Bohr-Rutherford diagrams for nitrogen and hydrogen show their electron distributions. The Lewis structure for NH₃ illustrates covalent bonding through shared electrons, making ammonia a covalent compound with nitrogen and hydrogen.
Bohr-Rutherford diagrams represent the distribution of electrons in an atom. For simplicity, let's consider the Bohr-Rutherford diagrams for nitrogen (N) and hydrogen (H) before bonding:
1. **Bohr-Rutherford Diagram for Nitrogen (N):**
- Nitrogen has an atomic number of 7.
- The first energy level (K) has 2 electrons, and the second energy level (L) has 5 electrons.
\[ \text{N: } \, \circ \, \circ \, \circ \, \circ \, \circ \, \circ \, \circ \]
2. **Bohr-Rutherford Diagram for Hydrogen (H):**
- Hydrogen has an atomic number of 1.
- The first energy level (K) has 1 electron.
\[ \text{H: } \, \circ \]
Now, let's draw the Lewis structure for ammonia (NH₃):
3. **Lewis Structure for NH₃:**
- Nitrogen (N) contributes 3 valence electrons.
- Each hydrogen (H) contributes 1 valence electron.
- The total number of valence electrons is 5 (from N) + 3 (from 3H) = 8.
\[ \text{NH₃: } \, \circ \, \underset{\times}{\text{N}} \, \, \, \, \, \, \underset{\times}{\text{H}} \, \, \, \, \, \, \, \underset{\times}{\text{H}} \]
The shared pairs of electrons are represented by lines or crosses (Xs).
**Formation of Ammonia (NH₃):**
- Ammonia (NH₃) forms through covalent bonding.
- Covalent bonds involve the sharing of electrons between nonmetals.
- Nitrogen and hydrogen are both nonmetals, and the sharing of electrons occurs to achieve a stable electron configuration.
Therefore, the formation of ammonia (NH₃) involves covalent bonding.