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btn-block" style="margin-bottom: 10px"><i class="fa fa-table"></i> Periodic 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"> Periodicity AHL (HL only) paper 1 questions <a href="#" class="mark-page-favorite pull-right" data-pid="2736" 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="../2075/paper-1-exam-questions.html">Paper 1 Exam Questions</a><i class="fa fa-fw fa-chevron-right divider"></i></li><li><span class="gray">Periodicity AHL (HL only) paper 1 questions</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><strong>Topics 13.1 and 13.2</strong></p> <p><strong>Paper 1 style questions </strong>are multiple choice. You are <strong>not permitted to use a calculator or the data book</strong> for these questions, but you should use a periodic table.</p> <p>A <strong>periodic table pop-up</strong> is available on the left hand menu.</p> <div class="greenBg"> <div class="tib-quiz" data-stats="7-834-2736"><div class="label label-default q-number">1</div><div class="exercise shadow-bottom"><div class="q-question"><p>What is the overall charge, <span class="math-tex">\(x\)</span>, on the cobalt (II) complex ion: [CoCl<sub>4</sub>]<span class="math-tex">\(^x\)</span></p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>2+</span></label> </p><p><label class="radio"> <input class="c" type="radio"> 2− </label></p><p><label class="radio"> <input type="radio"> <span>0 (no charge)</span></label> </p><p><label class="radio"> <input type="radio"> <span>+2</span></label> </p></div><div class="q-explanation"><p>The charge on the cobalt ion is 2+ (given by the Roman numerals, II). Each chloride ligand (Cl<sup>−</sup>) has a charge of 1−, so the overall charge will be 4− + 2+ = 2−.</p><p>(Charge is always expressed as number then sign, that is 2−, not −2.)</p><p><strong>2−</strong> 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">2</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of these statements is/are correct?</p><p><strong>1: </strong>Ligands are Lewis bases</p><p><strong>2: </strong>Zinc compounds are coloured</p><p><strong>3: </strong>Titanium (II) compounds are paramagnetic</p></div><div class="q-answer"><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 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>Ligands are molecules or negative ions that donate lone pair(s) of electrons to form coordinate (dative) bonds to a metal ion. <strong>Ligands are Lewis bases</strong>; metal ions are Lewis acids (electron pair donor/acceptor).</p><p>Zinc is not considered to be a transition element as its only stable ion is Zn<sup>2+</sup> with a full d sub-level, so it does <strong>not form coloured compounds</strong>.</p><p>Paramagnetic substances have unpaired electrons (and behave as if they are weakly magnetic when an external magnetic field is applied). Titanium (II) ions have unpaired electrons in their electronic configuration (1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup> 4s<sup>0</sup> 3d<sup>2</sup>). Remember that <strong>4s electrons are gained first and lost first</strong>, and that all orbitals in a given sub-level are filled <strong>singly first</strong>, before electrons pair-up; the two d-electrons will be unpaired. Therefore, <strong>titanium (II) compounds are paramagnetic.</strong></p><p>Thus <strong>1 and 3 only</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">3</div><div class="exercise shadow-bottom"><div class="q-question"><p>What is the effect on d-orbital splitting and wavelength of light absorbed of a stronger ligand in an octahedral transition metal complex ion?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>d-orbital splitting decreases and wavelength decreases</span></label> </p><p><label class="radio"> <input type="radio"> <span>d-orbital splitting increases and wavelength increases</span></label> </p><p><label class="radio"> <input type="radio"> <span>d-orbital splitting decreases and wavelength increases</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>d-orbital splitting increases and wavelength decreases</span></label> </p></div><div class="q-explanation"><p>The spectrochemical series shows the increasing strength of ligands.</p><p><img alt="" src="../../images/periodicity/spectrochemical-series.png" style="width: 360px; height: 20px;"></p><p>Stronger ligands cause a greater split in the d-orbitals, this means that the energy gap (ΔE) increases. However, energy of light is inversely proportional to wavelength, so as the energy gap increases the wavelength of light absorbed by the gap will decrease.</p><p>Therefore, <strong>d-orbital splitting increases and wavelength decreases</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">4</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of these statements about copper (I) (Cu<sup>+</sup>) and copper (II) (Cu<sup>2+</sup>) compounds is correct?</p></div><div class="q-answer"><p><label class="radio"><input class="c" type="radio"> Copper (I) compounds are diamagnetic and copper (II) compounds are paramagnetic</label></p><p><label class="radio"><input type="radio"> Copper (I) compounds are paramagnetic and copper (II) compounds are diamagnetic</label></p><p><label class="radio"><input type="radio"> Both copper (I) compounds and copper (II) compounds are paramagnetic</label></p><p><label class="radio"><input type="radio"> Both copper (I) compounds and copper (II) compounds are diamagnetic</label></p></div><div class="q-explanation"><p>Substances with all electrons paired are diamagnetic – they are not magnetic, but may be slightly repelled by magnetic fields. Copper (I) ions (Cu<sup>+</sup>) have electronic configuration 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup> 4s<sup>0</sup> 3d<sup>10</sup> (remember that <strong>4s electrons are gained first and lost first)</strong>, so copper (I) compounds are diamagnetic.</p><p>Paramagnetic substances have unpaired electrons (and behave as if they are weakly magnetic when an external magnetic field is applied). Copper (II) ions have unpaired electrons in their electronic configuration (1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>6</sup> 3s<sup>2</sup> 3p<sup>6</sup> 4s<sup>0</sup> 3d<sup>9</sup>). Therefore, copper (II) compounds are paramagnetic.</p><p>Thus <strong>Copper (I) compounds are diamagnetic and copper (II) compounds are paramagnetic</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">5</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which contributes to colour in transition metal complexes?</p><p><strong>1: </strong>The splitting of the d-orbitals in energy.</p><p><strong>2: </strong>The d-orbitals are partially filled with electrons.</p><p><strong>3: </strong>Light is emitted when electrons fall between split d-orbitals.</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>1, 2 and 3</span></label> </p><p><label class="radio"> <input class="c" 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></div><div class="q-explanation"><p>Transition metal complexes are coloured because:</p><ul><li>Ligands in an octahedral complex cause <strong>splitting of d-orbitals</strong> into two sets at different energies.</li><li>The energy gap corresponds to wavelengths of visible light.</li><li>Absorption of visible light <strong>promotes electrons from low to high energy d-orbitals and the colour observed is the complementary colour to the colour/frequency of light absorbed</strong> e.g. copper sulfate solution is blue – orange light is absorbed.</li><li>It is necessary for <strong>d-orbitals to be partially-filled </strong>or electrons have no space to move.</li></ul><p>Thus <strong>1 and 2 only</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">6</div><div class="exercise shadow-bottom"><div class="q-question"><p>What is the oxidation state of the iron, and the overall charge on the complex ion, in the compound [Fe(H<sub>2</sub>O)<sub>4</sub>(OH)<sub>2</sub>]NO<sub>3</sub>?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>Oxidation state +2; charge on the complex ion 0 (no charge)</span></label> </p><p><label class="radio"> <input class="c" type="radio"> Oxidation state +3; charge on the complex ion 1+ </label></p><p><label class="radio"> <input type="radio"> <span>Oxidation state +3; charge on the complex ion 0 (no charge)</span></label> </p><p><label class="radio"> <input type="radio"> <span>Oxidation state +4; charge on the complex ion 2+</span></label> </p></div><div class="q-explanation"><p>The nitrate ion (NO<sub>3</sub><sup>−</sup>) has a charge of 1−, so in order for the compound to be neutral, the overall charge on the complex ion must be 1+.</p><p>The charge on the iron ion is therefore 3+, since each hydroxide ligand (OH<sup>−</sup>) has a charge of 1− (the water ligands have no charge) and the overall charge on the complex ion is 1+ (3+ + 2− = 1+).</p><p>Charge is always expressed as number then sign, so the charge on the iron ion is 3+, but the oxidation state is +3.</p><p><strong>Oxidation state +3; charge on the complex ion 1+</strong> 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">7</div><div class="exercise shadow-bottom"><div class="q-question">Which colour of an octahedral cobalt (III) complex ion has the greatest d-orbital splitting?</div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>Violet</span></label> </p><p><label class="radio"> <input type="radio"> <span>Green</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>Orange</span></label> </p><p><label class="radio"> <input type="radio"> <span>Blue</span></label> </p></div><div class="q-explanation"><p>Ligands in an octahedral complex cause splitting of d-orbitals into two sets at different energies and the energy gap corresponds to wavelengths of visible light.</p><p>Absorption of visible light promotes electrons from low to high energy d-orbitals and the colour observed is <strong>the complementary colour to the colour/frequency of light absorbed.</strong></p><p>Recalling the colour wheel:</p><p><img alt="" src="../../images/periodicity/colourwheel.png" style="width: 120px; height: 120px;"></p><p>As a rule of thumb, the colour observed is the opposite of the (maximum frequency of light of the) colour absorbed. The observed colour orange has a complementary colour of absorbed light of blue, and blue light corresponds to the highest frequency/energy (lowest wavelength) of all the complementary colours (as given in the question).</p><p>Summary: Complementary colours are Orange→Blue, Violet→Yellow, Green→Red, Blue→Orange. And energy of light (absorbed): Blue > Yellow > Orange > Red (ROYGBIV)</p><p><strong>Orange </strong>is thus 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>Part of the spectrochemical series is shown below:</p><p>Br<sup>−</sup> < F<sup>−</sup> < H<sub>2</sub>O < CN<sup>−</sup></p><p>Which statement can be correctly deduced from the series?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>Br<sup>−</sup> is a stronger ligand than F<sup>−</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>A complex with H<sub>2</sub>O ligands is blue</span></label> </p><p><label class="radio"> <input type="radio"> <span>CN<sup>−</sup> ligands cause complexes to be violet</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>CN<sup>−</sup> ligands cause greater d-orbital splitting than H<sub>2</sub>O</span></label> </p></div><div class="q-explanation"><p>Ligands in an octahedral complex cause splitting of d-orbitals into two sets at different energies and the energy gap corresponds to wavelengths of visible light.</p><p>Absorption of visible light promotes electrons from low to high energy d-orbitals and the colour observed is the complementary colour to the colour/frequency of light absorbed.</p><p>The spectrochemical series indicates the strength of the ligands (I<sup>−</sup> the weakest; CN<sup>−</sup> and CO the strongest), with stronger ligands (better electron pair donors) causing greater d-orbital splitting.</p><p><img alt="" height="36" src="../../images/periodicity/spectrochemical-series.png" width="643"></p><p>The colour of complexes cannot be determined by the spectrochemical series, since colour also depends on the metal ion and its oxidation state.</p><p>Therefore the correct answer is <strong>CN<sup>−</sup> ligands cause greater d-orbital splitting than H<sub>2</sub>O</strong>.</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>Comparing [CuCl<sub>4</sub>]<sup>2−</sup> and [Cu(H<sub>2</sub>O)<sub>6</sub>]<sup>2+</sup> which of these statements is/are correct?</p><p><strong>1: </strong>[CuCl<sub>4</sub>]<sup>2−</sup> has greater d-orbital splitting because of the lower oxidation state of the copper</p><p><strong>2: </strong>Both complexes are octahedral</p><p><strong>3: </strong>The copper ion has electron configuration of [Ar]3d<sup>9</sup> in both complexes</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>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 3 only</span></label> </p><p><label class="radio"> <input type="radio"> <span>1 only</span></label> </p></div><div class="q-explanation"><p>The [CuCl<sub>4</sub>]<sup>2−</sup> complex is <strong>tetrahedral</strong>, the chloride ligands have a 1− charge and so the copper ion is <strong>Cu<sup>2+</sup></strong>.</p><p>The [Cu(H<sub>2</sub>O)<sub>6</sub>]<sup>2+</sup> complex is <strong>octahedral</strong>, water ligands have no charge and so the copper ion is <strong>also Cu</strong><sup>2+</sup>.</p><p>The copper ion therefore has electron configuration of <strong>[Ar]3d<sup>9</sup> in both complexes.</strong></p><p>The degree of d-orbital splitting, and hence the colour of the complex, varies with the metal and oxidation state of the transition metal ion and with the strength of the ligand. However, <strong>the oxidation state of the copper is the same in both complexes (+2)</strong> so statement 1 is incorrect.</p><p>Thus <strong>3 only</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">10</div><div class="exercise shadow-bottom"><div class="q-question"><p>What is the coordination number and the oxidation state of the iron ion in [Fe(CN)<sub>6</sub>]<sup>3–</sup> ?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>Coordination number 3 ; oxidation state +3</span></label> </p><p><label class="radio"> <input type="radio"> <span>Coordination number 3 ; oxidation state −3</span></label> </p><p><label class="radio"> <input type="radio"> <span>Coordination number 6 ; oxidation state −3</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>Coordination number 6 ; oxidation state +3</span></label> </p></div><div class="q-explanation"><p>The CN<sup>–</sup> ligand is a cyanide ion and has a 1− charge.</p><p>Each CN<sup>–</sup> forms one coordinate bond to the iron ion, and there are six ligands. Therefore there are a total of six coordinate bonds into the iron centre - the<strong> coordination number is 6</strong>.</p><p>The overall charge on the complex is 3−, so the iron ion must have a charge of 3+ (6− + 3+ = 3−). Therefore the oxidation state of the iron is +3.</p><p>Therefore the correct answer is <strong>Coordination number 6 ; oxidation state +3</strong>.</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 class="page-container panel-self-assessment" data-id="2736"> <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>Periodicity AHL (HL only) paper 1 questions</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> <div class="actions mt-xs-3"> <button id="save-my-progress" type="button" class="btn btn-sm btn-primary text-center btn-xs-block"> <i class="fa fa-fw fa-floppy-o"></i> Save </button> </div> </div></div> <div id="modal-feedback" class="modal fade" tabindex="-1" role="dialog"> <div class="modal-dialog" role="document"> <div class="modal-content"> <div class="modal-header"> <h4 class="modal-title">Feedback</h4> <button type="button" class="close hidden-xs hidden-sm" data-dismiss="modal" aria-label="Close"> <span aria-hidden="true">×</span> </button> </div> <div class="modal-body"> <div class="errors"></div> <p><strong>Which of the following best describes your feedback?</strong></p> <form method="post" style="overflow: hidden"> <div class="form-group"> <div class="radio"><label style="color: #121212;"><input type="radio" name="feedback-type" value="Recommendation"> Recommend</label></div><div class="radio"><label style="color: #121212;"><input type="radio" name="feedback-type" value="Problem"> Report a problem</label></div><div class="radio"><label style="color: #121212;"><input type="radio" name="feedback-type" value="Improvement"> Suggest an improvement</label></div><div class="radio"><label style="color: #121212;"><input type="radio" name="feedback-type" value="Other"> Other</label></div> </div> <hr> <div class="row"> <div class="col-md-6"> <div class="form-group"> <label for="feedback-name">Name</label> <input type="text" class="form-control" name="feedback-name" placeholder="Name" value=" "> </div> </div> <div class="col-md-6"> <div class="form-group"> <label for="feedback-email">Email address</label> <input type="email" class="form-control" name="feedback-email" placeholder="Email" value="@airmail.cc"> </div> </div> </div> <div class="form-group"> <label for="feedback-comments">Comments</label> <textarea class="form-control" name="feedback-comments" style="resize: vertical;"></textarea> </div> <input type="hidden" name="feedback-ticket" value="082b9c9c4ae3624d"> <input type="hidden" name="feedback-url" value="https://studyib.net/chemistry/page/2736/periodicity-ahl-hl-only-paper-1-questions"> <input type="hidden" name="feedback-subject" value="7"> <input type="hidden" name="feedback-subject-name" value="Chemistry"> <div class="pull-left"> </div> </form> </div> <div class="modal-footer"> <button type="button" class="btn btn-primary btn-xs-block feedback-submit mb-xs-3 pull-right"> <i class="fa fa-send"></i> Send </button> <button type="button" class="btn btn-default btn-xs-block m-xs-0 pull-left" data-dismiss="modal"> Close </button> </div> </div> </div></div> <style type="text/css" media="screen">/* Important part */
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