In a single molecule of CH4 you would have intramolecular forces that are covalent bonds. The intermolecular forces that exist between molecules of CH4 are called dispersion forces. These forces are the only intermolecular forces that occur between non-polar molecules.
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
It takes more heat to vaporize 12 grams of CH4 (methane) compared to 12 grams of Hg (mercury) because methane has weaker intermolecular forces and a lower boiling point. This means more energy is required to break the bonds between methane molecules to allow them to vaporize. Mercury has stronger intermolecular forces, so it requires less energy to vaporize.
Molecular formula: CH4 Structural formula: . H H C H . H CH4 (1 carbon and 4 hydrogen) it is NOT ch4 it is CH4; 4 being a subscript indicating 4 hydrogen atoms bonded into a single carbon atom
Formula: CH4
The compound CH4OH is called methanol. It is a type of alcohol often used as a solvent or fuel source.
The intermolecular forces in CH4 (methane) are London dispersion forces. Methane molecules are non-polar, so the only type of intermolecular force present is the weak temporary dipole-induced dipole interactions between molecules.
CH4 is a molecular solid. In this solid form, methane molecules are held together by intermolecular forces, such as Van der Waals forces, to form a solid structure.
Yes, CH4 (methane) does exhibit London dispersion forces due to temporary fluctuations in electron distribution around the molecule. These dispersion forces are the weakest intermolecular forces and are responsible for the non-polar nature of methane.
no
CH4 is not a polar compound.So it does exihibits london forces
CHF3 is a polar molecule. The fluorine atoms are electronegative and draw electrons towards their end of the molecule, leaving the hydrogen with a slight positive charge on it. So dipole-dipole forces will act between the molecules. The molecules will also exert dispersion forces on each other, but these are much weaker than the dipole-dipole forces.
CH4 (methane) is a nonpolar molecule, therefore its intermolecular forces are London dispersion forces. This is due to the temporary shifting of electron density within the molecule, creating weak attractions between neighboring molecules.
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
Metahne does not have a higher boiling point than methane. Fluoromethane, CH3F, has a boiling point of 195K, -78.2C, methane, CH4, has a boiling point of 109K approx -164 C. I make that fluoromethane has a higher temeprature boiling point than methane. This is what you would expect, London dispersion forces will be greater in CH3F as it has more electrons than CH4. CH3F is polar and there will be dipole dipole interactions which will not be present in CH4.
Ammonia (NH3) has hydrogen bonding intermolecular forces, whereas methane (CH4) does not. In addition, ammonia is polar, and so also has dipole-dipole forces and methane does not. Thus, it takes more energy (higher temperature) to boil and melt ammonia than it does methane.
It takes more heat to vaporize 12 grams of CH4 (methane) compared to 12 grams of Hg (mercury) because methane has weaker intermolecular forces and a lower boiling point. This means more energy is required to break the bonds between methane molecules to allow them to vaporize. Mercury has stronger intermolecular forces, so it requires less energy to vaporize.
Ethanol (C2H5OH) has a higher boiling point than methane (CH4) because it has stronger intermolecular forces, specifically hydrogen bonding, which requires more energy to overcome and boil. This results in a higher boiling point for ethanol compared to methane.