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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 core (SL and HL) paper 1 questions <a href="#" class="mark-page-favorite pull-right" data-pid="2425" 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 core (SL and HL) 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 3.1 and 3.2</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="7-644-2425"><div class="label label-default q-number">1</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which oxide when added to water will give the solution with the lowest pH?</p></div><div class="q-answer"><p><label class="radio"><input type="radio"> MgO</label></p><p><label class="radio"><input type="radio"> SiO<sub>2</sub></label></p><p><label class="radio"><input class="c" type="radio"> SO<sub>3</sub></label></p><p><label class="radio"><input type="radio"> Na<sub>2</sub>O</label></p></div><div class="q-explanation"><p>This question involves knowledge of structure and bonding as well as the acidic and basic nature of oxides.</p><p>Metal oxides (MgO and Na<sub>2</sub>O), if they react with water at all, will give alkaline solutions that therefore have a pH higher than 7.</p><p>Non-metal oxides may react with water to give acidic solutions that therefore have a pH lower than 7. However, SiO<sub>2</sub> (silica) is a giant covalent structure analogous to diamond, and does not react with water (sand is impure SiO<sub>2</sub>). Sulfur trioxide, SO<sub>3</sub>, will react (very exothermically) in water to give an acidic solution of sulfuric acid (H<sub>2</sub>SO<sub>4</sub>).</p><p><strong>SO<sub>3</sub></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>What is the correct trend in melting point going down group 1 and group 17?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>Decrease down group 1 and decrease down group 17</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>Decrease down group 1 and increase down group 17</span></label> </p><p><label class="radio"> <input type="radio"> <span>Increase down group 1 and increase down group 17</span></label> </p><p><label class="radio"> <input type="radio"> <span>Increase down group 1 and decrease down group 17</span></label> </p></div><div class="q-explanation"><p>Group 1 metals have metallic bonding and therefore giant structures. Melting points are relatively low for metals as the atoms are large and form 1+ ions so the attraction between the nucleus and ‘sea of electrons’ is not as strong as in other metals. Nonetheless strong metallic bonds must be broken. The melting points (values in data book) become <strong>lower down the group</strong> because of the increasing atomic/ion size leads to less attraction..</p><p>Group 17 non-metals; the halogens, have covalent bonding and simple molecular structures. The atoms get bigger down the group, so the diatomic halogen molecules get bigger down the group. These non-polar molecules have weak London dispersion forces that must be broken. The melting points (data book) become <strong>higher down the group</strong> as London dispersion forces get stronger as the number of electrons/molar mass of a molecule increases.</p><p>Thus,<strong> Decrease down group 1 and increase down group 17 </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>In which block are the elements (atomic numbers in brackets) Nd (60), Zn (30) and Xe (54) respectively?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>d-block; p-block; s-block</span></label> </p><p><label class="radio"> <input class="c" type="radio"> f-block; d-block; p-block </label></p><p><label class="radio"> <input type="radio"> <span>d-block; d-block; p-block</span></label> </p><p><label class="radio"> <input type="radio"> <span>f-block; d-block; d-block</span></label> </p></div><div class="q-explanation">The s-block is groups 1 and 2 (I and II); the d-block is groups 3-12; and the p-block is groups 13-18 (III to VIII). The lanthanides (elements 57-71) and actinides (elements 89-103), usually placed under the d-block, make up the f-block. (La and Ac themselves are usually considered to be in the f-block.) The correct answer is therefore: <strong>'f-block; d-block; p-block'.</strong></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 the following statements is/are true with regard to metals?</p><p><strong>1: </strong>Metals tend to form acidic oxides.</p><p><strong>2: </strong>Metals tend to be good conductors of electricity</p><p><strong>3: </strong>Metals tend to have lower ionisation energies than non-metals</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>1, 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 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>Metals tend to form basic (alkaline) oxides, not acidic oxides, so statement 1 is false.</p><p>Metals' outer electrons are delocalised and they have giant structures. Metals are often:<strong> good conductors of electricity</strong> and heat; high in melting and boiling point; malleable; ductile; sonorous; lustrous (shiny). Therefore statement 2 is true.</p><p>Metals have low electronegativity and tend to lose electrons when they react. The trend in ionisation energy across a period (from metals to non-metals) is a general increase. Therefore statement 3 is true.</p><p>Thus <strong>2 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">5</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which of the equations below represents the <em>first electron affinity </em>of chlorine?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>½Cl<sub>2</sub><sub>(g)</sub> → Cl<sup>+</sup><sub>(g)</sub> + e<sup>−</sup></span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>Cl<sub>(g)</sub> + e<sup>−</sup> → Cl<sup>−</sup><sub>(g)</sub></span></label> </p><p><label class="radio"> <input type="radio"> <span>Cl<sub>(g)</sub> → Cl<sup>+</sup><sub>(g)</sub> + e<sup>−</sup></span></label> </p><p><label class="radio"> <input type="radio"> <span>½Cl<sub>2(g)</sub> + e<sup>−</sup> → Cl<sup>−</sup><sub>(g)</sub></span></label> </p></div><div class="q-explanation"><p>First electron affinity and second electron affinity are definitions that need to be learned:</p><p>First electron affinity is the enthalpy change when <strong>one electron is gained </strong>by <strong>each atom</strong> <strong>in one mole</strong> of <strong>gaseous atoms</strong>.</p><p>Second electron affinity is the enthalpy change when <strong>one electron is gained </strong>by <strong>each 1− ion</strong> <strong>in one mole</strong> of <strong>gaseous ions</strong>.</p><p>Thus <strong>Cl<sub>(g)</sub> + e<sup>−</sup> → Cl<sup>−</sup><sub>(g) </sub></strong>is the correct answer, as this is the first electron affinity of chlorine.</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 series represents atoms in order of decreasing atomic radius?</p></div><div class="q-answer"><p><label class="radio"> <input class="c" type="radio"> <span>K > Na > Al > Si</span></label> </p><p><label class="radio"> <input type="radio"> <span>Na > K > Rb > Cs</span></label> </p><p><label class="radio"> <input type="radio"> <span>Ga > Al > Mg > Na</span></label> </p><p><label class="radio"> <input type="radio"> <span>Si > Al > Mg > Na</span></label> </p></div><div class="q-explanation"><p><strong>Across any period</strong> there is a general decrease in atomic radii due to increasing nuclear charge and electrons filling the same energy level. The electrons are in the same energy level, but the nuclear charge increases (number of protons increases), increasing the attraction between the nucleus and the electrons and pulling them in more tightly/closer to the nucleus. Overall the attraction between the outer electrons and the nucleus outweighs the increasing electron-electron repulsion.</p><p><strong>Down any group </strong>there is a general increase in atomic radii due to electrons filling energy levels that are further from the nucleus making the atoms bigger, despite the increase in nuclear charge.</p><p>Thus <strong>K > Na > Al > Si </strong>is the correct answer. K is lower than sodium in group 1, so Na will have a smaller atom radius, and Al and Si are elements further across period 3 than Na, so will have decreasing atomic radii.</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>Which oxides, when added to water, will give an alkaline solution?</p><p>1: P<sub>4</sub>O<sub>10</sub></p><p>2: SO<sub>3</sub></p><p>3: CaO</p></div><div class="q-answer"><p><label class="radio"><input type="radio"> 1 and 3 only</label></p><p><label class="radio"><input type="radio"> 2 only</label></p><p><label class="radio"><input class="c" type="radio"> 3 only</label></p><p><label class="radio"><input type="radio"> 1 and 2 only</label></p></div><div class="q-explanation"><p>Metal oxides (CaO), if they react with water at all, will give alkaline solutions (this does react).</p><p>Non-metal oxides (P<sub>4</sub>O<sub>10</sub> and SO<sub>3</sub>), if they react with water at all, will give acidic solutions (both of these do react).</p><p><strong>3 only</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">8</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which statement about trends is true in both groups 2<strong> and </strong>18?</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>Boiling points decrease</span></label> </p><p><label class="radio"> <input type="radio"> <span>Melting points increase</span></label> </p><p><label class="radio"> <input class="c" type="radio"> <span>Ionisation energies decrease</span></label> </p><p><label class="radio"> <input type="radio"> <span>Electronegativities increase</span></label> </p></div><div class="q-explanation"><p>Group 2 are metals, so have metallic bonding and therefore giant structures. The melting and boiling points become <strong>lower down the group</strong> because of the increasing atomic/ion size leads to less attraction.</p><p>Group 18 are non-metals; the noble gases, and exist as atomic gases. The melting and boiling points become <strong>higher down the group</strong> as London dispersion forces get stronger as the number of electrons/molar mass of the atoms increases.</p><p>Electronegativities decrease down all groups (and increase across periods).</p><p>Ionisation energies decrease down all groups (and show a general increase across periods).</p><p>Thus<strong> Ionisation energies decrease</strong><strong> </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">9</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which trends are generally correct across period 2 (Li to Ne)?</p><p><strong>1: </strong>Atomic radius decreases</p><p><strong>2: </strong>Boiling point increases</p><p><strong>3: </strong>1st ionisation energy increases</p></div><div class="q-answer"><p><label class="radio"> <input type="radio"> <span>1 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 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>Metals and Non-metals (or metalloids) with giant structures<strong> (Li, Be, B and C) </strong>have high melting/boiling points; strong covalent or metallic bonds are broken. Non-metals with simple molecular structures (<strong>N<sub>2</sub>, O<sub>2</sub></strong>, <strong>F<sub>2</sub></strong>) or gaseous atoms (<strong>Ne</strong>) have low melting/boiling points; only intermolecular forces need to be broken. So statement 2 is false as boiling point will peak at C (in the middle) across period 2.</p><p>Across <strong>any</strong> period there is a general decrease in atomic radii due to increasing nuclear charge and electrons filling the same energy level. The electrons are in the same energy level, but the nuclear charge increases (number of protons increases), increasing the attraction between the nucleus and the electrons and pulling them in more tightly/closer to the nucleus. Overall the attraction between the outer electrons and the nucleus outweighs the increasing electron-electron repulsion. Statement 1 is correct.</p><p>Across <strong>any </strong>period there is a general increase in 1<sup>st</sup> ionization energy due to increasing nuclear charge and electrons filling the same energy level. So the outermost electron becomes subject to greater attraction and more difficult to remove. Statement 3 is correct.</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">10</div><div class="exercise shadow-bottom"><div class="q-question"><p>Which element is <strong>not</strong> a metalloid?</p></div><div class="q-answer"><p><label class="radio"><input class="c" type="radio"> P</label></p><p><label class="radio"><input type="radio"> Ge</label></p><p><label class="radio"><input type="radio"> Si</label></p><p><label class="radio" style=" float: left; margin-right: 40px; "><input type="radio"> B</label></p></div><div class="q-explanation"><p>Metalloids lay on the diagonal between metals and non-metals. Beginning with Boron each successive element on the diagonal, <strong>and the one underneath it</strong>, are considered to be metalloids, ending in Astatine (which is not considered to be a metalloid):</p><p><img alt="" src="../../images/periodicity/metalloids-pt.png" style="width: 240px; height: 207px;"></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"><p>Which correctly describes the reaction between sodium and excess water?</p></div><div class="q-answer"><p><label class="radio"><input type="radio"> The reaction is endothermic and the products are sodium oxide and hydrogen</label></p><p><label class="radio"><input type="radio"> The reaction is endothermic and the products are sodium hydroxide and hydrogen</label></p><p><label class="radio"><input class="c" type="radio"> The reaction is exothermic and the products are sodium hydroxide and hydrogen</label></p><p><label class="radio"><input type="radio"> The reaction is exothermic and the products are sodium oxide and hydrogen</label></p></div><div class="q-explanation"><p>Group 1 metals react exothermically with water to give strongly alkaline solutions of the metal hydroxide and hydrogen gas, e.g. 2Na(s) + 2H<sub>2</sub>O(l) → 2NaOH(aq) + H<sub>2</sub>(g)</p><p>Therefore '<strong>The reaction is exothermic and the products are sodium hydroxide and hydrogen</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">12</div><div class="exercise shadow-bottom"><div class="q-question"><p>What is the trend in electronegativity across period 2 and down group 17?</p></div><div class="q-answer"><p><label class="radio"><input type="radio"> Electronegativity decreases across period 2 and decreases down group 17</label></p><p><label class="radio"><input class="c" type="radio"> Electronegativity increases across period 2 and decreases down group 17</label></p><p><label class="radio"><input type="radio"> Electronegativity decreases across period 2 and increases down group 17</label></p><p><label class="radio"><input type="radio"> Electronegativity increases across period 2 and increases down group 17</label></p></div><div class="q-explanation"><p>The most electronegative element is Fluorine (4.0) and the least is Francium (0.7). Therefore, electronegativity increases across all periods and up all groups. You don't need to know the values, but you do need to know the trend.</p><p>Therefore the correct answer is '<strong>Electronegativity increases across period 2 and decreases down group 17</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="2425"> <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 core (SL and HL) 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/2425/periodicity-core-sl-and-hl-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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