Because carbon and hydrogen have very similar electronegativity, the C-H bonds in CH3CH2CH3 are not very polar and it has a very small dipole moment and therefore weak dipole-dipole forces.
Ionic bonds are stronger than dipole-dipole attractions, hence NaF has the stronger attraction between particles. c. The formula NH3 represents a molecular substance possessing N-H bonds, ie a polar molecular compound with hydrogen bonds between molecules (enhanced by London forces).
But CH3CH2OH alone has hydrogen bonds that are much stronger than the intermolecular forces active in the other options. The boiling points of the hydrogen halides are listed below.
The intermolecular forces of CH3Cl have dipole-dipole forces and London dispersion forces. the chemical name of CH3Cl is chloromethane.
Answer and explanation: The F2 molecule has the lowest boiling point here because it exhibits van der Waals force. In contrast, NaF has the highest boiling point since it is a… See full answer below.
Quick answer: The main “IMF” in hydrogen fluoride (HF) is hydrogen bonding (since hydrogen is bonded to fluorine). Since the molecule is polar, there are also dipole-dipole forces in addition to the London dispersion forces (Van der Waals forces).
1. CH3CH2OH is completely water soluble. It can form hydrogen bonds with water and its hydrocarbon content is small.
The particularly strong intermolecular forces in ethanol are the result of a special class of dipole-dipole forces called hydrogen bonds.
In dimethyl ether (CH3−O−CH3) no H atoms are directly bonded to O and therefore no H bonding is possible in ethers.
1. Which intermolecular forces act in CH3Cl(s)? C, so dipole-dipole forces will be present.
CHCl3 is a polar molecule while CCl4 is a non-polar molecule. Dipole forces are the dominant intermolecular attractive forces between CHCl3 molecules, while the dominant intermolecular attractive forces within CCl4 molecules are London forces.
The hydrogen bonding propensities exhibited by the C-H protons in CHCl3 and CH2Cl2 are similar to those of the acetylenic C-C≡C-H proton. However, the participation of the Cl atoms of CHCl3 and CH2Cl2 in non-bonded interactions is rather limited: the propensity to form (O or N)-H…
HF is a polar molecule: dipole-dipole forces. Hydrogen is bonded to F. There are hydrogen bonds. There are also dispersive forces between HBr molecules.
The reason NaF would have the highest melting point is because if you look at the electronegativity values, fluorine has the highest and thus has the greatest attraction for the electrons in the ionic bond, making for a really strong sodium positive leads -ion and a strongly negative fluorine ion, which …
In HF each molecule has a hydrogen atom that can form a hydrogen bond and there are three lone pairs of electrons on the fluorine atom. The total number of hydrogen bonds is limited by the number of hydrogen atoms, and on average each HF molecule participates in two hydrogen bonds.
Yes, it’s true, dipole forces also occur between two ethanol molecules. here I am talking about the intraction between two dipoles in ethanol molecules. one dipole is carbon and another dipole is oxygen.