Consider the following ionization reactions : Reactions IE (i) X ( g ) → X + ( g ) + e ⊖ X 1 (ii) Y ( g ) → Y ( g ) + + e ⊖ Y 1 (iii) Y + ( g ) → Y + 2 ( g ) + e ⊖ Y 2 (iv) Z ( g )

Question

Consider the following ionization reactions :

Reactions	IE
(i) $X_{(g)} \to X^{+}_{(g)} + e^{⊖}$	$X_{1}$
(ii) $Y_{(g)} \to Y_{(g)}^{+} + e^{⊖}$	$Y_{1}$
(iii) $Y^{+}_{(g)} \to Y^{+ 2}_{(g)} + e^{⊖}$	$Y_{2}$
(iv) $Z_{(g)} \to Z_{(g)}^{+} + e^{⊖}$	$Z_{1}$
(v) $Z^{+}_{(g)} \to Z^{+ 2}_{(g)} + e^{⊖}$	$Z_{2}$
(vi) $Z^{+ 2}_{(g)} \to Z^{+ 3}_{(g)} + e^{⊖}$	$Z_{3}$

if X⁺ , Y⁺² and Z⁺³ ion have zero electron. (where X, Y & Z are belongs to upto 2^nd period) Select the CORRECT order(s) of corresponding IE.

TestHub · Accepted Answer

Based on the condition that X + , Y 2 + , and Z 3 + have zero electrons, the elements are identified as X = H ( Z = 1 ), Y = He ( Z = 2 ), and Z = L i ( Z = 3 ). For Option A: First ionization energy follows the order He > H > L i due to noble gas stability and smaller atomic size, so Y 1 ​ > X 1 ​ > Z 1 ​ is correct. For Option C: Z 3 ​ ( L i 2 + ), Y 2 ​ ( H e + ), and X 1 ​ ( H ) are hydrogen-like species where I E ∝ Z 2 , meaning Z 3 ​ > Y 2 ​ > X 1 ​ ( 122.4 e V > 54.4 e V > 13.6 e V ) is correct. For Option D: Successive ionization energies always increase ( Z 3 ​ > Z 2 ​ ), and since L i + ( Z 2 ​ = 75.6 e V ) has a higher nuclear charge than H e + ( Y 2 ​ = 54.4 e V ), Z 3 ​ > Z 2 ​ > Y 2 ​ is correct.

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Options:(select one or more)

Doubts & Discussion