Chem Notebook COmplete

The Learning Goal for this assignment is: The students will learn how the interactions between water
molecules account for the unique properties of water and how aqueous solutions form.
Take note over the following chapter. Use the Headings provided to organize your notes. Define and number all highlighted vocabulary (total 22 ) as well
as summarize and take notes over the sections. You may add pictures where needed. The pictures should be an appropriate size. Use Arial 12 for all
text. This document should be 2 pages and should be saved as a pdf before you submit it into Angel.
Chapter 15 Water and Aqueous Systems
Pages 488 - 507
15.1 Water and Its Properties
Water in the Liquid State
EQ: What factor causes the high surface tension, low vapor pressure, and high boiling point of water?
a. Many unique and important properties of water including its high surface tension, low vapor
pressure, and high boiling point result from hydrogen bonding.
Many of the characteristics of water are due to the structure in which water is organized, having one
oxygen and two hydrogen atoms makes the bonds highly polar.
Water is one of the liquids with the highest surface tensions.
1.Surface tension: The inward force, or pull, that tends to minimize the surface area of a liquid.
2.Surfactant: Is any substance that interferes with the hydrogen bonding between water molecules and thereby
reduces surface tension.
Water in the Solid State
EQ: How can you describe the structure of ice?
a. The structure of ice is a regular open framework of water molecules in a hexagonal arrangement.
Extensive hydrogen bonding in ice holds the water molecules further apart in a more ordered arrangement
This is what causes water in its solid form, ice, to float when dumped in a cup of water because it has a lower
density.
Summary: In this section it is now known that waters many of water’s unique characteristics is due to its
structure, especially how the hydrogen atoms are bonded together. In a liquid, these characteristics are high
surface tension, low vapor pressure, and high boiling point. As a solid, the characteristics caused by the
hydrogen bonding are density, arrangement of molecules, and the ability to float.
15.2 Homogeneous Aqueous Systems
Solutions
EQ: What types of substances dissolve most readily in water?
a. Substances that dissolve most readily in water include ionic compounds and polar covalent
compounds.
Water dissolves so many of the substances that it comes in contact with that you won’t find chemically
pure water in nature.
Solvents and solutes may be gases, liquids, or solids.
Nonpolar covalent compounds such as methane, and compounds found in oil, grease, and gasoline do not
Dissolve in water, however, they will dissolve in gasoline, this is do to the structure of the solvent and the
solute and the attractions and bonds that exist between them. There are nearly insoluble compounds
because the attractions among the ions are stronger than the attractions exerted by water.
3.Aqueous solution: is water that contains dissolved substances.
4.Solvent: The dissolving medium in a solution.
5.Solute: The dissolved particles in a solution.
6.Solvation: The process by which the positive and negative ions of an ionic solid become surrounded by
solvent molecules.
Electrolytes and Nonelectrolytes
EQ: Why are all ionic compounds electrolytes?
a. All ionic compounds are electrolytes because they dissociate into ions.
Conduction of an electric current requires ions that are mobile and, thus, able
to carry charges throughout a liquid, this is because they ionize in a solution.
Electrolytes are essential to all metabolic processes, including the ability for cells to
carry electrical impulses internally to communicate to other cells, also electrolytes are crucial to nerve and
muscle function, this is why it is always recommended to drink a liquid with significant amounts of electrolytes
when working out, playing a sport, or doing any other physical activity that uses up electrolytes.
Some polar molecular compounds are nonelectrolytes in the pure state but become electrolytes when they
dissolve in water.