Chemistry
Naming Ionic Compounds
Naming Ionic Compounds involves identifying the cation and anion present in the compound and naming them accordingly. The cation is named first, followed by the anion with the suffix "-ide" added to the end of its name. Roman numerals are used to indicate the charge of the cation if it is a transition metal.
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eBook - PDFChemistry
The Molecular Nature of Matter
- Neil D. Jespersen, Alison Hyslop(Authors)
- 2021(Publication Date)
- Wiley(Publisher)
In addition, when we first name a compound in this book, we will give the IUPAC name first, followed by the common name, if there is one, in parentheses. We will subsequently use the common name. Naming Ionic Compounds of Representative Elements In this section we discuss the nomenclature (naming) of simple inorganic ionic com- pounds. In general, inorganic compounds are substances that are not derived from hydro- carbons such as methane (CH 4 ), ethane (C 2 H 6 ), and other carbon–hydrogen compounds. In Naming Ionic Compounds, our goal is a name that someone else could use to write the formula. For ionic compounds, the name of the cation is given first, followed by the name of the anion. This is the same as the sequence in which the ions appear in the formula. If the metal in the compound forms only one cation, such as Na + or Ca 2+ , the cation takes the English name of the metal. The anion in a binary compound is formed from a nonmetal, and its name is created by adding the suffix -ide to the stem of the name for the nonmetal. An example TOOLS Naming Ionic Compounds 2.6 Nomenclature of Ionic Compounds 95 TABLE 2.5 Monatomic Negative Ions H − hydride C 4− carbide N 3− nitride O 2− oxide F − fluoride Si 4− silicide P 3− phosphide S 2− sulfide Cl − chloride As 3− arsenide Se 2− selenide Br − bromide Te 2− telluride I − iodide is KBr, potassium bromide. Table 2.5 lists some common monatomic (one-atom) negative ions and their names. It is also useful to know that the -ide suffix is usually used only for monatomic ions, with just two common exceptions—the hydroxide ion (OH ‒ ) and the cyanide ion (CN ‒ ). To form the name of an ionic compound, we simply specify the names of the cation and anion. We do not need to state how many cations or anions are present, since once we know what the ions are, we also know the charges of those ions, and we have all the information needed to assemble the correct formula as we just did in the previous section.
eBook - PDFChemistry
The Molecular Nature of Matter
- Neil D. Jespersen, Alison Hyslop(Authors)
- 2014(Publication Date)
- Wiley(Publisher)
Additionally, we will be able to take a formula and correctly name it, since up to this point we have used common names for substances. In addition, when we first name a compound in this book, we will give the IUPAC name first, followed by the common name, if there is one, in parentheses. We will subsequently use the common name. Naming Ionic Compounds of Representative Elements In this section we discuss the nomenclature (naming) of simple inorganic ionic compounds. In general, inorganic compounds are substances that are not derived from hydrocarbons such as methane (CH 4 ), ethane (C 2 H 6 ), and other carbon–hydrogen compounds. In Naming Ionic Compounds, our goal is a name that someone else could use to write the formula. For ionic compounds, the name of the cation is given first, followed by the name of the anion. This is the same as the sequence in which the ions appear in the formula. If the metal in the compound forms only one cation, such as Na + or Ca 2+ , the cation takes the English name of the metal. The anion in a binary compound is formed from a nonmetal and its name is created by adding the suffix -ide to the stem of the name for the nonmetal. An example is KBr, potassium bromide. Table 2.5 lists some common monatomic (one-atom) negative ions and their names. It is also useful to know that the -ide suffix is usually used only for monatomic ions, with just two common exceptions—the hydroxide ion (OH - ) and the cyanide ion (CN - ). To form the name of an ionic compound, we simply specify the names of the cation and anion. We do not need to state how many cations or anions are present, since once we know what the ions are we can assemble the correct formula as we just did in the previous section.
eBook - PDF- Rose Marie O. Mendoza(Author)
- 2023(Publication Date)
- Arcler Press(Publisher)
Note: Cations are always named before anions. Most transition metals, many actinides, and the heaviest elements of groups 13–15 can form more than one cation (Finke and Özkar, 2004). There is a systematic method used to name ionic compounds. Ionic compounds are named according to systematic procedures, although common names are widely used. Systematic nomenclature enables chemists to write the structure of any compound from its name and vice versa. Ionic compounds are named by writing the cation first, followed by the anion. If a metal can form cations with more than one charge, the charge is indicated by An Overview of Inorganic Compounds 28 roman numerals in parentheses following the name of the metal. Oxoanions are polyatomic anions that contain a single metal or nonmetal atom and one or more oxygen atoms (Boiocchi et al., 2004). 2.3. NAMING COVALENT COMPOUNDS As with ionic compounds, the system for naming covalent compounds enables chemists to write the molecular formula from the name and vice versa. This and the following section describe the rules for naming simple covalent compounds, beginning with inorganic compounds, and then turning to simple organic compounds that contain only carbon and hydrogen (Morris, 2011). When chemists synthesize a new compound, they may not yet know its molecular or structural formula. In such cases, they usually begin by determining its empirical formula, the relative numbers of atoms of the elements in a compound, reduced to the smallest whole numbers. Because the empirical formula is based on experimental measurements of the numbers of atoms in a sample of the compound, it shows only the ratios of the numbers of the elements present. The difference between empirical and molecular formulas can be illustrated with butane, a covalent compound used as the fuel in disposable lighters. The molecular formula for butane is C 4 H 10 . The ratio of carbon atoms to hydrogen atoms in butane is 4:10, which can be reduced to 2:5.
eBook - PDFChemistry
An Industry-Based Introduction with CD-ROM
- John Kenkel, Paul B. Kelter, David S. Hage(Authors)
- 2000(Publication Date)
- CRC Press(Publisher)
Ionic and covalent are words that describe the nature of the chemical combination involved. In this chapter, we examine these concepts in more detail in order to characterize the nature of chemical combination and the reasons why elements come together to form compounds in the way that they do. We also look at the schemes for naming common compounds and at the symbolism used for expressing chemical change in the formation and destruction of compounds. 2.2 Formulas of Ionic Compounds Positively charged ions are called cations (pronounced “cat-eye-uns”) and negatively charged ions are called anions (pronounced “ann-eye-uns”). Cations and anions come together to form formula units because oppositely charged ions attract each other electrostatically. Cations attract anions, and vice versa, in a manner similar to the way in which opposite poles of a magnet attract each other. If the cation has 26 Chemistry An Industry-Based Introduction with CD-ROM a charge of +1 (as opposed to +2 or +3), it attracts and exactly neutralizes one anion that has a charge of 1. With these two ions electrostatically stuck to each other, the result is a formula unit that has neither a positive charge nor a negative charge, but is neutral, or has no net charge. An ionic compound, with a set formula, has thus formed. For example, one sodium ion, Na + , and one chloride ion, Cl , by virtue of their equal but opposite charges, attract each other forming the formula unit depicted in Fig. 2.1(A). The result is a compound with the formula NaCl. 1 A similar one-to-one combination occurs between any cation with a charge of +1 and any anion with a charge of -1. Examples include the ammonium ion or any alkali metal ion (+1) combined with the nitrate ion, the hydroxide ion, or any monatomic ion formed from a halogen atom ( 1). These latter ions are called the “halide” ions: fluoride (F ), chloride (Cl ), bromide (Br ), and iodide (I ).
- Morris Hein, Scott Pattison, Susan Arena, Leo R. Best(Authors)
- 2014(Publication Date)
- Wiley(Publisher)
Thus we do not say calcium(II) chloride for CaCl 2 , but rather calcium chloride, since the charge of calcium is understood to be 12. In classical nomenclature, when the metallic ion has only two cation types, the name of the metal (usually the Latin name) is modified with the suffixes -ous and -ic to distinguish between the two. The lower-charge cation is given the -ous ending, and the higher one, the -ic ending. Examples: FeCl 2 ferrous chloride Fe 2 + (lower-charge cation) FeCl 3 ferric chloride Fe 3 + (higher-charge cation) CuCl cuprous chloride Cu + (lower-charge cation) CuCl 2 cupric chloride Cu 2 + (higher-charge cation) Table 6.4 lists some common metals that have more than one type of cation. Notice that the ous–ic naming system does not give the charge of the cation of an element but merely indicates that at least two types of cations exist. The Stock System avoids any pos- sible uncertainty by clearly stating the charge on the cation. iron(II) chloride iron(III) chloride FeCl 2 FeCl 3 charge: �2 �1 �3 �1 name: iron(II) chloride iron(III) chloride RULES FOR NAMING BINARY IONIC COMPOUNDS OF METAL FORMING TWO OR MORE TYPES OF CATIONS (STOCK SYSTEM) 1. Write the name of the cation. 2. Write the charge on the cation as a Roman numeral in parentheses. 3. Write the stem of the anion and add the suffix -ide. 108 CHAPTER 6 • Nomenclature of Inorganic Compounds Prefix Number mono 1 di 2 tri 3 tetra 4 penta 5 hexa 6 hepta 7 octa 8 nona 9 deca 10 Binary Compounds Containing Two Nonmetals Compounds between nonmetals are molecular, not ionic. Therefore, a different system for naming them is used. In a compound formed between two nonmetals, the element that occurs first in this series is written and named first: Si, B, P, H, C, S, I, Br, N, Cl, O, F The name of the second element retains the -ide ending as though it were an anion.
eBook - PDF- Rose Marie O. Mendoza(Author)
- 2023(Publication Date)
- Arcler Press(Publisher)
The word “ion” is then omitted when identifying ionic compounds, and the names of the anions and cations are combined, with cation always stated first then the anion mentioned last.. Remember that roman numerals are only used when talking about metals that has more than potential ionic state/ oxidation number or charge. Whenever the Na + and Cl – atoms combine to form NaCl, the resultant chemical is known as sodium chloride. When Mg 2+ and Cl – combine to form MgCl 2 , the resultant chemical is known as magnesium chloride. This follows the formula: Name of the metallic substance (cation) then the name of the non-metallic substance (anion) with its ending changed to -ide. Introduction to Ions and Ionic Compounds 17 When the metal component in an ionic bond contain more than one ionic charge/state, the roman numerical value representing its actual ionic charge is employed to determine that that specific ion is involved in the bond. For instance, if Fe 3 + and Cl – react to generate FeCl 3 , we’ll have to differentiate it from Fe 2 + and Cl – reacting to generate FeCl 2 . This indicate that FeCl 3 in another sense be written as Fe (III) Chloride, while FeCl 2 is alternatively written as Fe (II) Chloride (Wulfsberg et al., 2006; Thong et al., 2015). While it arises to Naming Ionic Compounds, the most significant thing to recall is that you’ll be capable of drawing the shape from the name and build the term from the structure. Let’s put our skills to the test! Practice Exercise 1 1. Name the formula of the compound when the following ions combine: (a) zinc and sulfur, (b) aluminun and oxygen, (c) Lead (+4) and chlorine, (d) mercury and fluorine, (e) Chro- mium (+6) and sulfur 2. Write the name of the following compound both in IUPAC and roman numeral system (for cations with multiple charges): (a) arsenic chloride, (b) Chromium (III) fluoride, (c) arsenic (V) nitride, (d) potassium bromide, (e) Barium oxide 1.6.
eBook - PDF- Morris Hein, Susan Arena, Cary Willard(Authors)
- 2016(Publication Date)
- Wiley(Publisher)
A s children, we begin to communicate with other people in our lives by learning the names of ob- jects around us. As we continue to develop, we learn to speak and use language to complete a wide vari- ety of tasks. As we enter school, we begin to learn of other languages—the languages of mathematics, of other cul- tures, of computers. In each case, we begin by learning the names of the building blocks and then proceed to more abstract concepts. Chemistry has a language all its own—a whole new way of describing the objects so familiar to us in our daily lives. For example, the seashell shown above is formed from the chemical calcium carbonate, commonly called limestone. It is the same chemical used in many calcium supple- ments for our diets. Once we learn the language, we can begin to understand the macroscopic and microscopic world of chemistry. © Exactostock /SuperStock Nomenclature of Inorganic Compounds C H A P T E R O U T L I N E 6.1 Common and Systematic Names 6.2 Elements and Ions 6.3 Writing Formulas from Names of Ionic Compounds 6.4 Naming Binary Compounds 6.5 Naming Compounds Containing Polyatomic Ions 6.6 Acids 6 6.2 • Elements and Ions 103 6.1 Common and Systematic Names Distinguish between the common and systematic names of chemical substances. Chemical nomenclature is the system of names that chemists use to identify compounds. When a new substance is formulated, it must be named in order to distinguish it from all other substances (FIGURE 6.1). In this chapter, we will restrict our discussion to the nomenclature of inorganic compounds—compounds that do not generally contain carbon. 3 or more Polyatomic compounds See Section 6.5 2 Binary compounds See Section 6.4 1 Element See Sections 3.1–3.4 Number of Elements Present FIGURE 6.1 Where to find rules for naming inorganic substances in this book. Common names are arbitrary names that are not based on the chemical composition of compounds.
eBook - PDF- David A. Ucko(Author)
- 2013(Publication Date)
- Academic Press(Publisher)
Table 7-2 lists the most common simple cations and anions. You can use this table to name many ionic compounds. As with covalent compounds, the formulas and names of ionic com-pounds are written with the most electronegative element last. Sodium chloride, NaCl, is a typical example. sodium chlor ide name of root of ending of cation anion anion 188 WRITING NAMES AND FORMULAS OF COMPOUNDS / 7.2 IONIC COMPOUNDS TABLE 7-2 Names of simple ions Cation Anion Symbol Name Symbol Name H + hydrogen ion fluoride ion Li + lithium ion c i -chloride ion Na + sodium ion Br bromide ion K + potassium ion I-iodide ion Mg 2 + magnesium ion O 2 oxide ion Ca 2+ calcium ion s 2 -sulfide ion Al 3+ aluminum ion N 3 nitride ion Other examples are: magnesium oxide, MgO; potassium sulfide, K 2 S ; calcium bromide, CaBr 2 ; aluminum chloride, A1C1 3 . As will be described in detail in Chapter Fifteen, atoms can be assigned oxidation numbers. These numbers reflect the way charges are distributed among the atoms in a molecule or formula unit. In the case of simple metal cations, the oxidation number of the metal is the same as the charge of the ion. For example, the oxidation number of sodium in N a + is + 1 . This number is said to represent the oxidation state of the element. Most transition metals have more than one oxidation state. To prop-erly identify the compound, the oxidation number must be written as a Roman numeral after the name of the metal. (The first six Roman numerals are: I, II, III, IV, V, VI.) For example, the name iron chloride is incomplete. It could mean either FeCl 2 , iron(II) chloride, or FeCl 3 , iron(III) chloride. Certain common elements, like iron, have only two major oxidation states, and an older system of naming used the endings -ous and Ac to distinguish these states. In that system, iron(II), F e 2 + , was ferrous ion, and iron(III), F e 3 + was ferric ion. In general, the lower state ends in -ous and the higher state in -ic.
eBook - PDF- John Kenkel(Author)
- 2010(Publication Date)
- CRC Press(Publisher)
Others will be discussed later . 3.3 Formulas of Ionic Compounds As we discussed in Chapter 1 (Section 1 .4 .2), all of the more than 13 mil-lion chemical compounds that exist consist of elements in chemical combi-nation . Compounds that are covalent or molecular have molecules as their fundamental particles . Compounds that are ionic have formula units as their fundamental particles . Molecules are composed of various numbers of differ-ent atoms in covalent chemical combination; formula units are composed of various numbers of different ions . Ionic and covalent are words that describe the nature of the chemical combination involved . In this chapter, we examine these concepts in more detail in order to characterize the nature of chemical combination and the reasons why elements come together to form compounds in the ways that they do . We also look at the schemes for naming common compounds and at the Table 3.1 The “Big Six” Polyatomic Ions Formula Name NO 3 − Nitrate SO 4 2 − Sulfate PO 4 3 − Phosphate CO 3 2 − Carbonate OH − Hydroxide NH 4 + Ammonium Basic Chemistry Concepts and Exercises 70 symbolism used for expressing chemical change in the formation and destruc-tion of compounds . Positively charged ions are called cations (pronounced cat-eye-uns) and negatively-charged ions are called anions (pronounced ann-eye-uns) . Cations and anions come together to form formula units because oppositely charged ions attract each other electrostatically . Cations attract anions, and vice versa, in a manner similar to the way in which opposite poles of a magnet attract each other . If a cation has a charge of + 1 (as opposed to + 2 or + 3), it attracts and exactly neutralizes one anion that has a charge of − 1 . With these two ions electrostatically “stuck” to each other, the result is a formula unit that has neither a positive charge nor a negative charge, but is neutral, or has no net charge . An ionic compound, with a set formula, has thus formed .
eBook - PDF- Leo J. Malone, Theodore O. Dolter(Authors)
- 2012(Publication Date)
- Wiley(Publisher)
PROCEDURE A quick glance at the periodic table reveals that the first element in each compound is a representative metal and the second is a representative nonmetal. Use the metal name unchanged, and change the ending of the nonmetals to -ide. E X A M P L E 4 - 1 Naming Binary Ionic Compounds 126 CHAPTER 4 The Periodic Table and Chemical Nomenclature Write the formulas for the following binary metal–nonmetal compounds: (a) aluminum fluoride and (b) calcium selenide. PROCEDURE From the names, recognize that these compounds are representative elements. Identify their charges based on their column on the periodic table. Determine how many of each element are necessary to produce a neutral compound. Use these as subscripts in the formula. SOLUTION (a) Aluminum is in Group IIIA, so it forms a cation with a +3 charge exclusively. Fluorine is in Group VIIA, so it forms an anion with a -1 charge. Since the positive charge must be balanced by the nega- tive charge, we need three F 1- anions to balance one Al 3+ ion [e.g., +3 + (3 * -1) = 0]. Therefore, the formula is written as Al 3+ + 3(F - ) = AlF 3 (b) Calcium is in Group IIA, so it forms a +2 cation. Selenium is in Group VIA, so it forms a -2 anion. Together the charges add to zero, so one of each atom is sufficient in the formula: Ca 2+ + Se 2- = CaSe ANALYSIS Another convenient way to establish the formula is to write the ions with their appropriate charges side by side. The numerical value of the charge on the cation becomes the subscript on the anion, and vice versa. The number 1 is understood instead of written as a subscript. This is known as the cross-charge method. Notice that, in (b), by exchanging values of the charge, we first indicate a formula of Ca 2 Se 2 . This is not a correct representation, however. Ionic compounds should be expressed with the simplest whole numbers for subscripts.
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