2.30 Describe how ionization energies support the idea of quantized energy levels in atoms.

How do ionization energies support the idea of quantized energy levels in atoms?

• Ionization energy is the energy required to remove an electron from an atom.

• The observed step-like pattern of ionization energies for elements indicates that electrons in atoms exist in discrete energy levels.

• Sharp increases in ionization energy occur when an electron is removed from a higher energy level, suggesting that these levels are distinct and quantized.

• Energy gaps between ionization energies reflect the differences between energy levels in an atom, supporting the concept of quantized energy states.

How do trends in ionization energies demonstrate quantized energy levels?

• First Ionization Energy: The energy needed to remove the first electron.

• Second Ionization Energy: The energy needed to remove a second electron, often much higher because it is removed from a more tightly bound electron (closer to the nucleus or from a filled shell).

• Trend: The large increase in ionization energy between successive electron removals (such as between the second and third ionization energies) indicates a jump from one energy level to another, more stable, and more tightly bound state.

• This confirms the idea that electrons occupy specific energy levels within an atom.

How do the ionization energies of sodium (Na) support the idea of quantized energy levels?

• First Ionization Energy of Sodium (Na): The energy required to remove one electron from the 3s orbital (outermost electron).

• Second Ionization Energy of Sodium (Na): Much higher because it involves removing an electron from a fully-filled inner shell (2p), which is more tightly bound to the nucleus.

• This significant increase between the first and second ionization energies suggests a jump from the outermost 3s level to the core 2p level, confirming that the electrons exist in distinct energy levels.

.

.