(1) What is the valence electron configuration for the krypton atom? (2) What is the valence electron configuration for the silicon atom? (1) What is the name of the element with a valence electron configuration of 2s²2p4? (2) What is the name of the element with a valence electron configuration of 4s24p6? (1) The element with a valence electron configuration of 2s 2p is in group and period (2) The element with a valence electron configuration of 3s²3p2 is in group and period

(1) What is the valence electron configuration for the krypton atom? (2) What is the valence electron configuration for the silicon atom? (1) What is the name of the element with a valence electron configuration of 2s²2p4? (2) What is the name of the element with a valence electron configuration of 4s24p6? (1) The element with a valence electron configuration of 2s 2p is in group and period (2) The element with a valence electron configuration of 3s²3p2 is in group and period

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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using the concept of effective nuclear charge, can you explain the fact that I1 < I2 < I3 < I4 < I5?
All of the following statements concerning the characteristics of the halogens are true except which: a) The first ionization energies decrease as the atomic numbers of the halogens increase. b) Fluorine is the best oxidizing agent. c) Fluorine atoms have the smallest radii. d) Iodine liberates free bromine from a solution of bromide ion. e) Fluorine is the most electronegative of the halogens.
Each of the following sets contains isoelectronic ions (ions containing the same number of electrons). Select the set that shows the correct trend in increasing size or increasing ionic radius. (A) O2– < F– < Na+ < Mg2+ ; (B) F– < O2– < Mg2+ < Na+; (C) Mg2+ < Na+ < F– < O2–; (D) Mg2+ < Na+ < F– < O2–;
23. Tin (in group 14) can form both Sn²+ and Snª+ ions, but magnesium (in group 2) forms only Mg²+ ions. (a) Write condensed ground-state electron configurations for the ions Sn²+, Sn++, and Mg²+. (b) Which neutral atoms have ground-state electron configurations identical to Sn²+ and Mg²+? (c) Which 2+ ion is isoelectronic with Sn++?
1.) Which element would have the least favorable favorable (least negative) electron affinity? S, Si, Al, Cl 2.) Which equation below illustrates the first electron affinity for gallium?
Nitrogen (N), phosphorus (P), and arsenic (As) are three elements that almost universally form ions with –3 charge when they form compounds with metals. First, (i) write the full and core electron configurations for N, P, and As. Then, using those configurations, (ii) explain why those three elements all form ions with the same charge.
Describe and explain each of the following atomic properties of the representative group of elements in the periodic table: (a) The trends of atomic size left-to-right across period and top-to-bottom down the group; (b) The trends of ionization energy left-to-right across period and top-to-bottom down the group
Which element in the 2nd period would have the largest difference in energy between its 4th and 5th lonization Energy? O Boron Carbon Beryllium Nitrogen
Which of the following atoms and ions is (are) isoelectronic with Si: Ar, S2+, Ne, Al3+, P3−, As3+?
3. What is the effective nuclear charge on3(a) the outer two electrons of B? 3(b) the inner two electrons of B? 3(c) Explain the four ionization energies of B being 801, 2427, 3660 and 25025kJ/mol?
Can you answer part B
(a) Identify the following neutral elements by their condensed electron configurations. (Enter the chemical symbol or name of the element.) (i) [Ar] 4s2 3d3 (ii) [Kr] 5s2 4d10 5p3 (iii) [Ar] 4s2 3d10 4p4