Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Explain why the first ionisation energy is lower for Al than Mg? O The valence electron in Al is less shielded from the nucleus and so the electron will observe a larger effective nuclear charge. O The valence electron is removed from the 3s orbital for Al rather than 3p orbital for Mg O This atomic radius of Al is larger therefore the valence electron is further away from the nucleus. O The valence electron in Mg is more shielded from the nucleus and so the electron will observe a larger effective nuclear charge. O The electronegativity of Mg is greater than Al and so will result in Mg having a higher tendency to attract covalently bound electrons. O The valence electron is removed from the 3p orbital for Al rather than 3s orbital for Mg

Explain why the first ionisation energy is lower for Al than Mg? O The valence electron in Al is less shielded from the nucleus and so the electron will observe a larger effective nuclear charge. O The valence electron is removed from the 3s orbital for Al rather than 3p orbital for Mg O This atomic radius of Al is larger therefore the valence electron is further away from the nucleus. O The valence electron in Mg is more shielded from the nucleus and so the electron will observe a larger effective nuclear charge. O The electronegativity of Mg is greater than Al and so will result in Mg having a higher tendency to attract covalently bound electrons. O The valence electron is removed from the 3p orbital for Al rather than 3s orbital for Mg

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter7: Chemical Bonding And Molecular Geometry
Section: Chapter Questions
Problem 7E: Write the electron configuration for each of the following ions: (a) As3 (b) I (c) Be2+ (d) Cd2+ (e)...
See similar textbooks
icon
Related questions
Question
Explain why the first ionisation energy is lower for Al than Mg? O The valence electron in Al is less shielded from the nucleus and so the electron will observe a larger effective nuclear charge. O The valence electron is removed from the 3s orbital for Al rather than 3p orbital for Mg O This atomic radius of Al is larger therefore the valence electron is further away from the nucleus. O The valence electron in Mg is more shielded from the nucleus and so the electron will observe a larger effective nuclear charge. O The electronegativity of Mg is greater than Al and so will result in Mg having a higher tendency to attract covalently bound electrons. O The valence electron is removed from the 3p orbital for Al rather than 3s orbital for Mg
Transcribed Image Text:Explain why the first ionisation energy is lower for Al than Mg? O The valence electron in Al is less shielded from the nucleus and so the electron will observe a larger effective nuclear charge. O The valence electron is removed from the 3s orbital for Al rather than 3p orbital for Mg O This atomic radius of Al is larger therefore the valence electron is further away from the nucleus. O The valence electron in Mg is more shielded from the nucleus and so the electron will observe a larger effective nuclear charge. O The electronegativity of Mg is greater than Al and so will result in Mg having a higher tendency to attract covalently bound electrons. O The valence electron is removed from the 3p orbital for Al rather than 3s orbital for Mg
AI-Generated Solution
AI-generated content may present inaccurate or offensive content that does not represent bartleby’s views.
steps

Unlock instant AI solutions

Tap the button
to generate a solution

SEE SOLUTION
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Principles of Modern Chemistry
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: Matter and Change
Chemistry: Matter and Change
Chemistry
ISBN:
9780078746376
Author:
Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:
Glencoe/McGraw-Hill School Pub Co
Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
Chemistry
ISBN:
9781337399425
Author:
Steven S. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS