Review Worksheet for Exam I
Chem 101, Summer 2006
1. Give the type of measurement for each of the following:
a) The amount of space taken up by a substance is its ____________________.
b) The amount of matter contained in a substance is its ____________________.
c) The amount of thermal kinetic energy of a substance is its ____________________.
2. Express the following measured numbers in scientific notation *Sig. Figs. Count
a) 680,000 km
b) 75.00 m
c) 0.0005 L
3. Complete the following metric relationships:
a) 1 g = __________ mg
b) 1 mm = __________ m
c) 1 Ci = __________ Ci
4. A graduated cylinder initially contains 20.3 mL of water. If you add a 41.7 g piece of
silver metal (density of silver = 10.5 g/mL), what is the new volume of water (including
metal) that you would read on the graduated cylinder? *Sig. Figs. Count
5. Write the symbols for the following elements:
Sodium ________
Bromine ________
Boron ________
Silver ________
6. Fill in the blanks with “precise” or “accurate”: The density of a sample of copper
was measured 10 times. The average value for the 10 measurements was close to the
literature value, so the results were _______________________.
measurements
had
a
wide
range
of
values,
so
the
However, the 10
results
were
not
_______________________.
7. A top-fuel dragster can reach speeds over 330 mi/hr in only 0.250 miles. How fast is
that in km/hr? (1 km = 0.621 mi)
8. Gallium has two naturally occuring isotopes. The isotope Ga-69 makes up 60.1 % of
the atoms and the isotope Ga-71 makes up 39.9 %. Calculate the atomic mass of
gallium. *Significant Figures Count
9. Complete each of the following nuclear equations:
a)
11C

7Be
b)
35S

________ + e-
c)
________ + 1n 
+ ________
14C
+ 1H
10. If the half-life of 11C is 20.0 min, what will be the remaining activity, after 60.0 min,
of a sample of 11C with an initial activity of 0.100 mCi?
11. If it takes 56 days for a sample of
approximate half-life of 32P?
32P
to decay from 250 Ci to 16 Ci, what is the
12. Give the maximum number of electrons that can be held in each of the following
shells:
1 ________
2 ________
3 ________
13. Give the maximum number of electrons that can be in each of the following
subshells:
s ________
p ________
d ________
14. Identify each of the following elements (give the name and symbol):
a) Has atomic number 15:
Name ____________________
Symbol ________
b) Is in group 2A and has 3 electron shells:
Name ____________________
Symbol ________
c) Has electron configuration 1s22s22p63s23p5:
Name ____________________
Symbol ________
15. If the atomic number is 6 and the mass number is 13,
a) What is the element?
_______________
b) How many electrons does it have?
_______________
c) How many neutrons does it have?
_______________
16. Write the electron configuration for potassium:
_______________________________________
17. Complete the following statements about metals and nonmetals:
a) ____________________ are bad conductors of electricity.
b) When they form ions, ____________________ typically lose electrons.
c) ____________________ usually form ionic bonds with ____________________ .
18. Write the electron-dot structures for the following ions and circle the ones with a
noble gas configuration:
a) S2-
b) P2-
c) Ca2+
19. What type of bond would you expect to form for each of the following pairs of
atoms (ionic, polar covalent or nonpolar covalent)? (circle your answer)
a) C and Br
Ionic
Polar Covalent
Nonpolar Covalent
b) O and H
Ionic
Polar Covalent
Nonpolar Covalent
c) Ca and I
Ionic
Polar Covalent
Nonpolar Covalent
20. For each of the following molecules, write the dot structure and use VSEPR theory
to predict the shape (linear, bent, trigonal planar, pyramidal or tetrahedral). State
whether each molecule is overall polar or nonpolar:
Molecule
Dot-Structure
Molecular Shape
Polar or Nonpolar
PCl3
BCl3
SiO2
21. For each of the following pairs of compounds, circle the one with the higher boiling
point:
a)
CH4
CHCl3
b)
PCl3
H2O
c)
HCl
KCl
22. Identify the main type of interactive force that occurs between molecules in each of
the following substances.
a) HCl
b) NH3
c) PH3
d) H2S
e) F2
f) CO2
23. Given that for water:
heat of fusion = 80. cal/g, heat of vaporization = 540 cal/g, specific heat = 1.00 cal/g ºC
a) Calculate the amount of heat consumed (in kcals) when 25 g of ice at -15 ºC first
warms to 0.0 ºC and then melts (hint: 2 steps). Show your work.
b) Calculate the amount of heat consumed (in kcals) when the 25 g of liquid water
warms from 0.0 ºC to 100.0 ºC, vaporizes, and then warms to 120 ºC (hint: 3 steps).
Show your work.
c) Draw a heating curve for the whole process occurring in parts a and b. It need not be
drawn to scale. (Label the x and y axes, the melting and boiling points and the physical
states: s, l and g.)