At room temperature, 20° C, water (H2O) is a liquid and oxygen (O2) is a gas. Based on kinetic molecular theory, which answer best explains the states of the two fluids?
You listed no answers. But in there somewhere should be hydrogen bonding and/or intermolecular forces.
The kinetic molecular theory provides a helpful explanation for the states of matter based on the behavior of individual particles at the molecular level. According to this theory, the states of matter are determined by the motion and interaction of the particles in a substance.
In the case of water (H2O) and oxygen (O2), their states at room temperature, 20°C, can be explained as follows:
1. Water (H2O): Water exists as a liquid at room temperature due to the intermolecular forces between its molecules. The kinetic energy of the water molecules is sufficient to overcome these attractive forces, allowing the molecules to freely move and flow. The proximity of the molecules in a liquid state allows for intermolecular forces to hold them together, giving water its characteristic fluidity.
2. Oxygen (O2): Oxygen exists as a gas at room temperature because the kinetic energy of its molecules is high enough to overcome the intermolecular forces between them. In the gaseous state, the oxygen molecules move rapidly and independently, exhibiting a random motion. The weak intermolecular forces are not sufficient to hold the oxygen molecules close together, resulting in a gas that can easily expand and fill the container it is in.
In summary, the kinetic molecular theory explains that the states of water and oxygen at room temperature are determined by the balance between the kinetic energy of the molecules and the intermolecular forces. Water is a liquid due to stronger intermolecular forces, whereas oxygen is a gas due to weaker intermolecular forces.