The closer the electron density is to the nucleus the _____ penetrating an orbital is

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To understand the statement, consider what “penetration” means in atomic orbitals: it refers to how much the electron density of a given orbital can extend toward the nucleus and experience the nucleus directly, as well as how effectively it can pass through the electron cloud of other electrons.
Option 1: "more". If the electron density is closer to the nucleus, the orbital has higher penetration. This is because electrons in orbitals with density near the nucleus have less shielding from inner electrons and can interact more directly with the nucleus. In general, s orbitals have their electron density concentrated closer to the nucleus and are said to penetrate more than p, d, or f orbitals. Therefore, closer electron density corresponds to greater penetration.
Option 2: "less". Claiming that closer electron density leads to less penetration contradicts the notion of penetration itself. The closer the density sits to the nucleus, the more the orbital penetrates, not less. Additionally, if an orbital density were further from the nucleus, it would be more shielded by other electrons and would exhibit lower penetration.
In summary, the idea that proximity of electron density to the nucleus increases an orbital’s penetration is consistent with fundamental concepts about penetration and shielding in atomic orbitals, while stating the opposite would conflict with those concepts.

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The closer the electron density is to the nucleus the _____ penetrating an orbital is

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