Classification of Elements & Periodicity in Properties Quiz - ICSE Class 11 Chemistry

Free practice quiz: Classification of Elements & Periodicity in Properties (ICSE Class 11 Chemistry). 39 multiple-choice questions with answers and explanations. Play online, no sign-up needed.

This ICSE Class 11 Chemistry practice quiz has 39 multiple-choice questions on Classification of Elements & Periodicity in Properties, and 39 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 statements is INCORRECT regarding the modern periodic law?

   1. The physical and chemical properties of elements are periodic functions of their atomic numbers.
   2. The position of an element in the periodic table is determined by its atomic number.
   3. Elements in the same group have similar chemical properties due to the same number of valence electrons.
   4. The periodic law states that the properties of elements are periodic functions of their atomic masses.
   Show answer

   Answer: D. The periodic law states that the properties of elements are periodic functions of their atomic masses.

   The modern periodic law, formulated by Moseley, states that the properties of elements are periodic functions of their atomic numbers, not atomic masses. The atomic number determines the electronic configuration, which in turn dictates the chemical behavior of an element.

2. Which pair of elements has similar chemical properties?

   1. Na and Mg
   2. Li and Na
   3. Be and B
   4. C and N
   Show answer

   Answer: B. Li and Na

   Elements in the same group of the periodic table have similar chemical properties because they have the same number of valence electrons. Lithium (Li) and Sodium (Na) are both alkali metals (Group 1) and have one valence electron (ns¹), leading to similar chemical behaviors.

3. The element with the electronic configuration [Xe] 4f⁷ 6s² belongs to which block of the periodic table and what is its group name?

   1. f-block, Lanthanoid
   2. d-block, Transition metal
   3. p-block, Halogen
   4. s-block, Alkali metal
   Show answer

   Answer: A. f-block, Lanthanoid

   The electronic configuration shows that the differentiating electrons are entering the 4f subshell. Elements where the last electron enters the f-orbital are called f-block elements. Specifically, the configuration [Xe] 4f⁷ 6s² corresponds to Europium (Eu), which is a Lanthanoid.

4. The elements of Group 17 are called:

   1. Alkali metals
   2. Alkaline earth metals
   3. Halogens
   4. Noble gases
   Show answer

   Answer: C. Halogens

   Group 17 elements in the periodic table are known as Halogens. Examples include Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), and Astatine (At). Alkali metals are in Group 1, Alkaline earth metals are in Group 2, and Noble gases are in Group 18.

5. Which of the following statements regarding the placement of elements in the periodic table is correct?

   1. Hydrogen is placed in Group 1 because it has one valence electron, but it also shares some properties with Group 17 elements.
   2. Helium, with electron configuration 1s², is placed in Group 18 due to its chemical inertness, despite having only 2 electrons.
   3. Elements with similar electronic configurations of their outermost shells are placed in the same group.
   4. All of the above
   Show answer

   Answer: D. All of the above

   Statement 1 is correct: Hydrogen has one valence electron like alkali metals (Group 1) and also resembles halogens (Group 17) by needing one electron to achieve a stable configuration. Statement 2 is correct: Helium's inertness and filled valence shell (1s²) dictate its placement with noble gases in Group 18. Statement 3 is correct: The periodic law states that elements with similar valence electron configurations exhibit similar chemical properties and are placed in the same group.

More questions in this quiz

Answers and explanations are in the full quiz.

1. Identify the element with the highest ionization enthalpy in the second period.
2. What is the correct order of increasing metallic character for the following elements?
3. Which of the following isoelectronic species has the smallest ionic radius?
4. The electronic configuration of an element is 1s²2s²2p⁶3s²3p⁶4s²3d⁵. What is the atomic number of this element?
5. Which of the following halogens has the highest electron gain enthalpy (least negative value)?
6. The element with the electronic configuration [Ar] 4s²3d¹⁰4p⁵ belongs to which block of the periodic table?
7. What is the correct order of increasing electronegativity?
8. The element with atomic number 13 is in which period and group?
9. Which of the following metals is an alkaline earth metal?
10. What is the common characteristic of elements in Group 18 (Noble Gases)?
11. The atomic radius generally decreases across a period due to:
12. Which of the following is NOT a transition element?
13. The first ionization energies of elements X, Y, and Z are 801, 1086, and 1251 kJ/mol respectively. If X, Y, and Z are consecutive elements in the same period, identify them.
14. Which of the following isoelectronic species has the largest ionic radius?
15. The element with atomic number 31 belongs to which period and block, and what is its group number?
16. Which trend is INCORRECT regarding the periodic properties in Group 1 (Alkali Metals)?
17. The sum of first and second ionization enthalpies of an element X is 2080 kJ/mol. The sum of third and fourth ionization enthalpies is 6000 kJ/mol. What is likely the group of element X?
18. Which of the following elements exhibits the highest electron affinity (most negative value)?
19. The elements that have atomic numbers from 57 to 71 are known as:
20. Which of the following is an exception to the general trend of increasing ionization enthalpy across a period?
21. Which of the following pairs of elements are isoelectronic?
22. The electronic configuration of an element is 1s²2s²2p⁶3s²3p⁶4s²3d⁷. To which block and group does this element belong?
23. Which property among the following generally decreases across a period?
24. The element with the electron configuration [Ar] 4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²4f¹⁴5d¹⁰6p¹ belongs to which period and block?
25. Which of the following statements about the periodic classification of elements is INCORRECT?
26. The element with atomic number 92 is _____, and it belongs to the _____ series.
27. Identify the element that has the highest metallic character within the period 3 of the periodic table.
28. The general electronic configuration of transition elements is:
29. Which of the following elements has the largest atomic radius?
30. The element with the electronic configuration 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²4f¹⁴5d¹⁰6p⁵ belongs to which group and block?
31. The ionization enthalpy order for elements of the second period is generally:
32. The correct order of increasing atomic radius for the following elements is:
33. Which element is likely to have the most stable electronic configuration among the following?
34. The metallic character of the elements of the second period follows the order:

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