out of sodium and potassium which will have stronger metallic character and why ?
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Metallic character depends upon ionization energy. Ionization energy is the minimum required energy to remove most loosely bounded electron from the outermost shell of an isolated gaseous atom in its neutral state.
It is an endothermic process. Hence ionization enthalpy is positive.
Ionization enthalpy depends on many factors but for your question it can be understood easily with one factor i.e. Atomic radius. On going down the group from Na to K, the atomic radius increases, as a result nucleus attraction on outermost electron decreases as distance from nucleus increases, so less energy is required to remove outermost electron from K as compared to Na.
Therefore K has more electropositive nature (tendency to form cation easily) than Na, i.e.
It is an endothermic process. Hence ionization enthalpy is positive.
Ionization enthalpy depends on many factors but for your question it can be understood easily with one factor i.e. Atomic radius. On going down the group from Na to K, the atomic radius increases, as a result nucleus attraction on outermost electron decreases as distance from nucleus increases, so less energy is required to remove outermost electron from K as compared to Na.
Therefore K has more electropositive nature (tendency to form cation easily) than Na, i.e.
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potassium will have more metallic character according to its position in modern periodic table as we know that in a group the metallic character increases as we move from top to bottom and potassium lies below aodium
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