This question is about the reaction between sodium and water.
Which statement about this reaction is correct?
| ☐ | A | Sodium sinks to the bottom of the water | |
| ☐ | B | A lilac flame is seen | |
| ☐ | C | A solution of sodium oxide is produced | |
| ☐ | D | Bubbles of hydrogen gas are produced |
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Which of the following could not be predicted about caesium, based on the trends seen in Group 1 metals?
| ☐ | A | It is soft | |
| ☐ | B | It has a relatively high melting point | |
| ☐ | C | It is very reactive | |
| ☐ | D | It has a relatively low density |
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A teacher adds a small piece of potassium to a large trough of water to form a solution.
When the reaction has completed she adds a few drops of universal indicator to the solution.
What is the most likely pH value of the solution?
| ☐ | A | 3 | |
| ☐ | B | 7 | |
| ☐ | C | 8 | |
| ☐ | D | 12 |
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Sodium and rubidium have similar chemical properties because their atoms
| ☐ | A | Form positive ions | |
| ☐ | B | Have the same number of electrons in their outer shell | |
| ☐ | C | Have the same electronic configuration | |
| ☐ | D | Readily gain electrons |
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This question is about some of the Group 1 alkali metals and their reactions.
| ☐ | A | Li (s) + H2O (g) → LiOH (aq) + H2 (g) | |
| ☐ | B | Li (s) + H2O (l) → LiOH (aq) + H2 (g) | |
| ☐ | C | 2Li (s) + 2H2O (l) → 2LiOH (aq) + H2 (g) | |
| ☐ | D | 2Li (s) + 2H2O (g) → 2LiOH (aq) + H2 (g) |
Place the following Group 1 metals in order from least to most reactive.
| least reactive | most reactive | |||||
| _______________ | → | _______________ | → | _______________ | → | _______________ |
.
Explain why francium is more reactive than rubidium.
Use the words in the boxes to complete the sentences. Each word may be used once, more than once or not at all.
| greater | electrostatic | weaker |
| stronger | less | thermal |
The distance between the outermost electron of francium and its nucleus is __________ than that of rubidium.
This means that the forces of attraction in francium are __________ .
Therefore, __________ energy is required to overcome the forces of attraction in francium.
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This question is about the elements in Group 1 of the Periodic Table and their reactions with water.
State why sodium and potassium are in Group 1 of the Periodic Table.
A reaction occurs when a small piece of sodium is added to a large volume of water in a trough.
| ☐ | A | 2 | |
| ☐ | B | 5 | |
| ☐ | C | 8 | |
| ☐ | D | 12 |
(1)
Give the name of a Group 1 metal that is less reactive than sodium.
A small piece of potassium is added to a large volume of water in a trough.
Give one observation that is made when potassium is added to water that is not made when sodium is added to water.
Complete the equation for the reaction of rubidium with water. State symbols are not required.
........Rb + ........H2O → ........RbOH + .........H2
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This question is about some of the Group 1 elements and their compounds.
A teacher adds a small piece of lithium to water in a trough.
A student does a flame test to see if a white solid contains sodium ions.
She cleans a platinum wire before using it for the flame test.
| ☐ | A | green | |
| ☐ | B | lilac | |
| ☐ | C | red | |
| ☐ | D | yellow |
Potassium sulfate (K2SO4) is an ionic compound.
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When lithium, a Group 1 metal, reacts with water, two products are formed.
Which is the correct balanced symbol equation, including state symbols, that represents this reaction?
| ☐ | A | Li (s) + 2H2O (l) → Li(OH)2 (l) + H2 (g) | |
| ☐ | B | 2Li (s) + 2H2O (l) → 2LiOH (aq) + H2 (g) | |
| ☐ | C | 2Li (s) + H2O (l) → Li2O (aq) + H2 (g) | |
| ☐ | D | 2Li (s) + 2H2O (l) → 2LiOH (l) + O2 (g) |
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This question is about some elements in Group 1 of the Periodic Table.
The table gives some statements about the reaction of potassium with water.
Place ticks (✔) in three boxes to show which three statements are correct.
| Statement | |
| potassium reacts more vigorously than sodium when added to water | |
| potassium sinks to the bottom of the water | |
| bubbles of oxygen gas are produced | |
| a lilac flame is seen | |
| potassium moves around | |
| a solution of potassium oxide is formed |
After the reaction of potassium with water is complete, a few drops of universal indicator are added to the solution formed. The universal indicator turns purple.
(1)
(1)
Sodium burns in oxygen to produce sodium oxide.
Complete the equation for this reaction.
..........Na + ..........O2 → ..........Na2O
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The position of an element in the Periodic Table can be used to predict its properties.
Which of the following statements could not be predicted using the trends in Group 1?
| ☐ | A | Rubidium has a lower melting point than lithium | |
| ☐ | B | Lithium is softer than potassium | |
| ☐ | C | Sodium will tarnish more quickly than lithium | |
| ☐ | D | Caesium is more reactive than potassium |
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This question is about sodium and potassium.
A trough is filled with water and a few drops of phenolphthalein indicator are added.
A small piece of sodium is dropped into the water. One of the products of the reaction is an alkali.
(2)
___Na (.......) + ___H2O (l) → ___NaOH (........) + H2 (g)
(1)
Explain why potassium is more reactive than sodium.
Refer to the electronic configurations of the atoms in your answer.
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This question is about some of the alkali metals and their compounds.
When a teacher drops a small piece of sodium into a trough of cold water, she observes bubbles of gas.
Give two other observations that would be made when sodium reacts with cold water.
Lithium reacts with fluorine to form the compound lithium fluoride.
(3)
|
Lithium ion
|
Fluoride ion
|
The table shows the electronic configurations of sodium and potassium.
| Element | Electronic configurations |
| sodium | 2.8.1 |
| potassium | 2.8.8.1 |
Explain, in terms of their electronic configurations, why potassium is more reactive than sodium.
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Lithium, sodium and potassium are the first three elements in Group 1 of the Periodic Table.
Suggest why these three elements are all stored in paraffin oil.
Caesium, Cs, is below potassium in Group 1.
A student investigates the temperature change in the reaction between dilute acids and solutions of Group 1 hydroxides.
He uses this apparatus.
This is the student’s method:
5 marksThese are the student’s results:
Temperature of hydrochloric acid = 19.9 °C
Maximum temperature of mixture = 26.5 °C
i)
Calculate the molar enthalpy change, ΔH, in kJ / mol for this reaction.
ΔH = .............................................. kJ / mol
(2)
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This question is about the reactions of Group 1 metals with water.
A teacher adds a piece of sodium to some water containing universal indicator.
The equation for this reaction is:
2Na (s) + 2H2O (l) → 2NaOH (aq) + H2 (g)
The sodium floats on the surface of the water and the universal indicator changes colour because an alkaline solution is formed.
The diagram represents an atom of lithium and an atom of sodium.
 |
 |
| lithium | sodium |
4 marks
The equation for the reaction is
2Li (s) + 2H2O (l) → 2LiOH (aq) + H2 (g)
The teacher collects 254 cm3 of hydrogen gas at room temperature and pressure (rtp).
Show by calculation that 1 mol of hydrogen gas has a volume of approximately 24000 cm3 at rtp.
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This question is about Group 1 metals and their reactions.
When lithium is added to water, bubbles of hydrogen gas are observed.
6 marks
The equation for the reaction between lithium and water is:
2Li (s) + 2H2O (l) → 2LiOH (aq) + H2 (g)
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This question is about some of the alkali metals and their compounds.
When a teacher drops a small piece of potassium into a trough of cold water, they observe bubbles of gas.
Give two other observations that would be made when potassium reacts with cold water.
When the reaction between potassium and cold water is complete, the teacher adds some universal indicator to the trough.
Explain the final colour of the universal indicator.
Suggest why the teacher does not repeat the experiment using hydrochloric acid instead of cold water.
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This question is about some Group 1 metal oxides.
When lithium is exposed to oxygen, it is oxidised and traces of lithium peroxides are produced.
Lithium oxide can also be produced by heating lithium hydroxide.
2LiOH → Li2O + H2O
State the type of reaction that occurs during this process.
The oxidation of potassium can produce potassium oxide, K2O, and potassium superoxide, KO2.
Compare the oxidation of potassium with the combustion of carbon.
4 marksPotassium superoxide is sometimes used as a water dehumidifier, carbon dioxide scrubber and oxygen generator on board space craft and submarines.
As it absorbs and reacts with carbon dioxide, it locks the carbon dioxide up as potassium carbonate and releases oxygen.
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