Why is fluorine more reactive than iodine but lithium less reactive than rubidium?

[matrix5]

I found in a text that had this question.

why should F, n row 2, be more reactive than iodine, in row 5, while Li, in row 2, is less reactive than Rb, in row 5?

BUT this does not agree with this text
http://richardbowles.tripod.com/chemistry/reactivity/reactivity.htm

as it is more reactive as you go down in the PTOE.

 

[Gokul43201]

Notice that your link doesn't say anything about non-metals, where reactivity decreases as you go down. The question is correct.

The reason for the decreasing reactivity down the halogen group shares the same basis as the reactivity trend among the metals (though the trend is reversed). The non-metals or electronegative elements react by gaining electrons, while the metals (electropositive elements) react by losing electrons. The reasons for the trends follow naturally from this.

 

[thepatientmental]

The reactivity of elements in a group or row on the Periodic Table of Elements (PTOE) is determined by their electron configuration and atomic structure. In general, as you move down a group on the PTOE, the reactivity of elements tends to increase due to the addition of more electron shells and a larger atomic radius. However, there are exceptions to this trend.

In the case of F and n in row 2, F is more reactive than n because it has a smaller atomic radius and a higher electronegativity. This means that F has a stronger ability to attract and gain electrons, making it highly reactive in chemical reactions. On the other hand, n has a larger atomic radius and lower electronegativity, making it less reactive.

For Li and Rb in row 2 and 5 respectively, the trend of increasing reactivity as you go down the group does not apply. This is because Li has a unique electron configuration with one valence electron, making it highly reactive in certain situations. Rb, on the other hand, has a full outer electron shell, making it less reactive compared to Li.

It is important to note that the reactivity of elements is also affected by other factors such as the presence of other elements in a compound and external conditions like temperature and pressure. Therefore, while the general trend of increasing reactivity as you go down a group on the PTOE holds true, there are exceptions that can be explained by the specific electron configurations and properties of each element.