The first ionisation potential of Na, Mg, Λl and Si (1) Na Λl Mg>Λl>Si (3) Na>Mg<Λl

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The first ionisation potential of Na, Mg, Λl and Si (1)...

The first ionisation potential of $\mathrm{Na}, \mathrm{Mg}, \Lambda \mathrm{l}$ and Si (1) $\mathrm{Na}<\mathrm{Mg}>\Lambda \mathrm{l}<\mathrm{Si}$ (2) $\mathrm{Na}>\mathrm{Mg}>\Lambda \mathrm{l}>\mathrm{Si}$ (3) $\mathrm{Na}>\mathrm{Mg}<\Lambda \mathrm{l}>\mathrm{Si}$ (4) $\mathrm{Na}>\mathrm{Mg}>\mathrm{Al}>\mathrm{Si}$

The first ionisation potential of $\mathrm{Na}, \mathrm{Mg}, \Lambda \mathrm{l}$ and Si
(1) $\mathrm{Na}<\mathrm{Mg}>\Lambda \mathrm{l}<\mathrm{Si}$
(2) $\mathrm{Na}>\mathrm{Mg}>\Lambda \mathrm{l}>\mathrm{Si}$
(3) $\mathrm{Na}>\mathrm{Mg}<\Lambda \mathrm{l}>\mathrm{Si}$
(4) $\mathrm{Na}>\mathrm{Mg}>\mathrm{Al}>\mathrm{Si}$

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Key Concepts

Periodic Trends

Periodic trends describe the systematic variations in many properties of the elements across the periodic table. For ionization energy, the trend generally increases from left to right within a period due to an increase in effective nuclear charge and decreases from top to bottom within a group due to increased electron shielding and larger atomic radii, although exceptions occur due to specific electron configurations.

Ionization Potential

Ionization potential (or ionization energy) is the energy required to remove an electron from an isolated gaseous atom or ion. It is a fundamental property that reflects the attraction between the nucleus and the outermost electron, and differences in ionization potential can be explained by factors such as nuclear charge, electron shielding, and distance of the electron from the nucleus.

Electron Configuration Effects

Electron configuration plays a crucial role in determining an element's ionization energy. Stability associated with filled or half-filled subshells can lead to deviations from the general periodic trend. In particular, slight variations in electron-electron repulsions and orbital energies can cause anomalies in the ordering of ionization energies, as seen when comparing elements with similar electronic shells.

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