Two sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required.In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next leastenergy, and so on.ionizationenergyionizationenergyrequiredrequiredНе» He + eFr - Fr + e?В — в +eНе- He + e?TI" + ev ?TI -Br - Br + e1 (least)23 (most)>

Given that : We have to rank the following two sets of ionizations by the increasing amount of…

Answered: Two sets of ionizations are shown in…

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 158CWP

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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.
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.
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
Write the symbol of each element described below. (a) largest atomic radius in Group 1 (b) smallest atomic radius in period 3 (c) largest first ionization energy in Group 2 (d) most electronegative in Group 16 (e) element(s) in period 2 with no unpaired p electron (f) abbreviated electron configuration is [Ar] 4s23d3 (g) A +2 ion with abbreviated electron configuration [Ar]3d5 (h) A transition metal in period 4 forming a +2 ion with no unpaired electrons
Answer the questions below concerning ground state electron configurations. (a) What element has the electron configuration [Ar]3d64s2? (b) What element has a 2+ ion with the configuration [Ar]3d5? Is the ion paramagnetic or diamagnetic? (c) Mow many unpaired electrons are in a Ni2+ ion? (d) The configuration for an element is given here. What is the identity of the element? Is a sample of the element paramagnetic or diamagnetic? How many unpaired electrons does a 3 ion of this element have? (e) What element has the following electron configuration? Write a complete set of quantum numbers for electrons 1-3.
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?

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