Transcript Lesson 6.2 Packet Answers

Answers to 6.2 Review and
Homework
Mrs. Wilson
6.1 Review
• Water has a bent molecular structure and permanent dipoles due to its highly
electronegative H-O bonds. It is polar.
• The partial + hydrogen ends attract the chloride anion away from the sodium cation.
Those hydrogen ends face the chloride.
• The partial – oxygen ends attract the sodium cation away from the chloride anion.
The oxygen ends face the sodium.
6.2
Homework
(pg. 30)
Nature of solute and solvent – Ionic and polar solutes dissolve in polar solvents, like
water. The solute and solvent have similar IMFs so a solute and solvent molecule can
associate with each other easily. Nonpolar solutes dissolve in nonpolar solvents for
the same reason. Solubility and Temperature – increase temperature for solids =
increased solubility (usually) because this increases avg. kinetic energy of solute and
solvent molecules
Nature of solute and solvent – Ionic and polar solutes dissolve in polar solvents, like water. The
solute and solvent have similar IMFs so a solute and solvent molecule can associate with each
other easily. Nonpolar solutes dissolve in nonpolar solvents for the same reason. Solubility
and Temperature – decrease temperature for gases = increased solubility because decreased
avg. KE will tend to keep nonpolar gases dissolved rather than escape the solvent. Solubility
and Pressure – increase pressure for gases = increased solubility (as P increases, gas
molecules have more collisions; more likely to be surrounded by solvent if they’re
colliding more frequently)
Inc. surface area and agitation = both factors allow solvation to occur faster (solvent can surround solute faster).