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Chemistry Y10 > Alkali Metals 2 > Flashcards

Alkali Metals 2 Flashcards

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1
Q

<p>Group 1 of the Periodic Table contains ..........</p>

A

<p>Lithium (Li)</p>

<p>Sodium (Na)</p>

<p>Potassium (K)</p>

<p>Rubidium (Rb)</p>

<p>Caesium (Cs)</p>

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2
Q

<p>Why do you think that the Group 1 metals are stored under oil?</p>

<p>A) To keep them moist and ready to react in experiments</p>

<p>B) To keep them out of contact with oxygen in the air</p>

<p>C) To lubricate the surface of the metal</p>

A

<p><strong>B</strong></p>

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3
Q

<p></p>

<p>The table below shows that Group 1 elements have low melting points for metals:<br></br><br></br></p>

<p>Group 1 metalMelting point (°C)</p>

<p>Lithium 180</p>

<p>Sodium 98</p>

<p>Potassium 63</p>

<p>Rubidium 39</p>

<p></p>

<p>Look at the table above. Which statement below is true?</p>

<p>A) There is no pattern in the melting points of the Group 1 metals as we go down the group.</p>

<p>B) The melting points of the Group 1 metals decrease as we go down the group.</p>

<p>C) The melting points of the Group 1 metals increase as we go down the group.</p>

A

<p><strong>B</strong></p>

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4
Q

<p>Predict the approximate melting point of caesium, theelementbelow rubidium in Group 1.</p>

<p>Between 40 °C and 50 °C</p>

<p>Between 20 °C and 30 °C</p>

<p>Between 60 °C and 70 °C</p>

A

<p>B</p>

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5
Q

<p>Which Group 1 metal is most difficult to cut with a knife and has the highest melting point?</p>

<p>Sodium</p>

<p>Lithium</p>

<p>Potassium</p>

<p>Rubidium</p>

<p>Caesium</p>

A

<p>Lithium</p>

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6
Q

<p>Liquid sodium is piped around some nuclear power stations to transfer heat. Which two properties of sodium make it suitable for this use?</p>

A

<p>It has a low melting point.</p>

<p>It is a good conductor of heat.</p>

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7
Q

<p>Group 1 metals are called thealkali metals. why?</p>

A

<p>They get their name from their reaction with water, which produces an alkaline solution</p>

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8
Q

<p>Which of the alkali metals shown below melts into a silver ball that moves around the surface of the water as it reacts?</p>

<p>Potassium</p>

<p>Sodium</p>

<p>Lithium</p>

A

<p>Sodium</p>

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9
Q

<p>You can collect the gas given off as lithium reacts with water. Which test shows that the gas collected is hydrogen?</p>

<p>A glowing splint re-lights</p>

<p>A lighted splint explodes with a squeaky 'pop'</p>

<p>Limewater turns milky</p>

A

<p>A lighted splint explodes with a squeaky 'pop'</p>

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10
Q

<p>What is thepH valueof the solution produced when the Group 1 metals react with water?</p>

<p>7</p>

<p>Greater than 7</p>

<p>Less than 7</p>

A

<p>Greater than 7</p>

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11
Q

<p>Which of the three metals is most reactive with water?</p>

<p>Lithium</p>

<p>Potassium</p>

<p>Sodium</p>

A

<p>Potassium</p>

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12
Q

<p>Caesium explodes when put into water, smashing the glass trough. Which statement do you think describes the pattern in reactivity as we go down Group 1?</p>

<p>The Group 1 metals get less reactive as we go down the group.</p>

<p>The Group 1 metals get more reactive as we go down the group.</p>

<p>There is no pattern in their reactivity.</p>

A

<p>The Group 1 metals get more reactive as we go down the group.</p>

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13
Q

<p>What is the equations ofthe reaction between rubidium and water?</p>

<p></p>

A

<p>2 Rb(s)+2 H2O(l)2 RbOH(aq)+H2(g)</p>

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14
Q

<p>What is the equation of the reaction lithiumand water?</p>

A

<p>lithium+waterlithium hydroxide+hydrogen<br></br>2 Li(s)+2 H2O(l)2 LiOH(aq)+H2(g)</p>

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15
Q

<p>What is the equation of the reaction sodium and water?</p>

A

<p>sodium+watersodium hydroxide+hydrogen<br></br>2 Na(s)+2 H2O(l)2 NaOH(aq)+H2(g)</p>

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16
Q

<p>What is the equation of the reaction potassiumand water?</p>

A

<p><br></br>potassium+waterpotassium hydroxide+hydrogen<br></br>2 K(s)+2 H2O(l)2 KOH(aq)+H2(g)</p>

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17
Q

<p>Which of the equations below show possible reactions of lithium?</p>

<p>A) 4 Li(s)+O2(g)2 Li2O(s)</p>

<p>B) Li(s)+Cl2(g)2 LiCl2(s)</p>

<p>C) 2 Li(s)+Cl2(g)2 LiCl(s) </p>

<p>D) Li(s)+O2(g)LiO2(s)</p>

A

<p>A & C</p>

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18
Q

<p>Write the equation showing the formation of potassium oxide is:<br></br><br></br></p>

A

<p>potassium+oxygenpotassium oxide<br></br>4 K(s)+O2(g)2 K2O(s)</p>

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19
Q

<p>The alkali metals react vigorously when heated with chlorine gas. Give an example:<br></br><br></br></p>

A

<p>sodium+chlorinesodium chloride<br></br>2 Na(s)+Cl2(g)2 NaCl(s)</p>

<p></p>

<p>potassium+chlorinepotassium chloride<br></br>2 K(s)+Cl2(g)2 KCl(s)</p>

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20
Q

<p>Summary</p>

A

<p>Group 1 elements are called the alkali metals.<br></br><br></br>They are soft metals that tarnish quickly in air.<br></br><br></br>The Group 1 metals get more reactive as we go down the group.<br></br><br></br>Their melting points decrease as we go down the group. The melting points are all low for metals, as are the densities of these elements.<br></br><br></br>The alkali metals are the most reactive group of metals in the Periodic Table. They form soluble compounds that are usually white.<br></br><br></br>They react vigorously with water, giving off hydrogen gas and producing an alkaline solution.<br></br><br></br>Because they are very reactive, they are stored under oil.</p>

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21
Q

<p>Name the product of the reaction between potassium and chlorine.</p>

<p>Potassium chloride</p>

<p>Potassium oxide</p>

<p>Potassium chlorate</p>

<p></p>

A

<p>Potassium chloride</p>

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22
Q

<p>Predict the colour of the product in the previous question.</p>

A

<p>White</p>

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23
Q

<p>Caesium+water…</p>

A

<p></p>

<p>caesium hydroxide+hydrogen</p>

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24
Q

<p>As theatomic numberof an alkali metal increases, its reactivity …</p>

A

<p>increases</p>

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25
Q

<p>Which gas is given off when an alkali metal reacts with water?</p>

A

<p>hydrogen</p>

26
Q

<p>Which of these alkali metals is easiest to cut with a knife?</p>

<p>Lithium</p>

<p>Sodium</p>

<p>Potassium</p>

A

<p>Potassium</p>

27
Q

<p>Which of the alkali metals has the highest melting point?</p>

<p>Lithium</p>

<p>Sodium</p>

<p>Potassium</p>

<p>Rubidium</p>

<p>Caesium</p>

A

<p>Lithium</p>

28
Q

<p>what is the electronic structure for the below atoms</p>

<p>Sodium </p>

<p>Potassium </p>

<p>Lithium </p>

A

<p>Sodium 2,8,1 </p>

<p>Potassium 2,8,8,1 </p>

<p>Lithium 2,1</p>

29
Q

<p>How many electrons are in the highest energy level (outer shell) of all the Group 1 metals?</p>

A

<p>1</p>

30
Q

<p>What is the charge on theionformed when an atom of an alkali metal reacts?</p>

A

<p>+1</p>

31
Q

<p>Which of these would make it easier for an atom to lose an electron?</p>

<p>The electron being nearer to the positively charged nucleus</p>

<p>The electron being further from the positively charged nucleus</p>

A

<p>The electron being further from the positively charged nucleus</p>

32
Q

<p>Why do the alkali metals get more reactive as we go down the group?</p>

A

<p>Because</p>

<p><br></br>This is because as we go down the group the outer electron of the atom is further from the attractive force of the nucleus. It is also shielded from the nucleus by more complete lower energy levels (full inner shells) of electrons.</p>

<p>If an electron is further from the attractive force of the nucleus, it is easier to remove it from the atom so it becomes more reactive</p>

33
Q

<p>Why the alkali metals are the most reactive group of metals in the Periodic Table?</p>

A

<p>the <strong>atoms </strong>of alkali metals all have just <strong>one</strong> electron in their highest energy level (outer shell) and It is relatively easy to lose this one electron</p>

<p>losing this outer electron, they form stable ions with a 1+ charge, e.g. Na+.</p>

34
Q

<p>As we go down Group 1,</p>

<p></p>

<p>The outer electron is more tightly held by the nucleus in larger atoms. <strong>True/False</strong></p>

<p>The outer electron is further from the attractive force of the nucleus in larger atoms. </p>

<p><strong>True/False</strong></p>

<p>The outer electron is shielded from the attractive force of the nucleus by more inner shells of electrons. <strong>True/False</strong></p>

<p>The outer electron in larger atoms is more strongly attracted by neighbouring atoms.</p>

<p><strong>True/False</strong></p>

A

<p>The outer electron is more tightly held by the nucleus in larger atoms. <strong>False</strong></p>

<p>The outer electron is further from the attractive force of the nucleus in larger atoms. </p>

<p><strong>True</strong></p>

<p>The outer electron is shielded from the attractive force of the nucleus by more inner shells of electrons. <strong>True</strong></p>

<p>The outer electron in larger atoms is more strongly attracted by neighbouring atoms.</p>

<p><strong>False</strong></p>

35
Q

<p>Are these statements true or false?</p>

<p>•Metals are on the right of the periodic table.</p>

<p>•Metal hydroxide is made when metals react with air.</p>

<p>•Group 1 metals are kept under oil.</p>

<p>•Hydrogen is produced when group 1 metals react with water.</p>

<p>•Hydrogen is tested with limewater.</p>

<p>•Lithium is the most reactive group 1 metal.</p>

A

<p>•Metals are on the right of the periodic table.<strong> (F)</strong></p>

<p>•Metal hydroxide is made when metals react with air. <strong>(F)</strong></p>

<p>•Group 1 metals are kept under oil. <strong>(T)</strong></p>

<p>•Hydrogen is produced when group 1 metals react with water. <strong>(T)</strong></p>

<p>•Hydrogen is tested with limewater. <strong>(F)</strong></p>

<p>•Lithium is the most reactive group 1 metal. <strong>(F)</strong></p>

36
Q

<p>•Name two group 1 metals</p>

<p>•Describe the trend in reactivity down period 1</p>

<p>•Explain the trend in reactivity down group 1</p>

<p>•Explain why group 1 metals are called the alkali metals</p>

<p>•What gas is produced when the group 1 metals react with water- how can we test for the presence of this gas?</p>

A

<p>•Name two group 1 metals</p>

<p><u><strong>Lithium and sodium</strong></u></p>

<p>•Describe the trend in reactivity down period 1</p>

<p><strong><u>they get more reactive as we go down the group and the reactions occur more rapidly</u></strong></p>

<p>•Explain the trend in reactivity down group 1</p>

<p><strong><u>As we move down the group the atoms have more shells of electrons and the atom gets bigger. and as the atom gets bigger the outer electrome is further from the nucleus so it is less strongly attached by the nucleus , and therefore it is more easily lost.</u></strong></p>

<p>•Explain why group 1 metals are called the alkali metals</p>

<p><strong><u>Because they react with water forming a metal hydroxide which is alkaline. PH above 7 (universal indicator is blue) (OH- ion)</u></strong></p>

<p>•What gas is produced when the group 1 metals react with water- how can we test for the presence of this gas?</p>

<p>Hydrogen which burns with a lilac flame.</p>

37
Q

<p></p>

<p>Alkali metals react with oxygen to form</p>

A

<p>metal oxides</p>

38
Q

<p>Alkali metals react with halogens to form</p>

A

<p>IONIC SALTS</p>

39
Q

<p>The alkali metals react with water to form</p>

A

<p>METAL HYDROXIDES</p>

40
Q

<p>The melting and the boiling point of halogens become ................... as we go down the group, and the molecules become ...........</p>

A

<p>increase, bigger</p>

41
Q

<p>Why Lithium, Sodium and Pottasium float on water?</p>

A

<p>Becasue they are less dense than water</p>

42
Q

<p>Chemical properties of group 1</p>

A

<ol> <li>they all react with water in the same way to form a hydroxide with the formula MOH</li> <li>they all react with oxygen to form oxide with the formula M2O</li> <li>they all react with halogens to form compunds with the formula MX</li> <li>they form ionic compunds which contain an M+ ion.</li></ol>

<p></p>

43
Q

<p>Physical properties of group 1</p>

<p>Li/Na/K/Rb/Cs/Fr</p>

<p>as we go down the group the</p>

<p>meting point ( increases/ decreases)</p>

<p>boiling point ( increases / decreases)</p>

<p>denisty g/cm3 ( increases/ decreases)</p>

<p>softness (increases / decreases)</p>

<p></p>

A

<p>meting point ( increases/ <u><strong>decreases</strong></u>)</p>

<p>boiling point ( increases / <u><strong>decreases</strong></u>)</p>

<p>denisty g/cm3 ( <u><strong>increases</strong></u>/ decreases)</p>

44
Q

<p>Physical properties of elements in group 1</p>

A

<ol> <li>melting points are very low</li> <li>densities is low</li> <li>very soft and easily cut with knife</li> <li>shiny and silver whne freshly cut but tarnish very quickly on exposure to air.</li></ol>

45
Q

<p>chemical properties depend on............</p>

<p>chemical properties of group 1 elements as we go down the group</p>

A

<p>the number of electrones in the outer shell</p>

<p>more reactive with water</p>

<p>more reactive with air tarnishes quickly</p>

<p>more reactive with halogens</p>

<p></p>

46
Q

<p>Write the equation of sodium reaction with water <strong>with state symbol</strong></p>

<p></p>

A

<p>2Na(s) + 2H2O(l) --> 2NAOH(aq) + H2(g)</p>

<p>Sodium is usually used ad molten sodium but to avoid confusion we write state symbol as (s)</p>

<p></p>

47
Q

<p>what is your observation for the sodium water reaction?</p>

A

<ol> <li>the sodium floats because it is less dense than water</li> <li>the sodium melts into a ball because its melting point is low and a lot of heat is produced by the reaction (exothermic)</li> <li>there is fizzing because hydrogen gas is produced.</li> <li>the sodium moves around on the surface of the water because the hydrogen isn't given off symmetrically around the ball, the sodium is pushed around the surface of the water by the hydrogen.</li> <li>the piece of sodium gets smaller an eventually disappears ( used up)</li> <li>test using universal indicator gives blue.</li></ol>

48
Q

<p>lithium reaction with water compared to sodium reaction with water</p>

<p>It is very similar except that it is (<strong>slower / faster)</strong></p>

<p><strong>lithium ( melts/ doesn't melt)?</strong></p>

A

<p>It is very similar except that it is <u><strong>slower</strong></u></p>

<p><strong>lithium ( melts/ <u>doesn't melt)</u></strong></p>

49
Q

<p>when lithium reacts with water it doesn't melt. explain why?</p>

A

<p>because the melting point of lithium is higher and the heat isn't produced so quickly so the lithium doesn't melt.</p>

50
Q

<p>lithium reaction with water is slower than sodium reaction with water</p>

<p>how can you observe this in the experiment?</p>

A

<p>lithium reaction</p>

<p>fizzes more slowly</p>

<p>lithium moves around the surface of water more slowly.</p>

<p>lithium takes longer to disappear.</p>

<p></p>

51
Q

<p>compare potasium reaction with water and sodium reactions with water</p>

A

<p>Potassium</p>

<p>fizzes more vigorously</p>

<p>moves around more quickly</p>

<p>disappears more quickly</p>

<p>disappears more quickly</p>

<p><strong><u>Key difference : with potassium the hydrogen bursts into flame but in sodium does not</u></strong></p>

52
Q

<ul> <li>compare rabidium and caesium reaction with water and sodium reaciton with water</li> <li>what is your predection about francium?</li></ul>

A

<p>rabidium and caesium reaction can be explosive.</p>

<p>Francium is even more explosive</p>

<p></p>

53
Q

<p><u><strong>VERY IMPORTANT</strong></u></p>

<p>write the water half equation when group 1 metal reacts with water. producing a hydroxide.</p>

<p></p>

<p>write the half equation when group1 metal reacts with water forming metal ions in solution( example sodium)</p>

<p></p>

<p></p>

A

<p>2H2O(l) + 2e- ---> 2OH-(aq) + H2(g)</p>

<p>Na(s) ---> Na+(aq) + e-</p>

54
Q

<p>burning group 1 metals in the qir we get vigorous reaction , state the different flame colours of burning</p>

<p>lithium</p>

<p>sodium</p>

<p>potassium</p>

A

<p>lithium : red flame to form lithium oxide</p>

<p>sodium : yellow flame to form sodium oxide</p>

<p>potassium : lilac flame to form potassium oxide</p>

<p></p>

55
Q

<p>when burning lithium , sodium and pottasium</p>

<p>what is the desctiption of the product formed?</p>

<p>what is the equation?</p>

<p>what other types of oxides can be formed?</p>

A

<p>It is a white powder in solid state, it isthe alkali metal oxide.</p>

<p>they all have the same equation</p>

<p>4M(s) + O2(g) ----> 2M2O(S)</p>

<p>other types of oxides</p>

<p>peroxides (M2O2)</p>

<p>and superoxides (MO2)</p>

<p>lithium can also form a nitride (Li3N)</p>

56
Q

<p>Explain why lithium , sodium and potassium are put in the same group in the periodic table?</p>

<p>VERY IMPORTANT</p>

A

<p>They all have one electrone in their outer shell . the elctronic configurations are:</p>

<p>lithium : 2,1</p>

<p>Sodium, 2,8,1</p>

<p>Potassium 2,8,8,1</p>

<p>also they have similar chemical properties such as</p>

<ol> <li>they react with water in the same way to form hydroxide with the formula MOH</li> <li>they react with oxygen to form oxide with the formula M2O</li> <li>they react with halogens to form compunds with formula MX</li> <li>they form ionic compunds which contain an M+ ion.</li> <li></li></ol>

57
Q

<p>summary of groups 1 main features</p>

A

<ol> <li>are metals</li> <li>are soft with melting point and densities which are very low for metal.</li> <li>have to be stored out of contact with air or water</li> <li>react rapidly with air to form coatings of the metal oxide</li> <li>react with water to produce alkaline solution of the metal hydroxide and hydrogen gas</li> <li>increase in reactivity as you do down the group</li> <li>form compunds in which the metal has a 1+ ion</li> <li>have mainly white colourless coumpunds which dissolve to produce colourless solutions.</li></ol>

<p></p>

58
Q

<p>find the names of the below letters</p>

<p><strong>B</strong> is a metal when dropped onto water it melts into a small ball and moves rapidly around the surface , a gas <strong>C</strong> is given off and this burns with a lilac flame a solution <strong>D</strong> is formed</p>

<p>write the reaction equation with state symbol</p>

A

<p>B = Potassium</p>

<p>C = hydrogen</p>

<p>D = Potassium hydroxide KOH</p>

<p></p>

<p>2K(s) + 2H2O(l) ---> 2KOH(aq) + H2(g)</p>

59
Q

<p>Explain why all metals in group 1 they react the same with water?</p>

A

<p>chemical properties depend on the number of electrons in the outer shell, and since they all have the same number of electrone in the outer shell (one) so they all have similar chemical properties and react the same with water.</p>

<p></p>

60
Q

<p>All metals in group 1 they react the same way with water</p>

<p>write the equation</p>

<p>write the equation for <u><strong>fracium</strong></u></p>

A

<p>2M+ 2H2O----> 2MOH+ H2</p>

<p></p>

<p>2Fr(s)+ 2H2O(l) ----> 2FrOH(aq)+ H2(g)</p>

61
Q

<p>predict the features of facium (Fr)</p>

A

<p>very soft</p>

<p>melting point is around the room temperature</p>

<p>has density over 2g/CM3</p>

<p>silvery metal tarnish instantly when cut</p>

<p>react with water violently forming fracium hydroxide and hydrogen</p>

<p>the solution FrOH is strongly alkaline</p>

<p>will form compounds that are white / clourless and dissolve in water giving a colourless solution.</p>

62
Q

<p>Congratulations you discovered a new alkali metal named Ed</p>

<p>is it more or less dense than fracium?</p>

<p>is the melting point higher or lower than fracium?</p>

<p>how many electrons does it have?</p>

<p>what is the equation to react with water?</p>

<p>is the solution acidic or akaline?</p>

<p>what is the equation to react with oxygen?</p>

<p>what is the equation to react with Cl</p>

<p>is it more or less reactive than fracium?</p>

<p></p>

A

<p>GUESS</p>

Chemistry Y10 (5 decks)

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