1. Electronic Configuration:
* Nitrogen has an atomic number of 7, meaning it has 7 electrons.
* The electronic configuration for nitrogen is 1s² 2s² 2p³
2. Orbital Diagram:
* 1s orbital: This orbital can hold up to 2 electrons. Represent it with a box: [1s]
- Fill the box with two arrows pointing up and down (↑↓) to represent the two electrons.
- [1s] ↑↓
* 2s orbital: This orbital also holds up to 2 electrons.
- [2s] ↑↓
* 2p orbitals: There are three 2p orbitals (2px, 2py, 2pz), each of which can hold up to 2 electrons.
- Represent each with a box: [2px] [2py] [2pz]
- Place one electron in each 2p orbital with the same spin (↑). This is called Hund's rule, which states that electrons will occupy orbitals individually before pairing up.
- [2px] ↑ [2py] ↑ [2pz] ↑
Complete Orbital Diagram for Nitrogen:
[1s] ↑↓ [2s] ↑↓ [2px] ↑ [2py] ↑ [2pz] ↑
Key Points:
* Aufbau Principle: Electrons fill orbitals in order of increasing energy.
* Hund's Rule: Electrons will occupy orbitals individually before pairing up.
* Pauli Exclusion Principle: No two electrons in an atom can have the same set of four quantum numbers. This means each orbital can hold a maximum of two electrons, with opposite spins.
