Konfigurasi Elektron - Aturan Penuh dan Setengah Penuh

Summary

In this informative session, the speaker discusses the principles of electron configuration, focusing on the stability associated with full and half-full subshells. Using chromium (Cr) and copper (Cu) as examples, the speaker explains how the electron configurations differ due to their stability preferences. Cr's configuration emphasizes the half-full stability of the d subshell, while Cu achieves stability through a fully filled d subshell. The session is designed to enhance understanding of electron configurations and their implications for chemical stability, concluding with an invitation for questions.

Takeaways

• 🔬 The fourth principle of electron configuration involves full and half-full orbital stability.
• 🔄 Atoms from group B exhibit stability when their d orbitals are either completely filled (D10) or half-filled (D5).
• ⚛️ Chromium (Cr), with atomic number 24, has a unique electron configuration that stabilizes at half-full.
• 📊 The electron configuration of Cr is 1s2 2s2 2p6 3s2 3p6 4s1 3d5 after one electron from 4s moves to 3d.
• 📉 Copper (Cu), with atomic number 29, prefers a fully filled d subshell configuration for stability.
• 🔢 The electron configuration of Cu is 1s2 2s2 2p6 3s2 3p6 4s1 3d10, achieving full stability.
• 📈 In the case of d orbitals, the distribution of electrons in boxes must follow the Aufbau principle.
• 🔄 Electrons fill the lowest energy orbitals first before moving to higher ones, following Hund's rule.
• 💡 The explanation emphasizes the importance of electron configurations in understanding atomic stability.
• 🤔 Viewers are encouraged to ask questions for further clarification on the topic.

Q & A

What is the main topic of the lesson discussed in the transcript?

The main topic is the principles of electron configuration, specifically focusing on full and half-full configurations in transition metals.

Which elements are specifically discussed in the lesson?

The lesson specifically discusses chromium (Cr) and copper (Cu).

What is the atomic number of chromium, and how is its electron configuration structured?

Chromium has an atomic number of 24, and its electron configuration is structured as 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁴.

Why is the configuration 4s¹ 3d⁵ considered more stable for chromium?

The configuration 4s¹ 3d⁵ is considered more stable because it achieves a half-full d subshell, which is energetically favorable.

What is the significance of full (D10) and half-full (D5) configurations in terms of stability?

Full (D10) and half-full (D5) configurations are significant because they are associated with lower energy states and increased stability for the atom.

What is the atomic number of copper, and what is its initial electron configuration before stability adjustments?

Copper has an atomic number of 29, and its initial electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁹.

How does copper achieve stability in its electron configuration?

Copper achieves stability by having one electron from the 4s orbital move to the 3d subshell, resulting in a configuration of 4s¹ 3d¹⁰, which is a fully filled d subshell.

What do the terms 'valence electrons' refer to in the context of the discussed elements?

Valence electrons refer to the electrons in the outermost shell (4s and 3d for both Cr and Cu) that are involved in chemical bonding and reactions.

What was the instructor's approach to explaining the filling of orbitals?

The instructor used a step-by-step method to explain the filling of orbitals, starting from the lowest energy level and emphasizing the stability of half-full and full configurations.

How does the instructor encourage student interaction at the end of the lesson?

The instructor encourages student interaction by inviting them to write comments or questions in the comments section to ensure they understand the material.