Lowest ionisation enthalpy in periods is shown by: (a) inert gases □(b) halogens □(c) alkali met

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Lowest ionisation enthalpy in periods is shown by: (a) inert...

Key Concepts

Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by electrons in an atom. It increases across a period as electrons are added to the same shell and the nucleus becomes more positively charged. This higher effective nuclear charge holds electrons more tightly, which is why elements toward the right side of the period typically have higher ionisation energies.

Alkali Metals

Alkali metals, which occupy the first group of the periodic table, have a very low ionisation enthalpy. This is due to their large atomic size and a single valence electron that is weakly held by the nucleus, making it relatively easy to remove compared to other elements in the same period.

Periodic Trends

Periodic trends describe the patterns in properties observed as one moves across periods or down groups in the periodic table. For ionisation enthalpy, there is an increasing trend from left to right within a period because the effective nuclear charge increases while atomic size decreases, making it harder to remove an electron.

Ionisation Enthalpy

Ionisation enthalpy (or ionisation energy) is the amount of energy required to remove an electron from a gaseous atom. It is influenced by factors such as the distance of the electron from the nucleus, nuclear charge, and electron shielding. This concept is fundamental for understanding reactivity and the periodic behavior of elements.

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