Fe compound name

Fe compound name DEFAULT

To determine a formula of a compound from its name you have to identify a compound as

Ionic Compound
•Ionic compounds are made from a metal and a nonmetal.

Covalent Compound
•Covalent compounds are made from two nonmetals.

Acid
•Acids are made from H and an anion. The anion may or may not be polyatomic.


Covalent compunds: write the element with a subscript that corresponds to the prefix.

For example, carbon tetraiodide...

Carbon is a nonmetal, and iodide is a nonmetal; therefore, carbon and iodide form a covalent compound. Thus, the covalent molecule nomenclature rules are used.

Carbon is C, idodide is I, and tetra means 4, so

carbon tetraiodide is CI4.

(hint: For our purposes, only covalent compounds use prefixes; therefore, the presence of a prefix means the compound must be covalent.)


Acids: add as many protons (H+) as needed to cancel the charge of the anion.

For example, hydrochloric acid...

The name has the word acid in it; therefore, it is an acid. Thus, the acid nomenclature rules are used.

Only acids based on monoatomic ions use the hydrosomething acid notation. The chloro is referring to the chloride anion, Cl-.

One proton is needed to cancel the charge of the chloride ion, so

hydrochloric acid is HCl.

Example, phosphoric acid...

The name has the word acid in it; therefore, it is an acid. Thus, the acid nomenclature rules are used.

The name doesn't use the hydrosomething acid notation, so the phosphoric must be referring to the polyatomic ion phosphate.

Three protons are needed to cancel the charge on the phosphate ion, PO43-, so

the formula is H3PO4.

Ionic compounds can be more difficult.

For example, iron (III) oxide...

Iron is a metal and oxygen (oxide) is a nometal; therefore, iron(III) oxid is an ionic compound. Thus, the nomenclature rules for ionic compounds are used.

The charges of the cations and the anions must be known to determine the formula of the compound.

Step 1 determine the charge of the cation.

Type I. Check the periodic table.

Type II. The name of a Type II cation contains the charge!

iron (III) means Fe3+

Step 2 Determine the charge of the anion.

Polyatomic anion. Remember the charge.

Monoatomic anion. Check the periodic table.

oxide is O2-.

Step 3 Combine ions so that the charges cancel.

2 (Fe3+) = +6
3 (O2-) = -6

Fe2O3

 

magnesium chloride
Mg is Mg2+
Cl is Cl-

MgCl2

 

  Back to
Nomenclature
Sours: https://www.westfield.ma.edu/PersonalPages/cmasi/gen_chem1/nomenclature/name_to_form.html

3.4: Ionic Nomenclature

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Learning Objectives

  • To use the rules for naming ionic compounds

After learning a few more details about the names of individual ions, you will be a step away from knowing how to name ionic compounds. This section begins the formal study of nomenclature, the systematic naming of chemical compounds.

Naming Ions

The name of a monatomic cation is simply the name of the element followed by the word ion. Thus, Na+ is the sodium ion, Al3+ is the aluminum ion, Ca2+ is the calcium ion, and so forth.

We have seen that some elements lose different numbers of electrons, producing ions of different charges (Figure 3.3). Iron, for example, can form two cations, each of which, when combined with the same anion, makes a different compound with unique physical and chemical properties. Thus, we need a different name for each iron ion to distinguish Fe2+ from Fe3+. The same issue arises for other ions with more than one possible charge.

There are two ways to make this distinction. In the simpler, more modern approach, called the Stock system, an ion’s positive charge is indicated by a roman numeral in parentheses after the element name, followed by the word ion. Thus, Fe2+ is called the iron(II) ion, while Fe3+ is called the iron(III) ion. This system is used only for elements that form more than one common positive ion. We do not call the Na+ ion the sodium(I) ion because (I) is unnecessary. Sodium forms only a 1+ ion, so there is no ambiguity about the name sodium ion.

The second system, called the common system, is not conventional but is still prevalent and used in the health sciences. This system recognizes that many metals have two common cations. The common system uses two suffixes (-ic and -ous) that are appended to the stem of the element name. The -ic suffix represents the greater of the two cation charges, and the -ous suffix represents the lower one. In many cases, the stem of the element name comes from the Latin name of the element. Table \(\PageIndex{1}\) lists the elements that use the common system, along with their respective cation names.

ElementStemChargeName
ironferr-2+ferrous ion
3+ferric ion
coppercupr-1+cuprous ion
2+cupric ion

The name of a monatomic anion consists of the stem of the element name, the suffix -ide, and then the word ion. Thus, as we have already seen, Cl is “chlor-” + “-ide ion,” or the chloride ion. Similarly, O2− is the oxide ion, Se2− is the selenide ion, and so forth. Table \(\PageIndex{2}\) lists the names of some common monatomic ions.

IonName
Ffluoride ion
Clchloride ion
Brbromide ion
Iiodide ion
O2−oxide ion
S2−sulfide ion
N3−nitride ion

The polyatomic ions have their own characteristic names, as discussed earlier.

Example \(\PageIndex{1}\)

Name each ion.

  1. Ca2+
  2. S2−
  3. SO32−
  4. NH4+
  5. Cu+

Solution

  1. the calcium ion
  2. the sulfide ion (from Table \(\PageIndex{2}\))
  3. the sulfite ion
  4. the ammonium ion
  5. the copper(I) ion or the cuprous ion (copper can form cations with either a 1+ or 2+ charge, so we have to specify which charge this ion has)

Exercise \(\PageIndex{1}\)

Name each ion.

  1. Fe2+
  2. Fe3+
  3. SO42−
  4. Ba2+
  5. HCO3

Example \(\PageIndex{2}\)

Write the formula for each ion.

  1. the bromide ion
  2. the phosphate ion
  3. the cupric ion
  4. the magnesium ion

Solution

  1. Br
  2. PO43−
  3. Cu2+
  4. Mg2+

Exercise \(\PageIndex{2}\)

Write the formula for each ion.

  1. the fluoride ion
  2. the carbonate ion
  3. the ferricion
  4. the potassium ion

Naming Compounds

Now that we know how to name ions, we are ready to name ionic compounds. We do so by placing the name of the cation first, followed by the name of the anion, and dropping the word ion from both parts. For example, what is the name of the compound whose formula is Ba(NO3)2?

Ba(NO3)2.jpg

The compound’s name does not indicate that there are two nitrate ions for every barium ion. You must determine the relative numbers of ions by balancing the positive and negative charges.

If you are given a formula for an ionic compound whose cation can have more than one possible charge, you must first determine the charge on the cation before identifying its correct name. For example, consider FeCl2 and FeCl3. In the first compound, the iron ion has a 2+ charge because there are two Cl ions in the formula (1− charge on each chloride ion). In the second compound, the iron ion has a 3+ charge, as indicated by the three Cl ions in the formula. These are two different compounds that need two different names. By the Stock system, the names are iron(II) chloride and iron(III) chloride. If we were to use the stems and suffixes of the common system, the names would be ferrous chloride and ferric chloride, respectively.

Example \(\PageIndex{3}\)

Name each ionic compound, using both Stock and common systems if necessary.

  1. Ca3(PO4)2
  2. (NH4)2Cr2O7
  3. KCl
  4. CuCl
  5. FeF2

Solution

  1. calcium phosphate
  2. ammonium dichromate (the prefix di- is part of the name of the anion)
  3. potassium chloride
  4. copper(I) chloride or cuprous chloride
  5. iron (II) fluoride or ferrous fluoride

Exercise \(\PageIndex{3}\)

Name each ionic compound, using both Stock and common systems if necessary.

Figure \(\PageIndex{1}\) is a synopsis of how to name simple ionic compounds.

3.7.jpg

Figure \(\PageIndex{1}\): A Guide to Naming Simple Ionic Compounds. Follow these steps to name a simple ionic compound.

KEY TAKEAWAY

  • Each ionic compound has its own unique name that comes from the names of the ions.

Contributors and Attributions

Sours: https://chem.libretexts.org/Courses/Eastern_Mennonite_University/EMU%3A_Chemistry_for_the_Life_Sciences_(Cessna)/03%3A_Ionic_Bonding_and_Simple_Ionic_Compounds/3.4%3A_Ionic_Nomenclature
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InChI=1S/2ClH.Fe/h2*1H;/q;;+2/p-2
NMCUIPGRVMDVDB-UHFFFAOYSA-L
iron dichloride
iron(II) chloride
iron(2+) chloride
[FeCl2] MolBase
FeCl2 IUPAC
ferrous chloride ChemIDplus
1398 Gmelin Registry Number Gmelin
7758-94-3 CAS Registry Number ChemIDplus
7758-94-3 CAS Registry Number NIST Chemistry WebBook
Sours: https://www.ebi.ac.uk/chebi/searchId.do?chebiId=CHEBI:30812

Transcript :

Chemistry in its element: iron

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You're listening to Chemistry in its element brought to you by Chemistry World, the magazine of the Royal Society of Chemistry.

(End promo)

Chris Smith

Hello, this week we turn to one of the most important elements in the human body. It's the one that makes metabolism possible and don't we just know it. There are iron man challenges, iron fisted leaders and those said to have iron in the soul. But there's a dark side to element number 26 too because its powerful chemistry means that it's also bad news for brain cells as Nobel Laureate Kary Mullis explains

Kary Mullis

For the human brain, iron is essential yet deadly. It exists on Earth mainly in two oxidation states - FeII and FeIII. FeIII is predominant within a few meters of the atmosphere which about two billion years ago turned 20% oxygen - oxidizing this iron to the plus three state which is virtually insoluble in water. This change from the relatively plentiful and soluble FeII, took a heavy toil on almost everything alive at the time.

Surviving terrestrial and ocean-dwelling microbes developed soluble siderophore molecules to regain access to this plentiful, but otherwise inaccessible essential resource, which used hydroxamate or catechol chelating groups to bring the FeIII back into solution. Eventually higher organisms including animals, evolved. And animals used the energy of oxygen recombining with the hydrocarbons and carbohydrates in plant life to enable motion. Iron was essential to this process.

But no animal, however, has been able to adequately deal, in the long run - meaning eighty year life spans - with the fact that iron is essential for the conversion of solar energy to movement, but is virtually insoluble in water at neutral pH, and, even worse, is toxic.

Carbon, sulfur, nitrogen. calcium, magnesium, sodium, maybe ten other elements are also involved in life, but none of them have the power of iron to move electrons around, and none of them have the power to totally destroy the whole system. Iron does. Systems have evolved to maintain iron in specific useful and safe configurations - enzymes which utilize its catalytic powers, or transferrins and haemosiderins, which move it around and store it. But these are not perfect. Sometimes iron atoms are misplaced, and there are no known systems to recapture iron that has precipitated inside of a cell.

In some tissues, cells overloaded with iron can be recycled or destroyed - but this doesn't work for neurons.

Neurons sprout thousands of processes during their existence - reaching out to form networks of connections to other neurons. During development of the adult human brain a large percentage of cells are completely eliminated, and some new ones are added. It is a learning process. But once an area of the brain is up and running, there is nothing that can be done biologically, if a large number of its cells stop working for any reason.

And the slow creep of precipitating iron over many decades is perhaps most often that reason. In less sophisticated tissues, like the liver, new stem cells can be activated, but in the brain, trained, structurally complex, interconnected neurons are needed, with thousands of projections that are accumulated over a lifetime of learning. So the result is slowly progressive neurodegenerative disease, like Parkinson's and Alzheimer's.

This same basic mechanism can result in a variety of diseases. There are twenty or thirty proteins that that deal with iron in the brain - holding iron and passing it from place to place. Every new individual endowed with a new set of chromosomes is endowed with a new set of these proteins. Some combinations will be better than others and some will be dangerous individually and collectively.

A mutation in a gene that codes for one of these proteins could disrupt its function - allowing iron atoms to become lost. These atoms that have been lost from the chemical groups that hold them will not always be safely returned to some structure like transferrin or haemoferritin. Some of them will react with water and be lost forever. Only they aren't really lost. They are piling up in the unlucky cell types that were the designated locations for expression of the most iron-leaky proteins. And oxides of iron are not just taking up critical space. Iron is very reactive. The infamous "Reactive Oxygen Species" which have been suspected of causing so many age related illnesses may just derive from various forms of iron.

It is time for specialists trained in chemistry, and with an eye to the chemistry of iron, to pay some attention to neurodegenerative disease.

Chris Smith

Kary Mullis telling the story of iron, the element that we can't do without, but which at the same time could hold the key to our neurological downfall. Next time on Chemistry in its Element Johnny Ball will tell the story of Marie Curie and the element that she discovered and then named after her homeland.

Johnny Ball

Pitchblende, a uranium bearing ore, seemed to be far too radio active than could be accounted for by the uranium. They sieved and sorted by hand ounce by ounce through tons of pitchblende in a drafty, freezing shed, before eventually tiny amounts of polonium were discovered.

Chris Smith

So be radioactive or at least podcast proactive and join us for the mysterious story of Polonium on next week's Chemistry in its Element. I'm Chris Smith, thank you for listening, see you next time.

(Promo)

Chemistry in its element is brought to you by the Royal Society of Chemistry and produced by thenakedscientists.com. There's more information and other episodes of Chemistry in its element on our website at chemistryworld.org/elements.

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Sours: https://www.rsc.org/periodic-table/element/26/iron

Compound name fe

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How To Name Ionic Compounds With Transition Metals

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