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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="../355/atomic-structure.html">Atomic Structure</a><i class="fa fa-fw fa-chevron-right divider"></i></li><li><span class="gray">Electron configuration</span></li> <span class="pull-right" style="color: #555" title="Suggested study time: 60 minutes"><i class="fa fa-clock-o"></i> 60'</span> </ol> <article id="main-article"> <p><img alt="" src="../../images/atomic-structure/electronconfig-1.png" style="float: left; width: 160px; height: 182px;">The electron configuration, that is the distribution or arrangement of electrons in the atom, can be described by the Bohr model of the atom and the quantum mechanical model of the atom. The Bohr model is simpler, with electrons found in shells around the nucleus. The quantum mechanical model is more complex and takes into account a broader range of evidence that we have about the positions of electrons in atoms. You need to know both models of the atom. Although <em>questions focused on electron configuration will always be asking about the quantum mechanical model</em> (and that is what is tested in questions here), you also need to be confident in understanding the Bohr model, which is used in describing chemical bonding and structure, later in the course.</p> <p>This topic is probably the most challenging in the whole course in terms of the abstract concepts covered, so do not be worried if understanding it all is difficult at the start. Breaking it down by learning the key information presented in the revision cards and repeatedly test yourself using the practice questions will help you get there in the end. </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>emission spectrum, absorption spectrum, continuous spectrum*, line spectrum*, energy level, sub-level, orbital, Aufbau principle, Hund's rule, Pauli exclusion principle</p> <div class="tib-flashcard"><a class="show-flashcards btn btn-success btn-xs-block btn-block " data-levels="1" data-mode="" data-topics="567" data-subject-id="7" data-n-flashcards="10" 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 model of the atom</p> </div> </div> <div class="panel-body"> <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 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 hydrogen emission spectrum</p> </div> </div> <div class="panel-body"> <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/291116913"></iframe></div> </div> <div class="panel-footer"> <div> </div> </div> </div> </div> </div> <div class="panel-body"> <div> <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 quantum mechanical model of the atom</p> </div> </div> <div class="panel-body"> <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/328600062"></iframe></div> </div> <div class="panel-footer"> <div> </div> </div> </div> </div> </div> <div class="panel-body"> <div> <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 quantum mechanical model and the periodic table</p> </div> </div> <div class="panel-body"> <div> <p>Understanding the relationship between electronic configuration and the arrangement of the periodic table.</p> <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/343225096"></iframe></div> </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> <div id="carousel-79" class="dynamic-gallery carousel slide" data-id="79"><div class="carousel-inner" role="listbox"><div class="item active"><a class="fancy" href="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132117.png" data-fancybox="gallery-79" title="" data-caption=""><img alt="" src="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132117.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-79/screen-shot-2018-10-30-at-123824.png" data-fancybox="gallery-79" title="" data-caption=""><img alt="" src="../../../std-galleries/7-79/screen-shot-2018-10-30-at-123824.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132133.png" data-fancybox="gallery-79" title="" data-caption=""><img alt="" src="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132133.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132151.png" data-fancybox="gallery-79" title="" data-caption=""><img alt="" src="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132151.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132205.png" data-fancybox="gallery-79" title="" data-caption=""><img alt="" src="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132205.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132224.png" data-fancybox="gallery-79" title="" data-caption=""><img alt="" src="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132224.png"></a></div><div class="item "><a class="fancy" href="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132239.png" data-fancybox="gallery-79" title="" data-caption=""><img alt="" src="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132239.png"></a></div></div><a class="left carousel-control" href="#carousel-79" role="button" data-slide="prev"><i class="fa fa-fw fa-chevron-left"></i></a><a class="right carousel-control" href="#carousel-79" 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/7-79/screen-shot-2018-10-25-at-132117-thumb128.jpg"><li><li data-index="1"><img title="Click to view" src="../../../std-galleries/7-79/screen-shot-2018-10-30-at-123824-thumb128.jpg"><li><li data-index="2"><img title="Click to view" src="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132133-thumb128.jpg"><li><li data-index="3"><img title="Click to view" src="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132151-thumb128.jpg"><li><li data-index="4"><img title="Click to view" src="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132205-thumb128.jpg"><li><li data-index="5"><img title="Click to view" src="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132224-thumb128.jpg"><li><li data-index="6"><img title="Click to view" src="../../../std-galleries/7-79/screen-shot-2018-10-25-at-132239-thumb128.jpg"><li></li></ol> </div> </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> <div class="tib-quiz" data-stats="7-111-713"><div class="label label-default q-number">1</div><div class="exercise shadow-bottom"><div class="q-question"><p>The electronic energy levels in an atom of hydrogen are:</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>getting closer together further from the nucleus</span></label> </p><p><label class="radio"> <input type="radio"> <span>evenly spaced apart </span></label> </p><p><label class="radio"> <input type="radio"> <span>randomly spaced apart</span></label> </p><p><label class="radio"> <input type="radio"> <span>getting closer together nearer to the nucleus</span></label> </p></div><div class="q-explanation"><p>The electronic energy levels are further apart at lower energy - nearer the nucleus. They get closer together in energy at higher energy - further away from the nucleus.</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>The electron transition between which two atomic energy levels <strong>emits</strong> the most energy?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>Second to seventh</span></label> </p><p><label class="radio"> <input type="radio"> <span>First to fourth</span></label> </p><p><label class="radio"> <input type="radio"> <span>Sixth to fourth</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>Third to first</span></label> </p></div><div class="q-explanation"><p>The question asks about emission - energy given out - so the transition must be from a <em>higher to lower</em> energy level. And as the energy gaps between the levels gets smaller at higher energy, third to first will be greater than sixth to fourth, so third to first 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">3</div><div class="exercise shadow-bottom"><div class="q-question"><p>What is the correct order of filling of electronic energy sub-levels in an atom (up to atomic number 36)?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>1s, 2s, 2p, 3s, 3p, 4s, 4d, 4p</span></label> </p><p><label class="radio"> <input type="radio"> <span>1s, 1p, 2s, 2p, 3s, 3p, 4s, 4p</span></label> </p><p><label class="radio"> <input type="radio"> <span>1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p</span></label> </p></div><div class="q-explanation"><p>The order of filling is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p. This must be learned. The periodic table can help since it is arranged in accordance with the filling of the electronic energy sub-levels in atoms.</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>What is the correct electronic configuration for an atom of sulfur?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>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> 4p<sup>2</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>1s<sup>2 </sup> 2s<sup>2</sup> 2p<sup>4</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>1s<sup>2 </sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>0</sup> 3p<sup>6 </sup></span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>1s<sup>2 </sup>2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>4</sup></span></label> </p></div><div class="q-explanation"><p>The sub-levels of an atom are filled in the following order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s. Remember that 's' sub-levels hold a maximum of 2 electrons, 'p' hold 6, and 'd' hold 10. A sulfur atom has sixteen electrons in total (atomic number is 16) so the electronic configuration for the sulfur atom is 1s<sup>2 </sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>4</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>Electron transitions in the hydrogen emission spectrum to levels n=1, n=2 and n=3 generate lines in which parts of the electromagnetic spectrum respectively?</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>n=1 in ultra-violet; n=2 in visible; n=3 in infra-red</span></label> </p><p><label class="radio"> <input type="radio"> <span>n=1 in infra-red; n=2 in ultra-violet; n=3 in visible</span></label> </p><p><label class="radio"> <input type="radio"> <span>n=1 in visible; n=2 in infra-red; n=3 in ultra-violet</span></label> </p><p><label class="radio"> <input type="radio"> <span>n=1 in ultra-violet; n=2 in infra-red ; n=3 in visible</span></label> </p></div><div class="q-explanation"><p>Electron transitions in the hydrogen emission spectrum from higher energy levels to n=1 result in emissions in the ultra-violet region (highest energy since these transitions have the largest gaps between energy levels). Transitions to n=2 are found in the visible region. Transitions to n=3 are found in the infra-red region (lowest energy since these transitions have the smallest gaps between energy levels).</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 description best describes the shape of a <em>p</em> orbital?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>A sphere</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>Two spheres side by side (touching)</span></label> </p><p><label class="radio"> <input type="radio"> <span>A circle</span></label> </p><p><label class="radio"> <input type="radio"> <span>Two circles side by side (touching)</span></label> </p></div><div class="q-explanation"><p>Orbitals are plots of electron position (90% probability) around the nucleus. They are three dimensional (not planar). An <em>s</em> orbital is a sphere; a <em>p</em> orbital is a three dimensional figure-of-eight. So the answer here that best decribes a <em>p </em>orbital is 'two spheres side by side (touching)'.</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>An atomic <strong>emission</strong> spectrum is produced when:</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>electrons move from electronic energy levels n=1 to n=2 </span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>electron transitions take place from a higher to a lower electronic energy level</span></label> </p><p><label class="radio"> <input type="radio"> <span>electron transitions take place from a lower to a higher electronic energy level</span></label> </p><p><label class="radio"> <input type="radio"> <span>electrons are excited to higher electronic energy levels</span></label> </p></div><div class="q-explanation"><p>Electron transitions (movements) from higher to lower energy levels result in energy being <strong>emitted</strong> (given out). Electron transitions from lower to higher energy levels result in energy being <strong>absorbed</strong> (taken in). The correct answer is '<em>electron transitions take place from a higher to a lower electronic energy level</em>' since it is the only answer that will result in energy being emitted (to give an emission spectrum) rather than absorbed.</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 maximum number of electrons that can be held the n=3 electronic energy level in an atom?</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>18</span></label> </p><p><label class="radio"> <input type="radio"> 2<span></span></label> </p><p><label class="radio"> <input type="radio"> <span>10</span></label> </p><p><label class="radio"> <input type="radio"> <span>8</span></label> </p></div><div class="q-explanation"><p>Each and every orbital can hold a maximum of two electrons. Any s sub-level contains one orbital and can therefore hold two electrons. Any p sub-level contains three orbitals and can therefore hold six electrons. Any d sub-level contains five orbitals and can therefore hold ten electrons. The n=3 energy level consists of the 3s, 3p and 3d sub-levels. Thus the answer is 18: 2 (3s) + 6 (3p) + 10 (3d). The 4s sub-level is filled before the 3d sub-level, which may cause some confusion here, but the 3d sub-level is still part of the n=3 energy level.</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>What is the maximum number of electrons that can be held in an orbital, a p sub-level, and the n=2 energy level respectively?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>1, 3, 4</span></label> </p><p><label class="radio"> <input type="radio"> <span>2, 8, 18</span></label> </p><p><label class="radio"> <input type="radio"> <span>2, 8, 8</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>2, 6, 8</span></label> </p></div><div class="q-explanation"><p>Each and every orbital can hold two electrons. Any s sub-level contains one orbital and can therefore hold two electrons. Any p sub-level contains three orbitals and can therefore hold six electrons. Any d sub-level contains five orbitals and can therefore hold ten electrons. The n=2 energy level consists of the 2s and 2p sub-levels. Thus the answer is 2, 6, 8: A maximum of 2 electrons can be held in an orbital, 6 in a p sub-level, and 8 in the n=2 energy level (2s and 2p; 2+6=8).</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 provide evidence for the existence of electrons in discrete energy levels?</p><p>1: The line emission spectrum of hydrogen</p><p>2: Electron spin</p><p>3: The mass spectrum of hydrogen</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>1 & 3 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>1, 2 & 3</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>1 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>1 & 2 only</span></label> </p></div><div class="q-explanation"><p>The line emission spectrum of hydrogen is composed of discrete lines that represent particular frequencies of light. Only certain frequencies are produced by electron transitions from higher to lower energy levels, suggesting that electrons only exist at certain energies within the atom. Thus the line emission spectrum provides evidence for the existence of electrons in discrete energy levels. Electron spin and the mass spectrum of hydrogen do not provide any evidence for this model.</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">11</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 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><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></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 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2</h4> <h5>Core (SL&HL): <a href="../2699/atomic-structure-core-sl-hl-paper-2-questions.html" title="Atomic Structure core (SL & HL) paper 2 questions">Atomic Structure core (SL & HL) paper 2 questions</a></h5> <h5>AHL (HL only): <a href="../2700/atomic-structure-ahl-hl-only-paper-2-questions.html" title="Atomic Structure AHL (HL only) paper 2 questions">Atomic 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="713"> <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>Electron configuration</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 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