1) For the following pairs of molecules/atoms, circle the species that has the h
ID: 1037726 • Letter: 1
Question
1) For the following pairs of molecules/atoms, circle the species that has the highest boiling point. (5) a. PH3 or NH3 b. HCl or HBr C. Ne or Kr d. CaHs or CH e. H2S or H20 2) Circle the intermolecular force(s) that is/are present in each of the following species. (8) a. Ne (dispersion forces, dipole-dipole forces, hydrogen bonding) b. HCl (dispersion forces, dipole-dipole forces, hydrogen bonding) c. CBrs (dispersion forces, dipole-dipole forces, hydrogen bonding) d. CHsF (dispersion forces, dipole-dipole forces, hydrogen bonding) e. NzHs (dispersion forces, dipole-dipole forces, hydrogen bonding) 3) Circle the intermolecular force that accounts for the difference in the following cases: (5) The boiling point of hydrogen fluoride (HF) is 20°C, while the boiling point of hydrogen chloride (HCI) is-85°C a. Hydrogen bonding, dipole-dipole interactions, or dispersion forces b. The boiling point of carbon tetrachloride (CCl4) is 77°C, while that of tetrabromomethane (CBra) is 190°c Hydrogen bonding, dipole-dipole interactions, or dispersion forces c. The boiling point of chlorine (Cla) is -34°C, while the boiling point of Hydrogen (H2) is -2530C Hydrogen bonding, dipole-dipole interactions, or dispersion forces d. The boiling point of ammonia (NHs) is -33°C, while that of nitrogen trifluoride is -129°C Hydrogen bonding, dipole-dipole interactions, or dispersion forcesExplanation / Answer
1.
a) NH3 has higher boiling point due to the presence of H-bonding.
b) HBr has higher boiling point due to bromine being a large atom has higher London dispersion forces which increase the boiling point.
c) Kr has the higher boiling point due to the presence of more London dispersion forces as Kr atom is bigger in size than Ne atom.
d) C3H8 has the higher boiling point due to the presence of strong London dispersion forces.
e) H2O has higher boiling point due to oxygen being more electronegative than sulfur can form stronger intermolecular H-bonding.
2.
a) Ne- dispersion forces
b) HCl - dipole-dipole and dispersion forces
c) CBr4 - dipole-dipole and dispersion forces.
d) CH3-F - dipole-dipole and dispersion forces
e) N2H4 - dispersion, dipole-dipole and H-bonding
3.
a) H-bonding
b) dispersion forces
c) dispersion forces
d) hydrogen bonding
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