Which of the following statements is INCORRECT regarding ionization energy? a. Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value. b.lonization energy increases for each successive electron being removed. c.In the same period, the second ionization energy of a group 1A element is higher than the second ionization energy of a group 2A element. d.The greatest increase in ionization energy is experienced on removal of electron from core noble gas configuration

Which of the following statements is INCORRECT regarding ionization energy? a. Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value. b.lonization energy increases for each successive electron being removed. c.In the same period, the second ionization energy of a group 1A element is higher than the second ionization energy of a group 2A element. d.The greatest increase in ionization energy is experienced on removal of electron from core noble gas configuration

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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Similar questions

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.
Write electron configurations for the following elements. a. The Group III A element in the same period as 4Be b. The Period 3 element in the same group as 5B c. The lowest-atomic-numbered metal in Group IIA d. The two Period 3 elements that have no unpaired electrons
An unknown element is a nonmetal and has a valence electron configuration of ns2np4 a. How many valence electrons does this element have? b. What are some possible identities for this element? c. What is the formula of the compound this element would form with potassium? d. Would this element have a larger or smaller radius than barium? e. Would lhis element have a greater or smaller ionization energy than fluorine?
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.
Which main group atom would be expected to have the lowest second ionization energy?
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
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
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.

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