Question

Name each of the following binary compounds. a. \(\mathrm{XeF}_{6}\) b. \(\mathrm{OF}_{2}\) c. AsI \(_{3}\) d. \(\mathrm{N}_{2} \mathrm{O}_{4}\) e. \(\mathrm{Cl}_{2} \mathrm{O}\) f. SF \(_{6}\)

Short answer

a. Xenon hexafluoride b. Oxygen difluoride c. Arsenic triiodide d. Dinitrogen tetroxide e. Dichlorine monoxide f. Sulfur hexafluoride

Step-by-step solution

Identify the elements in the compound

For each compound, we'll identify the two elements involved. a. \(\mathrm{XeF}_{6}\) - Xenon (Xe) and Fluorine (F) b. \(\mathrm{OF}_{2}\) - Oxygen (O) and Fluorine (F) c. AsI \(_{3}\) - Arsenic (As) and Iodine (I) d. \(\mathrm{N}_{2} \mathrm{O}_{4}\) - Nitrogen (N) and Oxygen (O) e. \(\mathrm{Cl}_{2} \mathrm{O}\) - Chlorine (Cl) and Oxygen (O) f. SF \(_{6}\) - Sulfur (S) and Fluorine (F)

Use naming rules and prefixes

We will use appropriate prefixes while naming these binary compounds. For ionic compounds containing metals and nonmetals, we simply name the elements and use the suffix -ide for the second element. For covalent compounds containing two nonmetals, we typically use Greek prefixes (mono, di, tri, tetra, penta, hexa...) to indicate the number of atoms of each element. a. \(\mathrm{XeF}_{6}\) - The compound is composed of Xenon and Fluorine. It's a covalent compound with six Fluorine atoms; therefore, its name is Xenon hexafluoride. b. \(\mathrm{OF}_{2}\) - The compound is composed of Oxygen and Fluorine. It's a covalent compound with two Fluorine atoms; therefore, its name is Oxygen difluoride. c. AsI \(_{3}\) - The compound is composed of Arsenic and Iodine. It's a covalent compound, with three Iodine atoms; therefore, its name is Arsenic triiodide. d. \(\mathrm{N}_{2} \mathrm{O}_{4}\) - The compound is composed of Nitrogen and Oxygen. It's a covalent compound with two Nitrogen atoms and four Oxygen atoms; therefore, its name is Dinitrogen tetroxide. e. \(\mathrm{Cl}_{2} \mathrm{O}\) - The compound is composed of Chlorine and Oxygen. It's a covalent compound with two Chlorine atoms and one Oxygen atom; therefore, its name is Dichlorine monoxide. f. SF \(_{6}\) - The compound is composed of Sulfur and Fluorine. It's a covalent compound with six Fluorine atoms; therefore, its name is Sulfur hexafluoride.

Key concepts

Chemical Nomenclature

Understanding the naming process, or chemical nomenclature, is crucial in chemistry, especially for binary compounds. Chemical nomenclature refers to the specific set of rules used to name chemical substances systematically. It's how chemists ensure clear communication about the makeup and properties of compounds.

Binary compounds consist of two different elements. This can include compounds formed from metals and nonmetals or nonmetals only. There are specific rules for naming these compounds. When dealing with nonmetals, which results in covalent compounds, using Greek prefixes is essential.

• The prefixes indicate the number of each type of atom present in the compound. For example, "mono" for one, "di" for two, "tri" for three, and so on.
• The first element in the compound keeps its elemental name, while the second adopts the suffix “-ide."

By adhering to these rules, one can accurately name compounds such as xenon hexafluoride (\(\mathrm{XeF}_{6}\)) or sulfur hexafluoride (\(\mathrm{SF}_{6}\)). This standardized system helps in avoiding confusion in the scientific community.

Covalent Compounds

Covalent compounds, also known as molecular compounds, are substances where atoms are bonded together by covalent bonds. These bonds form when two atoms share electrons in order to fulfill their outer shell electron requirements, leading to more stable molecules. Covalent compounds typically arise between nonmetal elements.

One key feature of covalent compounds is their varied physical properties. They can be gases, liquids, or solids at room temperature. Common characteristics also include lower melting and boiling points in comparison to ionic compounds.

• They are often poor conductors of electricity because they do not have charged particles that move freely.
• The naming of covalent compounds relies heavily on the use of prefixes to denote the number of each type of atom.

Some examples from our exercise include oxygen difluoride (\(\mathrm{OF}_{2}\)) and arsenic triiodide (\(\mathrm{AsI}_{3}\)). Proper naming follows the chemical nomenclature outlined earlier and reflects the compound's molecular composition and structure.

Molecular Formulas

The molecular formula of a compound is a concise way of expressing information about the atoms that constitute a molecule. It identifies not only the elements present but also the precise quantity of each atom within the molecule. This is especially crucial for understanding binary compounds and their properties.

For instance, sulfur hexafluoride (\(\mathrm{SF}_{6}\)) is expressed with the formula indicating one sulfur atom bonded with six fluorine atoms. Another example is dichlorine monoxide (\(\mathrm{Cl}_{2}\mathrm{O}\)), where there are two chlorine atoms and one oxygen atom.

Molecular formulas are not the same as chemical formulas or structural formulas. The molecular formula provides a straightforward depiction useful for stoichiometry and analysis but does not show how atoms are bonded or arranged spatially within the molecule.

• This form of representation is significant in identifying substances and predicting chemical reactions.
• Keeps track of atom count, which plays an essential role in reacting masses and limiting reactants in stoichiometric calculations.

Understanding molecular formulas enables students to bridge the gap between theoretical chemistry and tangible applications in labs and industry.