Which of the following ion is smallest ion?

More the nuclear charge on ion, electrons are more strongly attracted and thus size decreases. Hence, among the given ions Al3+ is the smallest ion.

Which is the smallest ion?

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.

Ionic Radii and Isoelectronic Series.

Ion Radius (pm) Atomic Number
N 3− 146 7
O 2− 140 8
F − 133 9
Na + 98 11

Which of the following ion has smallest ionic radius?

Hence Li+,B3+ are smaller than N3− and O2−. Among Li+ & B3+, B3+ is smaller as it has higher nuclear charge due to which its size is reduce as electrons are strongly attracted. Hence among given options, B3+ is smallest.

Which of the following has the smallest size?

Thus, Al3+ has the smallest size.

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. …

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Why is Al3+ smaller than Mg2+?

Identify the smallest ion among the following: i) Al3+ ii) Na+ iii) Ba2+ iv) Mg2+ More the nuclear charge on ion, electrons are more strongly attracted and thus size decreases. Hence, among the given ions Al3+ is the smallest ion. Was this answer helpful?

Which ion has largest radius?

Explanation: The ionic radii of cations follow the same trends as atomic radii. They increase from top to bottom and from right to left in the Periodic Table. Thus, the ion with the largest radius is closest to the lower left corner of the Periodic Table, and that is the K+ ion.

Which is the smallest radius?

Atomic radii vary in a predictable way across the periodic table. As can be seen in the figures below, the atomic radius increases from top to bottom in a group, and decreases from left to right across a period. Thus, helium is the smallest element, and francium is the largest.

Which ion has the smallest radius quizlet?

Ca2+ would have the smallest ionic radius because Calcium has a positive charge, and because this ion is a cation, cations will have the smallest radius. So therefore, elements with a positive charge, will have a smaller ionic radius.

Which is smallest in size N3 O2 F Na+?

Make life easier by first sorting them into Periodic Table order: N3- O2- F- Na+ Mg2+ Al3+ These are all isoelectronic with the structure 2,8. The smallest ion will be the one with the largest number of protons – Al3+; the biggest, the one with the least protons – N3-.

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Which has smaller size Na or Na+?

Answer. Na+ ion is smaller than Na because Na looses its one electron to become Na+ ion so the positive charge of nucleus per electron present will increase and it result more electrostatic force of attraction increases .

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.

Why is Na+ smaller than ne?

Consider also that Na+ has as many electrons as Ne, but Na+ has one more proton than Ne to attract the electrons closer to the nucleus, thus resulting in a smaller size compared to both Ne and Na.

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.

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