Question

Write the name for each of the following binary compounds of nonmetallic elements. a. \(\mathrm{XeF}_{6}\) b. \(\mathrm{SiCl}_{4}\) c. \(SeO\) d. \(\mathrm{XeF}_{4}\) e. \(\mathrm{AsBr}_{3}\) f. \(C l_{4}\)

Short answer

a. Xenon hexafluoride: \(\mathrm{XeF}_{6}\) b. Silicon tetrachloride: \(\mathrm{SiCl}_{4}\) c. Selenium monoxide: \(SeO\) d. Xenon tetrafluoride: \(\mathrm{XeF}_{4}\) e. Arsenic tribromide: \(\mathrm{AsBr}_{3}\) f. Tetrachlorine: \(Cl_{4}\)

Step-by-step solution

Identify the first element

The first element of the binary compound is the one that is written first in the formula. Identify the first element of each of the given compounds. a. Xe in \(\mathrm{XeF}_{6}\) b. Si in \(\mathrm{SiCl}_{4}\) c. Se in \(SeO\) d. Xe in \(\mathrm{XeF}_{4}\) e. As in \(\mathrm{AsBr}_{3}\) f. Cl in \(Cl_{4}\)

Identify the second element

The second element of the binary compound is the one that is written second in the formula. Identify the second element of each of the given compounds and change its ending to '-ide'. a. F (fluorine) in \(\mathrm{XeF}_{6}\) becomes fluoride b. Cl (chlorine) in \(\mathrm{SiCl}_{4}\) becomes chloride c. O (oxygen) in \(SeO\) becomes oxide d. F (fluorine) in \(\mathrm{XeF}_{4}\) becomes fluoride e. Br (bromine) in \(\mathrm{AsBr}_{3}\) becomes bromide f. Cl (chlorine) in \(Cl_{4}\) becomes chloride

Attach a prefix to indicate the number of atoms

Attach a prefix to indicate the number of atoms of each element in the compound. Prefixes are: 1. mono (only used for the second element) 2. di 3. tri 4. tetra 5. penta 6. hexa 7. hepta 8. octa 9. nona 10. deca a. hexafluoride for \(\mathrm{XeF}_{6}\) b. tetrachloride for \(\mathrm{SiCl}_{4}\) c. monoxide for \(SeO\) d. tetrafluoride for \(\mathrm{XeF}_{4}\) e. tribromide for \(\mathrm{AsBr}_{3}\) f. tetrachloride for \(Cl_{4}\)

Write the names of the binary compounds

Combine the elements with their prefixes to form the names of the binary compounds. a. Xenon hexafluoride: \(\mathrm{XeF}_{6}\) b. Silicon tetrachloride: \(\mathrm{SiCl}_{4}\) c. Selenium monoxide: \(SeO\) d. Xenon tetrafluoride: \(\mathrm{XeF}_{4}\) e. Arsenic tribromide: \(\mathrm{AsBr}_{3}\) f. Tetrachlorine: \(Cl_{4}\)

Key concepts

Chemical Nomenclature

Understanding chemical nomenclature is akin to learning a language that allows scientists and students to communicate chemical compositions succinctly and accurately. This system of naming compounds is regulated by international and national committees, ensuring that a compound's name imparts essential information about its constituents and structure.

In the case of binary compounds, which consist of two nonmetallic elements, these names usually end with '-ide'. This indicates that the compound is made from two different elements by adding the suffix '-ide' to the second element. For example, in the compound \(\mathrm{SiCl}_{4}\), silicon, the first element, retains its name, while chlorine changes to chloride.

Learning the intricacies of this system can be akin to solving a puzzle, with each piece representing a component of the compound's identity. This basis provides a reliable pathway for students to not only name compounds but also deduce possible structures and compositions from a given name.

Compounds of Nonmetallic Elements

Binary compounds composed of nonmetallic elements can be intriguing as they often form molecules with unique properties. These compounds are typically covalent, meaning the atoms share electrons to achieve stability. When naming them, it's crucial to consider both elements involved.

For instance, \(\mathrm{XeF}_{4}\) is a compound of xenon and fluorine, both nonmetals. The molecule is covalently bonded and described as xenon tetrafluoride, revealing both the nature of its bonds and the ratio of atoms within the molecule. Grasping the differences between compounds of nonmetallic elements versus those involving metals (which often form ionic bonds) is crucial for understanding their chemical behavior and potential reactions.

Prefixes in Compound Names

The use of prefixes in compound names serves as a direct way to signify the number of atoms of each element present within a molecule.

Let's illustrate how prefixes work through examples: For \(\mathrm{XeF}_{6}\), the prefix 'hexa-' indicates that there are six fluorine atoms bonded to a single xenon atom, hence xenon hexafluoride. Similarly, \(\mathrm{SiCl}_{4}\) is named silicon tetrachloride, with 'tetra-' reflecting the presence of four chlorine atoms.

These prefixes are essential tools, especially when dealing with molecules of the same elements but different ratios. They eliminate ambiguity and allow for a precise description of the substance at hand. For students learning to write and interpret these names, mastering prefixes is a fundamental aspect of chemical nomenclature that empowers them to communicate complex information efficiently.