Consider the following elementary reaction: k + br2 → kbr + br. (a) use simple bimolecular collision theory to determine the value of "kmax" at 600 k. use d12 = 0.400 nm and express k in l mol-1 s -1 .

(b) the observed rate constant at 600 k is ~ 1.4 x 1012 l mol-1 s -1 . this value is larger than what you should have calculated in part (a). we account for this atypical result via a harpoon mechanism. as the k atom approaches a br2 molecule, an electron jumps from k to br2. the resulting cation (k+ ) and anion (br2 – ) are then drawn toward one another, potentially causing a collision that may not have occurred without the attraction. use the observed rate constant to find an effective d12 for this reaction; that is, calculate the value of d12 required for collision theory to agree with experiment. we can use this value as an estimate of the distance over which the electron transfer occurs.

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.

i'm pretty sure it is letter c.) car

it takes on an electronical energy