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 calculations, show all working.

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Section A: Periodic Trends and Arrangement (Questions 1–5)

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

2. An element $X$ is in Group 2 and Period 3. (a) State the number of electrons in the outermost shell of $X$. [1] (b) State the number of electron shells in $X$. [1]

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

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4. Define the term "Period" as used in the Periodic Table. [1]

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5. Which group of elements is known as the "Alkali Metals"? [1]

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Section B: Group 1 and Group 17 Trends (Questions 6–10)

6. State the general trend in reactivity as you move down Group 1. [1]

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7. Explain why the reactivity of Group 1 elements increases as you move down the group. [3]

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8. State the general trend in reactivity as you move down Group 17. [1]

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9. Explain why the reactivity of Group 17 elements decreases as you move down the group. [3]

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10. Compare the physical state of Fluorine and Iodine at room temperature. [2]

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Section C: Transition Elements and Noble Gases (Questions 11–15)

11. List two characteristic properties of transition elements. [2]

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12. Why do transition elements often form colored compounds? [2]

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13. State one common use of transition elements in the industrial chemical process. [1]

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14. Explain why Noble Gases (Group 18) are chemically inert. [2]

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15. Which Noble Gas is commonly used in light bulbs to prevent the filament from oxidizing? [1]

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Section D: Application and Synthesis (Questions 16–20)

16. An element $Y$ is in Group 17 and Period 3. (a) Identify the element $Y$. [1] (b) State its electronic configuration. [1]

17. Sodium (Na) and Chlorine (Cl) react to form a compound. (a) State the formula of the compound formed. [1] (b) Describe the type of bonding in this compound. [1] (c) Explain the formation of this bond in terms of electron transfer. [2]

18. Element $Z$ has the electronic configuration 2, 8, 4. (a) State the Group and Period of element $Z$. [2] (b) State the number of valence electrons in $Z$. [1]

19. Why are Group 1 metals stored under oil? [2]

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20. Predict the relative reactivity of Potassium (K) compared to Lithium (Li). Justify your answer. [2]

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O-Level Chemistry Quiz - Periodic Table (Answer Key)

Section A: Periodic Trends and Arrangement

1. Atomic number [1]
2. (a) 2 [1] (b) 3 [1]
3. They have the same number of valence electrons [1], which determines their chemical reactivity/behavior [1].
4. A horizontal row of elements in the periodic table [1].
5. Group 1 [1]

Section B: Group 1 and Group 17 Trends

6. Reactivity increases down the group [1].
7. Atomic radius increases [1]. Outer electrons are further from the nucleus and shielding increases [1], weakening the attraction between the nucleus and the valence electron, making it easier to lose an electron [1].
8. Reactivity decreases down the group [1].
9. Atomic radius increases [1]. The distance between the nucleus and the outer shell increases and shielding increases [1], making it harder for the nucleus to attract and gain an electron [1].
10. Fluorine is a gas [1]; Iodine is a solid [1].

Section C: Transition Elements and Noble Gases

11. Any two: High melting/boiling points; Form colored compounds; Act as catalysts; Variable oxidation states [2].
12. They have partially filled d-orbitals [2].
13. Used as catalysts (e.g., Iron in Haber process) [1].
14. They have a full outer shell of electrons [1], making them stable and unreactive [1].
15. Argon [1].

Section D: Application and Synthesis

16. (a) Chlorine (Cl) [1] (b) 2, 8, 7 [1]
17. (a) NaCl [1] (b) Ionic [1] (c) Sodium loses one electron to become $\text{Na}^+$; Chlorine gains one electron to become $\text{Cl}^-$. Strong electrostatic attraction exists between the opposite ions [2].
18. (a) Group 14, Period 3 [2] (b) 4 [1]
19. They are highly reactive and would react with oxygen or moisture in the air [2].
20. Potassium is more reactive than Lithium [1] because it has a larger atomic radius/more shielding, making it easier to lose its valence electron [1].