Question

Name each of the following binary, nonionic compounds: (a) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (b) \(\mathrm{P}_{4} \mathrm{S}_{3}\) (c) \(\mathrm{OF}_{2}\) (d) \(\mathrm{XeF}_{4}\)

Short answer

(a) dinitrogen pentoxide, (b) tetraphosphorus trisulfide, (c) oxygen difluoride, (d) xenon tetrafluoride.

Step-by-step solution

Identify the Chemical Formula

Recognize the compound formula and identify the number of each type of atom present. For example, in (a) \(\mathrm{N}_2\mathrm{O}_5\), there are 2 nitrogen atoms and 5 oxygen atoms.

Apply Naming Rules for Binary Covalent Compounds

For binary covalent compounds, use prefixes to indicate the number of each type of atom. The prefixes are: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, and deca-. The first element does not use 'mono-' if there is only one atom of the first element.

Name Each Compound Part (a)

For \(\mathrm{N}_2\mathrm{O}_5\), use the prefix 'di-' for two nitrogen atoms, and 'penta-' for five oxygen atoms. The name is dinitrogen pentoxide.

Name Each Compound Part (b)

For \(\mathrm{P}_4\mathrm{S}_3\), use the prefix 'tetra-' for four phosphorus atoms, and 'tri-' for three sulfur atoms. The name is tetraphosphorus trisulfide.

Name Each Compound Part (c)

For \(\mathrm{OF}_2\), there is one oxygen atom, so no prefix is needed, and 'di-' for two fluorine atoms. The name is oxygen difluoride.

Name Each Compound Part (d)

For \(\mathrm{XeF}_4\), there is one xenon atom, so no prefix is needed, and 'tetra-' for four fluorine atoms. The name is xenon tetrafluoride.

Key concepts

Nomenclature

In chemistry, nomenclature is the system used to name chemical compounds. Each name provides information about the chemical composition of the compound, helping identify its elements and the proportions in which they are combined. For binary covalent compounds—compounds made from two different non-metal elements—the naming system relies on several rules. Typically, the first element's name comes first, followed by the second element’s name modified to end in '-ide.' The number of atoms of each element in the compound is indicated using specific prefixes. Understanding this systematic naming helps chemists around the world communicate more effectively and avoid confusion.

Chemical Formulas

Chemical formulas are not just random groupings of letters and numbers. They provide essential information about the elements present in a compound and the ratio of these elements. In a binary covalent compound, the chemical formula shows exactly which two non-metal atoms are bonded together.For example, in the compound \( \mathrm{N}_2\mathrm{O}_5 \), this formula reveals that there are two nitrogen atoms for every five oxygen atoms. Recognizing the correct chemical formula is the first step in naming a compound, as it guides you on how many atoms each element has, allowing you to apply the correct prefixes. Understanding how to read and write these formulas is crucial for both studying and experimenting in chemistry.

Prefixes in Chemistry

Chemistry uses specific prefixes to indicate the number of atoms of each element in a compound. These prefixes help to clearly specify how many atoms are involved and alleviate any ambiguity in the naming process. The most common prefixes include:

• Mono- (1)
• Di- (2)
• Tri- (3)
• Tetra- (4)
• Penta- (5)
• Hexa- (6)
• Hepta- (7)
• Octa- (8)
• Nona- (9)
• Deca- (10)

For instance, the name dinitrogen pentoxide indicates that there are two nitrogen atoms and five oxygen atoms. When using these prefixes, an important rule is to omit 'mono-' for the first element if there is only one atom.

Covalent Bonds

Covalent bonds are a type of chemical bond where atoms share pairs of electrons. This kind of bonding is common in compounds made from two non-metal elements, like the binary covalent compounds we've been discussing. Each covalent bond between two atoms involves the sharing of electrons to achieve stability in their outer electron shells, similar to noble gases. For example, in a molecule like \( \mathrm{OF}_2 \), oxygen shares electrons with two fluorine atoms to form a stable covalent bond. These bonds are essential for the structure and functionality of all kinds of compounds, influencing properties like their strength, flexibility, and reactivity.