Photo AI
Show, using dot and cross diagrams, the bond formation in a nitrogen molecule - Leaving Cert Chemistry - Question Question 1 - 2004
Question Question 1
Show, using dot and cross diagrams, the bond formation in a nitrogen molecule. Describe the bonding in the nitrogen molecule in terms of sigma ($ ext{σ}$) and pi ($ ... show full transcript
Worked Solution & Example Answer:Show, using dot and cross diagrams, the bond formation in a nitrogen molecule - Leaving Cert Chemistry - Question Question 1 - 2004
Step 1
Show, using dot and cross diagrams, the bond formation in a nitrogen molecule.
Answer
To illustrate the bond formation in a nitrogen molecule (N₂), we can use dot and cross diagrams:
- Each nitrogen atom has five valence electrons.
- The diagram can be represented as:
*N≡N*
In this representation, the dots represent valence electrons from one nitrogen atom, and the crosses represent valence electrons from the other nitrogen atom.
- In total, there are three electrons shared between the two atoms, indicating a triple bond, which consists of one sigma bond and two pi bonds.
Step 2
Describe the bonding in the nitrogen molecule in terms of sigma (σ) and pi (π) bonding.
Answer
The nitrogen molecule exhibits:
- One Sigma Bond (σ): The sigma bond in N₂ is formed by the head-on overlap of two sp³ hybrid orbitals from each nitrogen atom. This bonding involves sharing two electrons, which allows for the initial connectivity between the nitrogen atoms.
- Two Pi Bonds (π): The additional two bonds are pi bonds, formed by the side-to-side overlap of the unhybridized p orbitals from each nitrogen atom. These pi bonds exist above and below the plane of the atoms, creating a strong triple bond that stabilizes the molecule.
Step 3
What type of intermolecular forces would you expect to find in nitrogen gas? Explain your answer.
Answer
In nitrogen gas (N₂), the expected type of intermolecular forces are:
- Van der Waals / London Dispersion Forces: These forces are typically weak and arise due to temporary fluctuations in electron density that create instantaneous dipoles in adjacent molecules.
- Since nitrogen is a non-polar molecule, these intermolecular forces are the only significant interactions occurring between nitrogen gas molecules. The forces are temporary and non-permanent, resulting from the movement of electrons and their effect on the electron cloud.