Sodium is strongly metallic while chlorine is strongly non-metallic. Which of the following statements supports the formation of a stable ionic salt NaCl from sodium and chlorine?
a)Low value of ionisation energy of sodium and low electron affinity of chlorine
b)Low value of ionisation energy of sodium and high electron affinity of chlorine
c)Low value of ionisation energy of chlorine and high electron affinity of sodium
d)High value of ionisation energy of chlorine and high electron affinity of sodium
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Explanation:
Among the four options given in question; the correct one is option B
Low value of ionisation energy of sodium and high electron affinity of chlorine
As we move from left to right in periodic table, the electron affinity increases hence Chlorine has higher electron affinity
Also as we move from top to bottom, the ionisation energy would increase, sodium being on top hence it has lesser ionisation energy
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The statement that supports formation of a stable ionic salt NaCl from sodium and chlorine b) Low value of ionization energy of sodium and high electron affinity of chlorine.
Explanation:
- Ionization energy is the minimum amount of energy required to remove the valence electron (loosely bound).
- Electron affinity is the amount of energy released when the electron is attached to the neutral atom.
Na + Cl → NaCl
NaCl → Na⁺ + Cl⁻
- The attractive force between two ions are more, thus it forms a stable ionic bond.
- The high electron affinity of chlorine forms ions and low value of ionization energy of sodium makes the reaction stop with NaCl.
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