Name: ionic charges, formulas, and naming rules
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Ionic Compounds: Formulas and Nomenclature

Ionic compounds form ionic bonds between positively charged metal ions, or cations, and negatively charged nonmetal ions, or anions. These compounds are represented by chemical formulas.

Consider calcium fluoride. First, specify the ions of each element and their respective ionic charges. Start with the cations followed by anions.

Ionic charges can be determined from the group number of the element in the periodic table. Calcium from group 2 forms cations with an ionic-charge of 2+. Conversely, fluorine from group 17 forms anions with an ionic-charge of 1&minus;.

Next, the overall charge within the formula is balanced by employing a crisscross method. The cationic subscript is numerically matched to the anionic charge and vice versa, generating a charge-neutral chemical formula.&nbsp;

All ionic compounds are named by following a systematic naming convention called the chemical nomenclature. The chemical formula helps determine the name of the compound.&nbsp;

Binary ionic compounds name the metal cation first, succeeded by a parenthesized Roman-numeral indicating the metal charge if the metal can exist in different cationic states. The anion base-name ending with the suffix &lsquo;&ndash;ide&rsquo; follows last.&nbsp;

Consider the following three molecules. The cations are sodium or iron. The anions are iodide or bromide. Since sodium forms only a single type of cation, the parenthesized Roman-numeral is excluded. Iron forms two types of cations, which are displayed using parenthesized Roman-numerals. Thus, the names are sodium iodide, iron(II) bromide, and iron(III) bromide.

Polyatomic ionic compounds follow the same nomenclature rules, but apply the polyatomic anion name instead of the suffix &lsquo;-ide&rsquo;. Polyatomic anions containing oxygen, or oxyanions, are named based on the number of oxygen atoms.&nbsp;

For example, multiple polyatomic ionic compounds are formed between sodium and oxyanions of bromine.&nbsp;

The most common oxyanion of an element is named by combining the element&rsquo;s base-name with the suffix &lsquo;&ndash;ate&rsquo;. The suffix changes to &lsquo;&ndash;ite&rsquo; with one less oxygen, or it is given the prefix &lsquo;per&ndash;&rsquo; with one oxygen atom more.&nbsp;

Lastly, the oxyanion with one oxygen atom fewer than the oxyanion ending with &lsquo;&ndash;ite&rsquo; obtains the prefix &lsquo;hypo&ndash;&rsquo;. Therefore the ionic compounds are sodium perbromate, sodium bromate, sodium bromite, and sodium hypobromite.

Hydrated ionic compounds or hydrates like CaCl2∙2H2O contain chemically-associated water molecules. The ionic part is named first. The number of water molecules is indicated using Greek-numeral-prefixes followed by the suffix &lsquo;&ndash;hydrate.&rsquo; The chemical name of CaCl2∙2H2O is calcium chloride dihydrate.

ionic compounds: formulas and nomenclature

An element composed of atoms that readily lose electrons (a metal) can react with an element composed of atoms that readily gain electrons (a nonmetal) to produce ions through complete electron transfer. The compound formed by this transfer is stabilized by the electrostatic attractions (ionic bonds) between the oppositely charged ions.

Moving from the far right to the left on the periodic table, nonmetal elements often gain electrons to form anions with the same number of electrons as an atom of the next noble gas in the periodic table, and a negative charge equal to the number of groups moved left from the noble gases. That is, atoms of group 17 gain one electron and form anions with a 1&minus; charge; atoms of group 16 gain two electrons and form ions with a 2&minus; charge, and so on. For example, a neutral oxygen atom, with 8 protons and 8 electrons, readily gains two electrons. This results in an anion with 8 protons, 10 electrons, and a 2&minus; charge, and is symbolized as O2&minus;. The anion, O2&minus;, has the same number of electrons as the next noble gas &ndash; neon. The name of the anions is the name of the nonmetallic element with its ending replaced by the suffix -ide, so O2&minus; is called oxide.

Transition metals and some other metals often exhibit variable charges that are not predictable by their location in the table. For example, copper can form ions with a 1+ or 2+ charge, and iron can form ions with a 2+ or 3+ charge.

In every ionic compound, the total number of positive charges of the cations equals the total number of negative charges of the anions. Thus, ionic compounds are electrically neutral, even though they contain positive and negative ions. The formula of an ionic compound must have a ratio of ions such that the numbers of positive and negative charges are equal.

For example, if a compound contains aluminum and oxygen in the form of &nbsp;Al3+ and O2&minus;, the formula of the compound would be Al2O3. Two aluminum ions, each with a charge of 3+, would give us six positive charges, and three oxide ions, each with a charge of 2&minus;, would give us six negative charges. Thus, the compound will be electrically neutral, with the same number of positive and negative charges.

Many ionic compounds contain polyatomic ions as the cation, the anion, or both. Polyatomic ions are a group of bonded atoms that act as discrete units, carrying an overall charge. As with simple ionic compounds, these compounds must also be electrically neutral, so their formulas can be predicted by treating the polyatomic ions as discrete units. Parentheses are used in the formula to indicate polyatomic ions that behave as a unit. For example, the formula for calcium phosphate, one of the minerals in our bones, is Ca3(PO4)2. The compound contains the polyatomic ion PO43&minus;,&nbsp;consisting of one phosphorus atom and four oxygen atoms, and having an overall charge of 3&minus;. This formula indicates that there are three Ca2+ ions (total six positive charges) for every two PO43&minus; groups (total six negative charges). The compound is electrically neutral, and its formula shows a total count of three Ca, two P, and eight O atoms.

Ionic compounds are symbolized by formula, indicating the relative numbers of its constituent ions. For compounds containing only monatomic ions (such as NaCl) and for many compounds containing polyatomic ions (such as CaSO4), these formulas are just the empirical formulas. However, the formulas for some ionic compounds containing polyatomic ions are not empirical formulas. For example, the ionic compound sodium oxalate is composed of Na+ and C2O42&minus; ions combined in a 2:1 ratio, and its formula is written as Na2C2O4.&nbsp;

<h4>Nomenclature of Ionic Compounds</h4>

The name of a binary compound containing monatomic ions consists of the name of the cation (the name of the metal) followed by the name of the anion (the name of the nonmetallic element with its ending replaced by the suffix -ide). For example, the name for Na2O is sodium oxide.

Compounds containing polyatomic ions are also named similarly to those containing only monatomic ions, i.e., by naming first the cation and then the anion. For example, the name for CaSO4 is calcium sulfate.

Most of the transition metals and some main group metals can form two or more cations with different charges. Compounds of these metals with nonmetals are named with the same method as binary compounds, except the charge of the metal ion is specified by a Roman numeral in parentheses after the name of the metal.&nbsp;

The charge of a metal ion is determined from the formula of the compound and the charge of anion. For example, in a binary ionic compound of iron and chlorine, iron typically exhibits a charge of either 2+ or 3+, and the two corresponding compound formulas are FeCl2 and FeCl3. In such cases, the charge of the metal ion is included as a Roman numeral in parentheses immediately following the metal name. These two compounds are hence named iron(II) chloride and iron(III) chloride, respectively.&nbsp;

Ionic compounds that contain water molecules as integral components of their crystals are called hydrates. The name for an ionic hydrate is derived by adding a term to the name for the anhydrous (meaning &ldquo;not hydrated&rdquo;) compound that indicates the number of water molecules associated with each formula unit of the compound. The added word begins with a Greek prefix denoting the number of water molecules and ends with &ldquo;hydrate.&rdquo; For example, the anhydrous compound copper(II) sulfate also exists as a hydrate containing five water molecules and named copper(II) sulfate pentahydrate (penta = 5). Washing soda is the common name for a hydrate of sodium carbonate containing ten water molecules; the systematic name is sodium carbonate decahydrate (deca = 10).

Formulas for ionic hydrates are written by appending a vertically centered dot, a coefficient representing the number of water molecules, and the formula for water. For example, copper(II) sulfate pentahydrate is written as CuSO4∙5H2O.

This text is adapted from <a href="https://openstax.org/books/chemistry-2e/pages/2-6-molecular-and-ionic-compounds">Openstax, Chemistry 2e, Section 2.6: Molecular and Ionic Compounds and Openstax, Chemistry 2e, Section 2.7: Chemical Nomenclature</a>.

An element composed of atoms that readily lose electrons (a metal) can react with an element composed of atoms that readily gain electrons (a nonmetal) to ...

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ionic charges, formulas, and naming rules

Ionic compounds form when metals transfer electrons to nonmetals and create oppositely charged ions. The electrostatic attraction between the ions, called an ionic bond, holds the compound together. Many nonmetals gain electrons by moving toward the electron count of the next noble gas. Group 17 atoms usually gain one electron and form 1− ions, while group 16 atoms usually gain two electrons and form 2− ions.

Oxygen is a clear example. A neutral oxygen atom has 8 protons and 8 electrons. When it gains two electrons, it becomes O2− with 8 protons, 10 electrons, and a 2− charge. This ion has the same number of electrons as neon, and its name becomes oxide.

Some metals, especially transition metals and a few others, can form more than one positive ion. Copper can form 1+ or 2+ ions, and iron can form 2+ or 3+ ions. In every ionic compound, the total positive charge must match the total negative charge. That is why ionic compounds are electrically neutral, even though they contain charged particles. For example, aluminum and oxygen form Al2O3 because two Al3+ ions balance three O2− ions.

Many ionic compounds include polyatomic ions, which are groups of bonded atoms that act as one charged unit. These compounds must also stay electrically neutral, so the ions are treated as units when writing formulas. Parentheses show when a polyatomic ion appears more than once. Calcium phosphate is written as Ca3(PO4)2 because three Ca2+ ions balance two PO43− groups. This formula gives three calcium atoms, two phosphorus atoms, and eight oxygen atoms. Some ionic formulas match empirical formulas, such as NaCl and CaSO4, but others do not. Sodium oxalate, for example, is written as Na2C2O4 because Na+ and C2O42− combine in a 2:1 ratio.

Naming ionic compounds follows a set pattern. For binary compounds with monatomic ions, the cation name comes first, followed by the anion name with an -ide ending. Sodium oxide is the name for Na2O. Compounds with polyatomic ions are named the same way, so CaSO4 is calcium sulfate.

When a metal can form more than one charge, the name includes a Roman numeral to show the ion charge. The charge is found from the formula and the anion charge. Iron with chlorine forms FeCl2 and FeCl3, which are named iron(II) chloride and iron(III) chloride. Ionic hydrates are compounds that include water molecules in their crystal structure. Their names add a Greek prefix plus hydrate, such as copper(II) sulfate pentahydrate and sodium carbonate decahydrate. Hydrates are written with a dot and the water formula, as in CuSO4·5H2O.

Ionic Charges, Formulas, and Naming Rules

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Learn how ionic charges balance in formulas, how polyatomic ions are written with parentheses, and how to name ionic compounds and hydrates.

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Ionic Charges, Formulas, and Naming Rules

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