I cannot solve this problem..I want to get two same answer :( We have discussed

Question

I cannot solve this problem..I want to get two same answer :(

We have discussed why the alkali metals increase in reactivity as you go down the family on the periodic table, using the equation for the force of attraction between a nucleus and an electron:

Where F is the force, k is a constant related to charge, and d is the distance between the nucleus and an electron. We can also use this equation to understand the reactivity of the halogen family. Explain why the halogens decrease in reactivity as you go down the family on the periodic table. (See http://www.youtube.com/watch?v=u2ogMUDBaf4 as an example.)

Explanation / Answer

The reactivity of the alkali metals depends on the ease with which an electron is lost. From top to bottom in groups the size of atom increases because of number of shells increasing, which results larger atoms, due to this the nucluear attraction on outtermost electron decreases which leads to a greater reactivity.

where as in the case of halogens the reactivity depends on the involves acquisition of an electron. Fluorine has the highest electronegativity and iodine the lowest electronegativity of the halogens. The electronegativity is based in part on the ionization energy and the electron affinity which are both a function of the effective nuclear charge and the distance to the outermost energy level.

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