A. 150 B. 200 300 D. 400 E. 450 45. In which of the following substances are dip

Question

A. 150 B. 200 300 D. 400 E. 450 45. In which of the following substances are dipole-dipole forces the strongest intermolecular attractive force present? A. SO2 B. NH3 C. SO3 D. CaC12 E. CH3OH 46. What is the strongest intermolecular force of attraction between water molecules? A. ionic bond B. hydrogen bonding C. dipole-dipole forces D. London forces 47. Using the Clausius-Clapeyron equation, calculate the vapor pressure (in mmHg) of liquid bromine at 30 degree C. A. 220 B. 240 C. 260 Please turn the page to finish the exam. D. 280 E. 300

Explanation / Answer

1) since NH3 has hydrogren bonds, these hydrogens create high negative charge on nitrogen hence polarity increases, leads to formation of dipole with high attraction.

2) a hydrogen bond is an attraction between a slightly positive hydrogen on one molecule and a slightly negative atom on another molecule. Hydrogen bonds are dipole-dipole forces. The large electronegativity difference between hydrogen atoms and several other atoms, such as fluorine, oxygen and nitrogen, causes the bond between them to be polar. The other atoms have more affinity for the shared electrons, so they become slightly negatively charged and hydrogen becomes slightly positively charged. Hydrogen atoms are small, so they can cozy up close to other atoms. This allows them to come very close to the slightly negatively charged unshared electron pair of a nearby atom and create a bond with it.

3). the boiling point of any liquid, its vapor pressure equals the atmospheric pressure.

molar heat of vaporization of bromine =  29.96 kJ

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