3. Provide and explain the periodic trend for effective nuclear charge, Zeff- 4. Explain why the IE₁ of Na is 496 kJ/mol while IE₂ of Na is 4562 kJ/mol. 5. The EA₁ of O is -141 kJ/mol but the EA₂ of O is positive. Explain why. Also, explain why ionic compounds such as Li₂O and BeO exist despite the fact that it is unfavorable to form both the cation and the anion. 6. Consider the representative elements in the third period: Al, Ar, Cl, Mg, Na, P, S, Si. (a) Which of these elements are nonmetals? Metals? (b) Which (if any) of these elements are likely not to form ions? Which charge would you anticipate for an ion of each of the other elements? (c) Which of these elements will have the largest first ionization energy? (d) Rank these elements in order of increasing atomic radius. 7. Provide the ground-state electron configuration, indicate the valence electrons, and provide an orbital filling diagram for the valence electrons for each species below: (a) Ar (full configuration) (b) Ag (noble gas core) (c) Agt (noble gas core) (d) I (noble gas core) 8. Calculate the frequency and energy of light having a wavelength of 532 nm. We would classify this light as visible (green), would infrared light have a shorter/longer wavelength? Higher/lower energy? ulor formula (when applicable) for each compound described

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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Question #5 plz

3. Provide and explain the periodic trend for effective nuclear charge, Zeff.
4. Explain why the IE₁ of Na is 496 kJ/mol while IE₂ of Na is 4562 kJ/mol.
5. The EA₁ of O is -141 kJ/mol but the EA₂ of O is positive. Explain why. Also, explain why ionic
compounds such as Li₂O and BeO exist despite the fact that it is unfavorable to form both the
cation and the anion.
6. Consider the representative elements in the third period: Al, Ar, Cl, Mg, Na, P, S, Si.
(a) Which of these elements are nonmetals? Metals?
(b) Which (if any) of these elements are likely not to form ions? Which charge would
anticipate for an ion of each of the other elements?
(c) Which of these elements will have the largest first ionization energy?
(d) Rank these elements in order of increasing atomic radius.
7. Provide the ground-state electron configuration, indicate the valence electrons, and provide an
orbital filling diagram for the valence electrons for each species below:
(a) Ar (full configuration)
(b) Ag (noble gas core)
(c) Agt (noble gas core)
(d) I (noble gas core)
8. Calculate the frequency and energy of light having a wavelength of 532 nm. We would classify this
light as visible (green), would infrared light have a shorter/longer wavelength? Higher/lower energy?
Determine the empirical and molecular formula (when applicable) for each compound described
you

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Introduction

Electron affinity is the energy change that occurs when an isolated gas-phase atom gains an electron to form a negatively charged ion. Electron affinity is usually expressed in units of kilojoules per mole (kJ/mol). A positive electron affinity value means that energy is released when the electron is added, while a negative electron affinity value means that energy is required to add the electron.

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