Name____________________________________________ Date________________ Hour______
MST CHEMISTRY MIDTERM REVIEW
A. Scientific Measurement
Metric System
M
-
-
K
H
D
m
L
g
d
c
m
-
-
µ
Convert the following units:
1. 10.64 mL =
L
6. 13.2 kg =
g
2. 3200 m =
mm
7. 0.543 km =
mm
3. 14.32 L =
KL
8. 53 mL =
cL
4. 418 µg =
mg
9. 0.312 cg =
kg
10. 55 L =
µL
5. 0.000435 Km =
cm
Significant Figures
How many significant figures are in each of the following measurements?
11. 4.09 cm____
12. 10.450 L____
13. 0.00028 g____ 14. 10.10 mL____15. 10 m____
16. What are the SI units for the following: time, temperature, length, volume, mass?
17. What is the difference between precision and accuracy?
18. In a lab a student finds the density of copper to be 9.32g/cm3. If the actual density of copper is
8.96 g/cm3, what is the percent error?
B. Properties of Matter
Properties – Define the following:
19. solid20. liquid21. gas22. physical propertiesexamples:
23. chemical propertiesexamples:
24. physical changesexamples:
25. chemical changes26. indicators of chemical change
C. Atoms, Isotopes, Ions
Definitions- Define or fill in the following:
27. atomic number28. mass number29. isotope30. ion31. protons have a
charge and are found
.
32. neutrons have a
charge and are found
.
33. electrons have a
charge and are found
.
34. The
and
are about the same size and make up the mass
of the atom. The
are MUCH smaller and do not really affect the mass of
the atom.
35. Two isotopes are the same in this way:
. They are different in this way:
.
36. An ion is different from an atom because it has gained or lost
. It therefore has a
whereas an atom is neutral.
37. Complete the following table:
Symbol
Name
Atomic # Mass # # p+ # n # e8
barium
8
10
82
2
H
carbon-fourteen
Ca2+
20
sulfide
32
38. Another name for a positive ion is a
.
39. Another name for a negative ion is a
.
40. Metals
.
41. Nonmetals
electrons to form
electrons to form
.
42. Explain the difference between the mass number of an element and the average atomic mass of
the element.
Problems
43. A sample of silver is 52% 107Ag and 48% 108Ag. Calculate its average atomic mass.
44. A sample of lead is 1.37% 204Pb, 26.26% 206Pb, 20.82% 207Pb, and 51.55% 208Pb. What is the
average atomic mass of lead?
D. Names and Formulas of Ions
Writing Formulas- Write the formula, charge, and number of valence e-‘s for the most common ion /
indicated ion
45. Copper II ion
_____________
50. Copper I ion
46. Sulfide
_____________
51. Iron III ion ______________
47. Phosphide
_____________
52. Calcium ion
48. Mercury I ion
_____________
53. Vanadium ion
________________
49. Cobalt II ion
_____________
54. Barium ion
__________________
55. Prefixes are used when naming
56. Roman numerals are used to designate the
__________________
__________________
compounds.
of most transition metals.
57. What does Binary mean?
Drawing / Naming BICs Draw the Lewis Dot Structures and Show Formation of Ions for Each Pairing.
Then, Name the Binary Ionic Compound
58. Ca with O
59. Manganese II with Phosphorus
60. Lead IV with Selenium
61. Silver with Tellurium
F. Periodic Table Terms: Make sure you are familiar with, and can properly label the terms below on
the blank periodic chart.
group and family numbers
period
representative elements
transition elements
inner transition elements
metals
nonmetals
metalloids
alkali metals
alkaline earth metals
halogens
noble gases
lanthanide series
actinide series
In addition, make sure you know how to find the # of protons, electrons, neutrons and mass number of
atoms, ions and isotopes by using the periodic table.
G. Electrons in Atoms
78. What is the next atomic orbital in the series: 1s, 2s, 2p, 3s, 3p?
79. What is the electron configuration of potassium?
80. What is the number of electrons in the outermost energy level of an oxygen atom?
81. What is the maximum number of electrons in the second principal energy level?
82. According to the aufbau principle, electrons enter orbitals of ____________________ first.
83. What types of atomic orbitals (s, p, d, or f) are in the third principal energy level?
84. Stable electron configurations are likely to contain ____.
85. Describe the quantum mechanical model.
86. Explain Hund’s rule?
87. What does the Pauli Exclusion principle state?
H. The Periodic Table
88. Which of the following elements has the smallest radius: a) chlorine, or b) bromine?
89. What is the charge of a cation?
90. What is the element with the highest electronegativity value: a) calcium, or b) fluorine?
91. What element has the electron configuration of 1s22s22p63s23p2?
92. Elements that are characterized by the filling of f orbitals are classified as _____________.
93. As you move from left to right across the second period of the periodic table, ionization energy
_________________.
94. Cations form when an atom ______________ electrons.
95. What is the energy required to remove an electron from an atom in the gaseous state called?
96. How many electrons does the ion Ca2+ contain?
97. Vertical columns on the periodic table are called____________.
98. Horizontal rows on the periodic table are called_____________.
99. When a calcium atom loses two electrons to form a Ca2+ ion, the electrons are lost from what
orbital?
100. Write the shorthand electron configuration for bromine.
I. Ionic and Metallic Bonding
101. How many electrons does nitrogen gain in order to achieve a noble-gas electron
configuration?
102.
What particle is free to drift in metals?
103.
What are some properties of metallic bonding?
104.
What are the characteristics of ionic compounds?
105.
What is the formula of sodium nitride?
106.
What is the name given to the electrons in the highest occupied energy level of an atom?
107.
What is the basis of a metallic bond?
108. How many electrons are transferred from calcium to iodine when forming the compound
calcium iodide?
109.
The electron configuration of a fluoride ion (F1-) is:
110. An ionic bond is a bond between ________________________________
.
111. Which of the following pairs of elements is most likely to form an ionic compound: a)
magnesium and fluorine, or b) sodium and aluminum?
112.
The octet rule states that, in chemical compounds, atoms tend to have ________________.
113.
How many valence electrons are in bromine?
114.
Draw the electron dot structure for chlorine.
115.
What is a lone pair of electrons?
K. Nuclear Chemistry
116. Nitrogen-13 emits beta radiation and decays to Carbon-13 with a half-life of 10 min. Assuming
a starting mass of 2.00 grams of Nitrogen-13, how many grams will be present at the end of three
half-lives?
117.
Write an equation for the alpha decay of Pa-231.
118.
Write an equation for the beta decay of H-3.