The electron affinity of an element is typically defined as the energy change for the choose your answer... of an electron for choose your answer... in the choose your answer... phase. Its value is usually negative. The more negative the value, the choose your answer. the affinity of the element for the electron.

The electron affinity of an element is typically defined as the energy change for the choose your answer... of an electron for choose your answer... in the choose your answer... phase. Its value is usually negative. The more negative the value, the choose your answer. the affinity of the element for the electron.

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 37A

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Based on their positions in the periodic table, list the following ions in order of increasing radius: K+, Ca2+, Al3+, Si4+.
lement X, which has a valence shell configuration of ns2np4 , was isolated in a laboratory. Which of the following statements is(are) true concerning element X? Element X has chemical properties similar to those of the halogens. Element X has six valence electrons. When element X is reacted with calcium, the compound formed would most likely have the formula Ca2X . Element X needs to gain two electrons to attain a noble gas electron configuration. mg src=Images/HTML_99425-11-106AP_image001.jpg alt="" align="top"/>
The energy needed to remove one electron from a gaseous potassium atom is only about two-thirds as much as that needed to remove one electron from a gaseous calcium atom, yet nearly three times as much energy as that needed to remove one electron from K+ as from Ca+ . What explanation can you give for this contrast? What do you expect to be the relation between the ionization energy of Ca+ and that of neutral K?
Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and an orbital (as described by the more modern, wave mechanical picture of the atom).
The first ionization energy of helium is 2370kJmol1 , the highest for any element. (a) Define ionization energy and discuss why for helium it should be so high. (b) Which element would you expect to have the highest second ionization energy? Why? (c) Suppose that you wished to ionize some helium by shining electromagnetic radiation on it. What is the maximum wavelength you could use?
Atoms of which group in the periodic table have a valence shell electron configuration of ns2np2?
Which atom and/or ion is (are) isoelectronic with Br+:Se2+,Se,As,Kr,Ga3+,Cl?
Section 11.6 uses a "firefly" analogy to illustrate how the wave mechanical modal for the atom differs from Bohr’s. model. Explain this analogy.
In each of the following sets of elements, which element would he expected to have the highest ionization energy? msp;a.Cs,K,Lic.l,Br,Clb.Ba,Sr,Cad.Mg,Si,S
Consider the following statement "The ionization energy for the potassium atom is negative, because when K loses an electron to become K +, it achieves a noble gas electron configuration." Indicate everything that is correct in this statement. Indicate everything that is incorrect. Correct the incorrect information and explain.
Which of the following atoms and ions is (are) isoelectronic with S2+:Si4+,Ar,As3+,Si,Al3+?
The following statements either define or are closely related to the terms periodic law, period, and group. Match the terms to the appropriate statements. a. This is a horizontal arrangement of elements in the periodic table. b. Element 11 begins this arrangement in the periodic table. c. The element nitrogen is the first member of this arrangement. d. Elements 9, 17, 35 and 53 belong to this arrangement.