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2.4: Naming Covalent Compounds

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    Learning Objectives

    • To name covalent compounds that contain up to three elements.

    As with ionic compounds, the system that chemists have devised for naming covalent compounds enables us to write the molecular formula from the name and vice versa. In this and the following section, we describe the rules for naming simple covalent compounds. We begin with inorganic compounds and then turn to simple organic compounds that contain only carbon and hydrogen.

    Binary Inorganic Compounds

    Binary covalent compounds—that is, covalent compounds that contain only two elements—are named using a procedure similar to that used to name simple ionic compounds, but prefixes are added as needed to indicate the number of atoms of each kind. The procedure, diagrammed in  Figure \(\PageIndex{1}\) , uses the following steps:

    Figure \(\PageIndex{1}\)Naming a Covalent Inorganic Compound



    1. Place the elements in their proper order.

      1. The element farthest to the left in the periodic table is usually named first. If both elements are in the same group, the element closer to the bottom of the column is named first.
      2. The second element is named as if it were a monatomic anion in an ionic compound (even though it is not), with the suffix -ide attached to the root of the element name.
    2. Identify the number of each type of atom present.

      1. Prefixes derived from Greek stems are used to indicate the number of each type of atom in the formula unit (Table \(\PageIndex{1}\) ). The prefix mono- (“one”) is used only when absolutely necessary to avoid confusion, just as we omit the subscript 1 when writing molecular formulas.

        To demonstrate steps 1 and 2a, we name HCl as hydrogen chloride (because hydrogen is to the left of chlorine in the periodic table) and PCl5 as phosphorus pentachloride. The order of the elements in the name of BrF3, bromine trifluoride, is determined by the fact that bromine lies below fluorine in group 17.

        Table \(\PageIndex{1}\)  Prefixes for Indicating the Number of Atoms in Chemical Names

        Prefix Number
        mono- 1
        di- 2
        tri- 3
        tetra- 4
        penta- 5
        hexa- 6
        hepta- 7
        octa- 8
        nona- 9
        deca- 10
        undeca- 11
        dodeca- 12
      2. If a molecule contains more than one atom of both elements, then prefixes are used for both. Thus N2O3 is dinitrogen trioxide, as shown in Figure \(\PageIndex{1}\).
      3. In some names, the final a or o of the prefix is dropped to avoid awkward pronunciation. Thus OsO4 is osmium tetroxide rather than osmium tetraoxide.
    3. Write the name of the compound.

      1. Binary compounds of the elements with oxygen are generally named as “element oxide,” with prefixes that indicate the number of atoms of each element per formula unit. For example, CO is carbon monoxide. The only exception is binary compounds of oxygen with fluorine, which are named as oxygen fluorides. (The reasons for this convention will become clear in Chapter 7 "The Periodic Table and Periodic Trends" and Chapter 8 "Ionic versus Covalent Bonding".)
      2. Certain compounds are always called by the common names that were assigned long ago when names rather than formulas were used. For example, H2O is water (not dihydrogen oxide); NH3 is ammonia; PH3 is phosphine; SiH4 is silane; and B2H6, a dimer of BH3, is diborane. For many compounds, the systematic name and the common name are both used frequently, so you must be familiar with them. For example, the systematic name for NO is nitrogen monoxide, but it is much more commonly called nitric oxide. Similarly, N2O is usually called nitrous oxide rather than dinitrogen monoxide. Notice that the suffixes -ic and -ous are the same ones used for ionic compounds.

    Note the Pattern

    Start with the element at the far left in the periodic table and work to the right. If two or more elements are in the same group, start with the bottom element and work up.

    Example \(\PageIndex{1}\)

    Write the name of each binary covalent compound.

    1. SF6
    2. N2O4
    3. ClO2

    Given: molecular formula

    Asked for: name of compound


    A List the elements in order according to their positions in the periodic table. Identify the number of each type of atom in the chemical formula and then use Table \(\PageIndex{1}\)  to determine the prefixes needed.

    B If the compound contains oxygen, follow step 3a. If not, decide whether to use the common name or the systematic name.


    1. A Because sulfur is to the left of fluorine in the periodic table, sulfur is named first. Because there is only one sulfur atom in the formula, no prefix is needed. B There are, however, six fluorine atoms, so we use the prefix for six: hexa- (Table \(\PageIndex{1}\)). The compound is sulfur hexafluoride.
    2. A Because nitrogen is to the left of oxygen in the periodic table, nitrogen is named first. Because more than one atom of each element is present, prefixes are needed to indicate the number of atoms of each. According to Table \(\PageIndex{1}\), the prefix for two is di-, and the prefix for four is tetra-. B The compound is dinitrogen tetroxide (omitting the a in tetra- according to step 2c) and is used as a component of some rocket fuels.
    3. A Although oxygen lies to the left of chlorine in the periodic table, it is not named first because ClO2 is an oxide of an element other than fluorine (step 3a). Consequently, chlorine is named first, but a prefix is not necessary because each molecule has only one atom of chlorine. B Because there are two oxygen atoms, the compound is a dioxide. Thus the compound is chlorine dioxide. It is widely used as a substitute for chlorine in municipal water treatment plants because, unlike chlorine, it does not react with organic compounds in water to produce potentially toxic chlorinated compounds.


    Exercise \(\PageIndex{1}\)

    Write the name of each binary covalent compound.

    1. IF7
    2. N2O5
    3. OF2
    1. iodine heptafluoride
    2. dinitrogen pentoxide
    3. oxygen difluoride

    Example \(\PageIndex{2}\)

    Write the formula for each binary covalent compound.

    1. sulfur trioxide
    2. diiodine pentoxide

    Given: name of compound

    Asked for: formula


    List the elements in the same order as in the formula, use Table  \(\PageIndex{1}\)  to identify the number of each type of atom present, and then indicate this quantity as a subscript to the right of that element when writing the formula.


    1. Sulfur has no prefix, which means that each molecule has only one sulfur atom. The prefix tri- indicates that there are three oxygen atoms. The formula is therefore SO3. Sulfur trioxide is produced industrially in huge amounts as an intermediate in the synthesis of sulfuric acid.
    2. The prefix di- tells you that each molecule has two iodine atoms, and the prefix penta- indicates that there are five oxygen atoms. The formula is thus I2O5, a compound used to remove carbon monoxide from air in respirators.


    Exercise \(\PageIndex{2}\)

    Write the formula for each binary covalent compound.

    1. silicon tetrachloride
    2. disulfur decafluoride
    1. SiCl4
    2. S2F10


    The structures of some of the compounds in Example 8 and Example 9 are shown in Figure \(\PageIndex{2}\) along with the location of the “central atom” of each compound in the periodic table. It may seem that the compositions and structures of such compounds are entirely random, but this is not true. After you have mastered the material in Chapter 7 "The Periodic Table and Periodic Trends" and Chapter 8 "Ionic versus Covalent Bonding", you will be able to predict the compositions and structures of compounds of this type with a high degree of accuracy.


    Figure \(\PageIndex{2}\) The Structures of Some Covalent Inorganic Compounds and the Locations of the “Central Atoms” in the Periodic Table


    The compositions and structures of covalent inorganic compounds are not random. As you will learn in Chapter 7 "The Periodic Table and Periodic Trends" and Chapter 8 "Ionic versus Covalent Bonding", they can be predicted from the locations of the component atoms in the periodic table.



    Approximately one-third of the compounds produced industrially are organic compounds. All living organisms are composed of organic compounds, as is most of the food you consume, the medicines you take, the fibers in the clothes you wear, and the plastics in the materials you use. Section 2.1 "Chemical Compounds" introduced two organic compounds: methane (CH4) and methanol (CH3OH). These and other organic compounds appear frequently in discussions and examples throughout this text.

    The detection of organic compounds is useful in many fields. In one recently developed application, scientists have devised a new method called “material degradomics” to make it possible to monitor the degradation of old books and historical documents. As paper ages, it produces a familiar “old book smell” from the release of organic compounds in gaseous form. The composition of the gas depends on the original type of paper used, a book’s binding, and the applied media. By analyzing these organic gases and isolating the individual components, preservationists are better able to determine the condition of an object and those books and documents most in need of immediate protection.

    The simplest class of organic compounds is the hydrocarbons, which consist entirely of carbon and hydrogen. Petroleum and natural gas are complex, naturally occurring mixtures of many different hydrocarbons that furnish raw materials for the chemical industry. The four major classes of hydrocarbons are the alkanes, which contain only carbon–hydrogen and carbon–carbon single bonds; the alkenes, which contain at least one carbon–carbon double bond; the alkynes, which contain at least one carbon–carbon triple bond; and the aromatic hydrocarbons, which usually contain rings of six carbon atoms that can be drawn with alternating single and double bonds. Alkanes are also called saturated hydrocarbons, whereas hydrocarbons that contain multiple bonds (alkenes, alkynes, and aromatics) are unsaturated.


    The simplest alkane is methane (CH4), a colorless, odorless gas that is the major component of natural gas. In larger alkanes whose carbon atoms are joined in an unbranched chain (straight-chain alkanes), each carbon atom is bonded to at most two other carbon atoms. The structures of two simple alkanes are shown in Figure \(\PageIndex{3}\), and the names and condensed structural formulas for the first 10 straight-chain alkanes are in Table \(\PageIndex{2}\) . The names of all alkanes end in -ane, and their boiling points increase as the number of carbon atoms increases.


    Figure \(\PageIndex{3}\)  Straight-Chain Alkanes with Two and Three Carbon Atoms



    Table \(\PageIndex{2}\)The First 10 Straight-Chain Alkanes

    Name Number of Carbon Atoms Molecular Formula Condensed Structural Formula Boiling Point (°C) Uses
    methane 1 CH4 CH4 −162 natural gas constituent
    ethane 2 C2H6 CH3CH3 −89 natural gas constituent
    propane 3 C3H8 CH3CH2CH3 −42 bottled gas
    butane 4 C4H10 CH3CH2CH2CH3 or CH3(CH2)2CH3 0 lighters, bottled gas
    pentane 5 C5H12 CH3(CH2)3CH3 36 solvent, gasoline
    hexane 6 C6H14 CH3(CH2)4CH3 69 solvent, gasoline
    heptane 7 C7H16 CH3(CH2)5CH3 98 solvent, gasoline
    octane 8 C8H18 CH3(CH2)6CH3 126 gasoline
    nonane 9 C9H20 CH3(CH2)7CH3 151 gasoline
    decane 10 C10H22 CH3(CH2)8CH3 174 kerosene

    Alkanes with four or more carbon atoms can have more than one arrangement of atoms. The carbon atoms can form a single unbranched chain, or the primary chain of carbon atoms can have one or more shorter chains that form branches. For example, butane (C4H10) has two possible structures. Normal butane (usually called n-butane) is CH3CH2CH2CH3, in which the carbon atoms form a single unbranched chain. In contrast, the condensed structural formula for isobutane is (CH3)2CHCH3, in which the primary chain of three carbon atoms has a one-carbon chain branching at the central carbon. Three-dimensional representations of both structures are as follows:


    The systematic names for branched hydrocarbons use the lowest possible number to indicate the position of the branch along the longest straight carbon chain in the structure. Thus the systematic name for isobutane is 2-methylpropane, which indicates that a methyl group (a branch consisting of –CH3) is attached to the second carbon of a propane molecule. Similarly, you will learn in Section 2.6 "Industrially Important Chemicals" that one of the major components of gasoline is commonly called isooctane; its structure is as follows:


    As you can see, the compound has a chain of five carbon atoms, so it is a derivative of pentane. There are two methyl group branches at one carbon atom and one methyl group at another. Using the lowest possible numbers for the branches gives 2,2,4-trimethylpentane for the systematic name of this compound.


    The simplest alkenes are ethylene, C2H4 or CH2=CH2, and propylene, C3H6 or CH3CH=CH2 (part (a) in Figure 2.16 "Some Simple (a) Alkenes, (b) Alkynes, and (c) Cyclic Hydrocarbons"). The names of alkenes that have more than three carbon atoms use the same stems as the names of the alkanes (Table 2.7 "The First 10 Straight-Chain Alkanes") but end in -ene instead of -ane.

    Once again, more than one structure is possible for alkenes with four or more carbon atoms. For example, an alkene with four carbon atoms has three possible structures. One is CH2=CHCH2CH3 (1-butene), which has the double bond between the first and second carbon atoms in the chain. The other two structures have the double bond between the second and third carbon atoms and are forms of CH3CH=CHCH3 (2-butene). All four carbon atoms in 2-butene lie in the same plane, so there are two possible structures (part (a) in Figure \(\PageIndex{4}\) ). If the two methyl groups are on the same side of the double bond, the compound is cis-2-butene (from the Latin cis, meaning “on the same side”). If the two methyl groups are on opposite sides of the double bond, the compound is trans-2-butene (from the Latin trans, meaning “across”). These are distinctly different molecules: cis-2-butene melts at −138.9°C, whereas trans-2-butene melts at −105.5°C.


    Figure \(\PageIndex{4}\) Some Simple (a) Alkenes, (b) Alkynes, and (c) Cyclic Hydrocarbons


    The positions of the carbon atoms in the chain are indicated by C1 or C2.


    Just as a number indicates the positions of branches in an alkane, the number in the name of an alkene specifies the position of the first carbon atom of the double bond. The name is based on the lowest possible number starting from either end of the carbon chain, so CH3CH2CH=CH2 is called 1-butene, not 3-butene. Note that CH2=CHCH2CH3 and CH3CH2CH=CH2 are different ways of writing the same molecule (1-butene) in two different orientations.


    The name of a compound does not depend on its orientation. As illustrated for 1-butene, both condensed structural formulas and molecular models show different orientations of the same molecule. Don’t let orientation fool you; you must be able to recognize the same structure no matter what its orientation.


    Note the Pattern

    The positions of groups or multiple bonds are always indicated by the lowest number possible.


    The simplest alkyne is acetylene, C2H2 or HC≡CH (part (b) in Figure \(\PageIndex{4}\)​​​​​​​ ). Because a mixture of acetylene and oxygen burns with a flame that is hot enough (>3000°C) to cut metals such as hardened steel, acetylene is widely used in cutting and welding torches. The names of other alkynes are similar to those of the corresponding alkanes but end in -yne. For example, HC≡CCH3 is propyne, and CH3C≡CCH3 is 2-butyne because the multiple bond begins on the second carbon atom.

    Note the Pattern

    The number of bonds between carbon atoms in a hydrocarbon is indicated in the suffix:

    • alkane: only carbon–carbon single bonds
    • alkene: at least one carbon–carbon double bond
    • alkyne: at least one carbon–carbon triple bond

    Cyclic Hydrocarbons

    In a cyclic hydrocarbon, the ends of a hydrocarbon chain are connected to form a ring of covalently bonded carbon atoms. Cyclic hydrocarbons are named by attaching the prefix cyclo- to the name of the alkane, the alkene, or the alkyne. The simplest cyclic alkanes are cyclopropane (C3H6) a flammable gas that is also a powerful anesthetic, and cyclobutane (C4H8) (part (c) in Figure \(\PageIndex{4}\) ). The most common way to draw the structures of cyclic alkanes is to sketch a polygon with the same number of vertices as there are carbon atoms in the ring; each vertex represents a CH2 unit. The structures of the cycloalkanes that contain three to six carbon atoms are shown schematically in Figure \(\PageIndex{5}\)​​​​​​​ ​​​​​​​.


    Figure \(\PageIndex{5}\)​​​​​​​ The Simple Cycloalkanes



    Aromatic Hydrocarbons

    Alkanes, alkenes, alkynes, and cyclic hydrocarbons are generally called aliphatic hydrocarbons. The name comes from the Greek aleiphar, meaning “oil,” because the first examples were extracted from animal fats. In contrast, the first examples of aromatic hydrocarbons, also called arenes, were obtained by the distillation and degradation of highly scented (thus aromatic) resins from tropical trees.

    The simplest aromatic hydrocarbon is benzene (C6H6), which was first obtained from a coal distillate. The word aromatic now refers to benzene and structurally similar compounds. As shown in part (a) in Figure \(\PageIndex{6}\)​​​​​​​​​​​​​​, it is possible to draw the structure of benzene in two different but equivalent ways, depending on which carbon atoms are connected by double bonds or single bonds. Toluene is similar to benzene, except that one hydrogen atom is replaced by a –CH3 group; it has the formula C7H8 (part (b) in Figure \(\PageIndex{6}\)​​​​​​​​​​​​​​). As you will soon learn, the chemical behavior of aromatic compounds differs from the behavior of aliphatic compounds. Benzene and toluene are found in gasoline, and benzene is the starting material for preparing substances as diverse as aspirin and nylon.


    Figure \(\PageIndex{6}\)​​​​​​​ Two Aromatic Hydrocarbons: (a) Benzene and (b) Toluene



    Figure \(\PageIndex{7}\)​​​​​​​​​​​​​​​​​​​​​ illustrates two of the molecular structures possible for hydrocarbons that have six carbon atoms. As you can see, compounds with the same molecular formula can have very different structures.


    Figure \(\PageIndex{7}\)​​​​​​​​​​​​​​​​​​​​​Two Hydrocarbons with the Molecular Formula C6H12


    Example \(\PageIndex{3}\)

    Write the condensed structural formula for each hydrocarbon.

    1. n-heptane
    2. 2-pentene
    3. 2-butyne
    4. cyclooctene

    Given: name of hydrocarbon

    Asked for: condensed structural formula


    A Use the prefix to determine the number of carbon atoms in the molecule and whether it is cyclic. From the suffix, determine whether multiple bonds are present.

    B Identify the position of any multiple bonds from the number(s) in the name and then write the condensed structural formula.


    1. A The prefix hept- tells us that this hydrocarbon has seven carbon atoms, and n- indicates that the carbon atoms form a straight chain. The suffix -ane tells that it is an alkane, with no carbon–carbon double or triple bonds. B The condensed structural formula is CH3CH2CH2CH2CH2CH2CH3, which can also be written as CH3(CH2)5CH3.
    2. A The prefix pent- tells us that this hydrocarbon has five carbon atoms, and the suffix -ene indicates that it is an alkene, with a carbon–carbon double bond. B The 2- tells us that the double bond begins on the second carbon of the five-carbon atom chain. The condensed structural formula of the compound is therefore CH3CH=CHCH2CH3.


    3. A The prefix but- tells us that the compound has a chain of four carbon atoms, and the suffix -yne indicates that it has a carbon–carbon triple bond. B The 2- tells us that the triple bond begins on the second carbon of the four-carbon atom chain. So the condensed structural formula for the compound is CH3C≡CCH3.


    4. A The prefix cyclo- tells us that this hydrocarbon has a ring structure, and oct- indicates that it contains eight carbon atoms, which we can draw as


      The suffix -ene tells us that the compound contains a carbon–carbon double bond, but where in the ring do we place the double bond? B Because all eight carbon atoms are identical, it doesn’t matter. We can draw the structure of cyclooctene as



    Exercise \(\PageIndex{3}\)

    Write the condensed structural formula for each hydrocarbon.

    1. n-octane
    2. 2-hexene
    3. 1-heptyne
    4. cyclopentane
    1. CH3(CH2)6CH3
    2. CH3CH=CHCH2CH2CH3
    3. HC≡C(CH2)4CH3



    The general name for a group of atoms derived from an alkane is an alkyl group. The name of an alkyl group is derived from the name of the alkane by adding the suffix -yl. Thus the –CH3 fragment is a methyl group, the –CH2CH3 fragment is an ethyl group, and so forth, where the dash represents a single bond to some other atom or group. Similarly, groups of atoms derived from aromatic hydrocarbons are aryl groups, which sometimes have unexpected names. For example, the –C6H5 fragment is derived from benzene, but it is called a phenyl group. In general formulas and structures, alkyl and aryl groups are often abbreviated as R.


    Structures of alkyl and aryl groups. The methyl group is an example of an alkyl group, and the phenyl group is an example of an aryl group.



    Replacing one or more hydrogen atoms of a hydrocarbon with an –OH group gives an alcohol, represented as ROH. The simplest alcohol (CH3OH) is called either methanol (its systematic name) or methyl alcohol (its common name) (see "Different Ways of Representing the Structure of a Molecule"). Methanol is the antifreeze in automobile windshield washer fluids, and it is also used as an efficient fuel for racing cars, most notably in the Indianapolis 500. Ethanol (or ethyl alcohol, CH3CH2OH) is familiar as the alcohol in fermented or distilled beverages, such as beer, wine, and whiskey; it is also used as a gasoline additive (Section 2.6 "Industrially Important Chemicals"). The simplest alcohol derived from an aromatic hydrocarbon is C6H5OH, phenol (shortened from phenyl alcohol), a potent disinfectant used in some sore throat medications and mouthwashes.


    Ethanol, which is easy to obtain from fermentation processes, has successfully been used as an alternative fuel for several decades. Although it is a “green” fuel when derived from plants, it is an imperfect substitute for fossil fuels because it is less efficient than gasoline. Moreover, because ethanol absorbs water from the atmosphere, it can corrode an engine’s seals. Thus other types of processes are being developed that use bacteria to create more complex alcohols, such as octanol, that are more energy efficient and that have a lower tendency to absorb water. As scientists attempt to reduce mankind’s dependence on fossil fuels, the development of these so-called biofuels is a particularly active area of research.


    Covalent inorganic compounds are named by a procedure similar to that used for ionic compounds, using prefixes to indicate the numbers of atoms in the molecular formula. The simplest organic compounds are the hydrocarbons, which contain only carbon and hydrogen. Alkanes contain only carbon–hydrogen and carbon–carbon single bonds, alkenes contain at least one carbon–carbon double bond, and alkynes contain one or more carbon–carbon triple bonds. Hydrocarbons can also be cyclic, with the ends of the chain connected to form a ring. Collectively, alkanes, alkenes, and alkynes are called aliphatic hydrocarbonsAromatic hydrocarbons, or arenes, are another important class of hydrocarbons that contain rings of carbon atoms related to the structure of benzene (C6H6). A derivative of an alkane or an arene from which one hydrogen atom has been removed is called an alkyl group or an aryl group, respectively. Alcohols are another common class of organic compound, which contain an –OH group covalently bonded to either an alkyl group or an aryl group (often abbreviated R).


    • Covalent inorganic compounds are named using a procedure similar to that used for ionic compounds, whereas hydrocarbons use a system based on the number of bonds between carbon atoms.


    1. Benzene (C6H6) is an organic compound, and KCl is an ionic compound. The sum of the masses of the atoms in each empirical formula is approximately the same. How would you expect the two to compare with regard to each of the following? What species are present in benzene vapor?

      1. melting point
      2. type of bonding
      3. rate of evaporation
      4. structure
    2. Can an inorganic compound be classified as a hydrocarbon? Why or why not?

    3. Is the compound NaHCO3 a hydrocarbon? Why or why not?

    4. Name each compound.

      1. NiO
      2. TiO2
      3. N2O
      4. CS2
      5. SO3
      6. NF3
      7. SF6
    5. Name each compound.

      1. HgCl2
      2. IF5
      3. N2O5
      4. Cl2O
      5. HgS
      6. PCl5
    6. For each structural formula, write the condensed formula and the name of the compound.











    7. For each structural formula, write the condensed formula and the name of the compound.









    8. Would you expect PCl3 to be an ionic compound or a covalent compound? Explain your reasoning.

    9. What distinguishes an aromatic hydrocarbon from an aliphatic hydrocarbon?

    10. The following general formulas represent specific classes of hydrocarbons. Refer to Table \(\PageIndex{2}\) and Figure \(\PageIndex{4}\) and identify the classes.

      1. CnH2n + 2
      2. CnH2n
      3. CnH2n − 2
    11. Using R to represent an alkyl or aryl group, show the general structure of an

      1. alcohol.
      2. phenol.



      1. ROH (where R is an alkyl group)
      2. ROH (where R is an aryl group)


    1. Write the formula for each compound.

      1. dinitrogen monoxide
      2. silicon tetrafluoride
      3. boron trichloride
      4. nitrogen trifluoride
      5. phosphorus tribromide
    2. Write the formula for each compound.

      1. dinitrogen trioxide
      2. iodine pentafluoride
      3. boron tribromide
      4. oxygen difluoride
      5. arsenic trichloride
    3. Write the formula for each compound.

      1. thallium(I) selenide
      2. neptunium(IV) oxide
      3. iron(II) sulfide
      4. copper(I) cyanide
      5. nitrogen trichloride
    4. Name each compound.

      1. RuO4
      2. PbO2
      3. MoF6
      4. Hg2(NO3)2·2H2O
      5. WCl4
    5. Name each compound.

      1. NbO2
      2. MoS2
      3. P4S10
      4. Cu2O
      5. ReF5
    6. Draw the structure of each compound.

      1. propyne
      2. ethanol
      3. n-hexane
      4. cyclopropane
      5. benzene
    7. Draw the structure of each compound.

      1. 1-butene
      2. 2-pentyne
      3. cycloheptane
      4. toluene
      5. phenol



      1. N2O
      2. SiF4
      3. BCl3
      4. NF3
      5. PBr3

      1. Tl2Se
      2. NpO2
      3. FeS
      4. CuCN
      5. NCl3

      1. niobium (IV) oxide
      2. molybdenum (IV) sulfide
      3. tetraphosphorus decasulfide
      4. copper(I) oxide
      5. rhenium(V) fluoride











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