Question

imagine an electron in the 4d orbital of a neutral atom. decide how well each of the other electrons in the table below would screen this electron from the

Explanation:

Step1: Understand screening effectiveness

Screening effectiveness depends on the distance of the electron from the nucleus and the type of orbital. Electrons in lower - energy, more penetrating orbitals (like \(s\) orbitals) are closer to the nucleus and can screen more effectively.

Step2: Analyze each electron

• Electron in \(2s\) orbital: The \(2s\) orbital is closer to the nucleus compared to \(4s\), \(2p\), and \(4d\) orbitals. \(s\) orbitals have a higher probability of being close to the nucleus (more penetrating), so an electron in \(2s\) will screen the \(4d\) electron very effectively.
• Electron in \(4s\) orbital: \(4s\) is farther from the nucleus than \(2s\), but \(s\) orbitals are still more penetrating than \(p\) and \(d\) orbitals. So it will screen the \(4d\) electron effectively.
• Electron in \(2p\) orbital: \(p\) orbitals are less penetrating than \(s\) orbitals. The \(2p\) electron is at a similar principal quantum level (\(n = 2\)) as \(2s\), but due to lower penetration, it will screen the \(4d\) electron moderately.
• Electron in another \(4d\) orbital: \(d\) orbitals are the least penetrating. An electron in \(4d\) (same type of orbital) will screen the \(4d\) electron the least effectively as they are in the same outer - shell and have poor penetration.

Answer:

An electron in a \(2s\) orbital > An electron in a \(4s\) orbital > An electron in a \(2p\) orbital > An electron in another \(4d\) orbital.