Answer :
It seems there might be a typo in the given molecules. Usually, the chemical formulas are recognized in certain formats. For this answer, I'll assume the following correct notations for the molecules provided:
- CH₄ (methane)
- F₂ (fluorine)
- CH₃OH (methanol)
- H₂O (water)
Now, let's evaluate the type and strength of intermolecular forces present in each of these molecules to determine which has the weakest intermolecular forces.
1. CH₄ (Methane): Methane is a nonpolar molecule due to the symmetry and equal distribution of charges around the carbon atom. The only type of intermolecular forces it experiences are London dispersion forces (also known as Van der Waals forces), which are typically weak and arise due to the temporary dipole moments induced when electrons move around the molecule.
2. F₂ (Fluorine): Fluorine is a diatomic molecule composed of two fluorine atoms. Like methane, it is nonpolar and the intermolecular forces between fluorine molecules are London dispersion forces. Although these forces are weak in general, they can be slightly stronger in fluorine when compared to methane because of the larger number of electrons in fluorine that can create temporary dipoles.
3. CH₃OH (Methanol): Methanol contains a polar O-H bond, making the molecule polar overall. The polarity of methanol allows for stronger dipole-dipole interactions between molecules. Additionally, it can form hydrogen bonds because of the presence of the hydroxyl (-OH) group, making its intermolecular forces much stronger than those of nonpolar molecules.
4. H₂O (Water): Water is a well-known polar molecule with two hydrogen atoms and one oxygen atom, where the oxygen atom is more electronegative, pulling the shared electron density towards itself and creating a dipole. Water molecules can form multiple hydrogen bonds (each water molecule can form up to four hydrogen bonds), which are considerably stronger compared to other intermolecular forces like London dispersion forces or general dipole-dipole interactions.
Given these considerations, CH₄ would have the weakest intermolecular forces. It is nonpolar, meaning it lacks dipole-dipole interactions, and does not have the ability to form hydrogen bonds, so it relies solely on temporary London dispersion forces for interaction with other methane molecules.
- CH₄ (methane)
- F₂ (fluorine)
- CH₃OH (methanol)
- H₂O (water)
Now, let's evaluate the type and strength of intermolecular forces present in each of these molecules to determine which has the weakest intermolecular forces.
1. CH₄ (Methane): Methane is a nonpolar molecule due to the symmetry and equal distribution of charges around the carbon atom. The only type of intermolecular forces it experiences are London dispersion forces (also known as Van der Waals forces), which are typically weak and arise due to the temporary dipole moments induced when electrons move around the molecule.
2. F₂ (Fluorine): Fluorine is a diatomic molecule composed of two fluorine atoms. Like methane, it is nonpolar and the intermolecular forces between fluorine molecules are London dispersion forces. Although these forces are weak in general, they can be slightly stronger in fluorine when compared to methane because of the larger number of electrons in fluorine that can create temporary dipoles.
3. CH₃OH (Methanol): Methanol contains a polar O-H bond, making the molecule polar overall. The polarity of methanol allows for stronger dipole-dipole interactions between molecules. Additionally, it can form hydrogen bonds because of the presence of the hydroxyl (-OH) group, making its intermolecular forces much stronger than those of nonpolar molecules.
4. H₂O (Water): Water is a well-known polar molecule with two hydrogen atoms and one oxygen atom, where the oxygen atom is more electronegative, pulling the shared electron density towards itself and creating a dipole. Water molecules can form multiple hydrogen bonds (each water molecule can form up to four hydrogen bonds), which are considerably stronger compared to other intermolecular forces like London dispersion forces or general dipole-dipole interactions.
Given these considerations, CH₄ would have the weakest intermolecular forces. It is nonpolar, meaning it lacks dipole-dipole interactions, and does not have the ability to form hydrogen bonds, so it relies solely on temporary London dispersion forces for interaction with other methane molecules.
