32. The first ionisation energy of gallium is greater than that of aluminum and the first ionisation energy of thallium is greater than that of indium. What could be the possible explanation for this? A. This is the normal trend in ionisation energy. B. Both Ga and Tl prefer to lose three electrons rather than one. C. Both Ga and Tl follow transition elements which are excellent shielders of nuclear charge. D. Ga follows a series of transition elements and TI follows both a series of transition elements and inner transition elements which are poor shielders of nuclear charge.

32. The first ionisation energy of gallium is greater than that of aluminum and the first ionisation energy of thallium is greater than that of indium. What could be the possible explanation for this? A. This is the normal trend in ionisation energy. B. Both Ga and Tl prefer to lose three electrons rather than one. C. Both Ga and Tl follow transition elements which are excellent shielders of nuclear charge. D. Ga follows a series of transition elements and TI follows both a series of transition elements and inner transition elements which are poor shielders of nuclear charge.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter7: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 89E: Write the expected ground-state electron configuration for the following. a. the element with one...

See similar textbooks

Similar questions

Which main group atom would be expected to have the lowest second ionization energy?
The radius trend and the ionization energy trend are exact opposites. Does this make sense?
Explain why Al is a member of group 13 rather than group 3?
Write the expected ground-state electron configuration for the following. a. the element with one unpaired 5p electron that forms a covalent compound with fluorine b. the (as yet undiscovered) alkaline earth metal after radium c. the noble gas with electrons occupying 4f orbitals d. the first-row transition metal with the most unpaired electrons
The changes in electron affinity as one goes down a group in the periodic table are not nearly as large as the variations in ionization energies. Why?
Compare the configurations below with two electrons located in p orbitals. Which would be the most stable (have the lowest energy)? Which would be the least stable? Explain your answers.
(a) Explain why the sizes of atoms change when proceeding across a period of the periodic table. (b) Explain why the sizes of transition metal atoms change very little across a period.
Answer the following questions about first ionization energies. (a) Generally ionization energies increase on proceeding across a period, but this is not true for magnesium (738 kJ/mol) and aluminium (578 kJ/mol). Explain this observation. (b) Explain why the ionization energy of phosphorus (1012 kJ/mol) is greater than that of sulphur (1000 kJ/mol) when the general trend in ionization energies in a period would predict the opposite.
What is the difference between core electrons and valence electrons? Why do we emphasize the valence electrons in an atom when discussing atomic properties? What is the relationship between valence electrons and elements in the same group of the periodic table?