3 Ways to Name Chemical Compounds - wikiHow (2024)

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Co-authored byBess Ruff, MA

Last Updated: March 20, 2024Fact Checked

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1. 1

   Know what makes a compound ionic. Ionic compounds contain a metal and a nonmetal. Refer to the periodic table of elements to see what categories the elements in the compound belong to.

2. 2

   Build the name. For a two element ionic compound, the naming is simple. The first part of the name is the name of the metal element. The second part is the name of the nonmetal element, with the suffix “-ide.”

   • Here are some examples:
     • Al₂O₃. Al₂ = Aluminium; O₃ = Oxygen. So the name would be “aluminium oxide.”
     • FeCl₃. Fe = Iron; Cl₃ = Chlorine. So the name would be "iron chloride."
     • SnO₂. Sn = Tin; O₂ = Oxygen. So the name of this compound would be Tin Oxide.

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3. 3

   Recognize and name transition metals. Metals in the D and F blocks of the periodic table are known as transition metals. Their charge is written with a Roman numeral when writing out the compound name. This is because they can have more than one charge and make more than one compound.

   • Example: FeCl₂ and FeCl₃. Fe = Iron; Cl₂ = Chloride -2; Cl₃ = Chloride -3. The names would be iron(II) chloride and iron(III) chloride.

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1. 1

   See Also

   Naming ions and ionic compounds (article) | Khan Academy4.3: Chemical NomenclatureNaming Compounds – Introductory Chemistry2.12: Naming Chemical Compounds

   Understand what a polyatomic compound is. These compounds are built off of groups of atoms that are covalently bonded together, and the entire group has a positive or negative charge.^[1] You can do three basic things to polyatomic compounds, which will help you identify and understand these types of compounds:

   • Add a hydrogen to the beginning of the compound. The word “hydrogen” is added to the beginning of the compound name. This reduces the negative charge by one. For example, “carbonate” CO₃^2- becomes “hydrogen carbonate” HCO₃^-.
   • Remove an oxygen from the compound. The charge stays the same and the ending of the compound changes from “-ate” to “–ite”. For example: NO₃ to NO₂ goes from “nitrate” to “nitrite.”
   • Replace the central atom with another from the same periodic group. For example, sulfate SO₄^2- can become Selenate SeO₄^2-.
2. 2

   Memorize the most common ion groups. These are the basis for forming most polyatomic compounds.^[2] Listed in order of increasing negative charge, they are:

   • Hydroxide ion: OH^-
   • Nitrate ion: NO₃^-
   • Hydrogen carbonate ion: HCO₃^-
   • Permanganate ion: MnO₄^-
   • Carbonate ion: CO₃^2-
   • Chromate ion: CrO₄^2-
   • Dichromate ion: Cr₂O₇^2-
   • Sulfate ion: SO₄^2-
   • Sulphite ion: SO₃^2-
   • Thiosulfate ion: S₂O₃<2-
   • Phosphate ion: PO₄^3-
   • Ammonium ion: NH₄⁺

3. 3

   Build compound names based off the list. Associate whatever element(s) is attached to the group ion and name accordingly. If the element comes in front of the ion group, the name of the element is simply added to the beginning of the compound name.^[3]

   • Example: KMnO₄. You should recognize the MnO₄^- ion as permanganate. K is potassium, so the compound is named potassium permanganate.
   • Example: NaOH. You should recognize the OH^- ion as hydroxide. Na is sodium, so the compound is named sodium hydroxide.

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1. 1

   Understand a covalent compound. Covalent compounds are formed by two or more nonmetal elements. The name for the compound is based off how many atoms are present. The prefix attached is the Latin term for the number of molecules.^[4]

2. 2

   Learn the prefixes. Memorize the prefixes for up to 10 atoms:^[5]

   • 1 atom – “Mono-“
   • 2 atoms – “Di-“
   • 3 atoms – “Tri-“
   • 4 atoms – “Tetra-“
   • 5 atoms – “Penta-“
   • 6 atoms – “Hexa-“
   • 7 atoms – “Hepta-“
   • 8 atoms – “Octa-“
   • 9 atoms – “Nona-“
   • 10 atoms – “Deca-“

3. 3

   Name the compounds. Using the correct prefixes, name the new compound. You attach prefixes to any part of the compound that has multiple atoms.^[6]

   • Example: CO would be carbon monoxide and CO₂ would be carbon dioxide.
   • Example: N₂S₃ would be Dinitrogen trisulfide.
   • In most cases, the “mono-“ prefix can be omitted, because it is implied when it is not present. It is still used for carbon monoxide due to the term being in use since early chemistry.

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