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AQA GCSE Chemistry for Combined Sciences: Trilogy Oxford University Press Help C2 The periodic table Summary questions 1 a Where in the periodic table do you find: I the halogens + II the noble gases [1 mark] iii the alkali metals [1 mark] [1 mark] b In which groups would you find the three elements described below? I This is a metal that can be cut with a knife and is stored under oil. It reacts violently with water and forms ions with a 1+ charge. [I mark] It This is a very unreactive, monatomic gas. (f mark] iii This toxic gas is the most reactive of the all the non-metallic elements. It forms ions with a 1- charge and will also form covalent compounds. [t mark] 2 Astatine, At, is a halogen whose atomic number is 85. It lies at the bottom of Group 7, beneath lodine a How many electrons occupy its outermost shell (highest energy level)? Explain how you worked out your answer. [I mark] b Predict the state of astatine at 20°C [1 mark] c For the compound sodium astatide, predict: I its type of bonding [1 mark] ii its colour [1 mark] iii its chemical formula [1 mark] iv the word equation and the balanced symbol equation for its formation from its elements [2 marks] v whether or not you would see signs of a reaction if a solution of sodium astatide was mixed with chlorine water. Explain how you arrived at your answer. [2 marks] d Place the halogens, including astatine, in order of reactivity, with the most reactive element first. Explain your answer in detail (include the trend in reactivity and the how the trend can be explained, referring to the formation of halide ions). [6 marks] 3 Rubidium, Rb, is in Group 1 of the periodic table, lying directly beneath potassium. a Predict the following physical properties of rubidium, including its hardness, electrical conductivity, and melting point. [3 marks] b i What will be the charge on a rubidium ion? [1 mark] in Copy and complete the table below: Rubidium compound Chemical formula rubidum iodide rubidum fluoride rubidium lydroside Rubidium compound Chemical formula rubidum iodide rubidum fluoride rubidium lydroside [3 marks] c. Write down word equations and balanced symbol equations, including state symbols, for the following reactions: I rubidium and water [3 marks] it rubidium and chlorine. [2 marks] d Will the reactions of rubidium in part c be more or less vigorous than the same reactions using potassium? Explain your answer in detail by comparing the atoms of the two elements. [5 marks] 4 Group 0 is found as the last column in the periodic table, on the extreme right hand side. a Write the name and symbol of the first four elements in Group 0. [2 marks] b What is the name commonly given to the elements in Group 0? [t mark] c Explain which of the first four noble gases is the odd one out in terms of the number of electrons in its outermost shell. [3 marks] d Describe how the electronic structures of the Group 0 elements affects their chemistry. [1 mark] The Group 0 elements are found in trace amounts in the air. If air is gradually cooled down to extremely low temperatures, predict which of the first four elements would condense as a liquid first. Give a reason for your answer. [2 mark] 5 a Explain how Dmitri Mendeleev used atomic weights to construct his periodic table. [2 marks] b Explain how the scientific community were influenced to accept his periodic table. [6 marks] c Why, in 1869, could scientists not explain why some pairs of elements in his periodic table appeared to be in the wrong order according to their atomic weights? [3 marks] 6 a Explain how the atoms of metals and non-metals change when they react to form their ions, using magnesium as an example of a metallic element and oxygen as an example of a non-metallic element. [6 marks] b Suggest how the radius of a metal ion compares with the radius of the metal atom it was made from. Give a reason for your suggestion. [2 marks] 32

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AQA GCSE Chemistry for Combined Sciences: Trilogy Oxford University Press Help C2 The periodic table Summary questions 1 a Where in the periodic table do you find: I the halogens + II the noble gases [1 mark] iii the alkali metals [1 mark] [1 mark] b In which groups would you find the three elements described below? I This is a metal that can be cut with a knife and is stored under oil. It reacts violently with water and forms ions with a 1+ charge. [I mark] It This is a very unreactive, monatomic gas. (f mark] iii This toxic gas is the most reactive of the all the non-metallic elements. It forms ions with a 1- charge and will also form covalent compounds. [t mark] 2 Astatine, At, is a halogen whose atomic number is 85. It lies at the bottom of Group 7, beneath lodine a How many electrons occupy its outermost shell (highest energy level)? Explain how you worked out your answer. [I mark] b Predict the state of astatine at 20°C [1 mark] c For the compound sodium astatide, predict: I its type of bonding [1 mark] ii its colour [1 mark] iii its chemical formula [1 mark] iv the word equation and the balanced symbol equation for its formation from its elements [2 marks] v whether or not you would see signs of a reaction if a solution of sodium astatide was mixed with chlorine water. Explain how you arrived at your answer. [2 marks] d Place the halogens, including astatine, in order of reactivity, with the most reactive element first. Explain your answer in detail (include the trend in reactivity and the how the trend can be explained, referring to the formation of halide ions). [6 marks] 3 Rubidium, Rb, is in Group 1 of the periodic table, lying directly beneath potassium. a Predict the following physical properties of rubidium, including its hardness, electrical conductivity, and melting point. [3 marks] b i What will be the charge on a rubidium ion? [1 mark] in Copy and complete the table below: Rubidium compound Chemical formula rubidum iodide rubidum fluoride rubidium lydroside Rubidium compound Chemical formula rubidum iodide rubidum fluoride rubidium lydroside [3 marks] c. Write down word equations and balanced symbol equations, including state symbols, for the following reactions: I rubidium and water [3 marks] it rubidium and chlorine. [2 marks] d Will the reactions of rubidium in part c be more or less vigorous than the same reactions using potassium? Explain your answer in detail by comparing the atoms of the two elements. [5 marks] 4 Group 0 is found as the last column in the periodic table, on the extreme right hand side. a Write the name and symbol of the first four elements in Group 0. [2 marks] b What is the name commonly given to the elements in Group 0? [t mark] c Explain which of the first four noble gases is the odd one out in terms of the number of electrons in its outermost shell. [3 marks] d Describe how the electronic structures of the Group 0 elements affects their chemistry. [1 mark] The Group 0 elements are found in trace amounts in the air. If air is gradually cooled down to extremely low temperatures, predict which of the first four elements would condense as a liquid first. Give a reason for your answer. [2 mark] 5 a Explain how Dmitri Mendeleev used atomic weights to construct his periodic table. [2 marks] b Explain how the scientific community were influenced to accept his periodic table. [6 marks] c Why, in 1869, could scientists not explain why some pairs of elements in his periodic table appeared to be in the wrong order according to their atomic weights? [3 marks] 6 a Explain how the atoms of metals and non-metals change when they react to form their ions, using magnesium as an example of a metallic element and oxygen as an example of a non-metallic element. [6 marks] b Suggest how the radius of a metal ion compares with the radius of the metal atom it was made from. Give a reason for your suggestion. [2 marks] 32

AQA GCSE Chemistry for Combined Sciences: Trilogy Oxford University Press Help C2 The periodic table Summary questions 1 a Where in the periodic table do you find: I the halogens + II the noble gases [1 mark] iii the alkali metals [1 mark] [1 mark] b In which groups would you find the three elements described below? I This is a metal that can be cut with a knife and is stored under oil. It reacts violently with water and forms ions with a 1+ charge. [I mark] It This is a very unreactive, monatomic gas. (f mark] iii This toxic gas is the most reactive of the all the non-metallic elements. It forms ions with a 1- charge and will also form covalent compounds. [t mark] 2 Astatine, At, is a halogen whose atomic number is 85. It lies at the bottom of Group 7, beneath lodine a How many electrons occupy its outermost shell (highest energy level)? Explain how you worked out your answer. [I mark] b Predict the state of astatine at 20°C [1 mark] c For the compound sodium astatide, predict: I its type of bonding [1 mark] ii its colour [1 mark] iii its chemical formula [1 mark] iv the word equation and the balanced symbol equation for its formation from its elements [2 marks] v whether or not you would see signs of a reaction if a solution of sodium astatide was mixed with chlorine water. Explain how you arrived at your answer. [2 marks] d Place the halogens, including astatine, in order of reactivity, with the most reactive element first. Explain your answer in detail (include the trend in reactivity and the how the trend can be explained, referring to the formation of halide ions). [6 marks] 3 Rubidium, Rb, is in Group 1 of the periodic table, lying directly beneath potassium. a Predict the following physical properties of rubidium, including its hardness, electrical conductivity, and melting point. [3 marks] b i What will be the charge on a rubidium ion? [1 mark] in Copy and complete the table below: Rubidium compound Chemical formula rubidum iodide rubidum fluoride rubidium lydroside Rubidium compound Chemical formula rubidum iodide rubidum fluoride rubidium lydroside [3 marks] c. Write down word equations and balanced symbol equations, including state symbols, for the following reactions: I rubidium and water [3 marks] it rubidium and chlorine. [2 marks] d Will the reactions of rubidium in part c be more or less vigorous than the same reactions using potassium? Explain your answer in detail by comparing the atoms of the two elements. [5 marks] 4 Group 0 is found as the last column in the periodic table, on the extreme right hand side. a Write the name and symbol of the first four elements in Group 0. [2 marks] b What is the name commonly given to the elements in Group 0? [t mark] c Explain which of the first four noble gases is the odd one out in terms of the number of electrons in its outermost shell. [3 marks] d Describe how the electronic structures of the Group 0 elements affects their chemistry. [1 mark] The Group 0 elements are found in trace amounts in the air. If air is gradually cooled down to extremely low temperatures, predict which of the first four elements would condense as a liquid first. Give a reason for your answer. [2 mark] 5 a Explain how Dmitri Mendeleev used atomic weights to construct his periodic table. [2 marks] b Explain how the scientific community were influenced to accept his periodic table. [6 marks] c Why, in 1869, could scientists not explain why some pairs of elements in his periodic table appeared to be in the wrong order according to their atomic weights? [3 marks] 6 a Explain how the atoms of metals and non-metals change when they react to form their ions, using magnesium as an example of a metallic element and oxygen as an example of a non-metallic element. [6 marks] b Suggest how the radius of a metal ion compares with the radius of the metal atom it was made from. Give a reason for your suggestion. [2 marks] 32

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<p> <br />1. i. Group 7<br /> ii. Group 0<br /> iii. Group 1<br />b. i. Group 1<br /> ii. Group 0<br /> iii. Group 7<br />c. i. Rubidium reacts with water to form rubidium hydroxide and hydrogen gas: \( \text{Rb} + \text{H}_2\text{O} \rightarrow \text{RbOH} + \text{H}_2 \)<br /> ii. Rubidium reacts with chlorine to form rubidium chloride: \( \text{Rb} + \text{Cl}_2 \rightarrow \text{RbCl} \)<br />d. More vigorous<br />2. a. 7 electrons<br /> b. Solid<br /> c. i. Ionic bonding<br /> ii. Colorless or white<br /> iii. NaAt<br /> iv. Sodium reacts with astatine to form sodium astatide: \( \text{Na} + \text{At} \rightarrow \text{NaAt} \)<br /> d. No reaction<br /> e. Fluorine > Chlorine > Bromine > Iodine > Astatine<br />3. a. Soft, Good conductor, Low melting point<br /> b. i. +1<br /> b. ii. Smaller, Loss of an outer electron shell</p>

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<p><br />1. i. Halogens are found in Group 7 of the periodic table.<br /> ii. Noble gases are found in Group 0 (or 8) of the periodic table.<br /> iii. Alkali metals are found in Group 1 of the periodic table.<br />b. i. The described metal is an alkali metal, hence it belongs to Group 1.<br /> ii. The described gas is a noble gas, hence it belongs to Group 0.<br /> iii. The described gas is a halogen, hence it belongs to Group 7.<br />c. i. Rubidium reacts with water to form rubidium hydroxide and hydrogen gas. The balanced chemical equation is \( \text{Rb} + \text{H}_2\text{O} \rightarrow \text{RbOH} + \text{H}_2 \).<br /> ii. Rubidium reacts with chlorine to form rubidium chloride. The balanced chemical equation is \( \text{Rb} + \text{Cl}_2 \rightarrow \text{RbCl} \).<br />d. The reactions of rubidium will be more vigorous than potassium due to its larger atomic size, which makes rubidium more reactive.<br />2. a. Astatine has 7 electrons in its outermost shell as it is a member of Group 7.<br /> b. Astatine is predicted to be a solid at 20°C due to its position in the periodic table, below iodine which is a solid.<br /> c. i. Sodium astatide has ionic bonding due to the transfer of electrons from sodium to astatine.<br /> ii. Sodium astatide is likely colorless or white as most ionic compounds are.<br /> iii. The chemical formula for sodium astatide is NaAt.<br /> iv. Sodium reacts with astatine to form sodium astatide, represented by the equation \( \text{Na} + \text{At} \rightarrow \text{NaAt} \).<br /> d. There would be no reaction between sodium astatide and chlorine water as both are halogens and sodium astatide is stable.<br /> e. The order of reactivity among halogens decreases down the group due to increasing atomic size and decreasing electron affinity, hence the order is: Fluorine > Chlorine > Bromine > Iodine > Astatine.<br />3. a. Rubidium is soft, a good conductor of electricity, and has a low melting point due to its metallic nature and position in Group 1.<br /> b. i. A rubidium ion will have a charge of +1 due to the loss of one electron to achieve a stable electron configuration.<br /> b. ii. The radius of a metal ion is smaller than the radius of the metal atom it was made from due to the loss of an electron shell.</p>
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