Interpretation:
The ground state electronic configuration of
Concept Introduction:
Electronic configuration: The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.
Electrons occupy the lowest energy orbitals. The increasing order of orbital energy is
The energy order of the orbital for the first three periods is as follows,
The orbital which is closer to the nucleus has lower energy; therefore the
In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.
The subshell ordering by Aufbau principle is given below,
Want to see the full answer?
Check out a sample textbook solutionChapter 1 Solutions
Chemical Principles: The Quest for Insight
- • list the number of orbitals of each type (1s, 3p, etc) in an atom.arrow_forward• identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.arrow_forwardGiven the valence electron orbital level diagram and the description, identify the element or ion. a. A ground state atom b. An atom in an excited state (assume two electrons occupy the 1s orbital) c. A ground state ion with a charge of 1arrow_forward
- What is the maximum number of electrons that can be identified with each of the following sets of quantum numbers? In some cases, the answer may be none In such cases, explain why none is the correct answer. (a) n = 4, = 3, m = 1 (b) n = 6, = 1, m = 1, ms = 1/2 (c) n= 3, = 3, m = 3arrow_forwardOne bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit pararamagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for Li, N, Ni, Te, Ba, and Hg. Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: 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 Learning