Everything You Need To Know About Compound Names

One of the most important pieces of information to get from a compound name is whether it is an inorganic or organic molecule. This will give you an idea of where the elements come from (inorganic) or from living organisms (organic). For example, sodium chloride has the two elements coming from two different places: sodium comes from inorganic table salt, and chlorine comes from table salt used for cooking food. Copper sulfate on the other hand has copper coming from copper wire and sulfur coming since ancient times in its natural form as brimstone. VF5 compound name is an example of a non-organic compound.

The first letters or numbers of the compound name identify its type (inorganic or organic). The last number may be called its oxidation state. The types include: Metal Polarity, ionic charges, Lewis acids / bases, transition metals, coordination compounds and related metals. In addition to the six polarities listed above, there are also electron withdrawing species in transition metals like ruthenium and rhodium. 

The compound name of such a transition metal ion is Ru+5-5 instead of just Ru where it is a neutral atom with five unpaired electrons in the outermost shell. Another important class of compounds are those called coordination complexes.

Everything You Need To Know About Compound Names :

1. Metal Polarity

Metal Polarity – This category includes compounds with a positive and a negative charge. Compounds here have the metal connected to at least two different elements that can conduct electrons. Some examples of this type are potassium nitrate (with the nitrogen atom as the electron carrier) and lithium hydride (with hydrogen serving this function). This category also includes compounds with two positive or two negative ions that are bound together by relatively weak forces, such as calcium fluoride (CaF) and sodium chloride (NaCl).

2. Ionic Charges

Ionic Charges – Inorganic compounds where the metal is in its highest oxidation state are in this group. Examples of this type of compound include iron(III) sulfate, iron(III) carbonate, alkali metals and some transition metals like ruthenium and rhodium.

3. Lewis Acids / Bases

Lewis Acids / Bases – This category contains compounds like boron trifluoride, anions of the halogens, and compounds of the alkali metals with oxygen and fluorine such as sodium or potassium oxides and hydrogen fluoride. Most inorganic compounds are here. Most organic molecules are not included and will appear in a different category below.

4. Transition Metals

Transition Metals – Transition metals have some valence electrons in both their d- and s-orbitals that can become unpaired upon interaction with other species. Examples of this class are ruthenium and rhodium.

5. Coordination Complexes

Coordination Compounds – Inorganic compounds where the metal is bonded to more than one atom are in this category. They contain anions, carbocations, coordination complexes, and other types of compounds that have a central metal ion that can hold an electron by sharing it with another atom or compound. 

Metalloids like gold, platinum, and palladium are also included here because they usually have too few valence electrons to describe as metals but they do act as metals under certain conditions. Most complexes in this class carry ligands such as oxygen or nitrogen atoms. Examples of these compounds are sodium chloride, ammonium nitrate and ammonium sulfate. Compounds like these are known to have a very wide range of colors.

6. Related Metals

Related Metals – These are other members of the same group in the periodic table, or are compounds where a metal atom is bound to another metal like silver and gold. Examples of this type of compound include calcium fluoride and calcium oxide.

7. Halogens (Bromine, Chlorine, Fluorine, Iodine)

14 Elements in Group 17 has 2 electrons in their outer shell; the last two electrons are strongly attracted to each other. When these elements have eight electrons in their valence shell, they can form a bond with another halogen atom sharing an electron. This attraction is so strong that it happens spontaneously at room temperature. If a metal atom has other valence electrons, it is called an ion. If the metal atom has six or fewer electrons in its valence shell, the metal is a nonmetal. If a halogen atom has eight electrons in its valence shell (eight bonds), it has a very high electronegativity and attracts another halogen very strongly.

It is important to remember that halogens in general do not have bonding diatomic orbital and therefore do not form bonds with other atoms via sharing electrons. Halogens do react with other atoms, but they often lose an electron to form a covalent bond.

Some halogens are gases at room temperature and pressure. When they are combined with metals, they form diatomic ions: When an iodine atom forms this type of bond, the atom loses one of its three electrons in its outer shell.