We’re being asked to classify each ion as diamagnetic or paramagnetic.
Recall that for:
• diamagnetic: all of the electrons are paired
• paramagnetic: at least one electron is unpaired
For neutral element, Atomic Number = # of protons = # of electrons.
Step 1: Electron configuration
Atomic # = 30 → 30 e-
Nearest noble gas before Zn → Ar (18 e–).
The shorthand e– config. for Cu is:
Step 2: Orbital diagram
Outermost sublevel: 3d → 5 orbitals (d)
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
Classify these atoms and ions as paramagnetic or diamagnetic.
Frequently Asked Questions
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 Paramagnetism and Diamagnetism concept. You can view video lessons to learn Paramagnetism and Diamagnetism. Or if you need more Paramagnetism and Diamagnetism practice, you can also practice Paramagnetism and Diamagnetism practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Corbin's class at UCLA.