Chemistry 242 - Inorganic Chemistry II
Chapter 20 - The Halogens: Fluorine, Chlorine Bromine, Iodine and Astatine
- All elements except helium, neon and krypton fro some sort of halogen compound.
- The structures vary from ionic to covalent.
- Halides are often the source materials for thsynthesis of other substances.
- The halides are often the "generic" compounds used to illustrate the range of oxidation states for the other elements.
- The class of fluorocarbons is an important group of organic chemicals which often have unique properties.
Occurence and Isolation, and Properties of the Elements
- Occurs in fluorspar, CaF2, cryolite, Na3AlF6 and fluorapatie, 3Ca3(PO4)2.Ca(F,Cl)2. It is actually more abundant than chlorine.
- It is made by electrolysis, for example, of a misture of 2 to 3 parts of HF with KF which melts at 70 - 100 oC. It is a pale yellow gas, bp -118 oC.
- It is the most reactive of all the elements and attacks all the others except He, Ne and Ar so it has to be handled in special apparatus: stainless steel and copper because they become coated with a protective fluoride layer and are the materials of choice. (If all traces of HF are removed, fluorine can be handled in glass apparatus also, but this is nearly impossible.)
- Fluorine will also attack many compounds yielding flourides.
- The reason for its great reactivity seems to be connected with the weak F-F bond probably due to strong repulsion between the non-bonding (lone-pair) electrons. (In this respect it is similar to hydrazine and hydrogen peroxide.)
- Occurs mainly as rock salt, NaCl, potassium chloride and magnesium chloride.
- Chlorine is manufactured by the electrolysis of brine. At one time this was done using a mercury cathode, which also produced sodium amalgam, thence sodium hydroxide by hydrolysis. The sodium hydroxide was often recombined with the chlorine to form sodium hypochlorite (bleach) for use in the paper industry. The mercury is now recognized as a major polluent. Now "memberane" cells are used to prevent the electrolytes around the two electodes from mixing.
- Chlorine is a green gas bp -34.6 oC.
- It occurs with chlorine and can be obtained by displacement from bromides with chlorine.
- Bromine is a brown liquid, mp -7.2, bp 58.8 oC.
They can be made by:
- Direct reaction. In the case of fluorine, particularly, high oxidation states can be reached.
- Reaction with an oxide.
- Halogen exchange reactions.
- By dehydration of hydrated halides.
As a class of compounds, the halides illustrate the distinction between ionic solids, network solids and molecular compounds (which can be solids liquids or gases). This section deals with all three, its heading notwithstanding!
The particularly high electronegativity of fluorine leads to some special properties in its compounds:
- Broadly, the more covalent the halide, the more likely it is to be truly molecular. Examples would be BCl3 or IF3.
- As the compounds become less covalent, halogen bridges are found, leading first to dimers such as Al2Cl6.
- As the covalency continues to decrease, the amount of bridging increases and network solids can be found. An example is (AlF3)n in which all the aluminum is 6-coordinated and all the fluorines are bridging (2-coordinate). The bonding remains quite covalent.
- At the ionic limit one finds salts such as sodium chloride, where the forces between sodium and chloride ions are almost entirely electrostatic. Both ions are 6-coordinate in NaCl.
- The position along the above progression is influenced by factors such as the electronegativity of the components, their size, and the possibility of multiple bonding which might stabilize a monomeric molecular compound such as BF3 (pp - pp) or SF6 (dp - pp).
- CF3COOH is a strong acid unlike CH3COOH.
- NF3 and N(CF3)3 are not at all basic, unlike ammonia.
- -CF3 groups are quite inert to nucleophilic attack, unlike -CH3.
- -CF3 mimics a big halogen with an electronegativity around that of -Cl.
Fluorine forms two oxygen compounds:
Chlorine does not react directly with oxygen, but forms a dangerously exposive paramagnetic oxide ClO2 in the following reaction:
- Oxygen Fluoride, OF2 a yellow gas produced by:
F2 + NaOH(aq) OF2
- Dioxygen difluoride, O2F2 a yellow-orange solid produced by:
F2(g) + O2(g) O2F2 (Electric discharge through the reactants)
NaClO3 + SO2 + H2SO4 2ClO2 + 2NaHSO4
It is used as a chlorinating agent in organic synthesis well diluted with air!
Iodine forms one important oxide, I2O5, by dehydration of HIO3:
HIO3 I2O5 + H2O (240 oC)
Its use is as a reagent for quantitative analysis for carbon monoxide:
5CO + I2O5 I2 + 5CO2
then the iodine is titrated as triiodide with thiosulphate:
I2 + I- I3-
S2O32- + I3- 3I- + S4O62- (starch as indicator)
- The reaction of the halogens with water produces hypohalous acids, HOX, and halide ion in solution:
X2 + H2O HOX + H+ + X-
The pure compounds are unknown except HOF which is none too stable itself.
The solutions can be used to obtain the salts e.g. sodium hypochloride, bleach. The XO- ions disproprortionate further in basic solution, (IO- very rapidly even in neutral solution):
3XO- 2X- + XO3-
- For chlorine the following reactions are important:
- Production of chlorite, ClO2-, and chlorate, ClO3-:
ClO2 + 2OH- ClO2- + ClO3- + H2O
- Perchlorate is produced by electrolytic oxidation of chlorate:
ClO3- + H2O ClO4- + 2H+ + 2e-
- Periodate species are unlike the others due to the large size and low electronegativity of iodine. The following equilibria are important:
H5IO5 H+ + H4IO6- K = 10-3
H4IO6- IO4- + 2H2O k = 29
H4IO6- H3IO62- + H= k = 1x10-7
Periodate is used as an oxidizing agent in organic synthesis.
- The species are molecules or molecule ions, for example, BrCl, IF5, Br3+, I3-.
- The neutral species will be XX'n where n is odd and 7 or less and X' will be the lighter halogen. The range of isolable compounds is governed by steric effects.
- Most are made by direct reactions.
Organic Compounds of Fluorine
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