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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="../356/periodicity.html">Periodicity</a><i class="fa fa-fw fa-chevron-right divider"></i></li><li><span class="gray">First-row d-block elements</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/periodicity/vanadiumoxidationstates.jpg" style="width: 160px; height: 122px; float: left;">This section of the course is not in itself too conceptually challenging, but there are lots of links to other parts of the course. Ensure that you are confident with electronic structure (quantum mechanical model of the atom), know about dative bonds and shapes of molecules, and understand Lewis acids and bases. Then it is a matter of learning the content here.</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 transition element*, A ligand*, A dative (coordinate) bond*, A complex ion*, Coordination number*</strong>, Monodentate ligand, Polydentate ligand, Paramagnetism, Ferromagnetism, Diamagnetism</p> <div class="tib-flashcard"><a class="show-flashcards btn btn-success btn-xs-block btn-block " data-levels="1,3" data-mode="Normal" data-topics="633" data-subject-id="7" data-n-flashcards="10" style="text-align:center">Show flashcards</a></div><hr> </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-187" class="dynamic-gallery carousel slide" data-id="187"><div class="carousel-inner" role="listbox"><div class="item active"><a class="fancy" href="../../../std-galleries/7-187/screenshot-2020-07-22-at-160418.png" data-fancybox="gallery-187" title="" data-caption=""><img alt="" src="../../../std-galleries/7-187/screenshot-2020-07-22-at-160418.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-187/screenshot-2020-07-22-at-175017.png" data-fancybox="gallery-187" title="" data-caption=""><img alt="" src="../../../std-galleries/7-187/screenshot-2020-07-22-at-175017.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-187/screenshot-2020-07-22-at-160457.png" 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src="../../../std-galleries/7-187/screenshot-2020-07-22-at-160622-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="7-153-878"><div class="label label-default q-number">1</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following describes the typical properties of a transition metal?</p><p><strong>1: </strong>They have variable oxidation states.</p><p><strong>2: </strong>They display catalytic properties.</p><p><strong>3: </strong>They are Lewis acids.</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>2 and 3 only</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>1, 2 and 3</span></label> </p><p><label class="radio"> <input type="radio"> <span>1 and 3 only</span></label> </p></div><div class="q-explanation"><p>Transition metals have variable oxidation states, form complex ions with ligands (ligands donate electron pairs into the metal centre, so the transition metal is behaving as a Lewis acid), have coloured compounds, and display catalytic and magnetic properties. Thus 1,2 and 3 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">2</div><div class="exercise shadow-bottom"><div class="q-question">What are the electronic configurations of chromium and copper atoms respectively?</div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>[Ar] 4s<sup>1</sup> 3d<sup>5</sup> and [Ar] 4s<sup>2</sup> 3d<sup>9</sup></span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>[Ar] 4s<sup>1</sup> 3d<sup>5</sup> and [Ar] 4s<sup>1</sup> 3d<sup>10</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>[Ar] 4s<sup>2</sup> 3d<sup>4</sup> and [Ar] 4s<sup>1</sup> 3d<sup>10</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>[Ar] 4s<sup>2</sup> 3d<sup>4</sup> and [Ar] 4s<sup>2</sup> 3d<sup>9</sup></span></label> </p></div><div class="q-explanation">Chromium and copper have unusual electronic configurations that do not follow the Aufbau principle (filling electron energy levels in order, lowest energy first), since the half-filled singly oocupied d-orbital configurations ([Ar] 4s<sup>1</sup> 3d<sup>5</sup> and [Ar] 4s<sup>1</sup> 3d<sup>10</sup>) happen to be of lower energy than the expected configurations ([Ar] 4s<sup>2</sup> 3d<sup>4</sup> and [Ar] 4s<sup>2</sup> 3d<sup>9</sup>)</div><div class="q-explanation">Thus '[Ar] 4s<sup>1</sup> 3d<sup>5</sup> and [Ar] 4s<sup>1</sup> 3d10' is the correct answer, where [Ar] indicates the electron configuration of argon: 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup>.</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>Which of the following cannot act as a ligand?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>OH<sup>−</sup></span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>NH<sub>4</sub><sup>+</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>H<sub>2</sub>O</span></label> </p><p><label class="radio"> <input type="radio"> <span>NH<sub>3</sub></span></label> </p></div><div class="q-explanation"><p>A ligand must have a lone pair of electrons that can be donated to a metal centre to form a coordinate (dative) bond. All of the species written have a lone pair except for the ammonium ion (NH<sub>4</sub><sup>+</sup>) which does not, and is therefore 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>A complex ion has the formula [Ni(en)<sub>3</sub>]<sup>2+</sup>.</p><p>What is the coordination number of the nickel ion, and what is the denticity (number of coordinate bonds that a single ligand can form to a metal centre) of the 'en' ligand?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>3 ; bidentate</span></label> </p><p><label class="radio"> <input type="radio"> <span>3 ; monodentate</span></label> </p><p><label class="radio"> <input type="radio"> <span>6 ; monodentate</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>6 ; bidentate</span></label> </p></div><div class="q-explanation"><p>The 'en' ligand is 1,2-ethanediamine and its structure is shown in the data book (section 16 Ligands). As can be seen from the structure it has <strong>two amine groups</strong> capable of donating a pair of electrons and it is therefore <strong>bidentate</strong>.</p><p>If each 'en' forms two coordinate bonds to the nickel ion, and there are three ligands, there are a total of six coordinate bonds into the nickel centre - the<strong> coordination number is 6</strong>.</p><p>'6 ; bidentate' 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">5</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following d-block metal compounds is not coloured?</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>ZnO<sub>(s)</sub></span></label> </p><p><label class="radio"> <input type="radio"> <span>Fe<sub>2</sub>O<sub>3(s)</sub></span></label> </p><p><label class="radio"> <input type="radio"> <span>[Fe(H<sub>2</sub>O)<sub>5</sub>SCN]<sup>2+</sup><sub>(aq)</sub></span></label> </p><p><label class="radio"> <input type="radio"> <span>CuCO<sub>3(s)</sub></span></label> </p></div><div class="q-explanation"><p>Most transition metal compounds are coloured, but Zn is not considered to be a transition metal (despite being in the d-block) because it does not form ions with incomplete d-orbitals (It is only stable as Zn<sup>2+</sup> in which it has lost both 4s electrons and has a complete 3d sub-level). Without incomplete d-orbitals in the metal d-block compounds cannot be coloured, so Zinc compounds, like ZnO, are not coloured. ZnO is the correct answer.</p><p>ZnO is a white solid, CuCO<sub>3</sub> is a blue-green solid, Fe<sub>2</sub>O<sub>3</sub> is a red-brown solid, [Fe(H<sub>2</sub>O)<sub>5</sub>SCN]<sup>2+</sup> is a blood-red solution.</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>What is the overall (missing) charge on the copper (II) complex ion: [CuCl<sub>4</sub>] ?</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>2+</span></label> </p><p><label class="radio"> <input type="radio"> <span>0</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>2−</span></label> </p></div><div class="q-explanation"><p>The charge on the copper ion is 2+ (given by the Roman numerals, II). Each chloride ligand (four are found in the complex) has a charge of 1−, so the overall charge will be 2+ + (4×1−) = 2−.</p><p><strong>Charge i</strong>s always expressed as number then sign, that is 2−.</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>Some magnetic substances behave as if they are weakly magnetic when an external magnetic field is applied.</p><p>Which type of magnetism does this sentence descibe?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>No type of magnetism is correctly described</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>Paramagnetism</span></label> </p><p><label class="radio"> <input type="radio"> <span>Ferromagnetism</span></label> </p><p><label class="radio"> <input type="radio"> <span>Diamagnetism</span></label> </p></div><div class="q-explanation"><p>Ferromagnetic substances, like iron, are permanently magnetic.</p><p>Paramagnetic substances have unpaired electrons, and behave as if they are weakly magnetic when an external magnetic field is applied.</p><p>Diamagnetic substances have all electrons paired, are not magnetic at all, and may be weakly repelled by an external magnetic field.</p><p>Thus paramagnetism is the correct answer here.</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>Which of the following contributes to the ability of transition metals to show catalytic activity?</p><p><strong>1: </strong>The relatively high melting points.</p><p><strong>2: </strong>The ability to form variable oxidation states.</p><p><strong>3: </strong>The ability to adsorb substances onto their surface.</p></div><div class="q-answer"><p><label class="radio"> <input class="c" 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><p><label class="radio"> <input type="radio"> <span>1 and 3 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>1, 2 and 3</span></label> </p></div><div class="q-explanation"><p>Transition metals can often act as catalysts because of their ability to switch between oxidation states, and because substances can easily adsorb onto the surface of a metal.</p><p>There is no evidence that the relatively high melting points of transition metals contributes to their catalytic activity.</p><p>Thus '2 and 3 only' 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">9</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following contributes to the ability of transition metals to form variable oxidation states?</p><p><strong>1: </strong>The relatively (compared to group 1 and 2 metals) low first ionisation energies.</p><p><strong>2: </strong>The presence of singly-occupied d-orbitals.</p><p><strong>3: </strong>The closeness in energy of the s and d sub-levels.</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 type="radio"> <span>1 and 3 only</span></label> </p><p><label class="radio"> <input class="c" 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>Transition metals do not have low first ionisation energies when compared to the main group metals.</p><p>The electrons in singly occupied d-orbitals are relatively unstable, and the s and d sub-levels are very close to each other in energy (remember that 's-electrons' are gained first and lost first). These factors contribute to transtion metals having successive ionisation energies that do not have 'big jumps' and thus being able to have variable oxidation states; thus 2 and 3 only 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">10</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the following are paramagnetic?</p><p><strong>1: </strong>Oxygen atoms</p><p><strong>2: </strong>Zinc atoms</p><p><strong>3: </strong>Vanadium atoms</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>2 and 3 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>3 only</span></label> </p><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></div><div class="q-explanation"><p>Paramagnetic substances have unpaired electrons, and behave as if they are weakly magnetic when an external magnetic field is applied.</p><p>Diamagnetic substances have all electrons paired, are not magnetic at all, and may be weakly repelled by an external magnetic field.</p><p>Oxygen and vanadium atoms both have unpaired electrons in their electronic configurations (1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>4</sup> and 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup> 4s<sup>2</sup> 3d<sup>3</sup> respectively), but zinc atoms do not (1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup> 4s<sup>2</sup> 3d<sup>10</sup>). Remember that all orbitals in a given sub-level are filled singly first, before electrons pair-up.</p><p>Thus '1 and 3 only' 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"> <div> <h4>Paper 1</h4> <h5>Core (SL&HL): <a href="../2425/periodicity-core-sl-and-hl-paper-1-questions.html" title="Periodicity core (SL and HL) paper 1 questions">Periodicity core (SL and HL) paper 1 questions</a></h5> <h5>AHL (HL only): <a href="../2736/periodicity-ahl-hl-only-paper-1-questions.html" title="Periodicity AHL (HL only) paper 1 questions">Periodicity AHL (HL only) paper 1 questions</a></h5> <h4>Paper 2</h4> <h5>Core (SL&HL): <a href="../2737/periodicity-core-sl-hl-paper-2-questions.html" title="Periodicity core (SL & HL) paper 2 questions">Periodicity core (SL & HL) paper 2 questions</a></h5> <h5>AHL (HL only): <a href="../2738/periodicity-ahl-hl-only-paper-2-questions.html" title="Periodicity AHL (HL only) paper 2 questions">Periodicity AHL (HL only) paper 2 questions</a></h5> </div> </div> <div class="panel-footer"> <div> </div> </div> </div> <div class="page-container panel-self-assessment" data-id="878"> <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>First-row d-block 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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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