Question

Name each of the following ionic or covalent compounds: a. \(\mathrm{N}_{2}\) Earth's atmosphere b. \(\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) antacid c. \(\mathrm{FeSO}_{4}\) iron supplement in vitamins d. \(\mathrm{N}_{2} \mathrm{O}_{4}\) rocket fuel e. \(\mathrm{Cu}_{2} \mathrm{O}\) fungicide f. \(\mathrm{NI}_{3}\) contact explosive

Short answer

a. Dinitrogen (Nitrogen gas), b. Magnesium phosphate, c. Iron(II) sulfate (Ferrous sulfate), d. Dinitrogen tetroxide, e. Copper(I) oxide, f. Nitrogen triiodide.

Step-by-step solution

- Identify Compound Type

Determine if the compound is ionic or covalent. Ionic compounds consist of metals and non-metals, while covalent compounds consist entirely of non-metals.

- Name Covalent Compounds

For covalent compounds (entirely non-metals), use the prefixes (mono-, di-, tri-, etc.) to indicate the number of each atom present. Here are the names for the covalent compounds:a. \(\text{N}_2\): Dinitrogen (common name: nitrogen gas)d. \(\text{N}_2 \text{O}_4\): Dinitrogen tetroxidef. \(\text{NI}_3\): Nitrogen triiodide

- Name Ionic Compounds with Polyatomic Ions

For ionic compounds containing polyatomic ions and metals with fixed charges, use the name of the metal followed by the name of the polyatomic ion. Here are the names for these compounds:b. \(\text{Mg}_3(\text{PO}_4)_2\): Magnesium phosphatec. \(\text{FeSO}_4\): Iron(II) sulfate (common name: ferrous sulfate)e. \(\text{Cu}_2 \text{O}\): Copper(I) oxide

Key concepts

ionic compounds

Ionic compounds form when a metal reacts with a non-metal, transferring electrons to create ions. The metal loses electrons to become a positively charged cation, while the non-metal gains electrons to become a negatively charged anion. These opposite charges attract, forming an ionic bond. For example, in \(\text{Mg}_3(\text{PO}_4)_2\), magnesium (a metal) combines with phosphate (a polyatomic ion).
To name ionic compounds, start with the name of the metal, then add the name of the non-metal with an 'ide' suffix, or the name of the polyatomic ion unchanged.

• If the metal can form ions of different charges, specify the charge with Roman numerals in parentheses.
• For example, \(\text{FeSO_4}\) is named iron(II) sulfate, indicating iron's +2 charge.

covalent compounds

Covalent compounds, also known as molecular compounds, form when two non-metals share electrons to achieve stability. These bonds involve the sharing of electron pairs between atoms.

For example, consider \(\text{N}_2O_4\), which consists of nitrogen and oxygen. Here, nitrogen atoms share electrons with oxygen atoms to form the compound.

To name covalent compounds:

• Use prefixes to indicate the number of each type of atom: mono- (1), di- (2), tri- (3), tetra- (4), and so on.
• For instance, \(\text{N}_2O_4\) is called dinitrogen tetroxide.

chemical nomenclature

Chemical nomenclature is the systematic naming of chemical compounds based on their composition and structure.

For ionic and covalent compounds, the naming conventions differ:

• For ionic compounds, name the metal first, followed by the non-metal with an 'ide' suffix or use the polyatomic ion's name.
• For covalent compounds, use prefixes to indicate the number of atoms and add appropriate suffixes.

An example of this is \(\text{NI}_3\), named nitrogen triiodide, reflecting the presence of three iodine atoms bonded to one nitrogen atom.

Following these rules ensures clarity and consistency in chemical communication.

polyatomic ions

Polyatomic ions are ions composed of two or more atoms covalently bonded, carrying a net electrical charge. They act as a single unit in chemical reactions.

For example, in \(\text{Mg}_3(\text{PO}_4)_2\), the phosphate ion \(\text{PO}_4^{3-}\) is a polyatomic ion.
Common polyatomic ions include:

• Sulfate (\text{SO}_4^{2-})
• Nitrate (\(\text{NO}_3^{-}\))
• Hydroxide (\(\text{OH}^{-}\))

When naming compounds containing polyatomic ions, use the ion's name directly. For instance, \(\text{FeSO}_4\) is named iron(II) sulfate.

Understanding polyatomic ions is essential for accurately naming and writing chemical formulas.