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Question 1
Elements and their compounds exhibit similarities and differences based on their respective positions within the Periodic Table. |
a) | Considering only the elements in periods 1-3, name the element with the largest atomic radius.
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b) | Considering only the elements in periods 1-3, name the element with the largest ionic radius.
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c) | Considering only the elements in periods 1-3, name the element with the highest first ionisation energy.
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d) | Considering only the elements in periods 1-3, name the element with the largest electronegativity.
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e) | Describe what you would observe when magnesium is heated in steam. Write an equation for the reaction that occurs.
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f) | Describe what you would observe when silicon(IV) chloride reacts with water. Write an equation for the reaction that occurs. Suggest the pH of the resulting solution.
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Question 2
The elements in period 3, from sodium to phosphorus, can react with chlorine to form chlorides. |
a) | State and explain the changes in oxidation states which occurs when chlorine reacts with other period 3 elements.
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b) | Write an equation to show the reaction of sodium chloride when added to water.
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c) | Write an equation to show the reaction of phosphorus(V) chloride when added to water.
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d) | Complete the table to describe the structure and bonding in magnesium chloride, anhydrous aluminium chloride and phosphorus(V) chloride.
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Question 3
a) | State the meaning of the term periodicity.
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b) | Identify the element in Period 3 with the highest electronegativity value.
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c) | Identify the element in Period 3 with the largest atomic radius. Explain your answer.
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Question 4
Melting points show a trend across a period. The melting points of some period 3 elements are shown in the table below. |
a) | Explain the trend shown in melting point, in terms of structure and bonding.
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Question 5
a) | Define the term first ionisation energy.
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b) | State and explain the trend in first ionisation energy of the elements in group 2.
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c) | The first ionisation energy of aluminium is lower than that of magnesium. Give the full electronic configurations of an atom of aluminium and an atom of magnesium.
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d) | Explain the difference in the first ionisation energies of the two metals.
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Question 6
Successive ionisation energies provide evidence for the existance of different electron shells in atoms. |
a) | Write an equation to represent the third ionisation energy of nitrogen
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b) | On the axes below, add crosses to estimate the successive ionisation energies of nitrogen.
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c) | Explain why the first ionisation energy of nitrogen is higher than the first ionisation energy of carbon.
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Question 7
This question is about the periodicity of the period 3 elements. |
a) | State and explain the general trend in first ionisation energy across period 3.
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b) | Give one example of an element which deviates from the general trend in first ionisation energy across Period 3. Explain why this deviation occurs.
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c) | Identify the element in period 3 that has the highest melting point. Explain your answer in terms of structure and bonding.
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d) | Identify the metallic element in period 3 that has the highest melting point. Explain your answer in tems of structure and bonding
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Question 8
The log of the third ionisation energy for six elements is shown in the table below. |
a) | Plot a graph of these data
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b) | Use the graph in part a) to estimate the third ionisation energy for argon, in kJ mol-1. Give your answer to the nearest whole number.
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c) | Suggest why the third ionisation energy of chlorine and argon are similar in magnitude.
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Question 9
The melting points of the period 3 elements are shown in the table below. |
a) | Explain the trend in melting points across the elements of period 3 in terms of their structure and bonding.
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Question 10
This question is about some period 3 elements and their oxides. |
a) | Write an equation for the reaction of phosphorus with an excess of oxygen.
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b) | Describe a chemical test you could carry out to distinguish between phosphorus oxide and sodium oxide.
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c) | Element X forms an amphoteric oxide that has a very high melting point. Write the formula of this amphoteric oxide.
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d) | State the meaning of the term amphoteric.
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e) | Write two equations to show the amphoteric nature of aluminium oxide when it reacts with hydrochloric acid and with sodium hydroxide. State symbols are not required.
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Question 11
Period 3 oxides can exhibit acidic and/or basic properties depending on the identity of the period 3 element. |
a) | Write an equation for the reaction of sulfur trioxide with potassium hydroxide solution.
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b) | Write an equation for the reaction of an excess of magnesium oxide with phosphoric acid.
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c) | Write an equation for the reaction of sodium oxide with phosphorus(V) oxide in the absence of water.
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Question 12
Sulfur dioxide reacts with water to form a weakly acidic solution. Ions are formed when sulfur dioxide reacts with water. |
a) | Write an equation for this reaction.
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b) | Suggest why sulfur dioxide forms a weakly acidic solution. Refer to the equation in part a).
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c) | Suggest why silicon dioxide is described as an acidic oxide even though it doesn't dissolve in water.
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Question 13
a) | Explain why sodium oxide and magnesium oxide form alkaline solutions when added to water.
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b) | Give the approximate pH values of the resulting solutions formed when sodium oxide and magnesium oxide are added to water. Explain your reasoning.
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Question 14
The elements from sodium to sulur in period 3 all react with oxygen to form oxides. |
a) | Describe two observations for the reaction that takes place when sodium is heated in oxygen. Write an equation for this reaction.
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b) | Describe two observations for the reaction that takes place when phosphorus is heated in oxygen. Write an equation for this reaction.
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c) | Describe two observations for the reaction that takes place when magneisum is heated in steam. Write an equation for this reaction.
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Question 15
The question is about the elements of period 3 from sodium to phosphorus. |
Element X forms an oxide that has a very high melting point. This oxide reacts very slowly with water to form a weakly alkaline solution. Deduce the type of bonding in this oxide of X. |
a) | Identify element X.
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b) | Write a balanced symbol equation for the reaction between element X and hydrochloric acid.
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c) | Element Y forms an oxide that has a low melting point. This oxide dissolves in water to form an acidic solution. Deduce the type of bonding in this oxide of Y. Identify element Y.
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d) | Write an equation for the reaction between this oxide of Y and water.
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e) | Element Z forms an oxide that is insoluble in water. This oxide reacts with hydrochloric acid and with aqueous sodium hydroxide. Identify element Z. Give the formula for this oxide.
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f) | Give an equation for the reaction of this oxide with hydrochloric acid.
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| 1 | 2 | 3 | 4 | 5 | 6 |
| 7 | 8 | 9 | 10 | 11 | 12 |
| 13 | 14 | 15 |