Determine the molecular geometry about each interior atom and sketch each molecule. a. N₂

Verified step by step guidance

1. Identify the type of atoms and the number of bonds: In N₂, there are two nitrogen atoms bonded together.
2. Determine the type of bond between the nitrogen atoms: Nitrogen typically forms a triple bond with another nitrogen atom in N₂.
3. Apply the VSEPR theory: Since there are no lone pairs on either nitrogen atom and only a triple bond, the molecular geometry is linear.
4. Sketch the molecule: Draw two nitrogen atoms connected by three lines (representing the triple bond) in a straight line.
5. Conclude the geometry: The molecular geometry around each nitrogen atom in N₂ is linear due to the triple bond and absence of lone pairs.

Key Concepts

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences the shape of the molecule. Understanding molecular geometry is crucial for predicting the physical and chemical properties of substances.

VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs in the valence shell of the central atom. According to VSEPR, electron pairs will arrange themselves as far apart as possible to minimize repulsion, leading to specific molecular shapes such as linear, trigonal planar, or tetrahedral.

Diatomic Molecules

Diatomic molecules consist of two atoms, which can be of the same or different elements. In the case of nitrogen (N2), both atoms are nitrogen, and the molecule is linear due to the absence of lone pairs and the presence of a triple bond between the two nitrogen atoms. Understanding the characteristics of diatomic molecules is essential for analyzing their behavior and properties.