Interpretation:
The orbital diagram for Rubidium (
Concept Introduction:
An orbital is a region of space in which electrons are filled. It can hold up to two electrons.
An atomic orbital is the region of space in which the probability of finding the electrons is highest. It is subdivided into 4 orbitals such as
The orders in which orbitals are filled by the electrons are governed by three basic principles.
- 1. Aufbau principle: In the ground state of an atom, an electron enters the orbital with lowest energy first and subsequent electrons are fed in the order of increasing energies. The word 'aufbau' in German means 'building up'. Here, it refers to the filling up of orbitals with electrons.
- 2. Pauli exclusion principle: As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins.
- 3. Hund’s rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is paired and all electrons in singly occupied orbitals have the same spin.
The electron configuration is the distribution of electrons of an atom in atomic orbitals. By following these three principles, electronic configuration of a particular atom is written.
To find: Draw the orbital diagram for rubidium (
Want to see the full answer?
Check out a sample textbook solutionChapter 3 Solutions
Chemistry: Atoms First
- • list the number of orbitals of each type (1s, 3p, etc) in an atom.arrow_forwardWhat type of electron orbital (i.e., s, p, d, or f) is designated by an electron with quantum numbers (a) n=1,l=0,m l =0(b) n=3,l=2,m l =1? (c) n=4,l=3,m l =3arrow_forwardUsing orbital box diagrams, depict an electron configuration for each of the following ions: (a) Mg2+, (b) K+, (c) Cl, and (d) O2.arrow_forward
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning