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Bromine electron affinity

Bromine has a lower electron affinity and electrode potential than chlorine but is still a very reactive element. It combines violently with alkali metals and reacts spontaneously with phosphorus, arsenic and antimony. When heated it reacts with many other elements, including gold, but it does not attack platinum, and silver forms a protective film of silver bromide. Because of the strong oxidising properties, bromine, like fluorine and chlorine, tends to form compounds with the electropositive element in a high oxidation state. [Pg.322]

Reactions in Water. The ionization potential for bromine is 11.8 eV and the electron affinity is 3.78 eV. The heat of dissociation of the Br2 molecule is 192 kj (46 kcal). The reduction potentials for bromine and oxybromide anions in aqueous acid solutions at 25°C are (21) ... [Pg.281]

Which element of each of the following pairs has the higher electron affinity (a) oxygen or fluorine (b) nitrogen or carbon (c) chlorine or bromine (d) lithium or sodium ... [Pg.178]

Figure 5.16. Plot of data for the external heavy-atom quenching of pyrene fluorescence in benzene at 20°C. Polaro-graphic half-wave reduction potentials Ein are used as a measure of the electron affinity of the quencher containing chlorine (O), bromine ( ), or iodine (3). From Thomaz and Stevens<148) with permission of W. A. Benjamin, New York. Figure 5.16. Plot of data for the external heavy-atom quenching of pyrene fluorescence in benzene at 20°C. Polaro-graphic half-wave reduction potentials Ein are used as a measure of the electron affinity of the quencher containing chlorine (O), bromine ( ), or iodine (3). From Thomaz and Stevens<148) with permission of W. A. Benjamin, New York.
Which atom has the greatest electron affinity chlorine, bromine, iodine ... [Pg.843]

Unlike the metallic elements, halogens become less reactive going down the periodic table because of their generally decreasing electron affinity. Thus, their reactivity order is F2 > CI2 > Br2 > I2. Fluorine often reacts violently, chlorine and bromine somewhat less so, and iodine often sluggishly. [Pg.227]

The trend in oxidation potentials may be considered a composite trend, similar to that described for the E° values of the alkali metals (Chap. 6). For the halogens, the following quantities are involved heats of dissociation of the molecules, electron affinities of the atoms, hydration energies of the ions, heats of vaporization (for bromine and iodine only), and, finally, entropy or randomness effects. Aside from the entropy effects (which turn out to be quite small for the reactions being considered), the reduction of the halogen X to the hydrated ion X at room temperature may be represented in steps as follows ... [Pg.209]

Calculate the difference between the ionization energy of lithium and the electron affinity of bromine. Deduce whether the transfer of an electron from one to the other in the gas phase is spontaneous. [Pg.387]

If we had assumed the simple ionic model here, the Born-Mayer equation would have given a lattice energy of 178.4 kcal. per mole. The ionization energy of silver is 176.2 and the electron affinity of bromine (2) is — 79.1, from which the atomization energy of AgBr is 81.3 kcal. per mole, in error by nearly 40 kcal. Efforts to modify the Born-Mayer equation to take other factors into account (5) have not produced satisfactory results for such compounds. [Pg.192]

Fluorine is, in fact, an extremely powerful oxidising agent. In spite of lower dissociation energies bromine and iodine are weaker oxiding agents than chlorine this is due to their smaller electron affinities and smaller hydration energies. [Pg.392]

Consider the elements selenium (Se) and bromine (Br). Which has the higher first ionization energy Which has the higher electron affinity ... [Pg.201]

Bromine has a greater electron affinity than selenium. Gaining the extra electron changes the Br atom into Br, which has a particularly stable closed-shell electron configuration (the same as that of the noble gas atom krypton [Kr]). No such configuration is created when a Se atom gains an additional electron. [Pg.201]

Based on general trends, the electron affinity of fluorine would be expected to be greater than that of chlorine however, the value is less and is similar to the value for bromine. Explain. [Pg.267]

There he worked with George Glockler on the electron affinity of halogens (initially iodine and later bromine and chlorine as well) from space-charge effects—Calvin s problem was to measure the amount of energy released when a halogen atom captures an electron and for that he had first to devise the methods for doing so. [Pg.16]


See other pages where Bromine electron affinity is mentioned: [Pg.91]    [Pg.203]    [Pg.299]    [Pg.91]    [Pg.190]    [Pg.258]    [Pg.658]    [Pg.675]    [Pg.227]    [Pg.248]    [Pg.426]    [Pg.175]    [Pg.3]    [Pg.979]    [Pg.49]    [Pg.209]    [Pg.739]    [Pg.566]    [Pg.6]    [Pg.49]    [Pg.328]    [Pg.128]    [Pg.339]    [Pg.77]    [Pg.88]    [Pg.76]    [Pg.368]    [Pg.738]    [Pg.262]   
See also in sourсe #XX -- [ Pg.566 ]

See also in sourсe #XX -- [ Pg.209 , Pg.216 ]

See also in sourсe #XX -- [ Pg.322 ]

See also in sourсe #XX -- [ Pg.577 ]




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