• s–subshell can hold a maximum of 2 electrons
• p–subshell can hold a maximum of 6 electrons
• d–subshell can hold a maximum of 10 electrons
• f–subshell can hold a maximum of 14 electrons
When filling up the orbitals, take note of:
• Aufbau Principle: totally fill in the lowest energy orbital first
• Hund’s Rule: electron orbitals that are degenerate (same energy orbital) are first half-filled before they are totally filled
The orbital diagram is:
Lower level (2p) orbital is not yet filled but Higher level (3s) orbital has 1 electron
Does the electron configuration 1s22s22p43s1 correspond to an excited state? Identify the atom and write the ground-state electron configuration if appropriate. How many unpaired electrons are present in this species?
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the The Electron Configuration concept. You can view video lessons to learn The Electron Configuration. Or if you need more The Electron Configuration practice, you can also practice The Electron Configuration practice problems.
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Based on our data, we think this problem is relevant for Professor Abdelrahman's class at UGA.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.