Choose the orbital diagram that represents the ground state of N. Give the ground state electron configuration for Se.
[Ar]4s23d10p4
[Ar]4s24d10p4
[Ar]4s23d10p6
[Ar]4s23d10
[Ar]3d10p4
The correct answer and explanation is :
Let’s break this question into two parts.
1. Orbital Diagram for the Ground State of Nitrogen (N)
Nitrogen (N) has an atomic number of 7, meaning it has 7 electrons. The ground state electron configuration for nitrogen follows the Aufbau principle, Hund’s rule, and the Pauli exclusion principle.
- Electron Configuration of Nitrogen: 1s² 2s² 2p³.
This configuration tells us that nitrogen’s electrons fill the orbitals as follows:
- The 1s orbital holds 2 electrons.
- The 2s orbital holds 2 electrons.
- The 2p orbital holds 3 electrons.
Thus, for the orbital diagram of nitrogen, it would be represented as:
1s: ↑↓
2s: ↑↓
2p: ↑ ↑ ↑This diagram shows that nitrogen has 3 unpaired electrons in the 2p orbital, which is consistent with its chemical properties and position in the periodic table.
2. Ground State Electron Configuration for Selenium (Se)
Selenium (Se) has an atomic number of 34, so it has 34 electrons. To write the ground state electron configuration for selenium, we follow the same principles.
- The electron configuration of Se is: [Ar] 4s² 3d¹⁰ 4p⁴.
Here’s the breakdown:
- [Ar] refers to the electron configuration of Argon (18 electrons), which covers the first 18 electrons.
- After Argon, selenium’s remaining electrons are filled in the 4s, 3d, and 4p orbitals.
- The 4s orbital fills first, with 2 electrons.
- The 3d orbital then fills with 10 electrons.
- Finally, the 4p orbital fills with 4 electrons.
Thus, the full electron configuration for selenium is [Ar] 4s² 3d¹⁰ 4p⁴.
Conclusion
- The orbital diagram for nitrogen (N) would show 3 unpaired electrons in the 2p orbital.
- The electron configuration for selenium (Se) is [Ar] 4s² 3d¹⁰ 4p⁴, which places selenium in Group 16 of the periodic table, indicating it has 6 valence electrons (2 from 4s and 4 from 4p).