Classification of Elements & Periodicity Page 94 Q 3.27, Class 11 CBSE Chemistry

Classification of Elements & Periodicity Page 94 Q 3.28, Class 11 CBSE Chemistry

Classification of Elements & Periodicity Page 94 Q 3.29, Class 11 CBSE Chemistry

Classification of Elements & Periodicity Page 94 Q 3.30, Class 11 CBSE Chemistry

Classification of Elements & Periodicity Page 94 Q 3.31, Class 11 CBSE Chemistry

Classification of Elements & Periodicity Page 94 Q 3.32, Class 11 CBSE Chemistry

1. There will be total 20  MCQ in this test.
2. Please keep a pen and paper ready for rough work but keep your books away.
3. The test will consist of only objective type multiple choice questions requiring students to mouse-click their correct choice of the options against the related question number.
4. No negative marking for incorrect choice.
5. Please click on “Finish the Test” when you want to exit.
6. All the best – Happy Studying.

1. The element with lowest ionization energy among the following is:

 Li

 Na

 Rb

 K

Question 1 of 20

2. Isoelectronic species have:

 Same number of neutrons

  Same atomic mass

 Same number of electrons

 Same number of protons

Question 2 of 20

3. The cause of periodicity of properties of elements is due to the repetition of similar:

  Density

 Electronic configuration of atoms in the outermost energy shell

  Atomic number

 Atomic mass

Question 3 of 20

4. Tendency of an atom in a molecule to attract the shared pair of electron towards itself is called:

  Electronegativity

 Ionisation enthalpy

 Electron gain enthalpy

 Periodicity

Question 4 of 20

5. Identify the smallest ion among the following:

  Na⁺

 Mg²⁺

 K⁺

 Al³⁺

Question 5 of 20

6. Na⁺ is smaller than Na atom because:

 The effective nuclear charge is greater in case of sodium ion.

 Nucleus in each case contains different nucleons.

 Na+ is more stable than in Na atom.

  Sodium atom has one electron lesser than sodium ion.

Question 6 of 20

7. Electron gain enthalpy is most negative for:

  Fluorine

 Sulphur

 Phosphorus

 Chlorine

Question 7 of 20

8. Among the following the element with highest first ionization energy is:

  C

 Al

 Be

 Si

Question 8 of 20

9. Which of the following elements will have the largest atomic radii?

 Sr

 Al

  Li

 Ca

Question 9 of 20

10. For noble gases radius is measured as:

  Atomic radius

 Ionic radius

 van der Waals radius

 Metallic radius

Question 10 of 20

11. The electronegativity of following elements increases in the order of?

  Si, P, C, N

 P, Si, N, C

  C, N, Si, P

 N, Si, C, P

Question 11 of 20

12. Which of following statement is incorrect regarding ionization enthalpy:

 The greater increase in ionization enthalpy is experienced on removal of electron from core noble gas configuration

 Ionization enthalpy increases on moving from left to right along a period

 Ionization enthalpy decreases down the group

 Removal of electrons from orbitals bearing lower n value is easier than from orbital having higher n value

Question 12 of 20

13. Which of the following elements has the largest ionisation enthalpy?

  O

 F

 C

 N

Question 13 of 20

14. Anion O^– is isoelectronic with:

  Ne

 N^3-

 N^2-

 F^–

Question 14 of 20

15. What happens to atomic radius on going from left to right in a period in a periodic table?

  Remains constant

 Increases

 Decreases

 Decreases first and then remains constant

Question 15 of 20

16. When an electron is added to neutral gaseous atom to convert it into a negative ion, the enthalpy change accompanying the process is called:

  Ionisation enthalpy

 Electron gain enthalpy

 Lattice enthalpy

 Hydration enthalpy

Question 16 of 20

17. Which of the following is isoelectronic with F^–?

  Ne

 Ar

 Cl^–

 Mg⁺

Question 17 of 20

18. Among the following elements element with highest ionisation enthalpy is:

 N

 C

 O

 B

Question 18 of 20

19. The largest atomic radius among the following is of:

 Na

 Mg

 K

 Ca

Question 19 of 20

20. Electron gain enthalpy values of noble gases are positive because:

  They are all gases

 They are monoatomic

 They have smallest size

 They have stable electronic configuration

Question 20 of 20

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