Question

Unlike carbon, which can form extended chains of atoms, nitrogen can form chains of very limited length. Draw the Lewis electron dot structure of the azide ion, \(\mathrm{N}_{3}^{-} .\) Is the ion linear or bent?

Short answer

The azide ion \( \mathrm{N}_{3}^{-} \) is linear.

Step-by-step solution

Count Total Valence Electrons

The azide ion \( \text{N}_3^- \) is composed of three nitrogen atoms, each of which has 5 valence electrons. Since the ion carries a charge of \(-1\), we must add one additional electron to the total. Thus, the total valence electron count is \( 3 \times 5 + 1 = 16 \) electrons.

Arrange Atoms and Draw Initial Structure

In the azide ion, the nitrogen atoms will be arranged in a chain form: \( \text{N} - \text{N} - \text{N} \). Start by placing two electrons (a single bond) between each pair of nitrogen atoms, using \( 4 \) of the \( 16 \) available electrons.

Distribute Remaining Electrons

After forming single bonds, \( 12 \) electrons remain. Place them around the nitrogen atoms to complete their octets. Start by adding electrons to the outer nitrogen atoms (terminal nitrogens). Distribute them as follows: \( \text{N:} \ 6\ electrons, \text{N} - \text{N} - \text{N:} \ 6\ electrons \).

Check Octets and Form Multiple Bonds

Ensure each nitrogen atom has 8 electrons. Find that the central nitrogen (middle) only has 4 electrons. Rearrange by creating multiple bonds. Convert lone pairs from terminal nitrogens into double bonds. The final structure will be: \( \text{:N}\equiv\text{N}^+-\text{N}^-:\).

Verify Formal Charges

Calculate formal charges to ensure they sum to \(-1\). The left nitrogen has a charge of 0, the central nitrogen has a charge of +1, and the right nitrogen has a charge of -2. Thus, \( 0 + 1 - 2 = -1 \), which is correct for the azide ion.

Determine Molecular Geometry

The azide ion \( \text{N}_3^- \) has two double bonds on the central nitrogen, with no lone pairs, resulting in a linear shape. This is consistent with the VSEPR theory, which predicts a linear shape for systems with two bond pairs and no lone pairs on the central atom.

Key concepts

Azide Ion

The azide ion, represented as \( \text{N}_3^- \), is an interesting anion in chemistry primarily because of its linear configuration and the unique bonding of nitrogen atoms. Nitrogen, being in group 15 of the periodic table, does not typically form long chains. However, in the azide ion, three nitrogen atoms are linked.
This is possible due to the presence of three nitrogen atoms, which must accommodate additional electrons due to its negative charge.

• The azide ion has a characteristic linear structure.
• It involves a central nitrogen atom making multiple bonds with two terminal nitrogen atoms.
• The ion carries a net charge of \(-1\).

Understanding the azide ion's structure is important, as it gives insights into how nitrogen atoms can bond in specific conditions and influence compounds, like certain explosives.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in forming chemical bonds. In the case of the azide ion \( \text{N}_3^- \), counting the valence electrons is the starting point to draw its Lewis structure.
Each nitrogen atom has five valence electrons because it is in group 15 of the periodic table. For the azide ion:

• Three nitrogen atoms contribute \( 3 \times 5 = 15 \) electrons.
• An additional electron is added because of the \(-1\) charge, totaling 16 valence electrons.

The correct distribution of these valence electrons among the nitrogen atoms is key to drawing a stable Lewis electron dot structure, ensuring that both the octet rule is fulfilled and the ion's stability is maximized.

Formal Charges

Formal charges play a crucial role in determining the most stable Lewis structure for ions and molecules. They help in understanding the distribution of electrons among atoms in a molecule and in predicting possible resonance structures.
To calculate the formal charge on an atom:

• Start with the number of valence electrons in the free atom.
• Subtract the number of lone pair electrons.
• Subtract half the number of bonding electrons (shared in bonds).

In the azide ion, the formal charges were calculated to confirm stability:

• The leftmost nitrogen has a formal charge of 0.
• The central nitrogen carries a charge of +1.
• The rightmost nitrogen has a charge of -2.

These add up correctly to \(-1\), confirming the electron distribution aligns with the ion's charge. The calculation of formal charges ensures that the resonance structure chosen is not only possible but also the most energetically favorable.

Molecular Geometry

Molecular geometry concerns the three-dimensional arrangement of atoms within a molecule and influences the chemical reactivity and properties of the compound.
For the azide ion \( \text{N}_3^- \), its geometry is derived from the number of bonds and lone pairs around the central nitrogen atom, analyzed through the Valence Shell Electron Pair Repulsion (VSEPR) theory.
The azide ion's linear shape comes from:

• Two double bonds without any lone pairs on the central atom.
• Predicts a 180-degree angle between the atoms resulting in a linear form.

Understanding the geometry aids in predicting how the azide ion might interact with other entities in chemical reactions. The linear shape ensures direct alignment, potentially influencing how and where reactions occur.