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The size of isoelectronic species: F–, Ne and Na+ is affected by:
- a)Nuclear charge (n)
- b)Valence principal quantum number(n)
- c)Electron-electron interaction in the outer orbitals
- d)None of the factor because their size is the same
Correct answer is option 'A'. Can you explain this answer?
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Verified Answer
The size of isoelectronic species: F–, Ne and Na+ is affected by...
nuclear charge (Z). Isoelectronic species are the species belonging to different atoms or ions which have same number of electrons but different magnitudes of nuclear charges.
The size of an isoelectronic species increases with a decrease in the nuclear charge (Z). For example, the order of the increasing nuclear charge of F–, Ne, and Na+ is as follows:
F– < Ne < Na+
Z 9 10 11
Therefore, the order of the increasing size of F–, Ne and Na+ is as follows:
Na+ < Ne < F–
Most Upvoted Answer
The size of isoelectronic species: F–, Ne and Na+ is affected by...
Explanation:
Isoelectronic species have the same number of electrons, but they can have different nuclear charges. Therefore, the size of isoelectronic species is affected by several factors, such as:
Nuclear Charge: As the nuclear charge increases, the attraction between the nucleus and the electrons also increases. This results in a stronger pull on the electrons towards the nucleus, making the atomic radius smaller. Therefore, the size of isoelectronic species decreases with increasing nuclear charge.
Valence Principal Quantum Number: The valence principal quantum number represents the energy level of the outermost electrons. As the valence principal quantum number increases, the electrons are further away from the nucleus and the atomic radius increases. Therefore, the size of isoelectronic species increases with increasing valence principal quantum number.
Electron-Electron Interaction in the Outer Orbitals: The repulsion between the electrons in the outer orbitals can affect the size of isoelectronic species. If there are more electrons in the outer orbitals, the repulsion between them will increase, causing the atomic radius to increase. Therefore, the size of isoelectronic species increases with increasing electron-electron interaction in the outer orbitals.
Conclusion:
Therefore, option 'A' is the correct answer. The size of isoelectronic species is affected by the nuclear charge, which is the main factor that determines the atomic radius. As the nuclear charge increases, the size of isoelectronic species decreases.
Isoelectronic species have the same number of electrons, but they can have different nuclear charges. Therefore, the size of isoelectronic species is affected by several factors, such as:
Nuclear Charge: As the nuclear charge increases, the attraction between the nucleus and the electrons also increases. This results in a stronger pull on the electrons towards the nucleus, making the atomic radius smaller. Therefore, the size of isoelectronic species decreases with increasing nuclear charge.
Valence Principal Quantum Number: The valence principal quantum number represents the energy level of the outermost electrons. As the valence principal quantum number increases, the electrons are further away from the nucleus and the atomic radius increases. Therefore, the size of isoelectronic species increases with increasing valence principal quantum number.
Electron-Electron Interaction in the Outer Orbitals: The repulsion between the electrons in the outer orbitals can affect the size of isoelectronic species. If there are more electrons in the outer orbitals, the repulsion between them will increase, causing the atomic radius to increase. Therefore, the size of isoelectronic species increases with increasing electron-electron interaction in the outer orbitals.
Conclusion:
Therefore, option 'A' is the correct answer. The size of isoelectronic species is affected by the nuclear charge, which is the main factor that determines the atomic radius. As the nuclear charge increases, the size of isoelectronic species decreases.
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The size of isoelectronic species: F–, Ne and Na+ is affected by...
The size of the cation, anion and neutral molecule depending on neucelar charge of the atom. Increase the nuclear charge of atom increase the attraction power of nucleus to attract the electron towards itself. Here Na+, Ne and anion F both have same no electron or isoelectronic but but differ in nuclear charge. In case of cation Na its nuclear charge is more than neutral Ne and anion F.
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The size of isoelectronic species: F–, Ne and Na+ is affected by:a)Nuclear charge (n)b)Valence principal quantum number(n)c)Electron-electron interaction in the outer orbitalsd)None of the factor because their size is the sameCorrect answer is option 'A'. Can you explain this answer?
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