Consider the following data regarding arsenic: IE 947 kJ/mol IE3 2735 kJ/mol IE2= 1798 kJ/mol EA, -78 kJ/mol Which of the following statement is true? A. The 1st electron affinity of As is 1798 kJ/mol of energy absorbed B. The 2nd ionization energy of As is 2735 kJ/mol of energy released The 2nd electron affinity of As3 is 1798 kJ/mol of energy released C. The 2nd ionization energy of As is 947 kJ/mol of energy released D. The 2nd electron affinity of As is 78.1 kJ/mol of energy absorbed E.

Consider the following data regarding arsenic: IE 947 kJ/mol IE3 2735 kJ/mol IE2= 1798 kJ/mol EA, -78 kJ/mol Which of the following statement is true? A. The 1st electron affinity of As is 1798 kJ/mol of energy absorbed B. The 2nd ionization energy of As is 2735 kJ/mol of energy released The 2nd electron affinity of As3 is 1798 kJ/mol of energy released C. The 2nd ionization energy of As is 947 kJ/mol of energy released D. The 2nd electron affinity of As is 78.1 kJ/mol of energy absorbed E.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter2: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 11ALQ: Consider the following statement "The ionization energy for the potassium atom is negative, because...

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Similar questions

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?
6.80 Describe how valence electron configurations account for some of the similarities in chemical properties among elements in a group.
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?
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.
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.
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
The outermost electron in an alkali-metal atom is sometimes described as resembling an electron in the corresponding state of a one-electron atom. Compare the first ionization energy of lithium with the binding energy of a 2s electron in a one-electron atom that has nuclear charge Zeff , and determine the value of Zeff that is necessary for the two energies to agree. Repeat the calculation for the 3s electron of sodium and the 4s electron of potassium.
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.

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