Briefly explain london dispersion forces.
The London dispersion force is the weakest intermolecular force. The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. This force is sometimes called an induced dipole-induced dipole attraction. London forces are the attractive forces that cause nonpolar substances to condense to liquids and to freeze into solids when the temperature is lowered sufficiently.
Because of the constant motion of the electrons, an atom or molecule can develop a temporary (instantaneous) dipole when its electrons are distributed unsymmetrically about the nucleus.
A second atom or molecule, in turn, can be distorted by the appearance of the dipole in the first atom or molecule (because electrons repel one another) which leads to an electrostatic attraction between the two atoms or molecules.
Dispersion forces are present between any two molecules (even polar molecules) when they are almost touching.
Molecular Size
Dispersion forces are present between all molecules, whether they are polar or nonpolar.
London dispersion forces tend to be:
Molecular Shape
The shapes of molecules also affect the magnitudes of dispersion forces between them.
Which of the following statements about London dispersion forces is/are true? Group of answer choices London dispersion forces are stronger between molecules of 1-butanol than between molecules of 2-methyl-2-propanol. London dispersion forces are stronger than hydrogen bonding interactions. both a and b neither a nor b How many different alkene products (counting cis and trans isomers of a compound as a single product) could be produced when 3-methyl-3-pentanol is dehydrated? Group of answer choices 1 2 3 4
Classify the following mixtures of liquids into (A) those with London Dispersion forces between the two molecules (B) those with London Dispersion forces and dipole-dipole attraction between the two molecules (C) those with London Dispersion forces, dipole-dipole attraction and hydrogen bonding between the two molecules |1-propanol and 1-butanol 1,1,2,2-tetrachloroethane and ethanol methylbenzene and 1,2-dimethylbenzene trichloromethane and dichloromethane benzene and cyclohexane bromobutane and ethanol
Which molecules exhibit only London (dispersion) forces? CH3CI BCI3 NH3 Br2 CH4
What intermolecular forces of attraction are present among two molecules of N-methylethanamine? a. London Dispersion only b. London Dispersion and Dipole-Dipole c. Dipole-Dipole only d. Hydrogen Bonding only e. London Dispersion and Hydrogen Bonding f. Dipole-Dipole and Hydrogen Bonding g. London Dispersion, Dipole-Dipole and Hydrogen Bonding
Identify the intermolecular forces present in this compound. | HỒ CCH, London (dispersion) forces dipole-dipole interactions hydrogen bonding
Which compound(s) exhibit only London dispersion intermolecular forces? (Select all that apply.) NH2OH SO2 CH4 SF4 PF5 NH3
Which molecule has the largest size, and therefore the greatest London Dispersion forces? □ H20 H2Te H2s H2Se
Which of the following compounds would have the largest London dispersion forces? A. C8H18 B. C4H10 C. CH4 D. C15H32
London dispersion forces are the only significant factor affecting boiling point for all the following except? a. CHF3 b. CH4 c. SO3 d. Ar e. Br2
Which member of each pair has the greater polarizability (forming stronger dispersion forces)? Briefly explain your reasoning. a. CH 2 or butane b. Mg or Mg? c. XeCla or XeF