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18 Nov 2019
When the following substances are in the liquid state, which would be expected to have the lowest boiling point? a. Ne b. Ar c. Kr d. Cl_2 e. Br_2 Water has a much higher boiling point than hydrogen sulfide, H_2 S. This is best explained by a. H_2 S having greater polarity than H_2 O. b. stronger S-H covalent bonds than O-H covalent bonds. c. stronger London dispersion forces between H_2 O molecules than between H_2 S molecules. d. hydrogen bonding between H_2 O molecules, which does not occur in H_2 S. e. stronger O-H covalent bonds than S-H covalent bonds.
When the following substances are in the liquid state, which would be expected to have the lowest boiling point? a. Ne b. Ar c. Kr d. Cl_2 e. Br_2 Water has a much higher boiling point than hydrogen sulfide, H_2 S. This is best explained by a. H_2 S having greater polarity than H_2 O. b. stronger S-H covalent bonds than O-H covalent bonds. c. stronger London dispersion forces between H_2 O molecules than between H_2 S molecules. d. hydrogen bonding between H_2 O molecules, which does not occur in H_2 S. e. stronger O-H covalent bonds than S-H covalent bonds.
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Collen VonLv2
26 Jun 2019
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