Two elements 1 and 2 are in the same row of the periodic table but not next to each other. Element 1 has a larger atomic radius than element 2, which of the following are most likely to be true about their relative ionization energies and why? 1. Element 1 has a larger ionization energy 2. Element 2 has a larger ionization energy 3. They both have the same ionization energy Because 1. electrons in element 1 are more strongly attracted to the nucleus 2. electrons in element 2 are more strongly attracted to the nucleus 3. electrons are being removed from the same quantum shell O O O O O 1,3 O 2,3 O 3,2 O 3,3

Two elements 1 and 2 are in the same row of the periodic table but not next to each other. Element 1 has a larger atomic radius than element 2, which of the following are most likely to be true about their relative ionization energies and why? 1. Element 1 has a larger ionization energy 2. Element 2 has a larger ionization energy 3. They both have the same ionization energy Because 1. electrons in element 1 are more strongly attracted to the nucleus 2. electrons in element 2 are more strongly attracted to the nucleus 3. electrons are being removed from the same quantum shell O O O O O 1,3 O 2,3 O 3,2 O 3,3

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...

See similar textbooks

Similar questions

Write the condensed electron configuration for antimony, Sb. b. Antimony can have a valence of -3, +3, or +5. Use the condensed electron configurations of each to explain how each of these valences might form.
Number 6 please
Predict which element has the larger first ionization energy based on periodic trends. cannot be determined based on periodic trends Cs Sr Predict which element has the larger first ionization energy based on periodic trends. P cannot be determined based on periodic trends Predict which element has the larger first ionization energy based on periodic trends. Se Cl cannot be determined based on periodic trends Predict which element has the larger first ionization energy based on periodic trends. N S
Rank the following elements according to atomic size using periodic trends from smallest to largest. B, Ne, Li, N
9. As a general trend, as we go across a period we find that ionization energy increases. What is ionization energy, Explain why oxygen has a lower ionization energy than nitrogen.
Compare the following two elements, identified by their electron configurations: A - [He]2s 22p 5 B - [Ar]3d 64s 2 Select the answer(s) that has the correct comparison between elements.A - A is a nonmetal and B is a transition metal. B - B has the higher first ionization energy. C - A has the larger atomic radius. D - A forms negative ions and B forms positive ions.
Which of the following are characteristics of atomic electron configuration?
Two unknown elements in the lab: X and Y are given, if X has a larger Z than Y. Which element has a higher ionization energy? Explain.
Multiple Choice First ionization energies (IE1) generally increase as you move up the periodic table and to the right. Why is the first ionization energy of Se lower than As? Choose the best answer from the options below. a) The element As has 3 unpaired electrons in the p orbitals. Adding one more electron in Se will pair one of the p orbital electrons which is a slightly higher energy state and Se is then easier to ionize. b) The element As has a filled s orbital and adding one more electron in Se will begin to fill the p orbital electrons which is a slightly higher energy state and Se is then easier to ionize. c) The element As has a filled d orbital and adding one more electron in Se will begin to fill the p orbital electrons which is a slightly higher energy state and Se is then easier to ionize. d) The element As has 5 unpaired electrons in the d orbital. Adding one more electron in Se will pair one of the d orbital electrons which is a slightly higher energy state and Se is then…
What is the neutral atom that has its first two energy levels filled, has 1 electron in its third energy level, and has no other electrons? Enter the name of the element, not the abbreviation.
Using the graph of successive ionization energies what element could the graph represent? Al Si CI Ionization Energy (kJ/mol) 35000 30000 25000 20000 15000 10000 5000 0 IE1 IE2 Successive lonization Energies IE3 IE4 IES IE6 IE7 Briefly explain how you knew which element the graph represented? Make sure to discuss core and valence electrons and relative energies. B I U X2 X2 IE8
Removal of each successive electron from the same atom in the ionization process takes increasing amounts of energy. However, at some point in the process there is a considerable jump in the ionization energy. At what step in the ionization process would you expect magnesium to exhibit a sudden marked increase in its ionization energy? the fifth ionization the first ionization the third ionization the fourth ionization the second ionization 000 00