Periodic Properties & Variations Quiz - ICSE Class 10 Chemistry

Free practice quiz: Periodic Properties & Variations (ICSE Class 10 Chemistry). 55 multiple-choice questions with answers and explanations. Play online, no sign-up needed.

This ICSE Class 10 Chemistry practice quiz has 55 multiple-choice questions on Periodic Properties & Variations, and 55 of them come with an explanation. Try the 5 sample questions below (tap an option to check yourself), then play the full quiz online. No sign-up needed.

Sample questions

1. Which of the following trends is INCORRECT for elements across a period in the periodic table?

   1. Atomic radius generally decreases.
   2. Electronegativity generally increases.
   3. Ionization energy generally decreases.
   4. Metallic character generally decreases.
   Show answer

   Answer: C. Ionization energy generally decreases.

   Across a period, the nuclear charge increases while the shielding effect remains relatively constant. This stronger attraction pulls the valence electrons closer to the nucleus, causing the atomic radius to decrease. The increased effective nuclear charge also leads to a general increase in electronegativity. The tendency to lose electrons (metallic character) decreases as elements become more electronegative. Ionization energy generally increases across a period due to the increased effective nuclear charge, making it harder to remove an electron.

2. The ionization energies of the first three elements in a period are I1, I2, and I3. If I1 < I2 << I3, which group do these elements likely belong to?

   1. Group 1
   2. Group 2
   3. Group 13
   4. Group 14
   Show answer

   Answer: B. Group 2

   The first ionization energy (I1) refers to the removal of the first electron, the second ionization energy (I2) to the removal of the second electron from the same atom, and so on. A large jump in ionization energy occurs when an electron is removed from a more stable electron shell. If I1 < I2 << I3, it means the first two electrons are relatively easy to remove, but the third electron is much harder to remove. This indicates that the element has two valence electrons that are readily lost to achieve a stable electron configuration (like a noble gas). Elements in Group 2 have two valence electrons (ns^2), and their ionization energies follow this pattern: I1 < I2 << I3.

3. Which statement best explains the decrease in atomic radius across a period?

   1. The number of electron shells increases.
   2. The nuclear charge increases, pulling electrons closer.
   3. The shielding effect of inner electrons increases significantly.
   4. The attraction between protons and electrons decreases.
   Show answer

   Answer: B. The nuclear charge increases, pulling electrons closer.

   Across a period, elements gain protons in the nucleus, increasing the nuclear charge. The added electrons are in the same principal energy shell, so the shielding effect of inner electrons does not increase proportionally to the nuclear charge. The increased nuclear charge exerts a stronger attractive force on the valence electrons, pulling them closer to the nucleus and thus decreasing the atomic radius.

4. Which of the following oxides is basic?

   1. CO2
   2. SO3
   3. P4O10
   4. K2O
   Show answer

   Answer: D. K2O

   The oxides of metals are generally basic, while the oxides of nonmetals are generally acidic. Potassium (K) is an alkali metal. Carbon (C), Sulfur (S), and Phosphorus (P) are nonmetals. Therefore, Potassium oxide (K2O) is a basic oxide.

5. The formation of a stable oxide layer on the surface of Aluminum is due to:

   1. Its high metallic character.
   2. Its low ionization energy.
   3. The formation of a protective oxide film.
   4. Its inert nature.
   Show answer

   Answer: C. The formation of a protective oxide film.

   Aluminum is a reactive metal, but it forms a thin, tenacious, and impermeable layer of aluminum oxide (Al2O3) on its surface when exposed to air. This oxide layer passivates the metal, preventing further reaction with oxygen or other corrosive agents, thus making it appear less reactive than expected for its position in the periodic table.

More questions in this quiz

Answers and explanations are in the full quiz.

1. The element with the highest ionization energy is likely to be found in which region of the periodic table?
2. Which of the following elements has the largest atomic radius?
3. The electron affinity of an element is the energy change when an electron is added to a neutral atom in the gaseous state. Which of the following elements is expected to have the most negative electron affinity?
4. Which of the following statements about metallic character is TRUE?
5. The element with the smallest atomic radius and the highest electronegativity is most likely to be found in which part of the periodic table?
6. Which of the following oxides is likely to be amphoteric?
7. Consider the elements X, Y, and Z with atomic numbers 11, 17, and 19 respectively. Which of the following statements about their properties is correct?
8. Element 'A' is in Period 2, Group 16, and Element 'B' is in Period 3, Group 16. Which statement is INCORRECT?
9. Element 'A' is in Period 2, Group 17, and Element 'B' is in Period 3, Group 17. Which statement is INCORRECT?
10. Which of the following elements would have the highest melting point?
11. Which of the following ions is isoelectronic with Argon (Ar)?
12. Which of the following ions is isoelectronic with Neon (Ne)?
13. As we move down a group in the periodic table, which of the following properties generally increases?
14. The chemical reactivity of alkali metals increases from top to bottom. This is primarily due to:
15. Which pair of elements would be expected to form an ionic compound?
16. Which of the following halogens has the highest melting point?
17. Consider elements with electron configurations $1s^2 2s^2 2p^6 3s^1$ and $1s^2 2s^2 2p^6 3s^2 3p^5$. Which statement correctly compares their properties?
18. Elements in the same period of the periodic table generally have:
19. Which element is expected to have the lowest first ionization energy among the following?
20. The oxide of which element is expected to be the most acidic?
21. Elements in the same group of the periodic table share similar chemical properties primarily due to:
22. Which of the following elements has the highest electronegativity?
23. Which of the following trends is CORRECT for elements as we move from left to right across Period 3?
24. Consider elements X, Y, and Z. X is in Group 1, Period 2. Y is in Group 17, Period 2. Z is in Group 1, Period 3. Which of the following comparisons is INCORRECT?
25. Which of the following pairs of elements would form the most polar covalent bond?
26. The ability of an atom to attract a shared pair of electrons towards itself is called:
27. Which of the following is NOT a periodic property?
28. Elements in the same period have similar chemical properties if they:
29. The element with the most negative electron affinity is typically found in which region of the periodic table?
30. Which of the following statements about atomic radius is correct?
31. The element with electronic configuration $1s^2 2s^2 2p^6 3s^2 3p^3$ is in which period and group?
32. Which of the following properties does NOT show a clear trend across a period?
33. Elements in the same period have electrons in the same principal energy level. This means they have:
34. Which of the following elements is a metalloid?
35. The metallic character of elements decreases across a period and increases down a group. Based on this, which of the following elements is the most metallic?
36. Which of the following statements about ionization energies is correct?
37. Which of the following is the correct order of increasing atomic radius?
38. Which of the following elements will exhibit the most vigorous reaction with cold water?
39. The element with atomic number 13 is:
40. Which trend is generally observed as you move down Group 17 (halogens)?
41. Which pair of elements has the largest difference in electronegativity?
42. Which of the following properties generally increases for elements in Group 14 as we move down the group?
43. The element in Period 3 with the highest ionization energy is:
44. Which of the following is NOT a valid explanation for periodic trends?
45. The element with atomic number 20 is located in:
46. Which of the following pairs of oxides are amphoteric?
47. The metallic character of elements in the same period is influenced by:
48. Which of the following statements about electron affinity is correct?
49. The reason for the anomaly in the electron affinity of Oxygen compared to Sulfur is primarily attributed to:
50. Which of the following sets lists elements in order of increasing atomic radius?

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