How many electrons are unpaired in the orbitals of nitrogen?
The correct answer and explanation is:
The correct answer is: 3 unpaired electrons
Explanation:
To determine the number of unpaired electrons in nitrogen, we must examine its electron configuration and orbital diagram.
Step 1: Atomic Number of Nitrogen
Nitrogen has an atomic number of 7, which means it has 7 electrons in a neutral atom.
Step 2: Electron Configuration
The electron configuration of nitrogen is:
1s² 2s² 2p³
This means:
- Two electrons fill the 1s orbital.
- Two electrons fill the 2s orbital.
- Three electrons occupy the 2p orbitals.
Step 3: Filling the 2p Orbitals
The 2p subshell has three orbitals: 2px, 2py, and 2pz. According to Hund’s Rule, electrons will fill these orbitals singly before pairing up.
So, the 2p electrons are distributed as:
- 1 electron in 2px
- 1 electron in 2py
- 1 electron in 2pz
Each of these orbitals contains 1 unpaired electron, resulting in three unpaired electrons.
Orbital Diagram:
1s: ↑↓
2s: ↑↓
2p: ↑ ↑ ↑
px py pz
Each arrow represents an electron. Since the 2p orbitals each have a single electron with parallel spins, all three are unpaired.
Conclusion:
Nitrogen has 3 unpaired electrons in its ground-state electron configuration. This configuration explains several chemical properties of nitrogen, including its paramagnetism (attraction to a magnetic field) and its ability to form three covalent bonds, as seen in molecules like ammonia (NH₃).
Understanding the number of unpaired electrons is essential in predicting the magnetic behavior, reactivity, and bonding characteristics of an atom in chemistry.