Ionization Energies Practice Questions PDF

1. What is the de nition of the rst ionization energy? * A) The energy required to remove one electron from a neutral atom in its gaseous state. * B) The energy released when one electron is added to a neutral atom in its gaseous state. * C) The energy required to remove one proton from a neutral at...

1. What is the de nition of the rst ionization energy? * A) The energy required to remove one electron from a neutral atom in its gaseous state. * B) The energy released when one electron is added to a neutral atom in its gaseous state. * C) The energy required to remove one proton from a neutral atom. * D) The energy required to remove all electrons from a neutral atom. 2. What is the general trend in rst ionization energy across a period (from left to right) in the periodic table? * A) Increases * B) Decreases * C) Remains constant * D) Varies randomly 3. Why does the rst ionization energy generally increase across a period? * A) Nuclear charge decreases, and shielding remains constant. * B) Nuclear charge increases, and shielding remains constant. * C) Nuclear charge remains constant, and shielding increases. * D) Both nuclear charge and shielding decrease. 4. What is the general trend in rst ionization energy down a group in the periodic table? * A) Increases * B) Decreases * C) Remains constant * D) Varies randomly 5. Why does the rst ionization energy decrease down a group? * A) Shielding decreases, and the distance between the nucleus and outer electron increases. * B) Shielding increases, and the distance between the nucleus and outer electron decreases. * C) Shielding and the distance between the nucleus and outer electron both increase. * D) Shielding and the distance between the nucleus and outer electron both decrease. fi fi fi fi fi fi  6. Which element has a lower rst ionization energy, Neon (Ne) or Argon (Ar)? * A) Neon (Ne) * B) Argon (Ar) * C) They have the same rst ionization energy. * D) Cannot be determined from the information given. 7. The rst ionization energy decreases from beryllium (Be) to boron (B). Why is this? * A) Boron has a higher nuclear charge than beryllium. * B) In Boron, the 2s orbital shields the 2p orbital, weakening the nuclear attraction. * C) Boron has a smaller atomic radius than beryllium. * D) Boron has more electron-electron repulsion. 8. The rst ionization energy decreases from nitrogen (N) to oxygen (O). Why is this? * A) Oxygen's 2p orbitals contain a paired set of electrons that causes repulsion. * B) Oxygen has a smaller atomic radius than nitrogen. * C) Oxygen has a lower nuclear charge than nitrogen. * D) Oxygen has less shielding than nitrogen. 9. What is the equation representing the *second* ionization energy of an element X? * A) X(g) → X⁺(g) + e⁻ * B) X⁺(g) → X²⁺(g) + e⁻ * C) X⁻(g) → X(g) + e⁻ * D) X²⁺(g) → X³⁺(g) + e⁻ 10. What is the general trend for successive ionization energies of any given element? * A) They decrease. * B) They increase. * C) They remain constant. * D) They uctuate randomly. 11. Why do successive ionization energies generally increase? * A) The number of protons decreases with each electron removed. * B) The relative positive charge increases with each electron removed. fi fi fl fi fi  * C) The shielding effect increases with each electron removed. * D) The atomic radius increases with each electron removed. 12. In a graph of successive ionization energies, what do large "jumps" in the data indicate? * A) Electrons are being removed from the same energy level. * B) The element is changing into a different element. * C) Electrons are being removed from a new, inner energy level. * D) The element has become stable. 13. If there is a large jump between the 3rd and 4th ionization energies of an element, which group is the element most likely in? * A) Group 1 * B) Group 2 * C) Group 3 * D) Group 4 14. If there is a small jump between the 2nd and 3rd ionisation energies, and a large jump between the 9th and 10th ionisation energies, what group is that atom in? * A) group 1 * B) group 2 * C) group 7 * D) group 8 15. Why is the second ionization energy of sodium signi cantly higher than its rst ionization energy? * A) The second electron is removed from the same energy level as the rst. * B) The second electron removed is being taken from an energy level closer to the nucleus. * C) Sodium has a very high nuclear charge. * D) Sodium has a very small atomic radius. 16. Which of these elements is likely to have the *lowest* rst ionization energy? * A) Li * B) F * C) Ne * D) Na fi fi fi fi  17. Which would be the correct 7th ionisation energy for Phosphorous? * A) P7+(g) → P8+(g) + e- * B) P6+(g) → P7+(g) + e- * C) P5+(g) → P6+(g) + e- * D) P(g) → P+(g) + e- 18. On a graph plotting ionisation number against ionisation energy, where would you expect to see the greatest jump for a group 6 element? * A) Between the 1st and 2nd I.E * B) Between the 5th and 6th I.E * C) Between the 6th and 7th I.E * D) Between the 2nd and 3rd I.E 19. Which shows the correct order of elements from smallest to largest rst ionisation energies? * A) F, O, N * B) N, O, F * C) O, N, F * D) F, N, O 20. Which of the elements has the highest second ionisation energy in its period? * A) group 1 * B) group 2 * C) group 7 * D) group 8 21. The second ionisation energy of an element is... * A) Always lower than the rst ionisation energy * B) Always greater than the rst ionisation energy * C) Sometimes greater than the rst ionisation energy * D) Always equal to the rst ionisation energy. 22. Why might successive ionisation energies not always perfectly increase smoothly? * A) The experimental setup is awed. * B) There are variations due to electron con gurations and electron- electron repulsion. * C) The temperature changes during the experiment. fi fi fi fi fl fi fi * D) The data is plotted incorrectly. 23. The "peaks" in the 2nd I.E. graph correspond to which group of elements? * A) group 8 * B) group 7 * C) group 2 * D) group 1 24. The "troughs" in the 2nd I.E. graph correspond to which group of elements? * A) group 1 * B) group 2 * C) group 7 * D) group 8 25. Elements in the same group show a similar pattern in their successive ionization energies because: * A) They have the same number of protons. * B) They have similar outer electron con gurations and experience similar shielding effects. * C) They have the same atomic radius. * D) They have the same number of electron shells. fi