Arrange the following compounds in order of their increasing solubility in water.
1) H3C - CH3
2) HO - OH
3) H3C - OH
put 2 last. 1,3,2
To determine the increasing solubility in water, we need to consider the polarity and ability to form hydrogen bonds with water.
The general trend for solubility in water is: polar compounds > compounds that can form hydrogen bonds > non-polar compounds.
Let's analyze each compound:
1) H3C - CH3 (Methane)
Methane is a non-polar compound consisting of carbon and hydrogen atoms. It has no polarity and cannot form hydrogen bonds. Therefore, it has low solubility in water.
2) HO - OH (Hydrogen Peroxide)
Hydrogen peroxide is a polar compound that can form hydrogen bonds with water. It has high solubility in water due to its ability to interact with the water molecules through hydrogen bonding.
3) H3C - OH (Methanol)
Methanol is a polar compound with an -OH group. It can form hydrogen bonds with water and has a higher solubility compared to non-polar compounds like methane.
Therefore, the increasing solubility in water from least to highest is:
1) H3C - CH3 (Methane)
2) H3C - OH (Methanol)
3) HO - OH (Hydrogen Peroxide)
To determine the solubility of compounds in water, we need to consider the type of intermolecular forces present in the compound. The stronger the intermolecular forces, the more soluble the compound will be in water.
Let's analyze each compound:
1) H3C-CH3 (Ethane)
Ethane is a nonpolar compound since it consists of only carbon and hydrogen atoms bonded by nonpolar carbon-carbon and carbon-hydrogen bonds. Nonpolar compounds generally exhibit weak London dispersion forces, which are weaker than the intermolecular forces in water. As a result, ethane is insoluble in water.
2) HO-OH (Hydrogen Peroxide)
Hydrogen peroxide is a polar compound with hydrogen bonding. Oxygen and hydrogen atoms within the molecule have significantly different electronegativities, creating a polar bond. This polarity allows hydrogen peroxide to form hydrogen bonds with water molecules. These strong hydrogen bonds increase its solubility in water.
3) H3C-OH (Methanol)
Methanol is also a polar compound due to the presence of an oxygen atom bonded to a carbon atom. Oxygen is more electronegative than carbon, creating a polar C-O bond. Methanol can form hydrogen bonds with water molecules due to the presence of a hydroxyl (-OH) group. These hydrogen bonds make methanol soluble in water.
Based on this analysis, we can rank the compounds in increasing order of solubility in water:
1) H3C-CH3 (Ethane) - Insoluble in water.
2) H3C-OH (Methanol) - Soluble in water.
3) HO-OH (Hydrogen Peroxide) - Highly soluble in water.