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Ionic compounds are not soluble in organic solvents as they cant dissociate. How are the non polar compounds soluble in organic solvents?
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Pál Váradi Nagy
Ionic compounds are not soluble in organic solvents as they cant dissociate. How are the non polar compounds soluble in organic solvents?
There are 2 main intermolecular forces.
First one is hydrogen bonding between molecules. It exists between polar solutes and polar solvents, but another force called dispersion (London). We may say dispersion force exists only in non polar solutes and non polar solvents. That’s what you want to know. It is almost like hydrogen bonding. But instead of Hydrogen, it can be other atoms. Nitrogen in a molecule to another atom maybe Oxygen or other atoms S and many more in another molecule. This dispersion force is weaker, but it takes over when there is no hydrogen- oxygen bonding only exist only in polar. When we say hydrogen bonding, it’s only between hydrogen and oxygen! But dispersion forces can be oxygen and other atoms. or two different other atoms. Remember no hydrogen bonding.
There are four major classes Ionic bonds > Hydrogen bonding > Van der Waals dipole-dipole interactions > Van der Waals dispersion forces.
First one is hydrogen bonding between molecules. It exists between polar solutes and polar solvents, but another force called dispersion (London). We may say dispersion force exists only in non polar solutes and non polar solvents. That’s what you want to know. It is almost like hydrogen bonding. But instead of Hydrogen, it can be other atoms. Nitrogen in a molecule to another atom maybe Oxygen or other atoms S and many more in another molecule. This dispersion force is weaker, but it takes over when there is no hydrogen- oxygen bonding only exist only in polar. When we say hydrogen bonding, it’s only between hydrogen and oxygen! But dispersion forces can be oxygen and other atoms. or two different other atoms. Remember no hydrogen bonding.
There are four major classes Ionic bonds > Hydrogen bonding > Van der Waals dipole-dipole interactions > Van der Waals dispersion forces.
Be careful how you ask the question, many ionic compounds can dissolve in polar organic compounds, but water is simply better at it than acetone or formic acid.
Mr. Bloom’s answer is a good start. Water is not only polar (like the organic solvents I mentioned but it is probably the strongest hydrogen-bond former of any liquid susbstance. Hydrogen bonds stabilize many solutions of polar compounds (which is why if you add 1 liter of methanol to 1 liter of water, you will get less than 2 liters of solution: the hydrogen bonds to water by methanol disrupts the hydrogen-bonded network of water and create space for them within the original molecular framework of the water. Extremely poor hydrogen bonders (like alkanes and aryl hydrocarbons) are quite insoluble, but smaller polar (e.g., alcohols) or ionizing (carboxylic acids and amines) are much more soluble. But the ionizing compounds are polar, so this goes beyond your original question.
The point is that bond polarity plays a strong role in many properties and reactions of organic compounds.
Be careful how you ask the question, many ionic compounds can dissolve in polar organic compounds, but water is simply better at it than acetone or formic acid.
Mr. Bloom’s answer is a good start. Water is not only polar (like the organic solvents I mentioned but it is probably the strongest hydrogen-bond former of any liquid susbstance. Hydrogen bonds stabilize many solutions of polar compounds (which is why if you add 1 liter of methanol to 1 liter of water, you will get less than 2 liters of solution: the hydrogen bonds to water by methanol disrupts the hydrogen-bonded network of water and create space for them within the original molecular framework of the water. Extremely poor hydrogen bonders (like alkanes and aryl hydrocarbons) are quite insoluble, but smaller polar (e.g., alcohols) or ionizing (carboxylic acids and amines) are much more soluble. But the ionizing compounds are polar, so this goes beyond your original question.
The point is that bond polarity plays a strong role in many properties and reactions of organic compounds.
There are 2 main intermolecular forces.
First one is hydrogen bonding between molecules. It exists between polar solutes and polar solvents, but another force called dispersion (London). We may say dispersion force exists only in non polar solutes and non polar solvents. That’s what you want to know. It is almost like hydrogen bonding. But instead of Hydrogen, it can be other atoms. Nitrogen in a molecule to another atom maybe Oxygen or other atoms S and many more in another molecule. This dispersion force is weaker, but it takes over when there is no hydrogen- oxygen bonding only exist only in polar. When we say hydrogen bonding, it’s only between hydrogen and oxygen! But dispersion forces can be oxygen and other atoms. or two different other atoms. Remember no hydrogen bonding.
There are four major classes Ionic bonds > Hydrogen bonding > Van der Waals dipole-dipole interactions > Van der Waals dispersion forces.
There are 2 main intermolecular forces.
First one is hydrogen bonding between molecules. It exists between polar solutes and polar solvents, but another force called dispersion (London). We may say dispersion force exists only in non polar solutes and non polar solvents. That’s what you want to know. It is almost like hydrogen bonding. But instead of Hydrogen, it can be other atoms. Nitrogen in a molecule to another atom maybe Oxygen or other atoms S and many more in another molecule. This dispersion force is weaker, but it takes over when there is no hydrogen- oxygen bonding only exist only in polar. When we say hydrogen bonding, it’s only between hydrogen and oxygen! But dispersion forces can be oxygen and other atoms. or two different other atoms. Remember no hydrogen bonding.
There are four major classes Ionic bonds > Hydrogen bonding > Van der Waals dipole-dipole interactions > Van der Waals dispersion forces.
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Be careful how you ask the question, many ionic compounds can dissolve in polar organic compounds, but water is simply better at it than acetone or formic acid.
Mr. Bloom’s answer is a good start. Water is not only polar (like the organic solvents I mentioned but it is probably the strongest hydrogen-bond former of any liquid susbstance. Hydrogen bonds stabilize many solutions of polar compounds (which is why if you add 1 liter of methanol to 1 liter of water, you will get less than 2 liters of solution: the hydrogen bonds to water by methanol disrupts the hydrogen-bonded network of water and create space for them within the original molecular framework of the water. Extremely poor hydrogen bonders (like alkanes and aryl hydrocarbons) are quite insoluble, but smaller polar (e.g., alcohols) or ionizing (carboxylic acids and amines) are much more soluble. But the ionizing compounds are polar, so this goes beyond your original question.
The point is that bond polarity plays a strong role in many properties and reactions of organic compounds.
Be careful how you ask the question, many ionic compounds can dissolve in polar organic compounds, but water is simply better at it than acetone or formic acid.
Mr. Bloom’s answer is a good start. Water is not only polar (like the organic solvents I mentioned but it is probably the strongest hydrogen-bond former of any liquid susbstance. Hydrogen bonds stabilize many solutions of polar compounds (which is why if you add 1 liter of methanol to 1 liter of water, you will get less than 2 liters of solution: the hydrogen bonds to water by methanol disrupts the hydrogen-bonded network of water and create space for them within the original molecular framework of the water. Extremely poor hydrogen bonders (like alkanes and aryl hydrocarbons) are quite insoluble, but smaller polar (e.g., alcohols) or ionizing (carboxylic acids and amines) are much more soluble. But the ionizing compounds are polar, so this goes beyond your original question.
The point is that bond polarity plays a strong role in many properties and reactions of organic compounds.
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