Question
(d) Explain in terms of electrons, why potassium reacts more violently than sodium __
Answer
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Scarlett
Professional · Tutor for 6 years
Answer
All of the aforementioned reasons regarding atomic radius, placement of valence electrons, and ionization energy contribute to the violent reactivity of potassium compared to sodium in terms of their electron activity.
Explanation
Both potassium (K) and sodium (Na) reside within the alkali metals column of the periodic table. These metals exhibit reactivity with water, generating alkali (base) solutions, hydrogen gas, and heat as part of exothermic reactions. However, potassium has a more violent reaction with water compared to sodium arising from the following factors related to electron activity:1. Larger atomic radius: Potassium has a bigger atomic radius than sodium, meaning it has more electron shells. The larger radius allows for the further shielding of its outer shell from the forces of the nucleus. This, in turn, makes it easier to release valence electrons which can contribute to its reactivity potential. 2. Distant valence electrons: With potassium structurally having more electron shells, its valence electrons exist further from its nucleus. This diminishes the effective nuclear charge on the valence electrons, rendering it easier for these electrons to participate in chemical reactions.3. Lower ionization energy: Ionization energy refers to the necessary energy needed to extricate an electron from an atom. A lower ionization energy symbolizes less energy required to remove a valence electron, making it easier for that atom to react. Potassium has a lower ionization energy level than sodium.Therefore, the aforementioned reasons contribute to why potassium reacts more profoundly with water than sodium, influencing its differing chemotherapeutic characteristics.