Name the following ionic compounds: (e) Fe 2 (CO 3 ) 3

Hey everyone in this example we need to give the name of our compound F. E. S. 04. So we're going to analyze this atom by atom beginning with our F. E. Here. We want to recall that S. E. Is going to be according to our periodic table a metal. And that is due to the fact that it's in the transition metal section of our periodic table. And so this is referring to our compounds iron. So we do know that because it's in the transition middle section it can have multiple charges. So we're going to have to analyze our second compound to figure out the charge of this iron. Our second compound here we're sorry our second adam here is a sulfur bonded to an oxygen atom. We want to recognize that this is actually a poly atomic ion which we should recall as S. 042 minus for sulfate. And so We would recall that this poly atomic ion of course has this two minus charge that I wrote in here. So because we have a two minus charge on our sulfate an ion. But as a whole are compound is neutral. This means that our charge on iron had to be something to cancel out this -2. And so we would say that our charge for iron is going to be therefore F. E two plus to neutralize The -2 charge on selfie. And so overall we can name our iron now because we know that it should be iron with a roman numeral two Corresponding to its two plus charge. And so we have iron too. And then our name of our anti on here selfie. So this is actually going to be the answer to the name of our given compound FES 04, which is iron to sulfate. So if you have any questions, please leave them down below. Otherwise, I will see everyone in the next practice video.

Ch.2 - Atoms, Molecules, and Ions

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.2 - Atoms, Molecules, and Ions

Problem 72e

Chapter 2, Problem 72e

Name the following ionic compounds: (e) Fe₂(CO₃)₃

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Identify the cation and the anion in the compound. Here, the cation is Fe (iron) and the anion is CO3 (carbonate).

Determine the charge of the anion. The carbonate ion (CO3) has a charge of -2.

Since the compound is neutral overall, the total positive charge must balance the total negative charge. Here, there are three carbonate ions, each with a -2 charge, giving a total of -6.

To balance the -6 charge from the anions, the iron cation must have a total charge of +6. Since there are two iron atoms, each iron must have a charge of +3.

Name the compound by stating the name of the cation first, followed by the charge of the cation in Roman numerals in parentheses, and then the name of the anion. The compound is named Iron(III) Carbonate.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of positively charged cations and negatively charged anions. These oppositely charged ions attract each other, creating a stable compound. Understanding the nature of ionic bonds is essential for naming these compounds correctly.

Oxidation States

The oxidation state, or oxidation number, indicates the degree of oxidation of an atom in a compound. It helps in determining how many electrons an atom has gained, lost, or shared during the formation of a compound. In the given compound, Fe has an oxidation state of +2, which is crucial for correctly identifying the compound's name.

Nomenclature of Ionic Compounds

The nomenclature of ionic compounds involves naming the cation first followed by the anion. For transition metals, the oxidation state is often indicated in Roman numerals. In the case of Fe2(CO3)3, the name would reflect the iron's oxidation state and the carbonate ion, leading to the name 'Iron(II) Carbonate' for the compound.