Since the number of electrons are the same, size is determined by the number of protons. Al has 13 protons, therefore the nuclear charge is greatest and pulls the electrons closer, thus is the smallest. The N3- has 7 protons and the nuclear charge it the smallest of the series.
Which ion is smallest in size?
Consequently, the ion with the greatest nuclear charge (Al 3 +) is the smallest, and the ion with the smallest nuclear charge (N 3−) is the largest.
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Ionic Radii and Isoelectronic Series.
| Ion | Radius (pm) | Atomic Number |
|---|---|---|
| N 3− | 146 | 7 |
| O 2− | 140 | 8 |
| F − | 133 | 9 |
| Na + | 98 | 11 |
How do you determine the size of an isoelectronic ion?
Another isoelectronic series is P3–, S2–, Cl–, Ar, K+, Ca2+, and Sc3+ ([Ne]3s23p6). For atoms or ions that are isoelectronic, the number of protons determines the size. The greater the nuclear charge, the smaller the radius in a series of isoelectronic ions and atoms.
Which is bigger Al3+ or mg2+?
As you go from Na+ to Mg2+ to Al3+, the number of protons in the nucleus increases and so pulls the outer electrons in more and more. The same thing is true for the other set of ions as well. … The smallest ion will be the one with the largest number of protons – Al3+; the biggest, the one with the least protons – N3-.
Which is smaller mg2+ or Na+?
mg2+ would be the smaller ion this is because each ion has the same number of electrons however mg2+ has a greater number of protons and therefore is more charge dense and the outer electrons feel a greater pull from the nucleus. …
How do you order ion sizes?
In such a series, size decreases as the nuclear charge (atomic number) of the ion increases. The atomic numbers of the ions are S (16), Cl (17), K (19), and Ca (20). Thus, the ions decrease in size in the order: S2- > Cl– > K+ > Ca2+.
Is F and Cl Isoelectronic?
Isoelectronic ions are ions that have the same number of electrons. There are many ions that are isoelectronic.
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| Isoelectronic ions | number of electrons |
|---|---|
| 1. Na+, F- | 10 electrons |
| 2. S2-, Cl-, K+, Ca+2 | 18 electrons |
Are isoelectronic ions the same size?
An Isoelectronic Series is a group of atoms/ions that have the same number of electrons. … Since the number of electrons are the same, size is determined by the number of protons. Al has 13 protons, therefore the nuclear charge is greatest and pulls the electrons closer, thus is the smallest.
Which is bigger Se2 or Br?
The Br− ion is smaller than the Se2− ion because the Br− ion has a larger nuclear charge and more extra electrons than the Se2− ion.
Why is Li+ bigger than Mg2+?
Interestingly, the atomic radii of Li and Mg are 1.52 and 1.60 A respectively, and here also the difference is quite small. … 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 has more size Ne Na+ Mg2+ Al3+?
Answer. Hence, Na+ is the largest amongst the 3.
Which is bigger Na or Na+?
Yes Na+ is smaller than Na because Na+ is formed when an electron is lost from the Na atom,Thus the effective nuclear charge increases bcz the number of protons exceeds the number of electrons . This results in bringing the valence shell a little closer to the nucleus because of a very strong nuclear pull.
Which has largest radius?
Thus O2− has a minimum z-effective thus largest radius.
Why is Al3+ smaller than Na+?
Al3+ because they all have the same number of electrons, however Al3+ has the most protons and therefore greatest nuclear charge. In Al3+, the same number of electrons are being attracted by more protons in the nucleus, so the electrons are being pulled closer to the nucleus, reducing the size of the ionic radius.