Which has the smallest size Na+ Mg2+ Al3+?

The correct option is: a Al3+ Explanation:These are isoelectronic ions ions with same number of electrons and for isoelectronic ions greater the positive nuclear charge greater is the force of attraction on the electrons by the nucleus and the smaller is the size of the ion. Thus Al3+ has the smallest size.

Which is smaller Na+ or Mg2+?

(i) The sodium ion (Na+) is larger than the magnesium ion (Mg2+) due to two effects.

Which of the following has smallest size Na+ Mg2+ Cl?

Na+,Mg2+,O2−andF− all are isoelectronic but Mg2+ have 12 protons in his nucleus, so the attraction force on last shell is maximum and hence it have smallest size.

Which has larger size Mg2+ or Al3+?

Mg, Mg2+, Al, Al3+. Atomic radii decrease across a period, cations are smaller than their parent atoms. Among isoelectronic ions, the one with the larger positive nuclear charge will have a smaller radius. Hence the largest species is Mg and the smallest one is Al3+ .

Which is the smallest among NA Mg2+ Al3 and why?

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.

Which is smaller Na+ or Al3+?

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 smallest ion will be the one with the largest number of protons – Al3+; the biggest, the one with the least protons – N3-.

Is Mg2+ smaller than Al3+?

As they have equal number of electrons the electrons are not involving in determination of atomic radius. Hence atomic radius is totally depended on effective nuclear charge. Therefore radius of Al3+ is less than Mg2+.

Are Na+ and Mg2+ the same size?

Explain your answer. 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.

Which ions smallest size?

Na+,Mg2+,O2− and F− all are isoelectronic but Mg2+ has 12 protons in his nucleus, so the attraction force on the last shell is maximum and hence, it has the smallest size.

Which of the following has the smallest size NA B NA+ C NA d Cl+?

(d) Cl+ is the correct answer. Atomic size decreases across the period. Thus chlorine will be smaller in size in comparison to sodium. Since cation is always smaller than its parent atom, therefore, Cl+ ion will be smallest among the given options.

Why is Na+ smaller than 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 smallest size Na+?

-Greater the charge on the cation, smaller is the size of the cation and vice-versa. So, from the above given all cations, we can see that phosphorus has the greatest charge on it i.e. +5 and its electrons are very strongly attracted by the nucleus due to the increased nuclear and thus, has the smallest size.

What is the Order of ionic size of Na+ Mg2+ Al3+ and Si4+?

AIPMT 1993: Na+, Mg2+, Al3+ and Si4+ are isoelectronic. The order of their ionic size is (A) Na+ > Mg2+ < Al3+ < Si4+ (B) Na+ < Mg2+ > Al3+ > Si4+

Why does Al3+ have a lower ionic radius than Mg2+?

Mg2+ – 10electrons , 12protons. Here both have same no. of electrons but different no. of protons(Z). As Al3+ has more protons so its electrons would be attracted more towards nucleus resulting in a size smaller than mg2+. Therefore Al3+ will havea lower ionic radius(its not called atomic radius for ions) than mg2+.

Why does Si4+ have a smaller radius than Na+?

So you’re increasing the number of protons without increasing the number of electrons. That extra positive charge pulls in the electrons tighter – giving you a smaller radius. So the smallest will be Si4+ and the largest Na+. Sounds like a periodic trend that you might or will learn in chemistry.

Why Al3+ and Mg2+ are isoelectronic species?

Now try to understand the concept , Al3+ and Mg2+ are isoelectronic species that is they have equal number of electrons. As they have equal number of electrons the electrons are not involving in determination of atomic radius.