We are asked to determine which of the given ions have six d electrons in the outermost d subshell.
To do so, we shall follow these steps:
Step 1: Determine the ground-state electron configuration of the element.
Step 2: Determine the orbital involved.
Step 3: Write the electron configuration from the lowest to the highest energy level.
Step 4: Determine the electron configuration of the ion.
Step 1: You can determine the ground-state electron configuration of Osmium (Os) by locating the position of Os in the periodic table.
Ground-state means that the element is in its lowest energy form (not in an excited state). Neutral osmium means it has no charge, meaning no electrons are removed or added in the atom.
You can see in the above illustration of the periodic table that Os is in Period 6 and d-block.
Which of these ions have six d electrons in the outermost d subshell?
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 The Electron Configuration: Ions concept. You can view video lessons to learn The Electron Configuration: Ions. Or if you need more The Electron Configuration: Ions practice, you can also practice The Electron Configuration: Ions practice problems.
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Based on our data, we think this problem is relevant for Professor Smeureanu's class at HUNTER.