7.21 Specify the group of the periodic table in whicheach of the following elements is found: (a) [Ne]3s',(b) [Ne]3s°3p', (c) [Ne]3s°3p°, (d) [Ar]4s²3ď.

Electrons are filled in this order The outer electron configuration of the elements in group 1A is…

Answered: 7.21 Specify the group of the periodic…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 142QRT

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2. Given their electron configurations, identify the following elements and specify in what group of the periodic table do they belong: (a) [A13d104s24p4(b) [Rn]7s²(c) [Kr]4d10(d) [A]4s²3d8 3. Group the species that are isoelectronic: Be2+, F, Fe2+, N³-, He, S2', Co3+, Ar. 4. Two atoms have the electron configurations 1s2s2p6 and 1s22s2p63s1. The first ionization energy of one is 2080 kJ/mol, and that of the other is 496 kJ/mol. Pair each ionization energy with one of the given electron configurations. Justify your choice. 5. The bonds in beryllium hydride (BeH2) molecules are polar, and yet the dipole moment of the molecule is zero. Explain. 6. Predict and draw the molecular geometries (show bond angles) for these molecules: a. BH3 b. BrCl3 c. CF4
From the following partial (valence-level) orbital diagrams, write the condensed electron configurations and the respective group numbers. (Type your answer using the format [Ar] 4s2 3d10 4p2 for [Ar]4s23d104p2.) (a) 1 |个|↑|个|个 5s 4d 5p (b) T 个|个 2s 2p (a) electron configuration group number (b) electron configuration group number
Group 4A elements have much more negative electronaffinities than their neighbors in groups 3A and 5A (seeFigure 7.12). Which of the following statements best explainsthis observation? (i) The group 4A elements have much higherfirst ionization energies than their neighbors in groups 3Aand 5A. (ii) The addition of an electron to a group 4A elementleads to a half-filled np3 outer electron configuration.(iii) The group 4A elements have unusually large atomic radii.(iv) The group 4A elements are easier to vaporize than arethe group 3A and 5A elements.
(a) As we go down the periodic table, which subshell is filled first, the 3d or the 4s subshell? (b) Which electronic configuration has a lower energy, [Ar]3d44s2 or [Ar]3d54s1? Note: The notation [Ar] represents the filled configuration for argon. Suggestion: Which has the greater number of unpaired spins? (c) Identify the element with the electronic configuration in part (b).
Give the ground-state electron configurations of the fol- lowing elements: (a) C (b) Se (c) Fe
Use electron configurations to explain the following observations:(a) The first ionization energy of phosphorus is greaterthan that of sulfur. (b) The electron affinity of nitrogen islower (less negative) than those of both carbon and oxygen.(c) The second ionization energy of oxygen is greater thanthe first ionization energy of fluorine. (d) The third ionizationenergy of manganese is greater than those of both chromiumand iron.
On the basis of periodic trends, choose the more metallic element from each pair (if possible).(a) Sn or Te(b) P or Sb(c) Ge or In(d) S or Br
3. Which one of each of the following pairs has the higher electron affinity? Explain in detail for each case. (a) C or F (b) F or I (c) Te or I (d) O or S (e) S or Se
Using complete subshell notation (1s^22s^22p^6, and so forth), predict the electron configurations of the following ions. (a) N3– (b) Ca2+ (c) S– (d) Cs2+ (e) Cr2+ (f) Gd3+
Identify each element below, and give the symbols of the other elements in its group:(a) [Ar] 4s²3d¹⁰4p⁴(b) [Xe] 6s²4f¹⁴5d²(c) [Ar] 4s²3d⁵
54.Using complete subshell notation (1s22s22p6, and so forth), predict the electron configurations of the following ions. (a) N3– (b) Ca2+ (c) S– (d) Cs2+ (e) Cr2+ (f) Gd3+
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7.21 Specify the group of the periodic table in which each of the following elements is found: (a) [Ne]3s', (b) [Ne]3s°3p', (c) [Ne]3s°3p°, (d) [Ar]4s²3ď.