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The large decrease in electron affinity between lithium (Li) and beryllium (Be), despite the…

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Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 108QRT

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Similar questions

What is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.
An ion M2+ has the configuration [Ar]3d2, and an atom has the configuration [Ar]4s2. Identify the ion and the atom.
Atoms of Group 1 elements have the lowest first ionization energy of all the elements on the periodic table but subsequently have the largest increase between the first and second ionization energy that any other elements have. Explain why this is the case, based on the electronic structure of the atoms/ions.
Elements on the left side of the periodic table are more likely to form positive ions than those on the right. Use the trend in the ionization energy of the elements to explain this observation.
All of the following statements concerning the characteristics of the halogens are true except which: a) The first ionization energies decrease as the atomic numbers of the halogens increase. b) Fluorine is the best oxidizing agent. c) Fluorine atoms have the smallest radii. d) Iodine liberates free bromine from a solution of bromide ion. e) Fluorine is the most electronegative of the halogens.
Write the full electron configuration of the Period 2 element with the following successive IEs (in kJ/mol): IE1 = 801 IE2= 2427 IE3 = 3659 IE4= 25,022 IE5 = 32,822
Both the electron affinity and the ionization energy of chlorine are higher than the corresponding quantities for sulfur. Explain why in terms of the electronic structure of the atoms.
The gadolinium +3 ion (Gd3+) has advantageous magnetic properties for Magnetic Resonance Imaging (MRI) applications, specifically a high number of unpaired electrons. In fact, both neutral Gd and Gd3+ have a set of degenerate orbitals with seven unpaired electrons. a) Write the electron configuration for Gd and Gd3+ using the condensed noble gas notation. Identify which orbitals lose electrons to yield the +3 cation based on the above information. Explain your reasoning (2-3 sentences). b) Curium (Cm) is an actinide element named for Marie Curie. Cm is in the same group as Gd and also forms a +3 cation. Write the electron configuration for Cm and Cm3+. c) While +3 is the most common oxidation state for lanthanide elements, some can form +2 ions. Identify an isoelectronic ion to Gd3+ that has a +2 oxidation state and indicate which orbitals lose electrons to form that ion.
In one area of Australia, the cattle did not thrive despite the presence of suitable forage. An investigation showed the cause to be the absence of sufficient cobalt in the soil. Cobalt forms cations in two oxidation states, Co2+and Co3+. Write the electron structure of the two cations.
it is clear that the first ionization energy of He is very large. Would you expect the first ionization energy of H– (hydride ion) to be larger, smaller, or about the same as the first ionization energy of He, and why?
Write the full electron configuration of the period 2 element with the following successive ionization energies (kJ/mol): IE1 = 801 IE2 = 2427 IE3 = 3659 IE4 = 25, 022 IE5 = 32,822
5) Give the name and symbols for three ions that are isoelectronic with an unknown element whose electron configuration is [ Kr] 5s², 4d¹0, 5p6. 6) Give the box orbital diagram for the ground state configuration of barium. 7) Give the name and symbols for two ions that are isoelectronic with selenium ion. 8) Find the possible values for the quantum numbers of the highest energy electron meaning that outermost valence electron. a. Gallium b. Rubidium c. Sodium

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Account for the large decrease in electron affinity between lithium and beryllium despite the increase in nuclear charge.