Question

Give the systematic name for the following compounds that are found in everyday life: a. \(\mathrm{H}_{2} \mathrm{S}\) (rotten egg smell) b. \(\mathrm{SO}_{2}\) (smell of burnt matches) c. \(\mathrm{SF}_{6}\) (aerosol can propellant) d. \(\mathrm{Na}_{2} \mathrm{SO}_{3}\) (dried fruit preservative)

Short answer

a. Dihydrogen monosulfide b. Sulfur dioxide c. Sulfur hexafluoride d. Sodium sulfite

Step-by-step solution

a. \(\mathrm{H}_{2} \mathrm{S}\)

This compound consists of hydrogen (H) and sulfur (S). There are 2 atoms of hydrogen and 1 atom of sulfur. The systematic name will consist of the elements' names and the number of atoms in the form of prefixes. Systematic name: Dihydrogen monosulfide

b. \(\mathrm{SO}_{2}\)

This compound consists of sulfur (S) and oxygen (O). There is 1 atom of sulfur and 2 atoms of oxygen. The systematic name will include the elements' names and the count of atoms in the form of prefixes. Systematic name: Sulfur dioxide

c. \(\mathrm{SF}_{6}\)

This compound consists of sulfur (S) and fluorine (F). There is 1 atom of sulfur and 6 atoms of fluorine. As before, the systematic name will use the elements' names and prefixes to indicate the atom counts. Systematic name: Sulfur hexafluoride

d. \(\mathrm{Na}_{2} \mathrm{SO}_{3}\)

This compound is an ionic compound composed of sodium (Na) and sulfate (SO\(_3\)) ions. There are 2 sodium atoms and 1 sulfate ion (with 1 sulfur and 3 oxygen atoms). For ionic compounds, we name the cation (positive ion) first and the anion (negative ion) second. Systematic name: Sodium sulfite

Key concepts

Systematic Naming

Systematic naming is an essential aspect of chemical nomenclature, simplifying the understanding of compound formulas and their respective structures. This naming method utilizes a set of rules to generate consistent and descriptive names for chemical compounds, which are universally accepted and understood.

When it comes to naming compounds, systematic names are formed using the IUPAC (International Union of Pure and Applied Chemistry) conventions. These conventions require that the names reflect the composition of the compounds through proper use of prefixes and the elements' names:

• Binary compounds (those with two elements) often have names ending with '-ide'.
• Prefixes like 'mono-', 'di-', 'tri-', are employed to indicate the number of each type of atom present.
• The more electronegative element is listed second and its suffix is changed to '-ide'.

For instance, in dihydrogen monosulfide (\(\mathrm{H}_{2} \mathrm{S}\)), 'di-' indicates there are two hydrogen atoms, and 'mono-' suggests one sulfur atom. Adopting these guidelines ensures that compound names can be constructed and understood reliably across the globe.

Covalent Compounds

Covalent compounds consist of atoms bonded together by shared electrons. This sharing enables the molecules to achieve a stable electron configuration. Covalent bonds typically occur between nonmetal elements.

These compounds are named based on both the elements involved and the number of atoms for each element, reflected in prefixes that appear in the name. This guidance results in more precise and informative names.

For instance, let's break down covalent compounds from our examples:

• Sulfur dioxide (\(\mathrm{SO}_{2}\)): With 'di-' meaning two, it indicates two oxygen atoms are present along with one sulfur atom.
• Sulfur hexafluoride (\( \mathrm{SF}_{6}\)): The prefix 'hexa-' denotes the presence of six atoms of fluorine with one atom of sulfur.

The use of these systematic rules allows for the proper identification and differentiation of compounds based on their chemical formulas.

Ionic Compounds

Ionic compounds consist of positively charged ions, called cations, and negatively charged ions, called anions. These compounds are traditionally formed between metal and nonmetal elements.

The naming of ionic compounds follows a distinct protocol from covalent compounds. The cation is named first, followed by the anion. Since ionic compounds often involve complex ions or polyatomic ions, it's important to know the names and formulas of common polyatomic ions to effectively name ionic compounds.

An example from our original exercise is sodium sulfite (\(\mathrm{Na}_{2} \mathrm{SO}_{3}\)):

• 'Sodium' is the name of the metal cation (Na). It always retains its elemental name.
• 'Sulfite' refers to the polyatomic anion (\(\mathrm{SO}_{3}^{2-}\)).

Such systematic naming allows for efficient communication, ensuring that the structure and composition of compounds are accurately conveyed.