Order the electrons in the following orbitals according to their shielding ability: 4s, 4d, 4f.

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Understand the concept of electron shielding: Electron shielding refers to the ability of inner electrons to reduce the effective nuclear charge felt by outer electrons. Electrons in inner orbitals shield outer electrons from the full charge of the nucleus.

Recall the order of orbitals based on their principal quantum number and azimuthal quantum number: The principal quantum number (n) indicates the energy level, while the azimuthal quantum number (l) indicates the shape of the orbital. For the given orbitals, 4s (l=0), 4d (l=2), and 4f (l=3).

Recognize that the shielding ability of an electron is influenced by its penetration and distance from the nucleus: Electrons in orbitals with lower azimuthal quantum numbers (l) generally have greater penetration and are closer to the nucleus, thus providing more effective shielding.

Compare the orbitals based on their azimuthal quantum numbers: The 4s orbital (l=0) has the lowest azimuthal quantum number, followed by 4d (l=2), and then 4f (l=3). Therefore, 4s electrons have the greatest shielding ability, followed by 4d, and then 4f.

Order the orbitals based on their shielding ability: Based on the analysis, the order from greatest to least shielding ability is 4s > 4d > 4f.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electron Shielding

Electron shielding refers to the phenomenon where inner electrons partially block the attractive force of the nucleus on outer electrons. This effect influences the energy levels of electrons in different orbitals, as electrons in inner shells can reduce the effective nuclear charge experienced by outer electrons, affecting their energy and stability.

Orbital Energy Levels

Orbitals are regions in an atom where electrons are likely to be found, and they have different energy levels based on their shape and distance from the nucleus. The order of energy levels typically follows the Aufbau principle, where electrons fill lower-energy orbitals (like 4s) before higher-energy ones (like 4d and 4f), impacting their shielding ability.

Order of Orbital Shielding Ability

The shielding ability of orbitals increases with their angular momentum and principal quantum number. In the case of 4s, 4d, and 4f orbitals, the 4s orbital has the highest shielding ability due to its lower energy and proximity to the nucleus, while the 4f orbital has the lowest shielding ability because it is more complex and further from the nucleus, leading to less effective shielding.

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