Arrange the following in increasing
order of their specific charges
Na+, Mg2+, Al3+, li+, F-
(please answer with explanation)
Answers
Answer:
Explanation:
Sodium belongs to period 3, and beryllium belongs to period 2 in the periodic table. Also, the Be2+ ion has a higher charge than the Na+ ion. So, there cannot be any doubt about the positions of Na+ and Be2+ as the largest and the smallest ions among the four.
Now, coming to Li+ and Mg2+, the values of their radii are 0.74 A and 0.72 A respectively ('A' stands for angstrom unit). Thus, the lithium ion with +1 charge is only marginally larger than the magnesium ion having a charge of +2.
Interestingly, the atomic radii of Li and Mg are 1.52 and 1.60 A respectively, and here also the difference is quite small. These two elements are known to show the so called 'diagonal relationship' in some of their chemical properties due such closeness in atomic size. Despite the Mg atom having a slightly larger size, the Mg2+ ion is marginally smaller in size than the Li+ ion because of its higher nuclear charge.
Sodium belongs to period 3, and beryllium belongs to period 2 in the periodic table. Also, the Be2+ ion has a higher charge than the Na+ ion. So, there cannot be any doubt about the positions of Na+ and Be2+ as the largest and the smallest ions among the four.
Now, coming to Li+ and Mg2+, the values of their radii are 0.74 A and 0.72 A respectively ('A' stands for angstrom unit). Thus, the lithium ion with +1 charge is only marginally larger than the magnesium ion having a charge of +2.
Interestingly, the atomic radii of Li and Mg are 1.52 and 1.60 A respectively, and here also the difference is quite small. These two elements are known to show the so called 'diagonal relationship' in some of their chemical properties due such closeness in atomic size. Despite the Mg atom having a slightly larger size, the Mg2+ ion is marginally smaller in size than the Li+ ion because of its higher nuclear charge.