Which of the following best explains why the $1s$ peak in the photoelectron spectrum of oxygen appears at a higher binding energy than the $1s$ peak in the photoelectron spectrum of nitrogen?

A) Oxygen has a greater nuclear charge than nitrogen, resulting in a stronger electrostatic attraction between the nucleus and the $1s$ electrons.

B) Oxygen experiences less electron-electron repulsion among its core electrons, decreasing the energy required to eject a $1s$ electron.

C) Nitrogen possesses a half-filled $2p$ subshell, which confers anomalous stability that decreases the binding energy of its $1s$ electrons.

D) Oxygen has more valence electrons than nitrogen, which shield the core electrons and increase the effective nuclear charge.

Photoelectron spectroscopy Knowledge-Based Practice

Chemistry · Atomic Structure · Chemistry · Electrons in Atoms

1 Chemistry practice questions on Photoelectron spectroscopy. Questions that assess core concepts and understanding.

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Atomic Structure · Chemistry

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