London dispersión forces are only significant factor affecting boiling point for all of the following except Kr,H2SO4,C4, CL2,CH4
if molecule or atoms are non-polar londen sidpersion forces are significantly effect on boiling point.
if molecule is polar then dipole-dipole interactions effects the boiling point.
among all H2SO4 is polar so dipole -dipole interactions are significant.
answer = HSO4
London dispersión forces are only significant factor affecting boiling point for all of the following except...
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
h of the following statements is NOT true? London dispersion forces are present in all substances but are the only significant intermolecular forces in nonpolar substances. ) The density of the liquid state of a substance is greater than the density of its gaseous state. The thermal energy in a liquid allows the atoms within molecules to completely overcome the attractions between them so they flow. Most liquids can be converted to a gas by reducing pressure and/or heating. The...
Which compound(s) exhibit only London dispersion intermolecular forces? (Select all that apply.) NH2OH SO2 CH4 SF4 PF5 NH3
Question 6 (1 point) Water has a relatively high boiling point due to London dispersion forces. True O False
1. Check off (V) all the forces that apply to each of the following compounds Compound Intermolecular Force London Forces Hydrogen Bonding Dipole - Dipole BrF Cl2 H.S 2. In the liquid state, disruptive forces are a. roughly of the same magnitude as cohesive forces b. very weak compared to cohesive forces c. dominant over cohesive forces d. None of these 3. Between CIF and ClBr which compound would have a large boiling point? Explain the reason for your choice....
Please show steps (17) Which intermolecular forces are present in a sample of SF4? (A) London dispersion forces (B) Covalent Bonds (C) Dipole-dipole forces (D) Two of these (E) All of these (18) Which of the following does not increase with the strength of the intermolecular forces? (A) Melting Point (B) Boiling Point (C) Viscosity (D) Surface Tension (E) Ideal gas behavior
My answers: Not sure if they are correct. 1. a. London dispersion b. H-bonding, dipole-dipole, london dispersion c. London dispersion d. Ionic, london disperson 2. The second one because not a lot of H+ and less acidic. Need help understanding the meaning of the question. 3. Diethyl cannot h-bond because it does not provide intermolecular bonding engery while 1-b. can form h-bond making strong intermolecular bonds to take up greater engery to break molecules. 4. Not sure...
Rank the following chemical compounds from smallest to largest boiling point. Explain your answer in terms of intermolecular forces of attraction. CH4, H20, PH3
Question 9 0.2 pts Which one of the following substances has London dispersion forces as its only intermolecular force? (No hydrogen bonding, no dipole-dipole forces.) о сезон NH3 H2S O CH4 Question 10 0.2 pts True or False. Most of the substances used in this investigation are extremely volatile (easily evaporate) and should be used with care in a fume hood. True O False Question 11 O pts True or False. To avoid fainting or feeling light-headed in the lab...
2 For each pair, decide which substance has the stronger London forces and explain your answer: al CH CH Clor CH CH Br CH,CH.CH,Cl or (CH),CHCI b| CH CH CI or CH CH CH CI Consider the following compounds: CHCI CH BECHI al Based on London forces, which of these would you expect to have the weakest intermolecular forces? Explain your answer. b Based on London forces, which of these would you expect to have the greatest heat of vaporization?...