Question
Explain why compounds of $\mathrm{Sc}^{3+}$ are colorless, but compounds of $\mathrm{Ti}^{3}$ are colored.
Step 1
For Scandium ($\mathrm{Sc}^{3+}$), the electron configuration is $3s^{2} 3p^{6} 4s^{2} 3d^{1}$. When it loses three electrons, it forms a stable noble gas configuration, similar to Argon, with no electrons in the 3d or 4s orbitals. Show more…
Show all steps
Your feedback will help us improve your experience
Nadia Lara and 84 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Compounds containing the $\mathrm{Sc}^{3+}$ ion are colorless, whereas those containing the $\mathrm{Ti}^{3+}$ ion are colored. Explain.
Compounds of $\mathrm{Sc}^{3+}$ are not colored, but those of $\mathrm{Ti}^{3+}$ and $\mathrm{V}^{3+}$ are. Why?
Transcript
600,000+
Students learning Chemistry with Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD
