Concept explainers
Interpretation:
The
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 identify: Identify the symbol of the element with the given ground-state electron configuration
Want to see the full answer?
Check out a sample textbook solutionChapter 3 Solutions
Chemistry: Atoms First
- What is... a) the aproximate size of the nucleus b) groundstatearrow_forwardWhat element has the abbreviated electron configuration of [Kr]5s24d2?arrow_forwardwhat are likely possibilies for X if Xn + Cl -> XCl2 can you help explain how to solve this? Would it be any element in the 2nd s2 row (Be, Mg, Ca, Sr, Ba, Ra)?arrow_forward
- the element that has a valence electron configuration 3s23p5 isarrow_forwardA.) What is the grounds the electron configuration of 15p. B.) Show the orbital diagram. C.) Write the four quantum numbers associated with the last electron. D.) Is it paramagnetic or diamagnetic?arrow_forwardHow many unpaired electrons would you expect for chromium in [Cr(H2O)6]3+? Is this a paramagnetic or diamagnetic material?arrow_forward
- How many unpaired d-electrons could Re(CO)5 have? Which is more reasonable? Why?arrow_forwardWhich of the following is the expected electron configuration for a cadmium (II) cation (Z = 48)?arrow_forwardIf the ground state electron configuration of an element is [Ne] 3s23p1, what is the typical charge on the monatomic ion of the element?arrow_forward
- 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 Learning