Group 2 ionisation energy quiz

1. Which statement correctly defines the first ionisation energy of an element?

a) Energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions
b) Energy released when 1 mole of electrons is added to 1 mole of gaseous atoms
c) Energy to remove an electron from a solid sample of the element
d) Energy needed to break a covalent bond

2. What is the general trend in first ionisation energy down Group 2 (Be → Ba)?

a) It increases down the group
b) It decreases down the group
c) It stays constant
d) It fluctuates randomly

3. What best explains the decrease in first ionisation energy down Group 2?

a) Nuclear charge decreases down the group
b) Electron–electron repulsion decreases down the group
c) Distance of the outer electron from the nucleus decreases
d) Increased distance and increased shielding outweigh the increase in nuclear charge

4. Across Group 2, first ionisation energy decreases because atomic radius and increase down the group.

5. Which Group 2 element has the highest first ionisation energy?

a) Be
b) Mg
c) Ca
d) Ba

6. The first ionisation process is and is defined for atoms.

7. Which Group 2 element listed has the lowest first ionisation energy?

a) Be
b) Mg
c) Ca
d) Ba

8. In atoms, electrons in inner shells reduce the attraction between the nucleus and outer electrons (the shielding effect).

9. During the first ionisation of a Group 2 atom, what is removed?

a) A neutron
b) A proton
c) An electron from the outer s sub-shell
d) An electron from an inner p sub-shell

10. Why is magnesium's first ionisation energy lower than Beryllium's?

a) Mg has a smaller atomic radius and less shielding
b) Mg has a larger radius and more shielding than Be
c) Mg has a lower nuclear charge than Be
d) Mg has electrons in a lower principal energy level

11. For Mg, the largest “jump” in successive ionisation energies occurs between:

a) 1st and 2nd
b) 2nd and 3rd
c) 3rd and 4th
d) There is no notable jump

12. Down Group 2 the atoms get and the first ionisation energy gets .

13. “Effective nuclear charge” felt by a valence electron means:

a) The actual nuclear charge (Z) only
b) Net attractive charge after accounting for shielding
c) Number of neutrons in the nucleus
d) The atom’s overall charge

14. Which valence configuration represents a Group 2 atom?

a) n s²
b) n s¹
c) n p¹
d) n p⁶

15. Electrons in the same principal energy level shield each other only .