7.16 Consider the isoelectronic ions F and Nat. (a) Which ion issmaller? (b) Using Equation 7.1 and assuming that core elec-trons contribute 1.00 and valence electrons contribute 0.00to the screening constant, S, calculate Zeff for the 2p electronsin both ions. (c) Repeat this calculation using Slater's rules toestimate the screening constant, S. (d) For isoelectronic ions,how are effective nuclear charge and ionic radius related?

A. Na+ is the smallest as it has lost an electron from its outermost shell thereby pulled a bit more…

Answered: 7.16 Consider the isoelectronic ions F…

Chemistry

10th Edition

ISBN:9781305957404

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

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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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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
(1) What is the name of the element with a valence electron configuration of 2s22p3?fill in the blank 1(2) What is the name of the element with a valence electron configuration of 3s2?
Nitrogen has a greater first ionization energy than phosphorus. What is the best evidence to supportthis observation?
9. An element has the following first 5 ionization energies in MJ/mol: 0.7, 1.5, 2.1, 7.7, 10.5 Which group on the periodic table does this element likely belong to? Give your reasoning.
On the basis of periodic trends, determine the element in each pair with the higher first ionization energy (if possible).(a) Sn or I (b) Ca or Sr (c) C or P (d) F or S
Arrange in order of increasing ionization energy (a) the Group 1A elements Na, Cs, and K(b) the Period 4 elements As, Ca, and Br
(a)draw the orbital diagram for strontium ion(b) is this ion paramagnetic or diamagnetic explain (c) circle any electron and give the values for all four of its quantum numbers
3. a) Mg and Al are used as anode materials in X-ray Photoelectron Spectroscopy (XPS). Determine the energy of X-ray photons emitted by Mg and Al atoms when an electron from the 2nd shell fills a hole in the 1st shell and compare with the experimentally observed values for Mg Ka and Al Ka radiation given in the lecture. Use the Bohr model (without correction) when calculating the transition energy.
Select the group of the periodic table containing some elements with a condensed electron configuration of [X]ns2(n-1)dnp. Period Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display MAIN-GROUP ELEMENTS Metals (main-group) Metals (transition) MAIN-GROUP ELEMENTS Metals (inner transition). - 1A (1) 1 H 2A 1.008 (2) 3 4 2 LI Be Metalloids Nonmetals 8A (18) 2 ЗА 4A 5A 6A 7A He (13) (14) (15) (16) (17) 4.003 5 6 7 8 9 10 B C N F Ne 6.941 9.012 10.81 12.01 14.01 16.00 19.00 20.18 11 12 TRANSITION ELEMENTS 13 14 15 16 " w 3 Na Mg 38 4B 5B 68 7B 8B- 1B 2B AI Si P S 22.99 24.31 (3) (4) (5) (6) (7) (8) (9) (10) (11) 19 20 21 22 23 24 25 26 27 28 29 (12) 26.98 31 28.09 30.97 32.07 17 18 CI Ar 35.45 39.95 K Ca Sc Ti V Cr Mn Fe Co Ni 37 38 40 41 42 Zr Nb Mo 95.94 55 56 57 6 Cs Ba La 73 74 W 183.9 104 105 106 7 39.10 40.08 44.96 47.88 50.94 52.00 54.94 55.85 39 5 Rb Sr Y 85.47 87.62 88.91 91.22 92.91 72 Hf Ta 132.9 137.3 138.9 178.5 180.9 87 88 89 Fr Ra Ac Rf…
(a) Write the equation representing the 3rd ionization energy for Cr.(b) The electron affinity of K is 48 kJ/mol. Write the equation for which this is the energy change.
Knowing that atomic radius and ionization energy are two important properties of an atom that are periodic in nature. First, (i) define the term ionization energy. Then, (ii) state the directions along the periodic table (up, down, left, right) that a) atomic radius and b) ionization energy increase and (iii) explain the factors that lead to each of these trends.

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