chemistry

Scandium chloride

Scandium chloride is a chemistry topic covered in the lgStudy science library. This page brings together a partial reference excerpt, illustrations, worked examples, real-world applications and a short study plan, so you can understand Scandium chloride rather than just read about it. In short: Scandium(III) chloride is an inorganic scandium compound with the chemical formula ScCl3. It is a white, high-melting ionic compound, which is deliquescent and highly water-soluble.

Key takeaways

Scandium chloride belongs to chemistry; place it in that map before memorising details.
Learn the definition first, then one example that makes the definition concrete.
Connect Scandium chloride to a quantity you can measure, compute or draw — that is where exam questions come from.
Reproduce the core statement of Scandium chloride from memory before moving on to harder problems.

Reference excerpt

Scandium(III) chloride is an inorganic scandium compound with the chemical formula ScCl3. It is a white, high-melting ionic compound, which is deliquescent and highly water-soluble. This salt is mainly of interest in the research laboratory. Both the anhydrous form and hexahydrate (ScCl3·6H2O) are commercially available.

Structure ScCl3 crystallises in the layered BiI3 motif, which features octahedral scandium centres. Monomeric ScCl3 is the predominant species in the vapour phase at 900 K, the dimer Sc2Cl6 accounts for approximately 8%. The electron diffraction spectrum indicates that the monomer is planar and the dimer has two bridging Cl atoms each Sc being 4 coordinate.

Reactions

ScCl3 is a Lewis acid that absorbs water to give aquo complexes. According to X-ray crystallogrphy, one such hydrate is the salt trans-[ScCl2(H2O)4]Cl·2H2O. With the less basic ligand tetrahydrofuran, ScCl3 yields the adduct ScCl3(THF)3 as white crystals. This THF-soluble complex is used in the synthesis of organoscandium compounds. ScCl3 has been converted to its dodecyl sulfate salt, which has been investigated as a "Lewis acid-surfactant combined catalyst" (LASC) in aldol-like reactions.

Reduction Scandium(III) chloride was used by Fischer et al. who first prepared metallic scandium by electrolysis of a eutectic melt of scandium(III) chloride and other salts at 700-800 °C. ScCl3 reacts with scandium metal to give a number of chlorides where scandium has an oxidation state of less than +3, ScCl, Sc7Cl10, Sc2Cl3, Sc5Cl8 and Sc7Cl12. For example, reduction of ScCl3 with scandium metal in the presence of caesium chloride gives the compound CsScCl3 which contains linear chains of composition ScIICl−3, containing ScIICl6 octahedra sharing faces.

Uses Scandium(III) chloride is found in some halide lamps, optical fibers, electronic ceramics, and lasers.

References

Illustrations

Worked examples

Example 1 — a first encounter with Scandium chloride

Start with the simplest possible case. Write down what Scandium chloride claims or describes in one sentence, then invent the smallest concrete situation in which that sentence is true. In chemistry, the smallest case is usually a single object, a single equation or a single measurement. Check that every symbol or term in your sentence has a meaning in that case.

Example 2 — changing one variable

Take the situation from Example 1 and change exactly one quantity: double it, halve it, or set it to zero. Predict what should happen to Scandium chloride before you calculate. Comparing your prediction with the result is the fastest way to find out whether you understand the idea or only the words.

Example 3 — an exam-style question

Typical questions about Scandium chloride ask you to (a) state it precisely, (b) apply it to given data, and (c) explain a limitation. Practise writing all three answers in under five minutes; the third part is what separates a full-mark answer from an average one.

Applications of Scandium chloride

In research: Scandium chloride appears in chemistry research whenever the underlying quantities have to be modelled precisely. Papers usually cite it as a starting assumption and then explore where it breaks down.
In technology and industry: Engineering practice reuses Scandium chloride in design rules, simulations and safety margins. Knowing the idea lets you read a specification sheet and understand why the numbers look the way they do.
In the classroom: Scandium chloride is common in secondary-school and first-year university syllabi. It links to neighbouring topics Chlorides, Metal halides, Scandium compounds, so understanding it makes those chapters shorter.
In everyday life: Look for Scandium chloride outside the textbook — in sport, cooking, traffic, electronics or the sky above you. An example you found yourself is remembered far longer than one you were given.

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How to study Scandium chloride in 20 minutes

Read the reference excerpt below once, without taking notes.
Close the page and write down what Scandium chloride means in your own words.
Compare your version with the excerpt and mark what you missed.
Work through the three examples above with pen and paper.
Explain Scandium chloride out loud to somebody else — or to Teacher Smith in the lgStudy chat.

Frequently asked questions

What is Scandium chloride in simple terms?

Scandium(III) chloride is an inorganic scandium compound with the chemical formula ScCl3. It is a white, high-melting ionic compound, which is deliquescent and highly water-soluble.

Why does Scandium chloride matter?

Because it connects several chemistry ideas at once: it gives you a definition you can apply, a quantity you can calculate, and a way to check whether a result is plausible.

How should I study Scandium chloride?

Read the excerpt, restate it from memory, then work through the examples and applications listed on this page. The five-step study plan above takes about twenty minutes.

What does this page cover?

It gives you a compact reference excerpt plus original lgStudy explanations, examples, applications and study material on Scandium chloride.