Ionic radii are:a)Inversely proportional to effective nuclear chargeb)Inversely proportional to square of effective nuclear chargec)Directly proportional to effective nuclear charged)Directly proportional to square of effective nuclear chargeCorrect answer is option 'A'. Can you explain this answer?

Question

Answer

As the effective nuclear charge increases, the hold of nucleus increases, thus the shell contracts, as a result size decreases.

Answer

Option a is correct answer.
as effective nuclear charge increases ionic radii decreases

Answer

Introduction:
Ionic radii refer to the size of ions in a crystal lattice. It depends on various factors, including the effective nuclear charge experienced by the electrons in the ion. In this answer, we will explore the relationship between ionic radii and effective nuclear charge.

Explanation:
Ionic radii are primarily determined by the balance between the attractive forces between the electrons and the nucleus, and the repulsive forces between electrons. Effective nuclear charge refers to the net positive charge experienced by the electrons in the outermost energy level of an atom. It is influenced by the number of protons in the nucleus and the shielding effect of inner electron shells.

Inversely proportional relationship:
Ionic radii are inversely proportional to the effective nuclear charge. This means that as the effective nuclear charge increases, the ionic radius decreases. There are several reasons for this relationship:

1. Coulomb's law: According to Coulomb's law, the force of attraction between two charged particles is directly proportional to the product of their charges and inversely proportional to the square of the distance between them. As the effective nuclear charge increases, the attraction between the electrons and the nucleus becomes stronger, pulling the electrons closer to the nucleus and reducing the ionic radius.

2. Electron-electron repulsion: As the number of electrons increases, there is a greater degree of electron-electron repulsion, which pushes the electrons further apart. This repulsion counteracts the attractive force of the nucleus and increases the ionic radius.

3. Shielding effect: Inner electron shells shield the outermost electrons from the full effect of the nuclear charge. The more electron shells there are between the outermost electrons and the nucleus, the less the outer electrons will experience the full positive charge of the nucleus. This shielding effect reduces the effective nuclear charge experienced by the outer electrons and increases the ionic radius.

Conclusion:
In summary, ionic radii are inversely proportional to the effective nuclear charge. As the effective nuclear charge increases, the attraction between the electrons and the nucleus becomes stronger, resulting in a decrease in the ionic radius. This relationship can be explained by Coulomb's law, electron-electron repulsion, and the shielding effect of inner electron shells.

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