Question

Using the periodic table, draw Bohr-Rutherford Diagrams of each of the elements (one atom) before bonding. Then draw the NH3 molecule indicating all the shared electrons as either dots or crosses (as Xs), paying close attention to the valence electrons. Indicate whether the formation of ammonia is an ionic or a covalent bond and explain your reasoning.

Answer 1

The Bohr-Rutherford diagrams illustrate the electron arrangement in nitrogen (N) and hydrogen (H). The Lewis structure for NH₃ shows a covalent bond with shared electrons, reflecting the molecular bonding in ammonia.

1. **Bohr-Rutherford Diagrams:**

- **Nitrogen (N):**

- Atomic number of N: 7

- Bohr-Rutherford diagram: Show 7 electrons in orbits around the nucleus.

- **Hydrogen (H):**

- Atomic number of H: 1

- Bohr-Rutherford diagram: Show 1 electron in orbit around the nucleus.

2. **Lewis Structure for NH₃:**

- Nitrogen needs three more electrons to achieve a full valence shell.

- Each hydrogen provides one electron.

- Draw Nitrogen (N) with three dots around it, each representing a shared electron from a hydrogen atom.

Lewis Structure:

H H

\ /

N

3. **Bonding Type:**

- In ammonia (NH₃), the bond formed between nitrogen and hydrogen is a **covalent bond**.

- Covalent bonds involve the sharing of electrons between atoms.

The Lewis structure clearly shows the shared electrons between nitrogen and hydrogen atoms, confirming the covalent nature of the bond in ammonia.