The low value of the first ionization energy of Ag is attributed to... the high atomic radius and availability of a single 5s electron .b the high atomic radius and absence of electrons in Ss orbital the small atomic radius and availability of a single 5s electron the small atomic radius and absence of electrons in 5s orbital

The low value of the first ionization energy of Ag is attributed to... the high atomic radius and availability of a single 5s electron .b the high atomic radius and absence of electrons in Ss orbital the small atomic radius and availability of a single 5s electron the small atomic radius and absence of electrons in 5s orbital

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 102QRT

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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?
Cesium is used extensively in photocells and in television cameras because it has the lowest ionization energy of all the stable elements. (a) What is the maximum kinetic energy of a photoelectron ejected from cesium by 520 nm light? Note that if the wavelength of the light used to irradiate the cesium surface becomes longer than 660 nm, no photoelectrons are emitted. (b) Use the rest mass of the electron to calculate the velocity of the photoelectron in (a).
For each of the following pairs of atoms or ions, state which you expect to have the larger radius. (a) Na or K (b) Cs or Cs+ (c) Rb+ or Kr (d) K or Ca (e) Cl or Ar
6.80 Describe how valence electron configurations account for some of the similarities in chemical properties among elements in a group.
Chromium(IV) oxide is used in making magnetic recording tapes because it is paramagnetic. It can be described as a solid made up of Cr4+ and O2 . Give the electron configuration of Cr4+ in CrO2 , and determine the number of unpaired electrons on each chromium ion.
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.
Consider the following ionization energies for aluminum: Al(g)Al+(g)+eI1=580kJ/molAl+(g)Al2+(g)+eI2=1815kJ/molAl2+(g)Al3+(g)+eI3=2740kJ/molAl3+(g)Al4+(g)+eI4=11,600kJ/mol a. Account for the trend in the values of tbe ionization energies. b. Explain the large increase between I3 and I4
The first ionization energies of As and Se are 0.947 and 0.941 MJ/mol, respectively. Rationalize these values in terms of electron configurations.
Identify the atom or ion corresponding to each of the following descriptions: (a) an atom with ground-state electron configuration [Kr]4d105s25p1 (b) an ion with charge 22 and ground-state electron configuration [Ne]3s23p6 (c) an ion with charge +4 and ground-state electron configuration [Ar]3d3
Periodic Properties I A hypothetical element, X, has the following ionization energy values: First ionization energy: 900 kJ/mol Second ionization energy: 1750 kJ/mol Third ionization energy: 14,900 kJ/mol Fourth ionization energy: 21,000 kJ/mol Another element, Y, has the following ionization energy values: First ionization energy: 1200 kJ/mol Second ionization energy: 2500 kJ/mol Third ionization energy : 19,900 kJ/mol Fourth ionization energy: 26,000 kJ/mol a To what family of the periodic table would element X be most likely to belong? Explain? b What charge would you expect dement X to have when it forms an ion? c If you were to place elements X and Y into the periodic table, would element Y be in the same period as element X? If not in the same period, where might they be relative to each other in the periodic table? d Would an atom of Y be smaller or larger than an atom of X? Explain your reasoning.
Before the element scandium was discovered in 1879, it was known as “eka-boron.” Predict the properties of scandium from averages of the corresponding properties of its neighboring elements in the periodic table. Compare your predictions with the observed values in Appendix F.

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