Answer:
The state of matter (whether a substance is a gas, liquid, or solid) at a given temperature depends on various factors, including intermolecular forces and molecular structure. In the case of carbon dioxide (CO2) and water (H2O), their different states at room temperature can be attributed to the following reasons:
Intermolecular forces: The strength of intermolecular forces between molecules plays a crucial role in determining the state of matter. In the case of CO2, it consists of one carbon atom bonded to two oxygen atoms (O=C=O). CO2 molecules are held together primarily by relatively weak London dispersion forces. These forces are formed due to temporary fluctuations in electron density, and they are generally weaker compared to other intermolecular forces. As a result, CO2 has weaker intermolecular attractions, allowing the molecules to move more freely and exist as a gas at room temperature.
Polarity and hydrogen bonding: In contrast, water (H2O) is a polar molecule with two hydrogen atoms bonded to one oxygen atom. The oxygen atom in water is more electronegative than hydrogen, resulting in a partial negative charge on the oxygen and partial positive charges on the hydrogen atoms. This polarity leads to stronger intermolecular attractions, including hydrogen bonding. Hydrogen bonding occurs when the partially positive hydrogen atom of one water molecule is attracted to the partially negative oxygen atom of another water molecule. Hydrogen bonding is a relatively strong intermolecular force, which contributes to the higher boiling point of water compared to CO2. These intermolecular attractions keep water molecules closer together and make it more difficult for them to overcome these forces, resulting in the liquid state of water at room temperature.
In summary, the difference in intermolecular forces, particularly the presence of hydrogen bonding in water, contributes to its higher boiling point and the liquid state at room temperature, despite its lower molecular weight compared to carbon dioxide
Step-by-step explanation: