Question

Can someone help me with this please? The problem is in the picture

Answer 1

Arranging the ions in order of increasing ionic radius:

`Be^{+2` <
`Mg^{+2` <
`Ba^{+2` <
`Sr^{+2` <
`Ra^{+2`

Arranging the ions in order of increasing ionic radius:

P^(−3)< S^(−2) <CH^(−1) <
`Na^{+1` <
`Al^{+3` <
`Mg^{+2`

a) The ionic radii of ions follow a trend where ions with more electrons than protons have larger radii, and ions with fewer electrons than protons have smaller radii.

Arranging the ions in order of increasing ionic radius:

`Be^{+2` <
`Mg^{+2`<
`Ba^{+2` <
`Sr^{+2` <
`Ra^{+2`

All ions have a +2 charge, indicating that they have lost two electrons.

As you move down a group in the periodic table (from Be to Ra), the atomic radius increases. Therefore, ions of elements farther down the group generally have larger ionic radii.

b) The ionic radii of ions with the same charge generally follow the trend where ions with more electrons than protons have larger radii.

Arranging the ions in order of increasing ionic radius:

P ^−3 <S^−2 < CH^−1 <
`Na^{+1` <
`Al^{+3` <
`Mg^{+2`

All ions in this list have a charge of ±3.

The trend generally follows the number of electrons present, with P having the most electrons and Mg having the least. Therefore, the order is based on increasing electron count, resulting in increasing ionic radius.