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Skeletal formula
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<h2 id="the-skeleton">The skeleton</h2> <h3>Terminology</h3> <p>The skeletal structure of an organic compound is the series of atoms bonded together that form the essential structure of the compound. The skeleton can consist of chains, branches and/or rings of bonded atoms. Skeletal atoms other than carbon or hydrogen are called <a href="/facts/Heteroatom/QzxXyfCT">heteroatoms</a>.<a class="footnote-ref" id="fnref:3" href="#fn:3"><sup>3</sup></a> </p><p>The skeleton has hydrogen and/or various <a href="/facts/Substituent/6y9IE6G0">substituents</a> bonded to its atoms. Hydrogen is the most common non-carbon atom that is bonded to carbon and, for simplicity, is not explicitly drawn. In addition, carbon atoms are not generally labelled as such directly (i.e. with "C"), whereas heteroatoms are always explicitly noted as such ("N" for <a href="/facts/Nitrogen/Nf1QpGDz">nitrogen</a>, "O" for <a href="/facts/Oxygen/acyn6o8r">oxygen</a>, etc.) </p><p>Heteroatoms and other groups of atoms that give rise to relatively high rates of chemical reactivity, or introduce specific and interesting characteristics in the spectra of compounds are called <a href="/facts/Functional_group/GXkSPsjM">functional groups</a>, as they give the molecule a function. Heteroatoms and functional groups are collectively called "substituents", as they are considered to be a substitute for the hydrogen atom that would be present in the parent <a href="/facts/Hydrocarbon/Dcg95Ju5">hydrocarbon</a> of the organic compound. </p> <h3>Basic structure</h3> <p>As in Lewis structures, covalent bonds are indicated by line segments, with a doubled or tripled line segment indicating <a href="/facts/Double_bond/qDemMn0c">double</a> or <a href="/facts/Triple_bond/poDWRayX">triple bonding</a>, respectively. Likewise, skeletal formulae indicate <a href="/facts/Formal_charges/uqHf9WD7">formal charges</a> associated with each atom, with lone pairs usually being optional (see below). In fact, skeletal formulae can be thought of as abbreviated Lewis structures that observe the following simplifications: </p> <ul><li>Carbon atoms are represented by the vertices (intersections or termini) of line segments. For clarity, methyl groups are often explicitly written out as Me or CH3, while (hetero)<a href="/facts/Cumulene/UtxYSvxN">cumulene</a> carbons are frequently represented by a heavy <a href="/facts/Interpunct/FqdEx1gT">center dot</a>.</li> <li>Hydrogen atoms attached to carbon are implied. An unlabeled vertex is understood to represent a carbon attached to the number of hydrogens required to satisfy the <a href="/facts/Octet_rule/X9jxSsos">octet rule</a>, while a vertex labeled with a formal charge and/or nonbonding electron(s) is understood to have the number of hydrogen atoms required to give the carbon atom these indicated properties. Optionally, acetylenic and formyl hydrogens can be shown explicitly for the sake of clarity.</li> <li>Hydrogen atoms attached to a heteroatom are shown explicitly. The heteroatom and hydrogen atoms attached thereto are usually shown as a single group (e.g., OH, NH2) without explicitly showing the hydrogen–heteroatom bond. Heteroatoms with simple alkyl or aryl substituents, like methoxy (OMe) or dimethylamino (NMe2), are sometimes shown in the same way, by analogy.</li> <li>Lone pairs on <a href="/facts/Carbene/3WxNSStY">carbene</a> carbons must be indicated explicitly while lone pairs in other cases are optional and are shown only for emphasis. In contrast, formal charges and unpaired electrons on main-group elements are always explicitly shown.</li></ul> <p>In the standard depiction of a molecule, the <a href="/facts/Canonical_form_(chemistry)/5tymwoIP">canonical form</a> (resonance structure) with the greatest contribution is drawn. However, the skeletal formula is understood to represent the "real molecule" – that is, the weighted average of all contributing canonical forms. Thus, in cases where two or more canonical forms contribute with equal weight (e.g., in benzene, or a carboxylate anion) and one of the canonical forms is selected arbitrarily, the skeletal formula is understood to depict the true structure, containing equivalent bonds of fractional order, even though the delocalized bonds are depicted as nonequivalent single and double bonds. </p> <h3>Contemporary graphical conventions</h3> <p>Since skeletal structures were introduced in the latter half of the 19th century, their appearance has undergone considerable evolution. The graphical conventions in use today date to the 1980s. Thanks to the adoption of the <a href="/facts/ChemDraw/kUTTTf9J">ChemDraw</a> software package as a <i>de facto</i> industry standard (by <a href="/facts/American_Chemical_Society/Alf3uhaF">American Chemical Society</a>, <a href="/facts/Royal_Society_of_Chemistry/1fg4xnqR">Royal Society of Chemistry</a>, and <a href="/facts/Gesellschaft_Deutscher_Chemiker/Jn2DuBo6">Gesellschaft Deutscher Chemiker</a> publications, for instance), these conventions have been nearly universal in the chemical literature since the late 1990s. A few minor conventional variations, especially with respect to the use of stereobonds, continue to exist as a result of differing US, UK and European practice, or as a matter of personal preference.<a class="footnote-ref" id="fnref:4" href="#fn:4"><sup>4</sup></a> As another minor variation between authors, formal charges can be shown with the plus or minus sign in a circle (⊕, ⊖) or without the circle. The set of conventions that are followed by most authors is given below, along with illustrative examples. </p> <ol><li>Bonds between sp2 or sp3 hybridized carbon or heteroatoms are conventionally represented using 120° angles whenever possible, with the longest chain of atoms following a zigzag pattern unless interrupted by a <i>cis</i> double bond. Unless all four substituents are explicit, this is true even when stereochemistry is being depicted using wedged or dashed bonds (<i>see below</i>).<a class="footnote-ref" id="fnref:5" href="#fn:5"><sup>5</sup></a> </li><li>If all four substituents to a tetrahedral carbon are explicitly shown, bonds to the two in-plane substituents still meet at 120°; the other two substituents, however, are usually shown with wedged and dashed bonds (to depict stereochemistry) and subtend a smaller angle of 60–90°. </li><li>The linear geometry at sp hybridized atoms is normally depicted by line segments meeting at 180°. Where this involves two double bonds meeting (an <a href="/facts/Allene/54hMEu5N">allene</a> or <a href="/facts/Cumulene/UtxYSvxN">cumulene</a>), the bonds are separated by a dot. </li><li>Carbo- and heterocycles (3- to 8-membered) are generally represented as regular polygons; larger ring sizes tend to be represented by concave polygons.<a class="footnote-ref" id="fnref:6" href="#fn:6"><sup>6</sup></a> </li><li>Atoms in a group are ordered so that the bond emanates from the atom that is directly attached to the skeleton. For example, the <a href="/facts/Nitro_group/pem2BhMY">nitro group</a> NO2 is denoted —NO2 or O2N—, depending on the placement of the bond. In contrast, the isomeric <a href="/facts/Nitrite/qkz2XScK">nitrite group</a> is denoted —ONO or ONO—.<a class="footnote-ref" id="fnref:7" href="#fn:7"><sup>7</sup></a> </li></ol> <h2 id="implicit-carbon-and-hydrogen-atoms">Implicit carbon and hydrogen atoms</h2> <p>For example, the skeletal formula of <a href="/facts/Hexane/JxPecNPt">hexane</a> (top) is shown below. The carbon atom labeled C1 appears to have only one bond, so there must also be three hydrogens bonded to it, in order to make its total number of bonds four. The carbon atom labelled C3 has two bonds to other carbons and is therefore bonded to two hydrogen atoms as well. A <a href="/facts/Lewis_structure/PTgB3gtW">Lewis structure</a> (middle) and <a href="/facts/Ball-and-stick_model/0FQhyys8">ball-and-stick model</a> (bottom) of the actual molecular structure of hexane, as determined by <a href="/facts/X-ray_crystallography/WtI0F5DN">X-ray crystallography</a>, are shown for comparison. </p> <p>It does not matter which end of the chain one starts numbering from, as long as consistency is maintained when drawing diagrams. The condensed formula or the IUPAC name will confirm the orientation. Some molecules will become familiar regardless of the orientation. </p> <h2 id="explicit-heteroatoms-and-hydrogen-atoms">Explicit heteroatoms and hydrogen atoms</h2> <p>All atoms that are not carbon or hydrogen are signified by their <a href="/facts/Chemical_symbol/2Fe1VAL0">chemical symbol</a>, for instance Cl for <a href="/facts/Chlorine/y27UwYBM">chlorine</a>, O for <a href="/facts/Oxygen/acyn6o8r">oxygen</a>, Na for <a href="/facts/Sodium/eYuSPu2V">sodium</a>, and so forth. In the context of organic chemistry, these atoms are commonly known as heteroatoms (the <a href="/facts/Prefix/C4Lw8npg">prefix</a> <i>hetero-</i> comes from Greek <i>ἕτερος</i> héteros, meaning "other"). </p><p>Any hydrogen atoms bonded to heteroatoms <i>are</i> drawn explicitly. In <a href="/facts/Ethanol/3lCLfBSP">ethanol</a>, C2H5OH, for instance, the hydrogen atom bonded to oxygen is denoted by the symbol H, whereas the hydrogen atoms which are bonded to carbon atoms are not shown directly. </p><p>Lines representing heteroatom-hydrogen bonds are usually omitted for clarity and compactness, so a functional group like the <a href="/facts/Hydroxyl/1Hs2QAEv">hydroxyl</a> group is most often written −OH instead of −O−H. These bonds are sometimes drawn out in full in order to accentuate their presence when they participate in <a href="/facts/Reaction_mechanism/9lanyVuy">reaction mechanisms</a>. </p><p>Shown below for comparison are a skeletal formula (top), its <a href="/facts/Lewis_structure/PTgB3gtW">Lewis structure</a> (middle) and its ball-and-stick model (bottom) of the actual <a href="/facts/Molecular_geometry/7USG5zDn">3D structure</a> of the ethanol molecule in the gas phase, as determined by <a href="/facts/Rotational_spectroscopy/QakXReKL">microwave spectroscopy</a>. </p> <h2 id="pseudoelement-symbols">Pseudoelement symbols</h2> <p>There are also symbols that appear to be <a href="/facts/Chemical_symbol/2Fe1VAL0">chemical element symbols</a>, but represent certain very common substituents or indicate an unspecified member of a group of elements. These are called pseudoelement symbols or organic elements and are treated like univalent "elements" in skeletal formulae.<a class="footnote-ref" id="fnref:8" href="#fn:8"><sup>8</sup></a> A list of common pseudoelement symbols: </p> <h3>General symbols</h3> <ul><li>X for any (<a href="/facts/Pseudohalogen/9DMN43ya">pseudo</a>)<a href="/facts/Halogen/YeFgWHeA">halogen</a> atom (in the related <a href="/facts/Covalent_bond_classification_method/tb2L7ECf">MLXZ notation</a>, X represents a one-electron donor ligand)</li> <li>L <i>or</i> L<i>n</i> for a <a href="/facts/Ligand/6etB3qeW">ligand</a> or ligands (in the related MLXZ notation, L represents a two-electron donor ligand)</li> <li>M <i>or</i> Met for any <a href="/facts/Metal/PT8hNX6R">metal</a> atom ([M] is used to indicate a ligated metal, ML<i>n</i>, when the identities of the ligands are unknown or irrelevant)</li> <li>E <i>or</i> El for any <a href="/facts/Electrophile/1AHFg1zm">electrophile</a> (in some contexts, E is also used to indicate any <a href="/facts/P-block/BbzD5jUU">p-block</a> element)</li> <li>Nu for any <a href="/facts/Nucleophile/xYccoaJQ">nucleophile</a></li> <li>Z for conjugating electron-withdrawing groups (in the related MLXZ notation, Z represents a zero-electron donor ligand; <i>in unrelated usage, Z is also an abbreviation for the carboxybenzyl group</i>.)</li> <li>D for <a href="/facts/Deuterium/Bv4wfCkw">deuterium</a> (2H)</li> <li>T for <a href="/facts/Tritium/HWSa6EHy">tritium</a> (3H)</li></ul> <h3>Alkyl groups</h3> <ul><li>R for any <a href="/facts/Alkyl/vmEk8X4v">alkyl</a> group or even any <a href="/facts/Organyl/gqCNaN45">organyl</a> group (Alk can be used to unambiguously indicate an alkyl group)</li> <li>Me for the <a href="/facts/Methyl_group/fkM97EMD">methyl group</a></li> <li>Et for the <a href="/facts/Ethyl_group/ydVhnBwD">ethyl group</a></li> <li>Pr, <i>n</i>-Pr, <i>or</i> <i>n</i>Pr for the <a href="/facts/Propyl/fl8SMScE">(<i>normal</i>) propyl</a> group (<i>Pr is also the symbol for the element <a href="/facts/Praseodymium/2lnRJ9dH">praseodymium</a>. However, since the propyl group is monovalent, while praseodymium is nearly always trivalent, ambiguity rarely, if ever, arises in practice.</i>)</li> <li><i>i</i>-Pr <i>or</i> <i>i</i>Pr for the <a href="/facts/Isopropyl/fl8SMScE">isopropyl</a> group</li> <li>All for the <a href="/facts/Allyl_group/CDxPwyvF">allyl group</a> (uncommon)</li> <li>Bu, <i>n</i>-Bu <i>or</i> <i>n</i>Bu for the <a href="/facts/N-butyl/fbTF0UkI">(<i>normal</i>) butyl</a> group</li> <li><i>i</i>-Bu <i>or</i> <i>i</i>Bu (<i>i</i> often italicized) for the <a href="/facts/Isobutyl/fbTF0UkI">isobutyl</a> group</li> <li><i>s</i>-Bu <i>or</i> <i>s</i>Bu for the <a href="/facts/Secondary_butyl/fbTF0UkI"><i>secondary</i> butyl</a> group</li> <li><i>t</i>-Bu <i>or</i> <i>t</i>Bu for the <a href="/facts/Tertiary_butyl/fbTF0UkI"><i>tertiary</i> butyl</a> group</li> <li>Pn for the <a href="/facts/Pentyl/dpbJQMdd">pentyl</a> group (<i>or</i> Am for the synonymous <a href="/facts/Pentyl/dpbJQMdd">amyl</a> group, <i>although Am is also the symbol for <a href="/facts/Americium/rxL9Yc64">americium</a>.</i>)</li> <li>Np <i>or</i> Neo for the <a href="/facts/Neopentyl/8KHow6mz">neopentyl</a> group (<i>Warning: Organometallic chemists often use Np for the related <a href="/facts/Neophyl_chloride/Leesg0qU">neophyl</a> group, PhMe2C–. Np is also the symbol for the element <a href="/facts/Neptunium/pwp7Yvds">neptunium</a>.</i>)</li> <li>Cy <i>or</i> Chx for the <a href="/facts/Cyclohexane/FDAW5j8v">cyclohexyl</a> group</li> <li>Ad for the 1-<a href="/facts/Adamantane/tlvgCxYf">adamantyl</a> group</li> <li>Tr <i>or</i> Trt for the <a href="/facts/Trityl/35o8VWeP">trityl</a> group</li></ul> <h3>Aromatic and unsaturated substituents</h3> <ul><li>Ar for any <a href="/facts/Aromaticity/wK0DzRY6">aromatic</a> substituent <i>(Ar is also the symbol for the element <a href="/facts/Argon/QX6NRH6d">argon</a>. However, argon is inert under all usual conditions encountered in organic chemistry, so the use of Ar to represent an aryl substituent never causes confusion.)</i></li> <li>Het for any <a href="/facts/Heterocyclic_compound/8oYSjJxY">heteroaromatic</a> substituent</li> <li>Bn <i>or</i> Bzl for the <a href="/facts/Benzyl/kHmqYwqH">benzyl</a> group (<i>not to be confused with Bz for <a href="/facts/Benzoyl/VNyxpSK0">benzoyl</a> group; However, old literature may use Bz for benzyl group.</i>)</li> <li>Dipp for the 2,6-diisopropylphenyl group</li> <li>Mes for the <a href="/facts/Mesityl/4JCRbj1Y">mesityl</a> group</li> <li>Ph, Φ, <i>or</i> φ for the <a href="/facts/Phenyl_group/Ql9Yx5uu">phenyl group</a> (<i>the use of <a href="/facts/Phi/pUzerkKk">phi</a> for phenyl has been in decline</i>)</li> <li>Tol for the <a href="/facts/Toluene/Pzdt8dwD">tolyl</a> group, usually the <i>para</i> isomer</li> <li>Is <i>or</i> Tipp for the 2,4,6-triisopropylphenyl group (<i>the former symbol is derived from the synonym</i> <i>isityl</i>)</li> <li>An for the <a href="/facts/Anisole/ezvjrK1s">anisyl</a> group, usually the <i>para</i> isomer (<i>An is also the symbol for a generic <a href="/facts/Actinide/kHC4lxJV">actinoid element</a>. However, since the anisyl group is monovalent, while the actinides are usually divalent, trivalent, or even higher valency, ambiguity rarely, if ever, arises in practice.</i>)</li> <li>Cp for the <a href="/facts/Cyclopentadienyl_complex/rezSmzLI">cyclopentadienyl</a> group (<i>Cp was the symbol for cassiopeium, a former name for <a href="/facts/Lutetium/URlmnYG8">lutetium</a></i>)</li> <li>Cp* for the <a href="/facts/Cyclopentadienyl_complex/rezSmzLI">pentamethylcyclopentadienyl</a> group</li> <li>Vi for the <a href="/facts/Vinyl_group/SyXSgVnw">vinyl group</a> (uncommon)</li></ul> <h3>Functional groups</h3> <ul><li>Ac for the <a href="/facts/Acetyl/rRmtXdn3">acetyl</a> group <i>(Ac is also the symbol for the element <a href="/facts/Actinium/GMQtJ4Gm">actinium</a>. However, actinium is almost never encountered in organic chemistry, so the use of Ac to represent the acetyl group never causes confusion)</i>;</li> <li>Bz for the <a href="/facts/Benzoyl/VNyxpSK0">benzoyl</a> group; OBz is the <a href="/facts/Benzoate/7HrmrBYS">benzoate</a> group</li> <li>Piv for the <a href="/facts/Pivaloyl/dDnDBbo0">pivalyl</a> (<i>t</i>-butylcarbonyl) group; OPiv is the pivalate group</li> <li>Bt for the 1-benzotriazolyl group</li> <li>Im for the 1-imidazolyl group</li> <li>NPhth for the phthalimide-1-yl group</li></ul> <h3>Sulfonyl/sulfonate groups</h3> <p>Sulfonate esters are often <a href="/facts/Leaving_group/uowVfqwh">leaving groups</a> in nucleophilic substitution reactions. <i>See the articles on <a href="/facts/Sulfonyl_group/UbpYXVvN">sulfonyl</a> and <a href="/facts/Sulfonate/ApbgQMXB">sulfonate</a> groups for further information.</i> </p> <ul><li>Bs for the <a href="/facts/Brosyl_group/8EkwMKpY">brosyl</a> (<i>p</i>-bromobenzenesulfonyl) group; OBs is the brosylate group</li> <li>Ms for the <a href="/facts/Sulfonyl/UbpYXVvN">mesyl</a> (methanesulfonyl) group; OMs is the <a href="/facts/Mesylate/h0GRcGo6">mesylate</a> group</li> <li>Ns for the <a href="/facts/Sulfonyl/UbpYXVvN">nosyl</a> (<i>p</i>-nitrobenzenesulfonyl) group <i>(Ns was the chemical symbol for nielsbohrium, but that was renamed <a href="/facts/Bohrium/epvp3GWM">bohrium</a>, Bh)</i>; ONs is the nosylate group</li> <li>Tf for the <a href="/facts/Triflate/6sbvDSyt">triflyl</a> (trifluoromethanesulfonyl) group; OTf is the <a href="/facts/Triflate/6sbvDSyt">triflate</a> group</li> <li>Nf for the <a href="/facts/Nonaflate/b3YcHrKc">nonaflyl</a> (nonafluorobutanesulfonyl) group, CF3(CF2)3SO2; ONf is the <a href="/facts/Nonaflate/b3YcHrKc">nonaflate</a> group</li> <li>Ts for <a href="/facts/Tosyl/Q4qU62D1">tosyl</a> (<i>p-</i>toluenesulfonyl) group <i>(Ts is also the symbol for the element <a href="/facts/Tennessine/eGCBDvEr">tennessine</a>. However, tennessine is too unstable to ever be encountered in organic chemistry, so the use of Ts to represent tosyl never causes confusion)</i>; OTs is the <a href="/facts/Tosylate/Q4qU62D1">tosylate</a> group</li></ul> <h3>Protecting groups</h3> <p>A <a href="/facts/Protecting_group/f92hVwHl">protecting group</a> or protective group is introduced into a molecule by chemical modification of a functional group to obtain chemoselectivity in a subsequent chemical reaction, facilitating multistep organic synthesis. </p> <ul><li>Boc for the <a href="/facts/T-butoxycarbonyl/6JhCTnpt"><i>t-</i>butoxycarbonyl</a> group</li> <li>Cbz <i>or</i> Z for the <a href="/facts/Carboxybenzyl/pAduphpY">carboxybenzyl</a> group</li> <li>Fmoc for the <a href="/facts/Fluorenylmethyloxycarbonyl_protecting_group/d2Sv8MYc">fluorenylmethoxycarbonyl</a> group</li> <li>Alloc for the allyloxycarbonyl group</li> <li>Troc for the trichloroethoxycarbonyl group</li> <li>TMS, TBDMS, TES, TBDPS, TIPS, ... for various <a href="/facts/Silyl_ether/k6y8Th9E">silyl ether</a> groups</li> <li>PMB for the 4-methoxybenzyl group</li> <li>MOM for the methoxymethyl group</li> <li>THP for the 2-tetrahydropyranyl group</li></ul> <h2 id="multiple-bonds">Multiple bonds</h2> <p>Two atoms can be bonded by sharing more than one pair of electrons. The common bonds to carbon are single, double and triple bonds. Single bonds are most common and are represented by a single, solid line between two atoms in a skeletal formula. Double bonds are denoted by two parallel lines, and triple bonds are shown by three parallel lines. </p><p>In more advanced theories of bonding, non-<a href="/facts/Integer/PUwwrawx">integer</a> values of <a href="/facts/Bond_order/Tdb1zgTc">bond order</a> exist. In these cases, a combination of solid and dashed lines indicate the integer and non-integer parts of the bond order, respectively. </p> Examples of multiple bonds in skeletal formulae<a class="footnote-ref" id="fnref:9" href="#fn:9"><sup>9</sup></a> <h2 id="benzene-rings">Benzene rings</h2> <p>In recent years, <a href="/facts/Benzene/Fguue7nr">benzene</a> is generally depicted as a hexagon with alternating single and double bonds, much like the structure <a href="/facts/August_Kekul%25C3%25A9/w1lFwWY9">Kekulé</a> originally proposed in 1872. As mentioned above, the alternating single and double bonds of "1,3,5-cyclohexatriene" are understood to be a drawing of one of the two equivalent canonical forms of benzene (the one explicitly shown and the one with the opposite pattern of formal single and double bonds), in which all carbon–carbon bonds are of equivalent length and have a bond order of exactly 1.5. For aryl rings in general, the two analogous canonical forms are almost always the primary contributors to the structure, but they are nonequivalent, so one structure may make a slightly greater contribution than the other, and bond orders may differ somewhat from 1.5. </p><p>An alternate representation that emphasizes this delocalization uses a circle, drawn inside the hexagon of single bonds, to represent the delocalized <a href="/facts/Pi_orbital/3Q6LAGYK">pi orbital</a>. This style, based on one proposed by <a href="/facts/Johannes_Thiele_(chemist)/5upR3Kvg">Johannes Thiele</a>, used to be very common in introductory organic chemistry textbooks and is still frequently used in informal settings. However, because this depiction does not keep track of electron pairs and is unable to show the precise movement of electrons, it has largely been superseded by the Kekuléan depiction in pedagogical and formal academic contexts.<a class="footnote-ref" id="fnref:10" href="#fn:10"><sup>10</sup></a> </p> <h2 id="stereochemistry">Stereochemistry</h2> <p><a href="/facts/Stereochemistry/XkcRVNwd">Stereochemistry</a> is conveniently denoted in skeletal formulae:<a class="footnote-ref" id="fnref:11" href="#fn:11"><sup>11</sup></a> </p> <p>The relevant chemical bonds can be depicted in several ways: </p> <ul><li>Solid lines represent <a href="/facts/Covalent_bond/EzMLf3Pz">bonds</a> in the plane of the paper or screen.</li> <li>Solid wedges represent bonds that point out of the plane of the paper or screen, towards the observer.</li> <li>Hashed wedges or dashed lines (thick or thin) represent bonds that point into the plane of the paper or screen, away from the observer.<a class="footnote-ref" id="fnref:12" href="#fn:12"><sup>12</sup></a></li> <li>Wavy lines represent either unknown stereochemistry or a mixture of the two possible stereoisomers at that point.</li> <li>An obsolescent<a class="footnote-ref" id="fnref:13" href="#fn:13"><sup>13</sup></a> depiction of hydrogen stereochemistry that used to be common in <a href="/facts/Steroid/4AhMbgXt">steroid</a> chemistry is the use of a filled circle centered on a vertex (sometimes called H-dot/H-dash/H-circle, respectively) for an upward pointing hydrogen atom and two hash marks next to vertex or a hollow circle for a downward pointing hydrogen atom. </li></ul> <p>An early use of this notation can be traced back to <a href="/facts/Richard_Kuhn/vxBBKvr7">Richard Kuhn</a> who in 1932 used solid thick lines and dotted lines in a publication. The modern <a href="/facts/Natta_projection/M2J6dMXp">solid and hashed wedges</a> were introduced in the 1940s by <a href="/facts/Giulio_Natta/6FDwycRB">Giulio Natta</a> to represent the structure of high <a href="/facts/Polymer/eF32E50K">polymers</a>, and extensively popularised in the 1959 textbook <i>Organic Chemistry</i> by <a href="/facts/Donald_J._Cram/R2aB0NYA">Donald J. Cram</a> and <a href="/facts/George_S._Hammond/7zL93G0r">George S. Hammond</a>.<a class="footnote-ref" id="fnref:14" href="#fn:14"><sup>14</sup></a> </p><p>Skeletal formulae can depict <a href="/facts/Cis-trans_isomerism/vqlchJly"><i>cis</i> and <i>trans</i> isomers</a> of alkenes. Wavy single bonds are the standard way to represent unknown or unspecified stereochemistry or a mixture of isomers (as with tetrahedral stereocenters). A crossed double-bond has been used sometimes; it is no longer considered an acceptable style for general use but may still be required by computer software.<a class="footnote-ref" id="fnref:15" href="#fn:15"><sup>15</sup></a> </p> <h2 id="hydrogen-bonds">Hydrogen bonds</h2> <p><a href="/facts/Hydrogen_bond/85V86IIg">Hydrogen bonds</a> are generally denoted by dotted or dashed lines. In other contexts, dashed lines may also represent partially formed or broken bonds in a <a href="/facts/Transition_state/34PsdqRd">transition state</a>. </p> <h2 id="notes">Notes</h2> <h2 id="external-links">External links</h2> <ul><li><a href="http://www.chemguide.co.uk/basicorg/conventions/draw.html">Drawing organic molecules</a> from <i>chemguide.co.uk</i></li></ul> <h2 id="references">References</h2> <ol> <li id="fn:1"><p>IUPAC Compendium of Chemical Terminology (5 ed.). Research Triangle Park, NC: International Union of Pure and Applied Chemistry. 2025. doi:10.1351/goldbook.08208. <a href="https://goldbook.iupac.org/terms/view/08208" target="_blank">https://goldbook.iupac.org/terms/view/08208</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li> <li id="fn:2"><p>This term is ambiguous, because "Kekulé structure" also refers to Kekulé's famous proposal of a hexagon of alternating single and double bonds for the structure of benzene. <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li> <li id="fn:3"><p>IUPAC Recommendations 1999, Revised Section F: Replacement of Skeletal Atoms <a href="http://www.chem.qmul.ac.uk/iupac/sectionF/RF5.html" target="_blank">http://www.chem.qmul.ac.uk/iupac/sectionF/RF5.html</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li> <li id="fn:4"><p>Brecher, Jonathan (2008). "Graphical representation standards for chemical structure diagrams (IUPAC Recommendations 2008)". Pure and Applied Chemistry. 80 (2): 277–410. doi:10.1351/pac200880020277. hdl:10092/2052. ISSN 1365-3075. <a href="https://doi.org/10.1351%2Fpac200880020277" target="_blank">https://doi.org/10.1351%2Fpac200880020277</a> <a href="#fnref:4" class="footnote-back-ref">↩</a></p></li> <li id="fn:5"><p>To prevent a 'kink' from emerging and causing a structure to take up too much vertical space on a page, the IUPAC (Brecher, 2008, p. 352) makes an exception for long chain cis-olefins (such as oleic acid), allowing the cis double bond within them to be depicted with 150° angles, so that the zigzags on either side of the double bond can propagate horizontally. <a href="/wiki/Oleic_acid" target="_blank">/wiki/Oleic_acid</a> <a href="#fnref:5" class="footnote-back-ref">↩</a></p></li> <li id="fn:6"><p>Smaller rings may also be drawn as concave to show stereochemistry (such as the conformations of cyclohexane) or polycyclic molecules that cannot be drawn 'flat' without significant distortion (such as tropane and adamantane). <a href="/wiki/Cyclohexane_conformation" target="_blank">/wiki/Cyclohexane_conformation</a> <a href="#fnref:6" class="footnote-back-ref">↩</a></p></li> <li id="fn:7"><p>In cases where the atom has bonds coming from both the left and right (such as a secondary amine NH in the middle of a chain), some authors allow the group's formula to be stacked vertically whereas others draw an explicit vertical bond within the group. <a href="/wiki/Amine" target="_blank">/wiki/Amine</a> <a href="#fnref:7" class="footnote-back-ref">↩</a></p></li> <li id="fn:8"><p>Clayden, Jonathan; Greeves, Nick; Warren, Stuart; Wothers, Peter (2001). Organic Chemistry (1st ed.). Oxford University Press. p. 27. ISBN 978-0-19-850346-0. <a href="978-0-19-850346-0" target="_blank">978-0-19-850346-0</a> <a href="#fnref:8" class="footnote-back-ref">↩</a></p></li> <li id="fn:9"><p>In this gallery, double bonds have been shown in red and triple bonds in blue. This was added for clarity – multiple bonds are not normally coloured in skeletal formulae. <a href="#fnref:9" class="footnote-back-ref">↩</a></p></li> <li id="fn:10"><p>For instance, the acclaimed 1959 textbook by Morrison and Boyd (6th edition, 1992) uses the Thiele notation as its standard depiction of the aryl ring, while the 2001 textbook by Clayden, Greeves, Warren, and Wothers (2nd edition, 2012) uses the Kekulé notation throughout and warns students to avoid using the Thiele notation when writing mechanisms (p. 144, 2nd ed.). <a href="#fnref:10" class="footnote-back-ref">↩</a></p></li> <li id="fn:11"><p>Brecher, Jonathan (2006). "Graphical representation of stereochemical configuration (IUPAC Recommendations 2006)" (PDF). Pure and Applied Chemistry. 78 (10): 1897–1970. doi:10.1351/pac200678101897. S2CID 97528124. <a href="http://www.iupac.org/publications/pac/pdf/2006/pdf/7810x1897.pdf" target="_blank">http://www.iupac.org/publications/pac/pdf/2006/pdf/7810x1897.pdf</a> <a href="#fnref:11" class="footnote-back-ref">↩</a></p></li> <li id="fn:12"><p>American and European chemists use slightly different conventions for a hashed bond. Whereas most American chemists draw hashed bonds with short hash marks close to the stereocenter and long hash marks further away (in analogy to wedged bonds), most European chemists start with long hash marks close to the stereocenter that gradually become shorter moving away (in analogy to perspective drawing). In the past, the IUPAC has suggested the use of a hashed bond with hash marks of equal length throughout as a compromise but now prefers the American-style hashed bonds (Brecher, 2006, p. 1905). Some chemists use a thick bond and dotted bond (or hashed bond with equal length hashes) to depict relative stereochemistry and a wedged bond and hashed bond with unequal hashes to depict absolute stereochemistry; most others do not make this distinction. <a href="/wiki/International_Union_of_Pure_and_Applied_Chemistry" target="_blank">/wiki/International_Union_of_Pure_and_Applied_Chemistry</a> <a href="#fnref:12" class="footnote-back-ref">↩</a></p></li> <li id="fn:13"><p>The IUPAC now strongly deprecates this notation. <a href="#fnref:13" class="footnote-back-ref">↩</a></p></li> <li id="fn:14"><p>Jensen, William B. (2013). "The Historical Origins of Stereochemical Line and Wedge Symbolism". Journal of Chemical Education. 90 (5): 676–677. Bibcode:2013JChEd..90..676J. doi:10.1021/ed200177u. <a href="/wiki/William_B._Jensen" target="_blank">/wiki/William_B._Jensen</a> <a href="#fnref:14" class="footnote-back-ref">↩</a></p></li> <li id="fn:15"><p>Brecher, Jonathan (2006). "Graphical representation of stereochemical configuration (IUPAC Recommendations 2006)" (PDF). Pure and Applied Chemistry. 78 (10): 1897–1970. doi:10.1351/pac200678101897. S2CID 97528124. <a href="http://www.iupac.org/publications/pac/pdf/2006/pdf/7810x1897.pdf" target="_blank">http://www.iupac.org/publications/pac/pdf/2006/pdf/7810x1897.pdf</a> <a href="#fnref:15" class="footnote-back-ref">↩</a></p></li> </ol>