Please ,for the last example on using butane 
It was said that they're not isomers because they are still of the same shape but I am a bit confused with the last structure

<h2>Alkanes</h2>
<p><strong>Alkanes</strong>, or <strong>saturated hydrocarbons</strong>, contain only single covalent bonds between carbon atoms. Each of the carbon atoms in an alkane has <em>sp</em><sup>3</sup> <a data-lesson="hybrid-atomic-orbitals" data-subject="chemistry" data-tutorial="covalent-bonding-continued" href="https://app.ulearngo.com/chemistry/covalent-bonding-continued/hybrid-atomic-orbitals">hybrid orbitals</a> and is bonded to four other atoms, each of which is either carbon or hydrogen. The Lewis structures and models of methane, ethane, and pentane are illustrated in the figure below.</p>
<p>Carbon chains are usually drawn as straight lines in Lewis structures, but one has to remember that Lewis structures are not intended to indicate the geometry of molecules. Notice that the carbon atoms in the structural models (the ball-and-stick and space-filling models) of the pentane molecule do not lie in a straight line. Because of the <em>sp</em><sup>3</sup> hybridization, the bond angles in carbon chains are close to 109.5°, giving such chains in an alkane a zigzag shape.</p>
<p>The structures of alkanes and other <a data-lesson="what-are-organic-molecules" data-subject="chemistry" data-tutorial="organic-molecules" href="https://app.ulearngo.com/chemistry/organic-molecules/what-are-organic-molecules">organic molecules</a> may also be represented in a less detailed manner by condensed structural formulas (or simply, <em>condensed formulas</em>). Instead of the usual format for <a data-lesson="chemical-formulas" data-subject="chemistry" data-tutorial="atoms-molecules-ions" href="https://app.ulearngo.com/chemistry/atoms-molecules-ions/chemical-formulas">chemical formulas</a> in which each element symbol appears just once, a condensed formula is written to suggest the <a data-lesson="electronegativity-and-bonding" data-subject="chemistry" data-tutorial="bonding-atomic-combinations" href="https://app.ulearngo.com/chemistry/bonding-atomic-combinations/electronegativity-and-bonding">bonding</a> in the molecule. These formulas have the appearance of a Lewis structure from which most or all of the bond symbols have been removed. Condensed structural formulas for ethane and pentane are shown at the bottom of the figure below, and several additional examples are provided in the exercises at the end of this tutorial.</p>
<div class="wp-caption alignnone" style="width: 800px"><img alt="The figure illustrates four ways to represent molecules for molecules of methane, ethane, and pentane. In the first row of the figure, Lewis structural formulas show element symbols and bonds between atoms. Methane has a central C atom with four H atoms bonded to it. Ethane has a C atom with three H atoms bonded to it. The C atom is also bonded to another C atom with three H atoms bonded to it. Pentane has a C atom with three H atoms bonded to it. The C atom is bonded to another C atom with two H atoms bonded to it. The C atom is bonded to another C atom with two H atoms bonded to it. The C atom is bonded to another C atom with two H atoms bonded to it. The C atom is bonded to another C atom with three H atoms bonded to it. In the second row, ball-and-stick models are shown. In these representations, bonds are represented with sticks, and elements are represented with balls. Carbon atoms are black and hydrogen atoms are white in this image. In the third row, space-filling models are shown. In these models, atoms are enlarged and pushed together, without sticks to represent bonds. The molecule names and structural formulas are provided in the fourth row. Methane is named and represented with a condensed structural formula as C H subscript 4. Ethane is named and represented with two structural formulas C H subscript 3 C H subscript 3 and C subscript 2 H subscript 6. Pentane is named and represented as both C H subscript 3 C H subscript 2 C H subscript 2 C H subscript 2 C H subscript 3 and C subscript 5 H subscript 12." height="372" src="https://data.ulearngo.com/assets/59c8f65a-28e6-48ce-99ba-23bae2e85431" width="800"/><p class="wp-caption-text">Pictured are the Lewis structures, ball-and-stick models, and space-filling models for molecules of methane, ethane, and pentane.</p></div>
<p>A common method used by organic chemists to simplify the drawings of larger molecules is to use a <strong>skeletal structure</strong> (also called a line-angle structure). In this type of structure, carbon atoms are not symbolized with a C, but represented by each end of a line or bend in a line. Hydrogen atoms are not drawn if they are attached to a carbon. Other atoms besides carbon and hydrogen are represented by their elemental symbols. The figure below shows three different ways to draw the same structure.</p>
<div class="wp-caption alignnone" style="width: 800px"><img alt="In this figure, a hydrocarbon molecule is shown in three ways. First, an expanded formula shows all individual carbon atoms, hydrogen atoms, and bonds in a branched hydrocarbon molecule. An initial C atom is bonded to three H atoms. The C atom is bonded to another C atom in the chain. This second C atom is bonded to one H atom and another C atom above the chain. The C atom bonded above the second C atom in the chain is bonded to three H atoms. The second C atom in the chain is bonded to a third C atom in the chain. This third C atom is bonded to on H atom and another C atom below the chain. This C atom is bonded to two H atoms and another C atom below the chain. This second C atom below the chain is bonded to three H atoms. The third C atom in the chain is bonded to a fourth C atom in the chain. The fourth C atom is bonded to two H atoms and a fifth C atom. The fifth C atom is bonded to two H atoms and a sixth C atom. The sixth C atom is bonded to three H atoms. Second, a condensed formula shows each carbon atom of the molecule in clusters with the hydrogen atoms bonded to it, leaving C H, C H subscript 2, and C H subscript 3 groups with bonds between them. The structure shows a C H subscript 3 group bonded to a C H group. The C H group is bonded above to a C H subscript 3 group. The C H group is also bonded to another C H group. This C H group is bonded to a C H subscript 2 group below and a C H subscript 3 group below that. This C H group is also bonded to a C H subscript 2 group which is bonded to another C H subscript 2 group. This C H subscript 2 group is bonded to a final C H subscript 2 group. The final structure in the figure is a skeletal structure which includes only line segments arranged to indicate the structure of the molecule." height="308" src="https://data.ulearngo.com/assets/a153152e-0c04-4bb2-adf2-c0442c99bedd" width="800"/><p class="wp-caption-text">The same structure can be represented three different ways: an expanded formula, a condensed formula, and a skeletal structure.</p></div>
<div class="ns-school-emp">
<h2>Example</h2>
<div class="ns-school-defn">
<div data-type="example">
<h3>Drawing Skeletal Structures</h3>
<p>Draw the skeletal structures for these two molecules:</p>
<img alt="Figure a shows a branched molecule with C H subscript 3 bonded to C with C H subscript 3 groups bonded both above and below it. To the right of the central C, a C H is bonded which has a C H subscript 3 group bonded above and to the right and below and to the right. Figure b shows a straight chain molecule composed of C H subscript 3 C H subscript 2 C H subscript 2 C H subscript 2 C H subscript 2 C H subscript 2 C H subscript 3." src="https://data.ulearngo.com/assets/72fa178c-45ca-45e0-adcf-471389d928e6"/>
<h3>Solution</h3>
<p>Each carbon atom is converted into the end of a line or the place where lines intersect. All hydrogen atoms attached to the carbon atoms are left out of the structure (although we still need to recognize they are there):</p>
<img alt="Figure a shows a branched skeleton structure that looks like a plus sign with line segments extending up and to the right and down and to the left of the rightmost point of the plus sign. Figure b appears in a zig zag pattern made with six line segments. The segments rise, fall, rise, fall, rise, and fall moving left to right across the figure." src="https://data.ulearngo.com/assets/1c26a7cf-07b5-4b22-a17a-70a222a2bf87"/></div>
</div>
</div>
<div class="ns-school-emp">
<h2>Example</h2>
<div class="ns-school-defn">
<div data-type="example">
<h3>Interpreting Skeletal Structures</h3>
<p>Identify the chemical formula of the molecule represented here:</p>
<img alt="This figure shows a pentagon with a vertex pointing right, from which a line segment extends that has two line segments attached at its right end, one extending up and to the right, and the other extending down and to the right." src="https://data.ulearngo.com/assets/962cd79a-8371-47d6-b6c7-6d6149364655"/>
<h3>Solution</h3>

There are eight places where lines intersect or end, meaning that there are eight carbon atoms in the molecule. Since we know that carbon atoms tend to make four bonds, each carbon atom will have the number of hydrogen atoms that are required for four bonds. This compound contains 16 hydrogen atoms for a molecular formula of C<sub>8</sub>H<sub>16</sub>.

<p>Location of the hydrogen atoms:</p>
<img alt="In this figure a ring composed of four C H subscript 2 groups and one C H group in a pentagonal shape is shown. From the C H group, which is at the right side of the pentagon, a C H is bonded. From this C H, a C H subscript 3 group is bonded above and to the right and a second is bonded below and to the right." src="https://data.ulearngo.com/assets/dd9a31c0-5952-4b46-bc44-8a8c52546e54"/></div>
</div>
</div>
<p>All alkanes are composed of carbon and hydrogen atoms, and have similar bonds, structures, and formulas; noncyclic alkanes all have a formula of C<sub>n</sub>H<sub>2n+2</sub>. The number of carbon atoms present in an alkane has no limit. Greater numbers of atoms in the molecules will lead to stronger <a data-lesson="intermolecular-and-interatomic-forces" data-subject="chemistry" data-tutorial="states-of-matter" href="https://app.ulearngo.com/chemistry/states-of-matter/intermolecular-and-interatomic-forces">intermolecular</a> attractions (dispersion forces) and correspondingly different physical properties of the molecules. Properties such as melting point and boiling point (see the table below) usually change smoothly and predictably as the number of carbon and hydrogen atoms in the molecules change.</p>
<table summary="This table shows molecular formulas, melting points in degrees Celsius, boiling points in degrees Celsius, phases at S T P, and numbers of structural isomers for twelve alkanes. Methane, C H subscript 4 has a melting point of –182.5, a boiling point of –161.5, is a gas at S T P, and has 1 structural isomer. Ethane, C subscript 2 H subscript 6, has a melting point of –183.3, a boiling point of –88.6, is a gas at S T P, and has 1 structural isomer. Propane, C subscript 3 H subscript 8, has a melting point of –187.7, a boiling point of –42.1, is a gas at S T P, and has 1 structural isomer. Butane, C subscript 4 H subscript 10, has a melting point of –138.3, a boiling point of –0.5, is a gas at S T P, and has 2 structural isomers. Pentane, C subscript 5 H subscript 12, has a melting point of –129.7, a boiling point of 36.1, is a liquid at S T P, and has 3 structural isomers. Hexane, C subscript 6 H subscript 14, has a melting point of –95.3, a boiling point of 68.7, is a liquid at S T P, and has 5 structural isomers. Heptane, C subscript 7 H subscript 16, has a melting point of –90.6, a boiling point of 98.4, is a liquid at S T P, and has 9 structural isomers. Octane, C subscript 8 H subscript 18, has a melting point of –56.8, a boiling point of 125.7, is a liquid at S T P, and has 18 structural isomers. Nonane, C subscript 9 H subscript 20, has a melting point of –53.6, a boiling point of 150.8, is a liquid at S T P, and has 35 structural isomers. Decane, C subscript 10 H subscript 22, has a melting point of –29.7, a boiling point of 174.0, is a liquid at S T P, and has 75 structural isomers. Tetradecane, C subscript 14 H subscript 30, has a melting point of 5.9, a boiling point of 253.5, is a solid at S T P, and has 1858 structural isomers. Octadectane, C subscript 18 H subscript 38, has a melting point of 28.2, a boiling point of 316.1, is a solid at S T P, and has 60,523 structural isomers.">
<thead>
<tr>
<th colspan="6">Properties of Some Alkanes</th>
</tr>
<tr>
<th>Alkane</th>
<th>Molecular Formula</th>
<th>Melting Point (°C)</th>
<th>Boiling Point (°C)</th>
<th>Phase at STP</th>
<th>Number of Structural Isomers</th>
</tr>
</thead>
<tbody>
<tr>
<td>methane</td>
<td>CH<sub>4</sub></td>
<td>–182.5</td>
<td>–161.5</td>
<td>gas</td>
<td>1</td>
</tr>
<tr>
<td>ethane</td>
<td>C<sub>2</sub>H<sub>6</sub></td>
<td>–183.3</td>
<td>–88.6</td>
<td>gas</td>
<td>1</td>
</tr>
<tr>
<td>propane</td>
<td>C<sub>3</sub>H<sub>8</sub></td>
<td>–187.7</td>
<td>–42.1</td>
<td>gas</td>
<td>1</td>
</tr>
<tr>
<td>butane</td>
<td>C<sub>4</sub>H<sub>10</sub></td>
<td>–138.3</td>
<td>–0.5</td>
<td>gas</td>
<td>2</td>
</tr>
<tr>
<td>pentane</td>
<td>C<sub>5</sub>H<sub>12</sub></td>
<td>–129.7</td>
<td>36.1</td>
<td>liquid</td>
<td>3</td>
</tr>
<tr>
<td>hexane</td>
<td>C<sub>6</sub>H<sub>14</sub></td>
<td>–95.3</td>
<td>68.7</td>
<td>liquid</td>
<td>5</td>
</tr>
<tr>
<td>heptane</td>
<td>C<sub>7</sub>H<sub>16</sub></td>
<td>–90.6</td>
<td>98.4</td>
<td>liquid</td>
<td>9</td>
</tr>
<tr>
<td>octane</td>
<td>C<sub>8</sub>H<sub>18</sub></td>
<td>–56.8</td>
<td>125.7</td>
<td>liquid</td>
<td>18</td>
</tr>
<tr>
<td>nonane</td>
<td>C<sub>9</sub>H<sub>20</sub></td>
<td>–53.6</td>
<td>150.8</td>
<td>liquid</td>
<td>35</td>
</tr>
<tr>
<td>decane</td>
<td>C<sub>10</sub>H<sub>22</sub></td>
<td>–29.7</td>
<td>174.0</td>
<td>liquid</td>
<td>75</td>
</tr>
<tr>
<td>tetradecane</td>
<td>C<sub>14</sub>H<sub>30</sub></td>
<td>5.9</td>
<td>253.5</td>
<td>solid</td>
<td>1858</td>
</tr>
<tr>
<td>octadecane</td>
<td>C<sub>18</sub>H<sub>38</sub></td>
<td>28.2</td>
<td>316.1</td>
<td>solid</td>
<td>60,523</td>
</tr>
</tbody>
</table>
<p>Hydrocarbons with the same formula, including alkanes, can have different structures. For example, two alkanes have the formula C<sub>4</sub>H<sub>10</sub>: They are called <em>n</em>-butane and 2-methylpropane (or isobutane), and have the following Lewis structures:</p>
<p><img alt="The figure illustrates three ways to represent molecules of n dash butane and 2 dash methlylpropane. In the first row of the figure, Lewis structural formulas show element symbols and bonds between atoms. The n dash butane molecule shows 4 carbon atoms represented by the letter C bonded in a straight horizontal chain with hydrogen atoms represented by the letter H bonded above and below all carbon atoms. H atoms are bonded at the ends to the left and right of the left-most and right-most C atoms. In the second row, ball-and-stick models are shown. In these representations, bonds are represented with sticks, and elements are represented with balls. Carbon atoms are black and hydrogen atoms are white in this image. In the third row, space-filling models are shown. In these models, atoms are enlarged and pushed together, without sticks to represent bonds. The molecule names are provided in the fourth row." src="https://data.ulearngo.com/assets/8b9988af-a8af-48f4-b65d-b9d306e8a4ef"/></p>
<p>The <a data-lesson="compounds-2" data-subject="chemistry" data-tutorial="quantitative-aspects-chemical-change" href="https://app.ulearngo.com/chemistry/quantitative-aspects-chemical-change/compounds-2">compounds</a> <em>n</em>-butane and 2-methylpropane are structural isomers (the term constitutional isomers is also commonly used). Constitutional isomers have the same molecular formula but different spatial arrangements of the atoms in their molecules. The <em>n</em>-butane molecule contains an <em>unbranched chain</em>, meaning that no carbon atom is bonded to more than two other carbon atoms. We use the term <em>normal</em>, or the prefix <em>n</em>, to refer to a chain of carbon atoms without branching. The compound 2–methylpropane has a branched chain (the carbon atom in the center of the Lewis structure is bonded to three other carbon atoms)</p>
<p>Identifying isomers from Lewis structures is not as easy as it looks. Lewis structures that look different may actually represent the same isomers. For example, the three structures in the figure below all represent the same molecule, <em>n</em>-butane, and hence are not different isomers. They are identical because each contains an unbranched chain of four carbon atoms.</p>
<div class="wp-caption alignnone" style="width: 800px"><img alt="The figure illustrates three ways to represent molecules of n dash butane. In the first row of the figure, Lewis structural formulas show carbon and hydrogen element symbols and bonds between the atoms. The first structure in this row shows three of the linked C atoms in a horizontal row with a single C atom bonded above the left-most carbon. The left-most C atom has two H atoms bonded to it. The C atom bonded above the left-most C atom has three H atoms bonded to it. The C atom bonded to the right of the left-most C atom has two H atoms bonded to it. The right-most C atom has three H atoms bonded to it. The C atoms and the bonds connecting all the C atoms are red. The second structure in the row similarly shows the row of three linked C atoms with a single C atom bonded below the C atom to the left. The left-most C atom has two H atoms bonded to it. The C atom bonded below the left-most C atom has three H atoms bonded to it. The C atom bonded to the right of the left-most C atom has two H atoms bonded to it. The right-most atom has three H atoms bonded to it. All the C atoms and the bonds between them are red. The third structure has two C atoms bonded in a row with a third C atom bonded above the left C atom and the fourth C atom bonded below the right C atom. The C atom bonded above the left C atom has three H atoms bonded to it. The left C atom has two H atoms bonded to it. The right C atom has two H atoms bonded to it. The C atom bonded below the right C atom has three H atoms bonded to it. All the C atoms and the bonds between them are red. In the second row, ball-and-stick models for the structures are shown. In these representations, bonds are represented with sticks, and elements are represented with balls. Carbon atoms are black and hydrogen atoms are white in this image. In the third row, space-filling models are shown. In these models, atoms are enlarged and pushed together, without sticks to represent bonds." height="607" src="https://data.ulearngo.com/assets/26627952-e201-4839-a8d9-0f9549584195" width="800"/><p class="wp-caption-text">These three representations of the structure of n-butane are not isomers because they all contain the same arrangement of atoms and bonds.</p></div>

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Alkanes

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Alkanes

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