Why the ratio of ionic radii Na +/ Mg2+ is greater than 1?
Further explaination: Magnesium is further along the period than sodium is which means that the electrostatic attraction between the valence electrons and the nucleus is greater than that of sodium and the relative nuclear charge for a 2+ ion is larger than that of a 1+ ion.
Why is the ionic radius of Li greater than that of Be?
In lithium’s case, the outermost electron is being screened from the nucleus by two core electrons. That is why lithium has a larger atomic radius than beryllium. In fact, atomic radius decreases as you move from left to right across a period.
What is the ionic radius of an Mg2+ ion?
Metallic, Covalent and Ionic Radii(r)*
| Atom/Ion | r(pm) |
|---|---|
| Lu | 172 |
| Lu3+ | 86 |
| Mg | 160 |
| Mg2+ | 72 |
Is Li+ bigger than be2+?
Looking at the periodic table we can see that the three cations have equal number of electron (after removing electrons from the neutral atoms, B, Be and Li). However, B3+ will have the smallest radius followed by Be2+ . Li+ will have the largest ionic radius among the three. of electrons.
Which is larger Li+ or Na+?
As Na atom is larger than Li atom, therefore, Na+ ion is also bigger in size than Li+ion. (v) P or As: Both these atoms belong to group 15 of the periodic table. Since As is placed after P, therefore its size is large because atomic size increases down the group.
Why is the radius of Li+ so much smaller than the radius of Li?
A cation has less electron than the neutral form of the element. Remember that the atomic radius is dependent upon the number of electrons (i.e. high number of electrons means larger radius). Li+ has 1 electron less than Li. Therefore, Li+ is smaller than Li.
Why Mg2+ is smaller than Li+?
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.
Which out of Li+ and al3+ has bigger size explain?
For Al+3 it has 13 protons and 10 electrons. That implies higher charge density on nucleus compared to Li+ (p=3,e=2). Due to this higher effective charge density factor Al+3 attracts the outermost shell strongly and outermost shell contracts.