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For which of the following species 2^(nd...

For which of the following species `2^(nd) IE lt 1^(st) IE`

A

`Be`

B

`Ne`

C

`Na^(+)`

D

None of these

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question "For which of the following species is the second ionization energy (IE) less than the first ionization energy?", we need to understand the concepts of ionization energy and the behavior of atoms when they lose electrons. ### Step-by-Step Solution: 1. **Understanding Ionization Energy**: - Ionization energy is the energy required to remove an electron from an atom or ion. The first ionization energy (1st IE) is the energy required to remove the first electron, while the second ionization energy (2nd IE) is the energy required to remove the second electron. 2. **General Trend**: - For any neutral atom, the first ionization energy is always less than the second ionization energy. This is because once the first electron is removed, the resulting cation has a smaller radius and a higher effective nuclear charge, making it harder to remove a second electron. 3. **Reasoning**: - When you remove the first electron, you create a positively charged ion (cation). This cation is smaller in size compared to the neutral atom due to the increased effective nuclear charge acting on the remaining electrons. As a result, the second ionization energy is always greater than the first. 4. **Conclusion**: - Therefore, there are no species for which the second ionization energy is less than the first ionization energy. The answer to the question is that none of the given species will satisfy the condition `2nd IE < 1st IE`. ### Final Answer: - None of these.
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Knowledge Check

  • Energy levels A, B, C of a certain atom corresponding to increasing values of energy i.e., E_(A) lt E_(B) lt E_(C) . If lambda_(1), lambda_(2), lambda_(3) are the wavelengths of radiations correspnding to the transitions C to B, B to A and C to A respectively, which of the following statements is correct?

    A
    `lambda_(3) = lambda_(1)+lambda_(2)`
    B
    `lambda_(1)+lambda_(2)+lambda_(3) = 0`
    C
    `lambda_(3)^(2) = lambda_(1)^(2)+lambda_(2)^(2)`
    D
    `lambda =(lambda_(1)lambda_(2))/(lambda_(1)+lambda_(2))`

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    Along the period (rarr) atomic // ionic radii and metallic character decreases while IE , EN , non-metallic character and oxidising power increases. Down the group (darr) , atomic // ionic radii, metallic character and reducing character increase while IE and EN decrease. However, Delta_(eg)H^(ɵ) becomes less negative down a group but more negative along a period. Which of the following isoelectronic species has lowest IE_(1) ?

    Which of the following molecules has the highest IE (i) Ne (ii) F

    Which of the following are isoelectronic species i.e, those having the same number of electrons? Na^(+),K^+, Mg^(+), Ca^(2+), S^(2-), Ar

    Consider the following values of I.E.(eV) for elements W and X: {:("Element",I.E_(1),I.E_(2),I.E_(3),I.E_(4)),(W,10.5,15.5,24.9,79.8),(X,8,14.8,78.9,105.8):} Other two element Y and Z hav outer electronic configuration ns^(2)np^(4) and ns^(2)np^(5) respectively. then according to given information which of the following compound(s) is/are not possible?

    Energy levels A,B,C of a certain atoms corresponding to increasing values of energy level i.e., E_(A) lt E_(B) lt E_(C) . If lambda_(1), lambda_(2) and lambda_(3) are the wavelengths of radiations corresponding to the transitions C to B,B to A and C to A respectively which of the following statement is correct?

    Which of the following statement is correct regarding following species? (i) Cl overset(E.A.)to Cl^(-) (ii) Cl^(-) overset(I.E.)to Cl (iii) Cl overset (I.E.) to Cl^+ (iv) Cl^(+) overset(I.E.)to Cl^(2+)

    Which among the following elements have lowest value of IE_1 ?

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