N 3)R′ is obtained. [5] The Wijs solution, iodine monochloride dissolved in acetic acid, is used to determine the iodine value of a substance. It can also be used to prepare iodates, by reaction with a chlorate.
2 Cl 2 + 2 NaHCO 3 → Cl 2 O + 2 CO 2 + 2 NaCl + H 2 O. This reaction can be performed in the absence of water but requires heating to 150–250 °C; as dichlorine monoxide is unstable at these temperatures [4] it must therefore be continuously removed to prevent thermal decomposition. 2 Cl 2 + Na 2 CO 3 → Cl 2 O + CO 2 + 2 NaCl
A diagram showing the bond dipole moments of boron trifluoride. δ- shows an increase in negative charge and δ+ shows an increase in positive charge. Note that the dipole moments drawn in this diagram represent the shift of the valence electrons as the origin of the charge, which is opposite the direction of the actual electric dipole moment.
Structure of solid phosphorus pentachloride, illustrating its autoionization at higher concentrations. [7] In solutions of polar solvents, PCl 5 undergoes self-ionization. [8] Dilute solutions dissociate according to the following equilibrium: PCl 5 ⇌ PCl + 4 + Cl −. At higher concentrations, a second equilibrium becomes more prevalent: 2 ...
The molecular structure in the gas phase was determined by microwave spectroscopy; the bond length is r e = 1.628341(4) Å. [2]The bond length in the crystalline ClF is 1.628(1) Å; the lengthening relative to the free molecule is due to an interaction of the type F-Br···ClMe with a distance of 2.640(1) Å.
The electronic structure of a coordination complex can be described in terms of the set of ligands each donating a pair of electrons to a metal centre. For example, in hexamminecobalt(III) chloride, each ammonia ligand donates its lone pair of electrons to the cobalt(III) ion. In this case, the bonds formed are described as coordinate bonds.
In the solid state is present as a planar dimer I 2 Cl 6, with two bridging Cl atoms. [1] It can be prepared by reacting iodine with an excess of liquid chlorine at −70 °C, [2] or heating a mixture of liquid iodine and chlorine gas to 105 °C. [citation needed] In the molten state it is conductive, which may indicate dissociation: [2] I 2 Cl ...