Question

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

Answer 1

For (a) the order is
`\(Be^(2+) < Mg^(2+) < Ba^(2+) < Sr^(2+) < Ra^(2+)\)`, and for (b) the order is
`\(P^(3-) < S^(2-) < Cl^(-) < Al^(3+) < Na^(+) < Mg^(2+)\).`

a) **Arranging ions in increasing ionic radius:**

`\[ Be^(2+) < Mg^(2+) < Ba^(2+) < Sr^(2+) < Ra^(2+) \]`

Explanation: As we move down a group in the periodic table (from Be to Ra), the ionic radius increases due to the addition of more electron shells.

b) **Arranging ions in increasing ionic radius:**

`\[ P^(3-) < S^(2-) < Cl^(-) < Al^(3+) < Na^(+) < Mg^(2+) \]`

Explanation: Within a period, as we move from right to left, the ionic radius generally increases because there are fewer electrons, resulting in a smaller effective nuclear charge, leading to a larger radius.