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Methanol, CH3OH (CH4O) is a covalent molecular compound. It is liquid under normal conditions and there is hydrogen bonding between molecules
hydrogen fluoride Alcohols like methanol, ethanol. Solvents like dimethyl formamide (DMF) or dimethyl sulfoxide (DMSO)
it has hydrogen bond (H-O)
Generally speaking 'like dissolves like' so when you thinking if a molecule can dissolve in a particular solvent, you need to decide what type of bonding that solvent can exhibit and what bonding the molecule in question exhibits. So for example water can exhibit hydrogen bonding. This means for something to be able soluble in water, it too needs to be able to exhibit hydrogen bonding. Methane only contains hydrogen and carbon and thus, will not exhibit hydrogen bonding. However, methanol has carbon, hydrogen and oxygen and therefore, can exhibit hydrogen bonding. As a result, using the 'like dissolve like' approach we can see why methane will be insoluble in water but methanol will be soluble.
The polar group -OH of ethanol is bonded to water by hydrogen bonds.
Methanol, CH3OH (CH4O) is a covalent molecular compound. It is liquid under normal conditions and there is hydrogen bonding between molecules
Hygroscopic substances include cellulose fiber such as ethanol, methanol and diesel fuel. As hydrogen bonding causes pure ethanol to readily absorbs water from the air, ethanol is considered to be hygroscopic.
hydrogen fluoride Alcohols like methanol, ethanol. Solvents like dimethyl formamide (DMF) or dimethyl sulfoxide (DMSO)
Methanol because the longer the side chains the less polar it becomes
Methanol and ethanol differ only by one carbon and 2 hydrogens. Both have the hydroxyl group and, thus, have hydrogen bonding and dipole-dipole interactions. What makes them different are their London forces (London forces are directly proportional to the number of electrons in a molecule and molecular size). Since methanol is smaller than ethanol, there is a smaller intermolecular London force. Less force holing the molecules together means they're easier to be pulled apart, which implies a lower boiling point.
it has hydrogen bond (H-O)
Hydrogen bond form the intermolecular forces in methyl alcohol. That's the reason why methyl alcohol is soluble in water.
Ethanol has intermolecular hydrogen bonding where as diethylether does not have this kind of bonding. So BP of ethanol is higher than diethylether.
Generally speaking 'like dissolves like' so when you thinking if a molecule can dissolve in a particular solvent, you need to decide what type of bonding that solvent can exhibit and what bonding the molecule in question exhibits. So for example water can exhibit hydrogen bonding. This means for something to be able soluble in water, it too needs to be able to exhibit hydrogen bonding. Methane only contains hydrogen and carbon and thus, will not exhibit hydrogen bonding. However, methanol has carbon, hydrogen and oxygen and therefore, can exhibit hydrogen bonding. As a result, using the 'like dissolve like' approach we can see why methane will be insoluble in water but methanol will be soluble.
Yes, Hydrogen bonding is a hydrogen bonded to any Fluorine, Nitrogen or Oxygen.
The polar group -OH of ethanol is bonded to water by hydrogen bonds.
(ch3)3n