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REVIEW SHEET
SEMESTER ONE EXAM
PREAPCHEMISTRY
1. How do you dilute an acid with water?
2. If you spill something on your skin in the lab, what would you do?
3. When would you use the eye wash? The shower?
4. Who do you notify immediately when there is ANY lab accident?
5. You are suppose to smell the vapors of a certain chemical how do you do it?
What is it called?
6. What is the difference between weight and mass?
7. How do you measure the volume of an irregularly shaped object?
8. What would you do if a fire started in the lab?
9. A dip in the surface of a liquid that is considered to be the top of the liquid is
known as the ____________________.
10. ( True or False) You can measure a chemical directly on the pan of the balance.
11. How many significant digits would 10032 have? _________ 1.0023? ______
0.00075? _________ 30000?________ 100.00?_________
12. Express the following in the correct number of significant figures.
3.0 x 102 / 2.11 x 103=
265.2( 1.2)=
2.3 + 17.256=
13. Write the following in scientific notation.
123456
1200
.000234
14. 1100 yards = ______ mm ( 1 in = 2.54 cm)
15. 100 ml of iron and 100 ml of water will have the same mass (true or false)
16. When measuring a physical property the substance (is/ is not) changed after the
measurement.
17. When measuring a chemical property the substance (is/ is not) changed after the
measurement.
18. Name three chemical properties.
19. Name three physical properties.
20. What is a heterogeneous mixture? Give an example.
21. What is a homogeneous mixture? Give an example.
22. What are the three states of matter that we deal with in chemistry? Which is the
most dense?
23. A mixture is a substance that can be separated by _________methods.
A compound is a substance that can be only separated by ________ methods.
Give an example of each.
24. A cubic centimeter is equivalent to what volumetric measurement? _________
25. Name the following.
HCl
HBr
H2SO4
HNO2
Ca3(PO4)2
KI
P3N5
Fe2O3
26. Write formulas for the following
Copper II oxide
Dihydrogen monoxide
Sodium chloride
Calcium bromide
Barium chlorate
Potassium permanganate
Phosphoric acid
Hydroiodic acid
27. The formula K2SO4 represents how many atoms of potassium? _____
oxygen?_____ how many molecules?______.
28. What is the law of conservation of mass?
29.What is Dalton’s atomic theory? Which part(s) is/are incorrect?
29. What is the law of multiple proportions?
30. In an exothermic reaction the energy is a ________________ (product or
reactant).
In
an
endothermic
reaction
the
energy
is
a
_________________(product or reactant).
31. What are the seven diatomic elements?
32. What is the molecular mass of Ca(NO3)2?
33. What is the percent composition of NH4NO3?
34. How many moles are there in 15g (NH4)2SO4?
35. How many molecules are there in 35 g of H2SO4?
36. How many L of gas at STP does 24 g of N2 occupy?
37. What does STP stand for, and what is STP?
38. What is a hydrated crystal?
39. How could you tell when a hydrated crystal is dry?
40. Find the percent water of hydration in the following Na2SO4 10H2O.
41. Experimentally you found the percent water of hydration of a crystal to be 42%,
but theoretically you calculated that it should be 60%. Calculate the percent error.
42. Calculate the empirical formula given the following data.
48.64% C
8.16% H
43.20 % O
43. A compound was found to contain 49.98g carbon and 10.47g hydrogen. The
molecular mass of the compound is 58.12 g. Determine the molecular formula.
44. How many moles of sulfur are in 10 moles of SO3?______________
How many moles of oxygen are in 10 moles of SO3?______________
45. Write a balanced chemical equation for each of the following.
a. in water, iron(III) chloride reacts with sodium hydroxide, producing solid
iron(III) hydroxide and sodium chloride.
b. Solid zinc and aqueous hydrogen sulfate react to produce hydrogen gas
and aqueous zinc sulfate.
c. What are the reactants and products for b.
46. How many neutrons, protons and electrons does silicon have?
47. Why is the atomic mass not a whole number?
48. Draw orbital diagrams and electron configurations for Na and Al.
49. What periodic trends increase as you go from left to right on the periodic table?
50. What periodic trends decrease as you go from left to right?
51. What periodic trends decrease as you go from left to right? What happens as you
go from top to bottom?
52. What is a cation and how is it formed?
53. What is an anion and how is it formed?
54. How is the periodic table organized?
55. Give the contributions of the following scientists Mendeleev, Mosely, Seaborg to
the development of the periodic table.
56. Draw a picture and name the following scientists model of the atom. List their
experiments and what their model added to our current model of the atom.
Bohr, Thompson, Rutherford, Schroedenger
57. On the periodic table a vertical column is known as ___________or
___________.
58. On the periodic table a horizontal row is known as a __________ or
___________.
59. Group 1A is known as ___________. Group 2A is known as _______________.
Group 7A is known as _____________.
Group 8A is known as the
_____________.
60. The period of the periodic table corresponds to the _____________ the electron is
located on.
64. Hydrogen and bromine react to form hydrogen bromide (HBr). If you start with
49.7 g of bromine, how many grams of HBr will be formed?
65. Given Al + O2  Al2O3. How many grams of aluminum oxide will be produced
if you start with 63 g of Al and 86 L of oxygen at STP? (Hint: balance equations and
find limiting reactant)
66. Given: PbS + O2  PbO + SO2. If 200.0 g of PbS is burned and 170.0 g of PbO
is obtained, what is the percent yield? Percent error?
67. Given Zn + HCl  ZnCl2 + H2. How many liters of hydrogen gas at STP will
be produced if you start with 55 grams of HCl ?
68. If =2.04 X 10-7 cm, find frequency and energy.
69. If v= 1.89 x 1018 Hz, find wavelength and energy.
70. If E = 7.89 x 10-20 J, find frequency and wavelength.
71. How many protons and neutrons do these isotopes have?
a.
14
6C
b.
41
19K
c.
115
49In
72. Who was the first to discover that uranium underwent nuclear radiation?
73. When elements have the same number of protons , but different numbers of neutrons,
they are called ___________________________.
74. What will a radioactive isotope do to become stable?________________________
What is this process called?___________________________________________
75. The radioactive particle that is the same as an electron is ________________.
76. The process where an electron from the first energy level is added to the nucleus is
called ___________________________.
77. The radioactive emission that is a high form of energy with _______ mass and
__________ charge is known as __________________.
78. A positive electron is also known as __________ and has what Greek
symbol?_____________
79. What radioactive particle is the same as a helium nucleus?__________________
80. The time required for half of a radioactive sample to decay is known as
_____________ and has the symbol _______________________.
81. Physical and chemical properties of stable isotopes are (the same as/ different from)
radioactive isotopes.______________________
82. The breakup of a large unstable nucleus into more stable nuclei is known as
_____________.
83. What particle is used to start the chain reaction of U-235?_______________
84. The combining of light nuclei to form a heavier nucleus is called
________________.
85.
86.
87.
88.
T or F Fission produces more energy than fusion.____________
What process takes place on the sun and other stars? _____________
T or F Fusion is now used to produce electricity._______________
Give the seven particles you might use to balance nuclear equation.
89. Balance the following nuclear equations.
a. 4319K 4320Ca + _________
b.
223
92U

c.
11
6C +
____  115B
d.
13
7N
219 Th
90
+ __________
 0+1β + ______
90. Name the three types of radiation and circle the weakest type.