The ionization energy for a H atom 1s electron is 2.18x10-18 J and that for a 2p electron is 0.545x10-18). A 2p electron is further from the nucleus than a 1s electron would be, and as a result IE is lower. The 1s electron is closer to the nucleus than a 2p electron would be, therefore it is easier to remove the 1s electron. The 2p electron is shielded by the 1s electron and will be more easily removed. Electrons never occupy 2p orbitals in hydrogen. The 2p electron is shielded by the 1s electron, and as a result IE is lower.

The ionization energy for a H atom 1s electron is 2.18x10-18 J and that for a 2p electron is 0.545x10-18). A 2p electron is further from the nucleus than a 1s electron would be, and as a result IE is lower. The 1s electron is closer to the nucleus than a 2p electron would be, therefore it is easier to remove the 1s electron. The 2p electron is shielded by the 1s electron and will be more easily removed. Electrons never occupy 2p orbitals in hydrogen. The 2p electron is shielded by the 1s electron, and as a result IE is lower.

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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