SASS Chem Revision

Page 1 ST ANDREW’S SECONDARY SCHOOL NAME TEACHING GROUP DATE DD MM YYYY Chemistry 2023 JUNE HOLIDAY REVISION PRACTICE Metals, The Periodic Table, Electrochemistry & Rate of Reaction 4 topics each with 4 sets of questions: each set consists of just 2 questions – 1 MCQ & 1 Structured. only 0.25 h / 15 min / 900 s needed each day to complete 1 set! “An 🍎 each day keeps the 👨⚕ away” apple doctor “A set 📄 each day keeps the 👻 away” questions nightmares JUNE HOLIDAYS 20232930311234567891011121314151617181920212223242526 MONTUEWEDTHUFRISATSUNGCE O-LEVEL MTGCE O-LEVEL MT ’B’VESAK DAY Semester2 Metals (1)Metals (2)Metals (3)Metals (4)Periodic Table (1)Periodic Table (2)Periodic Table (3) Periodic Table (4)Electrochemistry (1)Electrochemistry (2)Electrochemistry (3)Electrochemistry (4)Rate of Rxn (1)Rate of Rxn (2)Rate of Rxn (3)Rate of Rxn (4) BEGINS Write your answers to each set of questions on writing papers.

Page 2 METALS (1) 1 Which of the following metal oxides is most easily reduced by carbon? A CuO B Fe2O3 C MgO D ZnO 2 The Statue of Liberty in New York City was constructed in Paris, France, in the 1880s and presented as a gift to the United States of America. Its structure consists of an iron frame wrapped around with a sheet of pure copper. Due to a chemical process called patination, the copper reacted with oxygen and water in the air and became blue-green. The following chemical equations outline the steps in patination. Step 1: 4Cu (s) + O2 (g) ® 2Cu2O (s) Step 2: 2Cu2O (s) + O2 (g) ® 4CuO (s) Step 3: 2CuO (s) + CO2 (g) + H2O (l) ® Cu2CO3(OH)2 (s) The patina formed on the surface of the statue prevented copper from further oxidation. (a) (i) Determine the oxidation state of copper in CuO, Cu2O and Cu2CO3(OH)2. [3] (ii) Using the oxidation states determined in (a)(i), state with reasoning, whether each of the steps in patination is a redox reaction. [3] The iron frame eventually undergoes corrosion. However, unlike patination, corrosion of iron is considered to be destructive. (b) (i) Suggest why the corrosion of iron is considered to be destructive. [1] (ii) Is the iron frame in the Statue of Liberty expected to corrode at a faster or slower rate than usual? Provide an explanation to your answer. [2] (iii) Even though the iron frame can be protected from corrosion by coating with paint, this method was never considered. Suggest a reason why. [1] METALS (2) 3 Which of the following metals does not react with cold water, but reacts with steam to produce hydrogen gas? A Calcium B Copper C Lead D Zinc 4 Aluminium is the most abundant metallic element found on Earth, making up about 8% of the Earth’s crust. It is also the most widely used non-ferrous metal today. Aluminium does not occur naturally in its metallic form. It was only in 1807 that aluminium was discovered by Sir Humphry Davy. An economically viable process to extract aluminium by electrolysis was developed later in 1886. (a) Give one use of aluminium. [1] (b) Suggest a reason why aluminium does not occur naturally in its metallic form. [1] (c) How does the extraction method for aluminium relate to its position in the reactivity series? [1] (d) Despite being the most abundant metal found on Earth, most of the aluminium used today is recycled. Suggest a reason why. [1] (e) Give one benefit and one drawback from recycling aluminium. [2]

Page 3 METALS (3) 5 Brass is a copper alloy that contains zinc. Which statements about brass are correct? 1 Brass conducts electricity because it contains mobile electrons. 2 Brass does not react with dilute hydrochloric acid. 3 Brass has a higher melting point than copper or zinc. 4 The density of brass is much higher than copper or zinc. A 1, 2, 3 and 4 B 1,2 and 4 only C 2 and 3 only D 1 only 6 A student conducted an experiment to investigate the sacrificial protection between metals. He immersed two different strips of metals in three beakers, A, B and C, containing equal volumes of dilute hydrochloric acid. The diagrams below show the metal strips in each beaker. (a) Suggest, with reasoning, two observations the student would make in all three beakers. [4] (b) In which beaker would the time required for the zinc metal stripe to completely dissolve be (i) the shortest? [1] (ii) the longest? [1] (c) Discuss how you deduce at your answers in (b). [2] zinciron Beaker A zincmagnesium Beaker B zincsilver Beaker C

Page 4 METALS (4) 7 Mercury is found to be more reactive than silver but less reactive than copper. Which of the following statements about mercury is correct? A Mercury can be obtained from its ore by roasting in air. B Mercury displaces zinc from aqueous zinc nitrate solution. C Mercury reacts with cold water to produce hydrogen gas. D Mercury reacts with dilute hydrochloric acid to produce hydrogen gas. 8 You are provided with the following set of substances: • Copper wire • Copper(II) sulfate powder • Distilled water • Iron(II) chloride powder • Iron wire Using only the substances provided above, describe an experiment to determine the order of reactivity between copper and iron accurately. You may assume that all apparatus found in a school laboratory are available for your use. Your answer should include: • balanced chemical equations for all reactions that occurred, • relevant observations made. [5] PERIODIC TABLE (1) 9 Which statements about the Periodic Table are correct? 1 Elements become less metallic in character going down a group. 2 Elements change from being metallic to non-metallic in character moving across a period. 3 Elements in the same group undergo similar chemical reactions. 4 The group number represents the number of electron shells in an atom. A 1, 2, 3 and 4 B 1 and 4 only C 2 and 3 only D 1 only 10 The electronic configuration of five elements, A – E, are listed in the table below. Element A B C D E Electronic configuration 2,4 2,8,2 2,8,7 2,8,8,1 2,8,18,8 (a) Using the letters A, B, C, D and E, state which element is (i) a Group II metal? [1] (ii) a halogen? [1] (iii) a noble gas? [1] (iv) an alkali metal? [1] (b) (i) Deduce the formula of the compound formed between elements A and C. [1] (ii) Draw a ‘dot-and-cross’ diagram to show the bonding present in the compound in (b)(i). Explain how this bonding is formed. [3]

Page 5 PERIODIC TABLE (2) 11 Which statement explains why neon is chemically unreactive? A It contains an equal number of electrons and neutrons. B It does not gain or lose electrons. C Its first electron shell is completely filled. D Its valence electron shell is completely filled. 12 Chlorine is a halogen that is commonly used as a disinfectant and bleaching agent due to its powerful oxidising properties. (a) Use ideas about electron transfer to explain why chlorine is a powerful oxidising agent. [2] (b) A chemical reaction occurs when chlorine gas is bubbled into a solution of sodium iodide. (i) Describe the observation made during this reaction. [1] (ii) Construct a balanced chemical equation, with state symbols, for this reaction. [1] (iii) Using ideas about oxidation state and electron transfer, explain how this reaction occurs.[2] PERIODIC TABLE (3) 13 The chemical nature of oxides formed by the elements across a period changes from basic to acidic. Which of the following statements best explains this? A The metallic nature of the elements decreases going across a period. B The non-metallic nature of the elements decreases