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Periodic Table Trends Quiz
How well do you know the periodic table? This quiz will challenge your knowledge of atomic and ionic radii, ionization energy, electronegativity, and other important trends. Perfect for high school chemistry students.
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1. Which of the following elements has the largest atomic radius?
Explanation: Atomic radius increases down a group due to the addition of electron shells.
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2. Which element has the highest ionization energy?
Explanation: Ionization energy decreases down a group because the outermost electron is further from the nucleus and easier to remove.
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3. Which of the following elements has the highest electronegativity?
Answer: (a) Oxygen (O). Explanation: Electronegativity increases down a group and across a period (excluding noble gases).
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4. Which of the following has the smallest atomic radius?
Answer: (d) Silicon (Si). Explanation: Atomic radius decreases across a period due to increasing nuclear charge pulling the electrons closer.
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5. Which element has the lowest ionization energy?
Answer: (c) Cesium (Cs). Explanation: Cesium is at the bottom left of the periodic table, where ionization energy is lowest.
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6. Which of these elements is the most electronegative?
Answer: (c) Fluorine (F). Explanation: Fluorine is the most electronegative element.
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7. Which of the following represents the correct order of increasing atomic radius?
Answer: (a) Cl < S < P < Si. Explanation: Atomic radius decreases across a period from left to right.
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8. Which of the following has the highest metallic character?
Answer: (a) Sodium (Na). Explanation: Metallic character decreases across a period and increases down a group.
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9. Which of the following elements has the highest electron affinity?
Fluorine is an exception due to its small size and interelectronic repulsions.
While fluorine is more electronegative, chlorine has the highest electron affinity due to its larger atomic size compared to fluorine, which reduces electron repulsion in its valence shell. As a result, chlorine releases more energy when it gains an electron.
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10. Which element has the lowest electronegativity?
Answer: (c) Francium (Fr). Explanation: Francium is at the bottom left of the periodic table, where electronegativity is lowest.
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11. Ionization energy generally increases across a period because:
Answer: (b) The nuclear charge increases. Explanation: Increased nuclear charge pulls electrons more strongly.
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12. Atomic radius generally decreases across a period because:
Answer: (b) The nuclear charge increases. Explanation: Increased nuclear charge pulls electrons closer to the nucleus.
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13. Which of the following is the correct order of increasing electronegativity?
Answer: (a) K < Na < Li < F. Explanation: Electronegativity increases across a period and up in a group.
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14. Which of the following elements is most likely to form a stable -2 ion?
Answer: (c) Oxygen (O). Explanation: Oxygen needs two electrons to complete its octet.
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15. Which of the following pairs represents elements with similar chemical properties?
Answer: (b) Potassium (K) and Rubidium (Rb). Explanation: Elements in the same group (vertical column) have similar chemical properties due to having the same number of valence electrons.
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