Write equations that show the processes that describe the first, second, and third ionization energies of an aluminum atom. Which process would require the least amount of energy?

검증된 단계별 안내

Step 1: Understand the concept of ionization energy. Ionization energy is the energy required to remove an electron from an atom in the gaseous state.

Step 2: Write the equation for the first ionization energy of aluminum. This involves removing the first electron from a neutral aluminum atom: \[ \text{Al(g)} \rightarrow \text{Al}^+(g) + e^- \]

Step 3: Write the equation for the second ionization energy of aluminum. This involves removing a second electron from the singly charged aluminum ion: \[ \text{Al}^+(g) \rightarrow \text{Al}^{2+}(g) + e^- \]

Step 4: Write the equation for the third ionization energy of aluminum. This involves removing a third electron from the doubly charged aluminum ion: \[ \text{Al}^{2+}(g) \rightarrow \text{Al}^{3+}(g) + e^- \]

Step 5: Determine which process requires the least amount of energy. The first ionization energy generally requires the least energy because it involves removing an electron from a neutral atom, which is less energetically demanding than removing electrons from positively charged ions.

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Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It is a measure of how strongly an atom holds onto its electrons. The first ionization energy refers to the removal of the first electron, while subsequent ionization energies involve removing additional electrons from the resulting cations. Generally, ionization energy increases with each successive electron removed due to the increasing positive charge of the ion.

Aluminum's Electron Configuration

Aluminum has an atomic number of 13, with an electron configuration of [Ne] 3s² 3p¹. This configuration indicates that aluminum has three valence electrons in its outer shell. Understanding the electron configuration is crucial for predicting the ionization processes, as the first ionization energy will involve removing the 3p electron, while the second and third will involve removing the 3s electrons, which are held more tightly due to increased nuclear charge.

Trends in Ionization Energy

Ionization energy trends can be observed across periods and groups in the periodic table. Generally, ionization energy increases across a period due to increasing nuclear charge and decreases down a group due to increased distance from the nucleus and electron shielding. For aluminum, the first ionization energy will be the lowest because it involves removing the least tightly held electron, while the second and third ionization energies will require progressively more energy due to the increased positive charge of the ion.