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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.
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 ...
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.
When treated with water, beryllium chloride forms a tetrahydrate, BeCl 2 •4H 2 O ([Be(H 2 O) 4]Cl 2). BeCl 2 is also soluble in some ethers. [7] [8] When suspended in diethyl ether, beryllium chloride converts to the colorless dietherate: [9] BeCl 2 2 O(C 2 H 5) 2 → BeCl 2 (O(C 2 H 5) 2) 2. This ether ligand can be displaced by other Lewis ...
At high temperature and pressure, RbCl adopts the caesium chloride (CsCl) structure (NaCl and KCl undergo the same structural change at high pressures). Here, the chloride ions form a simple cubic arrangement with chloride anions occupying the vertices of a cube surrounding a central Rb + .
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.
Colourless diboron tetrachloride (m.p. -93 °C) is a planar molecule in the solid, (similar to dinitrogen tetroxide, but in the gas phase the structure is staggered. [4] It decomposes (disproportionates) at room temperatures to give a series of monochlorides having the general formula (BCl) n , in which n may be 8, 9, 10, or 11.
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