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Iron(II) citrate

Iron(II) citrate 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 Iron(II) citrate rather than just read about it. In short: Ferrous citrate, also known as iron(II) citrate or iron(2+) citrate, describes coordination complexes containing citrate anions with Fe2+ formed in aqueous solution. Although a number of complexes are possible (or even likely), only one complex has been crystallized.

Iron(II) citrate — main illustration
Iron(II) citrate — illustration

Key takeaways

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

Reference excerpt

Ferrous citrate, also known as iron(II) citrate or iron(2+) citrate, describes coordination complexes containing citrate anions with Fe2+ formed in aqueous solution. Although a number of complexes are possible (or even likely), only one complex has been crystallized. That complex is the coordination polymer with the formula [Fe(H2O)6]2+{[Fe(C6H5O7)(H2O)]−}2.2H2O, where C6H5O73- is HOC(CH2CO2−)2(CO2−, i.e., the triple conjugate base of citric acid wherein the three carboxylic acid groups are ionized. Ferrous citrates are all paramagnetic, reflecting the weak crystal field of the carboxylate ligands.

Ferrous citrates are produced by treating disodium citrate Na2C6H6O7 with sources of iron(II) aquo complexes, such as iron(II) sulfate. Ferrous citrates are all highly unstable in air, converting to ferric citrates. It is a nutrient supplement approved by the FDA.

See also Iron(III) citrate Ammonium ferric citrate

References

Illustrations

Iron(II) citrate illustration
Iron(II) citrate illustration
Iron(II) citrate: Structure of the anionic coordination polymer {[Fe(C6H5O7)(H2O)]−}n.[3] (legend: red = O, gray = C, blue = Fe, white = H).
Structure of the anionic coordination polymer {[Fe(C6H5O7)(H2O)]−}n.[3] (legend: red = O, gray = C, blue = Fe, white = H).

Worked examples

Example 1 — a first encounter with Iron(II) citrate

Start with the simplest possible case. Write down what Iron(II) citrate 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 Iron(II) citrate 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 Iron(II) citrate 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 Iron(II) citrate

In research
Iron(II) citrate 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 Iron(II) citrate 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
Iron(II) citrate is common in secondary-school and first-year university syllabi. It links to neighbouring topics Citrates, Iron(II) compounds, Organic compound stubs, so understanding it makes those chapters shorter.
In everyday life
Look for Iron(II) citrate 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 Iron(II) citrate in 20 minutes

  1. Read the reference excerpt below once, without taking notes.
  2. Close the page and write down what Iron(II) citrate means in your own words.
  3. Compare your version with the excerpt and mark what you missed.
  4. Work through the three examples above with pen and paper.
  5. Explain Iron(II) citrate out loud to somebody else — or to Teacher Smith in the lgStudy chat.

Frequently asked questions

What is Iron(II) citrate in simple terms?

Ferrous citrate, also known as iron(II) citrate or iron(2+) citrate, describes coordination complexes containing citrate anions with Fe2+ formed in aqueous solution. Although a number of complexes are possible (or even likely), only one complex has been crystallized.

Why does Iron(II) citrate 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 Iron(II) citrate?

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 Iron(II) citrate.

Tags

  • Citrates
  • Iron(II) compounds
  • Organic compound stubs

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