Identify the element, using theelement symbol, represented bythis electron configuration:2 2 6 2 6101s 2s 2p 3s² 3p 4s² 3d 4p.Identify the element, using the element symbol, represented bythis electron configuration: 1s22s22p63s23p64s23d104p1.

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Answered: Identify the element, using the element…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter8: The Periodic Table: Structure And Trends

Section: Chapter Questions

Problem 8.89QE

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Similar questions

Arrange the following groups of atoms in order of increasing size. a. Rb, Na, Be b. Sr, Se, Ne c. Fe, P, O
Using orbital box diagrams, depict an electron configuration for each of the following ions: (a) Mg2+, (b) K+, (c) Cl, and (d) O2.
6.82 A particular element has the following values for its first four ionization energies: 900, 1760, 14, 850, and 21,000 kJ/mol. Without consulting a list of ionization energy values, determine what group in the periodic table this element belongs in.
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?
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 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
Describe the major trends that emerge when atomic radii are plotted against atomic number. Describe the trends observed when first ionization energies are plotted against atomic number.
(a) What element has the configuration 1s22s22p63s2ps? (b) Using spdf notation and an orbital box diagram, show the electron configuration of phosphorus.
Order the atoms in each of the following sets from the least negative electron affinity to the most. a. N, O, F b. Al, Si, P
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.
Which ion with a +1 charge has the electron configuration 1s22s22p63s23p63d104s24p6? Which ion with a —2 charge has this configuration?
Read the labels of several commercial products and identify monatomic ions of at least six main group elements contained in the products. Write the complete electron configurations of these cations and anions.

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Identify the element, using the element symbol, represented by this electron configuration: 2 2 6 2 6 10 1s 2s 2p 3s² 3p 4s² 3d 4p. Identify the element, using the element symbol, represented by this electron configuration: 1s22s22p63s23p64s23d104p1.