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class="gray">Hybridization</span></li> <span class="pull-right" style="color: #555" title="Suggested study time: 45 minutes"><i class="fa fa-clock-o"></i> 45'</span> </ol> <article id="main-article"> <p> <img alt="" src="../../images/test-images/screenshot-2020-07-16-at-11.36.21.png" style="width: 160px; height: 134px; float: left;">It is really important that you are confident with your molecular shapes (covalent structure 4.3) and formation of sigma and pi bonds (further aspects of covalent bonding 14.1) before you try to get to grips with hybridization. Hybridization is a section of the course that is very challenging conceptually. The challenge is that hybridization is an abstract adjustment to an abstract model! However, the important thing to remember is that it is <em>just </em>a change to our model. We use VSEPR to explain the shapes of molecules through the Lewis (dot-cross) model of bonding. And we use hybridization to allow us to explain the shapes of molecules through the quantum mechanical model of the atom; to adjust the arrangement of the atomic orbitals in three-dimensional space. If, despite efforts, you are struggling to get your head around hybridization; the last slide of the revision cards has a useful rule-of-thumb that you can apply to help deal with exam questions.</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> <h5><strong>hybridization*</strong>, sp<sup>3</sup> hybridization, sp<sup>2</sup> hybridization, sp hybridization</h5> <div class="tib-flashcard"><a class="show-flashcards btn btn-success btn-xs-block btn-block " data-levels="3" data-mode="Normal" data-topics="610" data-subject-id="7" data-n-flashcards="4" 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>Understanding Hybridization</p> </div> </div> <div class="panel-body"> <div>Understanding that sp<sup>3</sup>, sp<sup>2</sup> and sp hybridization are adjustments to our quantum mechanical model of the atom to account for molecular shapes.</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/444475544"></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> 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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="7-140-886"><div class="label label-default q-number">1</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which words are missing from the sentence below to give the best definition of hybridisation:</p><p>Hybridisation is the mixing of _______________ _______________ on the same atom, to produce hybrid orbitals.</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>atomic orbitals</span></label> </p><p><label class="radio"> <input type="radio"> <span>electron density</span></label> </p><p><label class="radio"> <input type="radio"> <span>energy levels</span></label> </p><p><label class="radio"> <input type="radio"> <span>molecular orbitals</span></label> </p></div><div class="q-explanation"><p>'atomic orbitals' is the correct answer.</p><p>Hybridisation is a theory used to justify the shape of molecules when considering the combination of <strong>atomic orbitals</strong> to form sigma and pi bonds.</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 s orbitals and how many p orbitals combine to produce an sp<sup>3</sup> hybrid orbital?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>3 s and 3 p</span></label> </p><p><label class="radio"> <input type="radio"> <span>1 s and 1 p</span></label> </p><p><label class="radio"> <input type="radio"> <span>3 s and 1 p</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>1 s and 3 p</span></label> </p></div><div class="q-explanation"><p>The hybrid orbital name gives this answer: sp<sup>3</sup> has a 1 s orbital hybridising with 3 p orbitals. This, for example, occurs in a tetrahedrally bonded carbon atom.</p><p>Row A shows the electrons in the outermost atomic orbitals of an isolated C atom.</p><p>Row B shows the electrons in the hybrid orbitals when the four atomic orbitals have mixed to produce four hybrid (sp<sup>3</sup>) orbitals.</p><p><img alt="" height="195" src="../../images/chemical-bonding-and-structure/hybridisation-c.png" width="319"></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>Look at the sketch below:</p><p><img alt="" height="189" src="../../images/chemical-bonding-and-structure/hybridisation-c.png" width="308"></p><p>It represents the hybridisation of a carbon atom from an isolated state (row A), to a state in which the carbon is bonded tetrahedrally (row B).</p><p>Which of the following can be said to be true in going from A to B?</p><p><strong>1: </strong>The total energy of the orbitals remains the same.</p><p><strong>2: </strong>Each and every orbital has the same energy when in A and it does in B.</p><p><strong>3: </strong>The orbitals in A and B have different shapes.</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>1, 2 and 3</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>1 and 3 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>2 and 3 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>1 and 2 only</span></label> </p></div><div class="q-explanation"><p>When the atomic orbitals of any atom hybridise (mix), the total energy of the orbitals remains the same. However, the energy of individual orbitals (that hybridise) will change, and the shapes of the orbitals (that hybridise) will change. See the sketch below:</p><p>Thus '1 and 3 only' is the correct answer.</p><p><img alt="" height="344" src="../../images/chemical-bonding-and-structure/sp3hybrid.png" width="410"></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>Consider propene CH<sub>3</sub>CHCH<sub>2</sub>. What is the hybridisation of each carbon atom in the order they are written?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>sp<sup>3</sup> ; sp<sup>2</sup> ; sp<sup>3</sup></span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>sp<sup>3</sup> ; sp<sup>2</sup> ; sp<sup>2</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>sp<sup>2</sup> ; sp ; sp<sup>3</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>sp<sup>3</sup> ; sp ; sp<sup>2</sup></span></label> </p></div><div class="q-explanation"><p>The carbon-carbon bonds are C–C=C. The rule of thumb for remembering hydridisation in carbon:</p><p>All single bonds, carbon is sp<sup>3</sup> hybridised.</p><p>One double bond (and two singles), carbon is sp<sup>2</sup> hybridised.</p><p>One triple bond (and one single) or two double bonds, carbon is sp hybridised.</p><p>Thus the correct answer here is: sp<sup>3</sup>; sp<sup>2</sup> ; sp<sup>2</sup></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>What are the shapes of the bonds around the carbon atoms in sp<sup>3</sup>, sp<sup>2</sup> and sp hybridised carbons respectively?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>tetrahedral ; trigonal pyramidal ; bent</span></label> </p><p><label class="radio"> <input type="radio"> <span>the shapes cannot be determined</span></label> </p><p><label class="radio"> <input type="radio"> <span>tetrahedral ; tetrahedral; tetrahedral</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>tetrahedral ; trigonal planar ; linear</span></label> </p></div><div class="q-explanation"><p>The correct answer is 'tetrahedral ; trigonal planar ; linear'.</p><p>sp<sup>3</sup> carbons have 4 single bonds arranged tetrahedrally; the four sp<sup>3</sup> hydrid orbitals move as far apart as possible in 3D space (tetrahedral).</p><p>sp<sup>2</sup> carbons have one double bond and 2 single bonds arranged in a trigonal planar shape; the three sp<sup>2 </sup>hydrid orbitals move as far apart as possible in 3D space (trigonal planar), and the non-hybridised p orbital sits above the plane forming a pi bond.</p><p>sp carbons have one triple bond and 2 single bonds (or two double bonds) arranged in a linear shape; the two sp hydrid orbitals move as far apart as possible in 3D space (linear), and the non-hybridised p orbitals sit perpendicular to the plane of the bonds, and each other, forming pi bonds.</p><p>In the diagram below hybrid orbitals are represented by <strong>lines </strong>(for clarity).</p><p><img alt="" src="../../images/chemical-bonding-and-structure/hybrid-shapes.png" style="width: 438px; height: 231px;"></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 of the following describes the bonding in carbon dioxide CO<sub>2</sub>?</p><p><strong>1: </strong>The carbon is sp hybridised.</p><p><strong>2: </strong>The shape of the molecule is linear.</p><p><strong>3: </strong>There are 2 sigma and 2 pi bonds in total in the molecule.</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>1 and 2 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>1 and 3 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>2 and 3 only</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>1, 2 and 3</span></label> </p></div><div class="q-explanation"><p>'1, 2 and 3' is the correct answer.</p><p>O=C=O; carbon dioxide has two double bonds. Each double bond consists of one sigma and one pi bond (so two of each in total).</p><p>The carbon atom is sp hybridised and has a linear shape around it (full explanantion below):</p><p>sp<sup>3</sup> carbons have 4 single bonds arranged tetrahedrally; the four sp<sup>3</sup> hydrid orbitals move as far apart as possible in 3D space (tetrahedral).</p><p>sp<sup>2</sup> carbons have one double bond and 2 single bonds arranged in a trigonal planar shape; the three sp<sup>2 </sup>hydrid orbitals move as far apart as possible in 3D space (trigonal planar), and the non-hybridised p orbital sits above the plane forming a pi bond.</p><p>sp carbons have one triple bond and 2 single bonds (or two double bonds) arranged in a linear shape; the two sp hydrid orbitals move as far apart as possible in 3D space (linear), and the non-hybridised p orbitals sit perpendicular to the plane of the bonds, and each other, forming pi bonds.</p><p>In the diagram below hybrid orbitals are represented by <strong>lines </strong>(for clarity).</p><p><img alt="" src="../../images/chemical-bonding-and-structure/hybrid-shapes.png" style="width: 438px; height: 231px;"></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">7</div><div class="exercise shadow-bottom"><div class="q-question"><p>What is the hybridization of the <strong>nitrogen </strong>atom in aminomethane (below)?</p><p><img alt="" src="../../images/chemical-bonding-and-structure/screenshot-2020-07-20-at-10.53.34.png" style="width: 120px; height: 101px;"></p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>sp hybridized</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>sp<sup>3</sup> hybridized</span></label> </p><p><label class="radio"> <input type="radio"> <span>sp<sup>2</sup> hybridized</span></label> </p><p><label class="radio"> <input type="radio"> <span>It is not hybridized</span></label> </p></div><div class="q-explanation"><p>When identifying the hybridization of a given atom, it is best to use our 'rule-of-thumb'; that the geometry of the<strong> electron domains</strong> (see molecular shapes in the covalent structure section 4.3) tells us the hybridization:</p><p><strong>Tetrahedral electron domains means sp<sup>3</sup> hybridization.</strong></p><p><strong>Trigonal planer electron domains means sp<sup>2</sup> hybridization.</strong></p><p><strong>Linear electron domains means sp hybridization.</strong></p><p>The nitrogen atom here has electron domains that are tetrahedrally arranged (although the bonds are trigonal pyramidal around the central atom) so it must be sp<sup>3</sup> hybridized.</p><p><strong>sp<sup>3</sup> hybridized</strong> 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">8</div><div class="exercise shadow-bottom"><div class="q-question"><p>What is the hybridization of the <strong>oxygen </strong>atom in propanone (below)?</p><p><img alt="" src="../../images/chemical-bonding-and-structure/screenshot-2020-07-20-at-11.07.59.png" style="width: 120px; height: 108px;"></p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>sp<sup>3</sup> hybridized</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>sp<sup>2</sup> hybridized</span></label> </p><p><label class="radio"> <input type="radio"> <span>It is not hybridized</span></label> </p><p><label class="radio"> <input type="radio"> <span>sp hybridized</span></label> </p></div><div class="q-explanation"><p>When identifying the hybridization of a given atom, it is best to use our 'rule-of-thumb'; that the geometry of the<strong> electron domains</strong> (see molecular shapes in the covalent structure section 4.3) tells us the hybridization:</p><p><strong>Tetrahedral electron domains means sp<sup>3</sup> hybridization.</strong></p><p><strong>Trigonal planer electron domains means sp<sup>2</sup> hybridization.</strong></p><p><strong>Linear electron domains means sp hybridization.</strong></p><p>The oxygen atom here has electron domains that are arranged in a trigonal planar manner so it must be sp<sup>2</sup> hybridized.</p><p><strong>sp<sup>2</sup> hybridized</strong> 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="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> </div> </div> </div> <div class="page-container panel-self-assessment" data-id="886"> <div class="panel-heading">MY PROGRESS</div> <div class="panel-body understanding-rate"> <div class="msg"></div> <label class="label-lg">Self-assessment</label><p>How much of <strong>Hybridization</strong> have you understood?</p><div class="slider-container text-center"><div id="self-assessment-slider" class="sib-slider self-assessment " data-value="1" data-percentage=""></div></div> <label class="label-lg">My notes</label> <textarea name="page-notes" class="form-control" rows="3" placeholder="Write your notes here..."></textarea> </div> <div class="panel-footer text-xs-center"> <span id="last-edited" class="mb-xs-3"> </span> 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}</style><div id="modal-periodic-table" class="modal fade" tabindex="-1" role="dialog"> <div class="modal-dialog modal-lg" role="document" style="width: 90vw;"> <div class="modal-content"> <div class="modal-header"> <h4 class="modal-title">Periodic table</h4> <button type="button" class="close" data-dismiss="modal" aria-label="Close"> <span aria-hidden="true">×</span> </button> </div> <div class="modal-body"> <img src="../../../img/periodic-table/periodic-table-2020.png" style="max-width: 1400px; height: auto"> </div> <div class="modal-footer"> <button type="button" class="btn btn-default btn-xs-block m-xs-0 pull-right" data-dismiss="modal" aria-hidden="true"> Close </button> </div> </div> </div></div> <div id="fc-viewer" class="modal fade modal-flashcard" tabindex="-1" role="dialog"><div class="modal-dialog" role="document"><div class="modal-content"><div class="modal-header" style="background-color: #fafafa;"><div class="row" style="width: 100%;"><div class="col-md-12 tags-heading"><div style="display: flex; justify-content: space-between; align-items: center;"><p id="fc-viewer-info" style="width: 80%;"></p><button type="button" class="close" data-dismiss="modal" aria-label="Close"><span aria-hidden="true">×</span></button></div></div></div></div><div id="flashcard-body" class="modal-body"><div class="row" style="margin: 0;"><div class="col-md-8 fc-viewer-main"><div class="fc-viewer-inner"><div id="fc-viewer-main-front"><div class="fc-viewer-content"></div><span class="mark-favorite" style="position: absolute; top: 10px; right: 10px; font-size: 22px;"><i class="fa fa-lg fa-star-o"></i></span><span id="issue-report" class="issue-report hidden-xs hidden-sm" title="Report a problem"><i class="fa fa-fw fa-lg fa-exclamation-circle" style="font-size: 1.5em;"></i> </span> </div><div id="fc-viewer-main-back" class="reverse-flashcard green-bg"><div class="fc-viewer-content"></div><span class="mark-favorite" style="position: absolute; top: 10px; right: 10px; font-size: 22px;"><i class="fa fa-lg fa-star-o"></i></span></div></div></div><div class="col-md-4 fc-viewer-controls"><div class="fc-viewer-controls-middle"> <div class="fc-viewer-controls-middle-inner fc-back"><div class="fc-viewer-controls-answers mt-xs-0 mx-xs-0"><button id="right-answer" class="btn btn-success text-center btn-block" title="Mark this flashcard as CORRECT"><i class="fa fa-check"></i> Correct</button><button id="wrong-answer" class="btn text-center bg-red btn-block" title="Mark this flashcard as INCORRECT"><i class="fa fa-remove"></i> Incorrect</button></div><table class="table stats"><tr><td>Times flipped</td><td id="fc-viewer-tflipped" class="text-right">0</td></tr><tr><td>Marked as <em>correct</em></td><td id="fc-viewer-right" class="text-right">0</td></tr><tr><td>Marked as <em>incorrect</em></td><td id="fc-viewer-wrong" class="text-right">0</td></tr></table><a href="#" class="btn btn-default btn-sm btn-block text-center reset-stats hidden-xs hidden-sm" title="Reset stats for this flashcard" style="margin: 10px 0;"><i class="fa fa-undo"></i> Reset</a> <div class="fc-notes-container hidden-xs hidden-sm"><textarea class="form-control notes fc-back card-notes" rows="4" placeholder="Write your own notes here..." style="resize: none;">
</textarea><a href="#" class="btn btn-default btn-sm btn-block text-center save-notes" title="Save personal notes for this flashcard" style="margin-bottom: 10px;"><i class="fa fa-pencil"></i> Save notes</a> </div><div class="fc-viewer-actions-sm hidden-md hidden-lg"><button type="button" class="btn btn-sm btn-xs-block reset-stats"><i class="fa fa-fw fa-undo"></i>Reset</button> <button type="button" class="btn btn-sm btn-xs-block" data-toggle="modal" data-target="#card-notes-sm-modal"><i class="fa fa-fw fa-pencil"></i>Notes</button><button type="button" class="btn btn-sm btn-xs-block" data-toggle="modal" data-target="#report-problem-sm-modal"><i class="fa fa-fw fa-exclamation-circle"></i>Report error</button></div> </div></div><div class="fc-viewer-controls-bottom hidden-xs hidden-sm"><div class="fc-move"> <button class="btn bg-turquoise text-center disabled" rel="prev" title="Previous flashcard"><i class="fa fa-fw fa-chevron-left"></i>Prev</button><button class="btn bg-turquoise text-center disabled" rel="next" title="Next flashcard">Next<i class="fa fa-fw fa-chevron-right"></i></button></div><div class="fc-actions"><button class="btn btn-default btn-block text-center shuffle"><i class="fa fa-random"></i> Shuffle</button><div class="fc-progress"><div class="progress"><div class="progress-bar"></div></div><div class="text-right"><span class="fc-viewer-results-counter"></span></div></div></div></div><div class="fc-close-sm hidden-md hidden-lg"><button id="fc-xs-close" type="button" class="btn btn-default btn-block text-center" data-dismiss="modal" aria-label="Close">Close</button> <hr class="thin"> <div class="fc-actions" style="width: 100%;"> <button class="btn btn-default btn-block text-center shuffle"> <i class="fa fa-random"></i> Shuffle </button><div class="fc-progress"><div class="progress"><div class="progress-bar"></div></div><div class="text-right"><span class="fc-viewer-results-counter hidden-md hidden-lg"></span></div></div> </div></div></div></div></div><div class="modal-footer"><div id="report-error-container" class="report-problem"><div class="row"><div class="col-md-8"><div class="msg"></div><div class="form-group"><label>Report a problem for flashcard <span class="fc-viewer-id"></span></label><textarea class="form-control issue-description" cols="4"></textarea></div><button type="button" class="btn btn-primary pull-right send-report disabled"><i class="fa fa-paper-plane"></i>Send</button><button id="close-send-report" type="button" class="btn btn-default" style="margin-left: 0;">Close</button></div></div></div></div></div></div></div><div id="card-notes-sm-modal" class="modal fade overlay-modal" 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">Notes</h4></div><div class="modal-body p-xs-3"><textarea class="form-control notes fc-back card-notes p-xs-3" rows="8" style="resize: none;">
</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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