Why is water a liquid but carbon dioxide a gas at room temperature.
Well i believe it is bc H20 needs alot of energy to bc a gas bc of the molecular bonds on it, while CO2 requires less energy to become a gas so that is why it becomes a gas at room temp
I suspect this a question aimed at hydrogen bonds. The water molecule is capable of hydrogen bonding. Thus additional energy above that required to separate the molecules due to van der waals forces is needed in the case of water. This additional energy is reflected in the higher bp of water when compared to carbon dioxide.
This question also comes up when describing phase diagrams, if you are working on these then let us know.
Water is a liquid at room temperature because of its unique molecular structure and intermolecular forces. To understand this, we must examine the differences between water (H2O) and carbon dioxide (CO2) at the molecular level.
The water molecule consists of two hydrogen atoms covalently bonded to one oxygen atom. This molecular structure results in a bent or V-shape configuration, with the oxygen atom at the center and the hydrogen atoms forming an angle of about 104.5 degrees. This bent structure creates a polar molecule, with the oxygen atom having a slight negative charge and the hydrogen atoms having slight positive charges. This polarity leads to strong intermolecular forces, specifically hydrogen bonding, between neighboring water molecules.
On the other hand, the carbon dioxide molecule consists of one carbon atom double-bonded to two oxygen atoms. This linear molecular structure results in a non-polar molecule, with no significant charge separation. As such, the intermolecular forces between carbon dioxide molecules are weak van der Waals forces.
The strength of intermolecular forces determines the state of matter a substance will exist in at a given temperature. In the case of water, the strong hydrogen bonds between molecules allow them to stick together relatively tightly. These hydrogen bonds require a significant amount of energy to break, which is why water is a liquid at room temperature. The hydrogen bonds restrict the movement of water molecules, causing them to remain condensed and flow as a liquid.
In contrast, carbon dioxide molecules have weaker intermolecular forces, resulting in a lower boiling point and the ability to transition directly from a solid to a gas (sublimation) at room temperature. Carbon dioxide molecules have more freedom of movement due to the weak van der Waals forces between them, allowing them to escape the liquid phase and become a gas.
In summary, the different molecular structures and intermolecular forces of water and carbon dioxide determine their states of matter at room temperature. Water's polar nature and stronger hydrogen bonds result in a liquid state, whereas carbon dioxide's non-polar nature and weaker intermolecular forces allow it to exist as a gas.