Interpretation:
The reason for the slight increase in the first ionization energies of manganese, iron, and cobalt but the considerable increase in gallium, germanium, and arsenic has to be determined.
Concept Introduction:
The energy that is needed to remove an electron from the isolated, neutral gaseous atom is known as ionization energy. It is represented by
Want to see the full answer?
Check out a sample textbook solutionChapter 8 Solutions
Chemistry: Principles and Practice
- We expect the atomic radius to increase going down a group in the periodic table. Can you suggest why the atomic radius of hafnium breaks this rule? (See data below.)arrow_forward6.82 A particular element has the following values for its first four ionization energies: 900, 1760, 14, 850, and 21,000 kJ/mol. Without consulting a list of ionization energy values, determine what group in the periodic table this element belongs in.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning