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table</button> <div class="hidden-xs hidden-sm"> <button class="btn btn-default btn-block text-xs-center" data-toggle="modal" data-target="#modal-feedback" style="margin-bottom: 10px"><i class="fa fa-send"></i> Feedback</button> </div> </div> <div class="col-md-9" id="main-column"> <h1 class="page_title"> Covalent bonding <a href="#" class="mark-page-favorite pull-right" data-pid="881" title="Mark as favorite" onclick="return false;"><i class="fa fa-star-o"></i></a> </h1> <ol class="breadcrumb"> <li><a href="../../../chemistry.html"><i class="fa fa-home"></i></a><i class="fa fa-fw fa-chevron-right divider"></i></li><li><a href="../357/bonding-and-structure.html">Bonding and Structure</a><i class="fa fa-fw fa-chevron-right divider"></i></li><li><span class="gray">Covalent bonding</span></li> <span class="pull-right" style="color: #555" title="Suggested study time: 30 minutes"><i class="fa fa-clock-o"></i> 30'</span> </ol> <article id="main-article"> <p><img alt="" src="../../images/test-images/screenshot-2020-03-09-at-15.35.26-1.png" style="width: 160px; height: 90px; float: left;">Our model of covalent bonding is based on the Bohr model of the atom. We often think of a covalent bond as a shared pair of electrons (which it is) but be aware of the full definition that needs to be learned: A covalent bond is the electrostatic attraction between two nuclei and a pair of shared electrons.</p> <hr class="hidden-separator"> <div class="panel panel-has-colored-body panel-turquoise"> <div class="panel-heading"><a class="expander" href="#"><span class="fa fa-plus"></span></a> <div> <p>Key concepts</p> </div> </div> <div class="panel-body"> <div> <div class="panel-body"> <div> <p>Ensure you are confident using the terms below and learn the asterisked* definitions</p> <p><strong>a covalent bond*</strong>, <strong>bond polarity/dipole*</strong>, <strong>electronegativity*</strong>, electrostatic attraction, bonding pair, lone (non-bonding) pair</p> <div class="tib-flashcard"><a class="show-flashcards btn btn-success btn-xs-block btn-block " data-levels="1" data-mode="Normal" data-topics="605" data-subject-id="7" data-n-flashcards="6" style="text-align:center">Show flashcards</a></div><hr> <div class="panel panel-has-colored-body panel-has-border panel-turquoise"> <div class="panel-heading"><a class="expander" href="#"><span class="fa fa-plus"></span></a> <div> <p>The Bohr atom</p> </div> </div> <div class="panel-body"> <div>A reminder from <strong>electron configuration</strong> (section 2.2) that our Lewis (dot-cross) diagrams are based on the Bohr model of the atom.</div> <div> </div> <div class="video-embed vimeo"><iframe allow="accelerometer; autoplay; encrypted-media; gyroscope; picture-in-picture" allowfullscreen="" mozallowfullscreen="" webkitallowfullscreen="" height="420" width="100%" src="https://player.vimeo.com/video/283707909"></iframe></div> </div> <div class="panel-footer"> <div> </div> </div> </div> </div> </div> </div> </div> <div class="panel-footer"> <div> </div> </div> </div> <div class="panel panel-yellow panel-has-colored-body"> <div class="panel-heading"><a class="expander" href="#"><span class="fa fa-plus"></span></a> <div> <p>Essentials</p> </div> </div> <div class="panel-body"> <div> <p> The revision cards contain all of the essential content:</p> <div id="carousel-179" class="dynamic-gallery carousel slide" data-id="179"><div class="carousel-inner" role="listbox"><div class="item active"><a class="fancy" href="../../../std-galleries/7-179/screenshot-2020-03-09-at-171209.png" data-fancybox="gallery-179" title="" data-caption=""><img alt="" src="../../../std-galleries/7-179/screenshot-2020-03-09-at-171209.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-179/screenshot-2020-03-09-at-171233.png" data-fancybox="gallery-179" title="" data-caption=""><img alt="" src="../../../std-galleries/7-179/screenshot-2020-03-09-at-171233.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-179/screenshot-2020-03-09-at-171256.png" data-fancybox="gallery-179" title="" data-caption=""><img alt="" src="../../../std-galleries/7-179/screenshot-2020-03-09-at-171256.png"></a></div></div><a class="left carousel-control" href="#carousel-179" role="button" data-slide="prev"><i class="fa fa-fw fa-chevron-left"></i></a><a class="right carousel-control" href="#carousel-179" role="button" data-slide="next"><i class="fa fa-fw fa-chevron-right"></i></a></div><ol class="std-carousel-indicators"><li data-index="0"><img title="Click to view" src="../../../std-galleries/7-179/screenshot-2020-03-09-at-171209-thumb128.jpg"><li><li data-index="1"><img title="Click to view" src="../../../std-galleries/7-179/screenshot-2020-03-09-at-171233-thumb128.jpg"><li><li data-index="2"><img title="Click to view" src="../../../std-galleries/7-179/screenshot-2020-03-09-at-171256-thumb128.jpg"><li></li></ol> </div> </div> <div class="panel-footer"> <div> </div> </div> </div> <div class="panel panel-has-colored-body panel-green"> <div class="panel-heading"><a class="expander" href="#"><span class="fa fa-plus"></span></a> <div> <p>Test yourself</p> </div> </div> <div class="panel-body"> <div> <div class="panel-body"> <div> <div class="tib-quiz" data-stats="7-134-881"><div class="label label-default q-number">1</div><div class="exercise shadow-bottom"><div class="q-question"><p>What is a covalent bond?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>The electrostatic attraction between molecules with dipoles.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The electrostatic attraction between oppositely charged ions.</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>The electrostatic attraction between nuclei and shared pairs of electrons.</span></label> </p><p><label class="radio"> <input type="radio"> <span>The electrostatic attraction between nuclei and delocalised electrons.</span></label> </p></div><div class="q-explanation"><p>The correct answer is <em>the electrostatic attraction between nuclei and shared pairs of electrons</em>. The other explanations represent different types of bonding (ionic, metallic and intermolecular).</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">2</div><div class="exercise shadow-bottom"><div class="q-question"><p>How many electrons in total are shared between nitrogen atoms in an N<sub>2</sub> molecule?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>2</span></label> </p><p><label class="radio"> <input type="radio"> <span>3</span></label> </p><p><label class="radio"> <input type="radio"> <span>1</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>6</span></label> </p></div><div class="q-explanation"><p>The bond between the two nitrogen atoms is a triple bond (N≡N). Each bond consists of a pair of electrons, thus 3 × 2 = 6 electrons is the correct answer.</p><p>The number of bonds that non-metals atoms are likely to form can be predicted by their <strong>valency</strong>, and corresponds to the number of electrons needed for a full valence shell.</p><table border="0" cellpadding="0" cellspacing="0" style="width:100%;"><tbody><tr><td>Group number - old (new system)</td><td>IV (14)</td><td>V (15)</td><td>VI (16)</td><td>VII (17)</td></tr><tr><td>Electrons in outer (Bohr) shell</td><td>4</td><td>5</td><td>6</td><td>7</td></tr><tr><td>Valency</td><td>4</td><td>3</td><td>2</td><td>1</td></tr><tr><td>Example</td><td>C</td><td>N</td><td>O</td><td>Cl</td></tr></tbody></table><p>Metals tend not to form covalent bonds. Hydrogen has a valency of 1.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">3</div><div class="exercise shadow-bottom"><div class="q-question"><p>Ethane, ethene and ethyne have single, double and triple bonds respectively between the carbon atoms:</p><p>C–C ; C=C ; C≡C</p><p>Which is the shortest and which is the strongest of the bonds?</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>C≡C is the shortest and the strongest</span></label> </p><p><label class="radio"> <input type="radio"> <span>C–C is the shortest and C≡C is the strongest</span></label> </p><p><label class="radio"> <input type="radio"> <span>C–C is the shortest and the strongest</span></label> </p><p><label class="radio"> <input type="radio"> <span>C≡C is the shortest and C–C is the strongest</span></label> </p></div><div class="q-explanation"><p>The shorter the bond, the stonger the bond, since the electrostatic attraction between the shared electrons and the nuclei becomes greater the closer they are. <strong>Triple</strong> bonds are stronger and shorter than <strong>double </strong>bonds which are stronger and shorter than <strong>single</strong> bonds due to the greater number of electrons in the bond.</p><p>Thus:<em> C≡C is the shortest and the strongest</em>, is the correct answer.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">4</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which is the <strong>best </strong>definition of electronegativity?</p><p>A measure of...</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>the ability of an atom to attract a shared pair of electrons in a covalent bond.</span></label> </p><p><label class="radio"> <input type="radio"> <span>the ability of an atom to attract electrons.</span></label> </p><p><label class="radio"> <input type="radio"> <span>the number of electrons in an atom. </span></label> </p><p><label class="radio"> <input type="radio"> <span>the relative atomic radius of an atom. </span></label> </p></div><div class="q-explanation"><p>Electronegativity is defined as '...the relative ability of an atom to attract a shared pair of electrons in a covalent bond'.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">5</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following bonds is the most polar?</p><p>F–O ; O–C ; O–N; N–C</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>N–C</span></label> </p><p><label class="radio"> <input type="radio"> <span>F–O</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>O–C</span></label> </p><p><label class="radio"> <input type="radio"> <span>O–N</span></label> </p></div><div class="q-explanation"><p>Polarity of a bond can be estimated by looking at the difference in electronegativity of the elements of the atoms involved. Electronegativity values can be found in the data book:</p><table border="0" cellpadding="0" cellspacing="0" style="width: 100%;"><tbody><tr><td style="text-align: center;">C</td><td style="text-align: center;">N</td><td style="text-align: center;">O</td><td style="text-align: center;">F</td></tr><tr><td style="text-align: center;">2.6</td><td style="text-align: center;">3.0</td><td style="text-align: center;">3.4</td><td style="text-align: center;">4.0</td></tr></tbody></table><p>The C–O bond with a 0.8 difference is the most polar.</p><p>When you don't have a data book, remember that electronegativity increases moving right and upwards across the periodic table. All of the bonds given are made up of elements next to each other in the periodic table except for the C–O bond, which has greater separation and is therefore likely to be the most polar.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="label label-default q-number">6</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which representation shows the correct dipoles for the bonds in a molecule of an alcohol (hydroxyl functional group)?</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>C<sup>δ+</sup>–O<sup>δ–</sup>–H<sup>δ+</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>C<sup>δ–</sup>–O<sup>δ–</sup>–H<sup>δ+</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>C<sup>δ–</sup>–O<sup>δ+</sup>–H<sup>δ–</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>C<sup>δ+</sup>–O<sup>δ–</sup>–H<sup>δ–</sup></span></label> </p></div><div class="q-explanation"><p>Polarity of a bond can be estimated by looking at the difference in electronegativity of the elements of the atoms involved. Electronegativity values can be found in the data book:</p><table border="0" cellpadding="0" cellspacing="0" style="width:100%;"><tbody><tr><td style="text-align: center;">C</td><td style="text-align: center;">O</td><td style="text-align: center;">H</td></tr><tr><td style="text-align: center;">2.6</td><td style="text-align: center;">3.4</td><td style="text-align: center;">2.2</td></tr></tbody></table><p>When you don't have a data book, remember that electronegativity increases moving right and upwards across the periodic table. Hydrogen is an exception; remember that it has an electronegativity very similar to, but slightly less than carbon.</p><p>Here the oxygen atom is more electronegative than both carbon and hydrogen, so will carry the δ– charge; both C and H will carry a δ+ charge as they are less electronegative than O.</p></div><div class="actions"><span class="score" data-score="0"></span><button class="btn btn-default btn-sm btn-xs-block text-xs-center check"><i class="fa fa-check-square-o"></i> Check</button></div></div><div class="totals"><span class="score"></span><button class="btn btn-success btn-block text-center check-total"><i class="fa fa-check-square-o"></i> Check</button></div></div><hr> </div> </div> </div> </div> <div class="panel-footer"> <div> </div> </div> </div> <div class="panel panel-has-colored-body panel-default"> <div class="panel-heading"><a class="expander" href="#"><span class="fa fa-plus"></span></a> <div> <p>Exam-style questions</p> </div> </div> <div class="panel-body"> <h4>Paper 1</h4> <h5>Core (SL&HL): <a href="../2161/bonding-and-structure-core-sl-and-hl-paper-1-questions.html" title="Bonding and Structure core (SL and HL) paper 1 questions">Bonding and Structure core (SL and HL) paper 1 questions</a></h5> <h5>AHL (HL only): <a href="../2703/bonding-and-structure-ahl-hl-only-paper-1-questions.html" title=" Bonding and Structure AHL (HL only) paper 1 questions">Bonding and Structure AHL (HL only) paper 1 questions</a></h5> <h4>Paper 2</h4> <h5>Core (SL&HL): <a href="../2704/bonding-structure-core-sl-hl-paper-2-questions.html" title="Bonding & Structure core (SL & HL) paper 2 questions">Bonding & Structure core (SL & HL) paper 2 questions</a></h5> <h5>AHL (HL only): <a href="../2705/bonding-structure-ahl-hl-only-paper-2-questions.html" title="Bonding & Structure AHL (HL only) paper 2 questions">Bonding & Structure AHL (HL only) paper 2 questions</a></h5> </div> <div class="panel-footer"> <div>lent bonding is based on the Bohr model of the atom. 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</textarea></div><div class="modal-footer p-xs-3"><button type="button" class="btn btn-sm btn-primary btn-xs-block save-notes"><i class="fa fa-fw fa-pencil"></i>Save</button><button type="button" class="btn btn-sm btn-default btn-xs-block mx-xs-0" data-dismiss="modal" aria-label="Close">Close</button></div></div></div></div><div id="report-problem-sm-modal" class="modal fade overlay-modal report-problem" tabindex="-1" role="dialog"><div class="modal-dialog modal-sm" role="document"><div class="modal-content"><div class="modal-header p-xs-3"><h4 class="modal-title text-center my-xs-2">Report a problem for flashcard <span class="fc-viewer-id"></span></h4></div><div class="modal-body p-xs-3"><div class="msg"></div><div class="form-group mb-xs-0"><textarea class="form-control issue-description p-xs-3" rows="8"></textarea></div></div><div class="modal-footer p-xs-3"><button type="button" class="btn btn-sm btn-primary text-center btn-xs-block mb-xs-3 disabled send-report"><i class="fa fa-fw fa-paper-plane"></i>Send</button><button type="button" class="btn btn-sm btn-default text-center btn-xs-block mx-xs-0" data-dismiss="modal" aria-label="Close">Close</button></div></div></div></div> <div id="fcgame-viewer" class="modal fade modal-flashcard" tabindex="-1" role="dialog"> <div class="modal-dialog modal-lg modal-dialog-fcgame" role="document"> <div class="modal-content mc-flashcard modal-content-fcgame"> <div class="modal-header" style="background-color: #fafafa;"> <div class="row text-center" style="width: 100%;"> <div class="col-md-12"> <div style="display: flex; justify-content: space-between; align-items: center;"> <div class="text-left"> Your time: <span class="chronometer c-mobile" id="chronometer">00:00:</span> <span class="chronometer msec c-mobile" id="chronometer-msec">000</span> <br> Your best time: <span class="chronometer c-mobile" id="best-record"></span> </div> <button type="button" class="close" data-dismiss="modal" aria-label="Close"> <span aria-hidden="true">×</span> </button> </div> </div> </div> </div> <div id="fcgame-body" class=" modal-body modal-body-fcgame"> <div class="row-fluid"> <div class="col-lg-12 col-md-12 col-sm-12 fc-content" id="fc-content" style="padding: 15px;"></div> </div> </div> <div id="end-game" style="display: none;"> <div class="col-lg-10 col-lg-offset-1 col-md-10 col-md-offset-1 col-sm-10 col-sm-offset-1 result shadow-bottom"> <div id="end-game-dismiss"></div> <div id="end-game-results"></div> <div id="show-percent" style="margin-bottom: 30px;font-size: 16px;"></div> </div> <div id="end-game-fc" class="col-lg-12"></div> </div> <div id="start-game" class="col-lg-12 col-md-12 col-sm-12 centered"> <div style="width: 200px;"> <button class="btn btn-success btn-xs-block" id="play-game" style="display: block; width: 100%; margin: 10px 0;">Start</button> <button class="btn btn-default btn-xs-block" id="cancel-game" style="display: block; width: 100%; margin: 10px 0;">Cancel</button> </div> </div> <div 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