Draw the partial (valence-level) orbital diagram and write the symbol, group number, and period number of the element with the following configuration: [Kr] 5s² 4d¹ Part 1 of 4 Partial (valence-level) orbital diagram: Part 2 of 4 Symbol: Part 3 of 4 Group number: Part 4 of 4 Period number: Energy X 1 レ S

Draw the partial (valence-level) orbital diagram and write the symbol, group number, and period number of the element with the following configuration: [Kr] 5s² 4d¹ Part 1 of 4 Partial (valence-level) orbital diagram: Part 2 of 4 Symbol: Part 3 of 4 Group number: Part 4 of 4 Period number: Energy X 1 レ S

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter6: The Periodic Table And Atomic Structure

Section: Chapter Questions

Problem 6.82PAE: 6.82 A particular element has the following values for its first four ionization energies: 900,...

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Which of the following statements is(are) true? a. F has a larger first ionization energy than does Li. b. Cations are larger than their parent atoms. c. The removal of the first electron from a lithium atom (electron configuration is ls2 2s1 ) is exothermic-that is, removing this electorn gives off energy. d. The He atom is larger than the H+ ion. e. The Al atorn is smaller than the Li atom.
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?
Does the information on alkali metals in Table 2-8 of the text confirm the general periodic trends in ionization energy and atomic radius? Explain.
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
Write the orbital diagram for (a) Li(b) P(c) F(d) Fe
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.
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.
Write an orbital diagram for the ground state of the zinc atom. Is the atomic substance diamagnetic or paramagnetic?
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
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
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
r Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For example, the second ionization energy is the energy to remove a second electron from an element. Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the 1s orbital. l> X Y First 170 200 second 350 400 Third 1800 3500 fouth 2500 5000 entify the elements X and Y. There may be more than one answer. so explain completely.

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