Lesson 6 Ionization Energy and PES(Photo electron scpectroscopy)

1. In Photoelectron Spectroscopy (PES), what does the height of a peak in a PES spectrum represent? A) Number of orbitals B) Ionization energy of electrons C) Number of electrons in a given subshell D) Energy required to remove a proton

• C) Number of electrons in a given subshell

• B) Ionization energy of electrons

• D) Energy required to remove a proton

• A) Number of orbitals

2. Which of the following best explains why first ionization energy generally increases across a period? A) Atomic radius increases B) Shielding effect increases C) Nuclear charge increases while shielding remains relatively constant D) Electrons are added to higher energy levels

• A) Atomic radius decreases

• B) Shielding effect decreases

• D) Electrons are removed from lower energy levels

• C) Nuclear charge increases while shielding remains relatively constant

3. In a PES spectrum of nitrogen (N) and oxygen (O), why does oxygen have a lower first ionization energy despite having a higher nuclear charge? A) Oxygen has fewer electrons than nitrogen B) Electrons in oxygen experience more repulsion due to paired electrons in the 2p subshell C) Oxygen has a larger atomic radius than nitrogen D) Oxygen's 2s electrons are easier to remove than nitrogen's 2s electrons

• C) Oxygen has a smaller atomic radius than nitrogen

• D) Oxygen's 2p electrons are more stable than nitrogen's 2p electrons

• A) Oxygen has a higher electronegativity than nitrogen

• B) Electrons in oxygen experience more repulsion due to paired electrons in the 2p subshell

4. Which element will have the highest first ionization energy? A) Sodium B) Magnesium C) Chlorine D) Argon

• F) Calcium

• G) Fluorine

• D) Argon

• E) Potassium

5. What is the primary purpose of Photoelectron Spectroscopy? A) To measure the mass of an atom B) To determine the energy levels of electrons C) To analyze molecular structures D) To identify chemical bonds

• B) To determine the energy levels of electrons

• D) To identify chemical bonds

• C) To analyze molecular structures

• A) To measure the mass of an atom

6. How does the presence of d and f orbitals affect ionization energy trends? A) They increase ionization energy B) They decrease ionization energy C) They have no effect D) They only affect transition metals

• A) They increase atomic radius

• C) They enhance electron affinity

• B) They decrease ionization energy

• D) They only affect lanthanides and actinides

7. Which of the following elements has the lowest first ionization energy? A) Helium B) Lithium C) Potassium D) Neon

• C) Potassium

• Boron

• Sodium

• Magnesium

8. What is the relationship between atomic size and ionization energy? A) Larger atoms have higher ionization energy B) Smaller atoms have higher ionization energy C) Atomic size has no effect on ionization energy D) Ionization energy is constant across all sizes

• C) Atomic size has a direct proportional effect on ionization energy

• A) Larger atoms have lower ionization energy

• D) Ionization energy increases with atomic size

• B) Smaller atoms have higher ionization energy

9. In which group of the periodic table would you expect to find elements with the highest ionization energies? A) Alkali metals B) Alkaline earth metals C) Halogens D) Noble gases

• F) Lanthanides

• E) Transition metals

• D) Noble gases

• G) Actinides

10. What effect does increasing nuclear charge have on ionization energy? A) It decreases ionization energy B) It increases ionization energy C) It has no effect D) It only affects nonmetals

• C) It increases electron affinity

• A) It decreases atomic radius

• B) It increases ionization energy

• D) It only affects metals