O Level Chemistry Periodic Table Quiz

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O-Level Chemistry Quiz - Periodic Table

Name: ____________________
Class: ____________________
Date: ____________________
Score: ________ / 45

Duration: 60 Minutes
Total Marks: 45

Instructions:

• Answer all questions in the spaces provided.
• Use a pen for writing and a pencil for diagrams.
• Show all working clearly for calculation questions.

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Section A: Periodic Trends and Group 1 (1-7)

1. Elements in the Periodic Table are arranged in order of increasing ___________ number. [1]

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2. Explain why elements in the same group of the Periodic Table exhibit similar chemical properties. [2]

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3. As you move across a period from left to right, the nature of the elements changes from ___________ to ___________. [1]

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4. An element X is in Group 1 of the Periodic Table. (a) State one physical property of element X. [1]

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   (b) Describe the reaction of element X with water. [2]

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5. Compare the reactivity of potassium and sodium. Which is more reactive? Explain your answer in terms of electronic structure. [3]

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6. Write the balanced chemical equation for the reaction between lithium and water. Include state symbols. [2]

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7. Predict the charge of the ion formed by an element in Group 17. Explain your reasoning. [2]

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Section B: Group 17 and Group 18 (8-14)

8. State the general term used to describe the elements in Group 17. [1]

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9. Describe the trend in the physical state of the halogens as you move down Group 17 from fluorine to iodine. [2]

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10. Chlorine water is added to a solution of potassium bromide. (a) State whether a reaction occurs. [1]

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    (b) State the observation made. [1]

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    (c) Explain this observation in terms of reactivity. [2]

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11. Write the ionic equation for the displacement reaction between chlorine and bromide ions. [2]

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12. Explain why the reactivity of Group 17 elements decreases down the group. [3]

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13. Element Y is a noble gas in Group 18. (a) Explain why element Y is chemically inert. [2]

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    (b) State one common use of a noble gas in industry or medicine. [1]

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14. Which noble gas is most likely used to provide an inert atmosphere for high-temperature reactions? [1]

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Section C: Transition Elements and Reactivity Series (15-20)

15. State two characteristic properties of transition elements that distinguish them from Group 1 elements. [2] (i) ________________________________________________________________________ (ii) _______________________________________________________________________

16. Transition metals are often used as catalysts. Define the term catalyst. [2]

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17. In the reactivity series, magnesium is placed above copper. (a) Which metal is more likely to lose electrons to form a positive ion? [1]

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    (b) Predict whether copper(II) oxide can be reduced by magnesium. Explain your answer. [2]

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18. Describe the conditions required for the rusting of iron. [2]

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19. Explain how sacrificial protection prevents the rusting of a steel pipe. [3]

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20. A metal M reacts with steam to produce a metal oxide and hydrogen gas. (a) Is metal M more or less reactive than sodium? Justify your answer. [2]

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    (b) Write the general equation for the reaction of metal M with steam. [2]

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Answer Key - O-Level Chemistry Quiz: Periodic Table

1. Proton (1)

2. They have the same number of valence electrons / electrons in their outer shell (1), which determines their chemical reactivity (1).

3. Metallic to non-metallic (1)

4. (a) Soft / Low density / Silvery-white (Any one) (1) (b) Reacts vigorously with water (1) to produce a colorless solution of alkali and hydrogen gas / effervescence (1).

5. Potassium is more reactive (1). It has more shells/a larger atomic radius (1), so the outer electron is further from the nucleus and more easily lost (1).

6. $2\text{Li(s)} + 2\text{H}_2\text{O(l)} \rightarrow 2\text{LiOH(aq)} + \text{H}_2\text{(g)}$ (2) Award 1 mark for correct formulas, 1 mark for balancing and state symbols.

7. $1-$ (1). They have 7 valence electrons and need to gain one electron to achieve a stable noble gas configuration (1).

8. Halogens (1)

9. They change from gas (fluorine/chlorine) (1) to liquid (bromine) to solid (iodine) (1).

10. (a) Yes (1) (b) The solution turns orange/brown (1) (c) Chlorine is more reactive than bromine (1), so it displaces bromine from the bromide solution (1).

11. $\text{Cl}_2\text{(aq)} + 2\text{Br}^-\text{(aq)} \rightarrow 2\text{Cl}^-\text{(aq)} + \text{Br}_2\text{(aq)}$ (2)

12. As you go down the group, the atomic radius increases (1). The outer shell is further from the nucleus, increasing the shielding effect (1), making it harder for the atom to attract and gain an electron (1).

13. (a) It has a full valence shell / stable octet (1), so it does not need to gain, lose, or share electrons to become stable (1). (b) Argon for light bulbs / Helium for balloons / Neon for signage (Any one) (1).

14. Argon (1)

15. Any two: High melting/boiling points (1), High density (1), Variable oxidation states (1), Form colored compounds (1), Act as catalysts (1).

16. A substance that increases the rate of a chemical reaction (1) without being chemically changed or consumed in the process (1).

17. (a) Magnesium (1) (b) Yes (1). Magnesium is more reactive than copper and can therefore displace copper from its oxide (1).

18. Both water (moisture) (1) and oxygen (air) must be present (1).

19. A more reactive metal (e.g., zinc/magnesium) is attached to the iron (1). This metal oxidizes preferentially/loses electrons more easily than iron (1), preventing the iron from reacting with oxygen/water (1).

20. (a) Less reactive (1). Sodium reacts violently with cold water, whereas metal M requires steam (higher temperature) to react (1). (b) $2\text{M(s)} + 3\text{H}_2\text{O(g)} \rightarrow \text{M}_2\text{O}_3\text{(s)} + 3\text{H}_2\text{(g)}$ (or similar balanced equation for valency 1 or 2) (2).