Arrange the following Elements from greatest to least tendency to accept an electron.?

Rank from greatest to least tendency to accept an electron. To rank items as equivalent, overlap them.

Sr, Sn, Rb, Te, I

I > Te > Sn > Sr > Rb.

Explanation:

Atoms can accept additional electrons if the valence energy level is not full, which is true for all the elements except the noble gases (period 18 in the periodic table

Two factors must you consider to predict the ability to gain an electron:

The size of the atom The effective nuclear charge.

Starting with the second factor, the larger the attraction exerted by the effective nuclear charge the greater the tendency to accept an additional electron.

In a given period (row), the effective nuclear charge increases as you move to the right, since the number of protons (positive charge) increases, while the main energy level (size of the atom) remains constant.

From that, you can predict that as you move from left to right across a period on the periodic table, the tendency to accept and addtional electron increases (as said excluding the noble gases who have no room in their valence shell to accept any electrons).

The five given elements, Sr, Sn, Rb, Te, and I, are in the same period (row) number 5. So, you can use the just explained tendency to rank them from greatest to least tendency to accept an electron.

As said, the elements that are more to the right have a greater tendency to accept electrons as compared to the elements that are more to the left in the same row.

Ordering the elements from left to right they are:

Rb, Sr, Sn, Te, and I.

Which means that I (iodine) will have the greatest tendency to accept an electron and Rb will have the least tendency.

Therefore, the rank from greatest to least tendency to accept an electron is:

I > Te > Sn > Sr > Rb.