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Why the first ionisation enthalphy of so...

Why the first ionisation enthalphy of sodium is lower than that of magnesium while its second ionisation enthlpy is higher than that of magnesium ?

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The `1^(st)` ionization enthalphy of magnesium is higher than of Na due to higher nuclear charge and slightly smaller atomic radius of Mg than Na . After the loss of first electron , `Na^(+)` formed has the electronic configuration of neon (2,8) . The higher stability of the completely filled noble gas configuration leads to very high second ionization enthalpy for sodium.
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SURA PUBLICATION-PERIODIC CLASSIFICATION OF ELEMENTS-II. WRITE BRIEF ANSWER TO THE FOLLOWING QUESTIONS.
  1. Successive ionization energy values increase Why ?

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  2. Energy of an electron in the ground state of the hydrogen atom is -2....

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  3. The electronic configuration of atom is one of the important factor wh...

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  4. In what period and group will an element with Z=118 will be present?

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  5. Justify that the fifth period of the periodic table should have 18 el...

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  6. Elements a,b,c and d have the following electronic configurations: ...

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  7. Give the general electronic configuration of lanthanides and actides?

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  8. Why halogens act as oxidising agents?

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  9. Mention any two anomalous properties of second period elements.

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  10. Explain the pauling method for the determination os ionic radius.

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  11. Explain the periodic trend of ionisation potential.

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  12. Explain the diagonal relationship

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  13. Why the first ionisation enthalphy of sodium is lower than that of mag...

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  14. By using paulings method calculate the ionic radii of K^(+)andCl^(-) ...

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  15. Explain the following give appropriate reasons. (i) Ionisation po...

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  16. First ionisation potential of C- atom is greater than that of B atom ,...

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  17. The electron affinity values of Be, Mg are zero and those of N (0.02 e...

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  18. The formation of F^(-)(g) from F(g) is exothermic while that of O^(2-...

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  19. What is screening effect ?

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  20. Briefly give the basis for pauling's scale of electronegativity.

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