0
What else can I help you with?
What is the strongest intermolecular force present in ammonia?
The strongest intermolecular force in ammonia is hydrogen bonding. This occurs because the nitrogen atom in ammonia can form a hydrogen bond with a hydrogen atom from another ammonia molecule, resulting in a relatively strong attraction between the molecules.
What is the predominant intermolecular force of methane ammonia nitrogen triflouride?
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
Is acetone and water are miscible?
yes Regarding intermolecular forces, acetone has the chemical formula C3H60, through Hydrogen Bonds, the partial positive charge of Hydrogen in acetone is attracted to the partial negative charge of Oxygen in water. Also, inversely the Hydrogen in water is attracted to the Oxygen in Acetone. A dipole-dipole bond is also formed between the two substances due to the difference in charges. They there fore have an affinity for one another, and to be separated (as an example through fractional or simple distillation) the dipole dipole bonds and hydrogen bonds would need to be broken.
What are the type of intermolecular force present in AlH3?
AlH3 alane is a covalent solid and is a giant molecule, so no intermolecular forces will be present. Planar AlH3 molecules have been isolated at very low temperatures. AlH3 molecules would be predicted to have no dipole moment due to their shape. The only intermolecular forces would be London dispersion forces.
What kind of intermolecular forces are present in CS2?
Dipole forces and London forces are present between these molecules.
What is the inter molecular force in Acetone?
The intermolecular force in acetone (CH3COCH3) is dipole-dipole interaction. This is because acetone contains a carbonyl group that creates a partial negative charge on the oxygen atom and a partial positive charge on the carbon atom, leading to attraction between different acetone molecules.
What type of intermolecular force is acetone?
Acetone exhibits dipole-dipole interactions and London dispersion forces. The oxygen in the carbonyl group of acetone creates a partial negative dipole, while the carbon and hydrogen atoms exhibit London dispersion forces.
What is the force of attrction called?
intermolecular force
What kind of of force is dipole-dipole force?
This is an intermolecular force.
Why do mixtures of acetone and chloroform exhibit significant negative deviations from Raoult's law?
Mixtures of acetone and chloroform exhibit negative deviations from Raoult's law because the molecules of acetone and chloroform have different intermolecular interactions. Acetone forms stronger intermolecular interactions with chloroform than with itself, leading to a decrease in vapor pressure and lower than expected boiling point. This results in the formation of more stable mixed solvent molecules, causing negative deviations from Raoult's law.
What is the major force that governs the interaction between acetone and chloroform?
The major force that governs the interaction between acetone and chloroform is dipole-dipole interactions.
What is the source of intermolecular force?
Gravity!
Is high vapor boiling point a week intermolecular force?
Boiling point is a property not a force; but a high boiling point indicate a strong intermolecular force.
Which kind of force is a dipole -dipole force?
Intermolecular attraction
What is the intermolecular force of Ar?
The intermolecular force in Ar (argon) is London dispersion forces, which are the weakest type of intermolecular force. This force is caused by temporary fluctuations in electron distribution around the atom, leading to temporary dipoles.
What interaction is not a type of intermolecular force?
Intramolecular forces are not intermolecular forces !
Why acetone evaporates faster than chloroform and benzene?
Acetone evaporates faster than chloroform and benzene because it has a lower boiling point and higher vapor pressure. This means acetone molecules have more kinetic energy, allowing them to overcome intermolecular forces and escape into the air more readily. Chloroform and benzene have stronger intermolecular forces, requiring more energy to break these bonds and evaporate.
