Define physical and chemical properties, provide three examples of each, discuss their reversibility, and
explain the fundamental differences between them.
2. Density is a physical property of a molecule that’s measured as mass per unit volume.
(a) Given that density is usually expressed in the units of g/cm3
, calculate the density of a cube of plastic that
has a mass of 2.331 g and an edge length of 1.500 cm (volume of a cube is V = l
3
).
(b) Draw two liquids in a graduated cylinder on a separate sheet of paper. You won’t submit the drawing as part
of your answer. Liquid A has a density of 1.004 g/cm3 and Liquid B has a density of 0.6223 g/cm3
. Assume they
don’t mix. Label which liquid is on top and which liquid is on bottom, and then draw the cube where you would
expect it to be if it’s dropped into the graduated cylinder with these two liquids.
Explain the location for liquid A, liquid B, and the cube in the graduated cylinder.
3. Three quantum numbers are derived from Schrodinger’s equation that describe the probability of finding
an electron around a nucleus: the principal quantum number, the angular momentum quantum number, and
the magnetic quantum number. Explain each quantum number, including associated shapes, numbers,
letters, and values.
4. Write the full electron configuration for phosphorus, atomic symbol P, then draw an orbital box diagram
on a separate piece of paper that accounts for all of the electrons in phosphorus. You don’t need to include
the orbital box diagram as part of your answer. Based on your drawing, explain why phosphorus is either
paramagnetic or diamagnetic.
5. Compare and contrast the alkali metals and the alkaline earth metals. Discuss their physical and
chemical properties, their magnetic properties, and their electron configurations.
6. Explain the bonding that occurs between sodium and chlorine. Specifically, what kind of bonding takes
place, what’s the name of the resulting compound, and what properties would you expect this compound to
have with respect to water?
7. Explain the bonding in carbon tetrachloride, CCl4—specifically, explain whether it’s covalent or ionic.
8. Explain the layout of the modern periodic table, including rows, columns, groups, and blocks. Be sure to explain
what’s in each part of the periodic table.

3
For chemical drawings, you can use the Chemical Equation editor in the submission box for the assignment.
9. Draw the Lewis structure for sulfur tetrafluoride, SF4, and then draw the electron pair geometry. What’s the
name of the molecular shape of sulfur tetrafluoride? Note: You can draw this on paper, take a picture, and
paste the picture in your document.
10. Draw the structure of water. Is water considered polar or nonpolar? Why? Note: You can draw this on paper,
take a picture, and paste the picture in your document.
11. When someone is injured, responding medical personnel may use either hot packs or cold packs to treat the
injuries. These are examples of miniature chemical reactions. Using hot packs and cold packs as an example,
explain the terms endothermic reaction and exothermic reaction.
12. Combustion reactions take place between a fuel and oxygen and produce carbon dioxide and water. Balance
the following combustion reaction.
13. Aqueous lead (II) nitrate, Pb(NO3)2 undergoes a double displacement reaction with aqueous sodium chloride,
NaCl, in which a precipitate forms. If the precipitate contains lead, write the balanced chemical equation for
this reaction. Be sure to include the states of each of the reactants and products.
14. Explain the four basic types of chemical reactions. Be sure to include a sample equation for each type. Describe
how rate relationships and activation energy are important in chemical reactions.
15. Write the equilibrium expression for the following reaction. Based upon the value of K, would you expect there
to be more or less product in the equilibrium mixture? Why?

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