1 Answer ALL parts of this question.(a) Explain the following observations in first ionisation energies (IE1).(i)There is a large decrease in IE₁ between He and LI, Ne and Naand, Ar and K.IE: is lower for Al than Mg.IE₁ is lower than IE2.(ii)(iii)(b) Explain the trend in effective nuclear charge (Z) going from left to rightacross periods in the periodic table and with reference to Z*, rationalisewhy the ionic radii of the following anions decrease in the order shown:As > Se²> Br.

First ionization energy(IE1) is the energy required to remove the first electron from a gaseous…

Answer ALL parts of this question. (a) Explain the following observations in first ionisation energies (IE1₁). (i) There is a large decrease in IE1 between He and LI, Ne and Na and, Ar and K. (ii) (iii) IE₁ is lower for Al than Mg. IE₁ is lower than IE2. (b) Explain the trend in effective nuclear charge (Z) going from left to right across periods in the periodic table and with reference to Z", rationalise why the ionic radii of the following anions decrease in the order shown: As> Se²-> Br.

Answer ALL parts of this question. (a) Explain the following observations in first ionisation energies (IE1₁). (i) There is a large decrease in IE1 between He and LI, Ne and Na and, Ar and K. (ii) (iii) IE₁ is lower for Al than Mg. IE₁ is lower than IE2. (b) Explain the trend in effective nuclear charge (Z) going from left to right across periods in the periodic table and with reference to Z", rationalise why the ionic radii of the following anions decrease in the order shown: As> Se²-> Br.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter6: The Periodic Table And Atomic Structure

Section: Chapter Questions

Problem 6.82PAE: 6.82 A particular element has the following values for its first four ionization energies: 900,...

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