t t t Which one of the following atoms characterized by these electron configurations would have the greatest electron affinity? O1s22s22p63s23p2 O1s22s22p63s23p6 01s22s22p5 01s22s22p4 O1s22s22p63s23p4

t t t Which one of the following atoms characterized by these electron configurations would have the greatest electron affinity? O1s22s22p63s23p2 O1s22s22p63s23p6 01s22s22p5 01s22s22p4 O1s22s22p63s23p4

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 105AP

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The successive ionization energies for an unknown element are I1 = 896 kJ/mol I2 = 1752 kJ/mol I3 = 14,807 kJ/mol I4 = 17,948 kJ/mol To which family in the periodic table does the unknown element most likely belong?
The electron affinity of the lutetium atom (element 71) was measured using the technique of photoelectron spectroscopy with an infrared laser (the essay on p. 310 describes this instrumental method, using X rays). In this experiment, a beam of lutetium negative ions, Lu, was prepared and irradiated with a laser beam having a wavelength at 1064 nm. The energy supplied by a photon in this laser beam removes an electron from a negative ion, leaving the neutral atom. The energy needed to remove the electron from the negative ion to give the neutral atom (both in their ground states) is the electron affinity of lutetium. Any excess energy of the photon shows up as kinetic energy of the emitted electron. If the emitted electron in this experiment has a kinetic energy of 0.825 eV, what is the electron affinity of lutetium?
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.
Which of the following represents the change in electron configuration that is associated with the first ionization of strontium? a) [Kr]5s15p1 → [Kr]5s1 + e- b) [Kr]5s2 + e- → [Kr]5s25p1 c) [Kr]5s2 → [Kr]5s15p1 d) [Kr]5s2 → [Kr]5s1 + e-
Which is the correct electronic configuration for X (atomic number 34) in the ground state? 1s22s22p63s23p63d104s04p6 1s22s22p63s23p63d104s24p4 1s22s22p63s23p64s24d104p4 1s22s22p63s23p63d104s03p6
An element has 19 electrons in its neutral state. What is the ground state electron configuration of the ion that it would form? о 1s²2s²2p63s²3p6 1s²2s²2p63s23p64s² 1s²2s22p63s23p64s² 1s22s22p63s23p64s²3d²
Given the following electron configurations: I) 1s²2s²2p63s²3p6 II) 1s22s²2p 3s² III) 1s²2s²2p63s¹ Which one shows the smallest second ionization energy? OI and II 01 OII and III O III O II 4
Match the full and abbreviated electron configurations for the following atoms: 1s22s22p6 [Ne] [Ar] 1s22s22p63s23p6 [Ne] 3s23p1 1s22s22p63s23p1 1. Al (full electron configuration) 2. Al (abbreviated electron configuration) 3. S2- (full electron configuration) 4. S2- (abbreviated electron configuration) 5. Na+ (full electron configuration) 6. Na+ (abbreviated electron configuration)
Which ion with a +1 charge has the electron configuration 1s22s22p63s23p63d104s24p6? Which ion with a –2 charge has this configuration?
Written below are the electron configurations of of five different atomic species: A: 1s22s22p63s1 B: 1s22s22p3 C: 1s22s22p63s23p63d10 D: 1s22s22p63s23p64s23d10 E: 1s22s22p63s23p64s23d104p4 Which configuration is representative of a transition metal cation?
Which of the following is a correct electron configuration notation? Ca2+-1s22s22p63s23p64s2 F-1s22s22p6 O2--1s22s22p2 Te-1s22s22p63s23p64s23d104p65s24d105p5 Sb-1s22s22p63s23p64s23d104p65s24d105p3
What is the symbol for the atom that has the electron configuration 1s22s22p63s23p64s23d104p65s24d2?