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Name:______________________________
Chemistry Mid-Year Review L2
Into Unit
1. Why is Chemistry often called the central science?
2. What are the different branches of Chemistry?
3. State the Law of Conservation of Matter.
_____4. Group 1
_____5. Group 18
_____6. Group 17
_____7. Group 2
A.
B.
C.
D.
E.
F.
Transition metals
Alkali metals
Alkaline Earth metals
Noble gases
Inner transition metals
Halogens
Scientific Method
A. Experiment
D. Conclusion
G. Observation
B. Variable
E. Hypothesis
H. Law
C. Control
F. Theory
10. ______ In an experiment, one ____________ is tested at a time to determine how it
affects result.
11. ______ This is a Statement of what happens without explaining why
12. ______ This explains why/ how things happen
13. ______When you don’t do anything different than normal in an experiment, it serves
as a __________ group.
14. ______ Is a possible answer to a question
Name:______________________________
Math in Chemistry
15. List the SI base units for the following:
Distance __________
Mass _____________
Time _______________
Temperature __________
16. For the following, list the number of significant figures in each:
A. 0.0000095________________
B. 745672345 _________________
C. 0.0346001________________
D. 29480000___________________
17. How many liters in 1 Mega liter?
18. How many seconds in 0.75 years?
19. Herbert has to make some measurements. He takes a 16oz weight, and masses it to
be 32.21oz, 32.19oz, 32.20oz, and 32.32oz.
Do his measurements exhibit high precision? ______________
Do his measurements exhibit high accuracy?______________________
Explain!
20. Measurements are always uncertain because
A. Instruments aren’t designed for measurements
B. All measurements involve some estimation
C. People don’t know how to use instruments
D. None of the above
E. All of the above
21. 598 mL – 6.6 mL =
a. 591.4 mL
c. 604.6 mL
b. 591 mL
d. 605 mL
22. 42800 / 401
a. 107
c. 106.73
b. 106.7
d. 106.733
Name:______________________________
23. Complete the following: 564 cm = ________ meters
a. 564 m
b. 56.4 m
c. 5.64 m
d. 56400 m
24. 8.56 L X 6.2315 L X 4.163 L =
a. 222.1 L3
b. 222.06 L3
3
c. 220 L
d. 222 L3
25. What is the density of a wood block with a volume of 16.5 mL and a mass of 6.39g?
a. 0.3872 g/mL
b. 0.387 g/mL
c. 0.388 g/mL
d. 0.39 g/mL
26. Calculate the density of matter that has a volume of 12.4 ml and a mass of 4.20
grams.
27. Assuming that one drinks 24oz of coffee a day, 365 days a year, how many Liters of
coffee does the person consume in a year? (1.000oz= 29.57 mL)
28. Hugh was born 6.391875 X 103 days ago. How old (in years, with 1yr= 365.25 days)
is Hugh?
Matter
29. An element
a. can be broken down into simpler substances
b. are used to make other elements
c. are used to make compounds
d. are never found in the periodic table of elements
30. Physical means can be used to separate
a. elements
b. pure substances
b. mixtures
d. compounds
31. Anything that takes up space and has mass is called
a. matter
b. mass
c. volume
d. stuff
Name:______________________________
32. A change in the force of Earth’s gravity on an object will affect its
a. mass
b. density
c. weight
d. kinetic energy
33. Chemical proprieties
a. include changes of state of a substance
b. include mass and color
c. include changes that alter the identity of a substance
d. can be observed without altering the identity of a substance
34. Identify each as an element, compound, or mixture. For mixtures, identify it as
homogeneous or heterogeneous.
_______________________ A. Orange juice
_______________________ B. NaCl
_______________________ C. Fog
_______________________ D. Ink
_______________________ E. 14 Karat gold
_______________________ F. Ice
_______________________ G. Molybdenum
_______________________ H. octane (C8H18)
35. The four states of matter are: __________________________________________
_________________________________________________________________.
36. State below if the form (shape) of each state is constant, as well as the volume.
37. Explain the arrangement of molecules in solids, liquids, and gases.
Name:______________________________
38. Classify each of the following as either a physical or chemical change.
_______________________ A. Bending a piece of wire
_______________________ B. Burning coal
_______________________ C. Cooking a steak
_______________________ D. Dissolving sugar in water
_______________________ E. Souring milk
_______________________ F. Stretching a rubber band
The Atom
39. For the following elements, provide information as to group, block and metal status as
indicated on the top of the chart.
Element
K
19
Ba
56
Ti
22
Al
13
Se
34
Sb
51
Xe
54
Pm
61
Group name
Metal, Nonmetal, or
Metalloid?
Name:______________________________
40. Write the complete chemical symbol for an atom with 35 protons, 45 neutrons, and
36 electrons.
41. Element X has two natural isotopes. The isotope with mass 62.9265 amu has a
relative abundance of 69.17%. The isotope with mass 64.9278 amu has a relative
abundance of 30.83%.
What is the average atomic mass of element X?
What is the identity of element X?
42. Fill in the sections of the table that are empty.
Element
# of
protons
# of
neutrons
Cr
# of
electrons
Mass #
Charge
(+, , 0)
52
0
28
37
48
36
Br
36
80
5
11
I
3+
74
0
Nomenclature
43. Give the common ion for the following:
S
O
C
B
N
Cl
I
H
44. What are the 3 types of bonds?
45. Which type of bond occurs with a transfer of electrons?
Na
Ca
Mg
Ag
Name:______________________________
46. Which type of bond occurs with a sharing of electrons?
47. Beryllium Bromide (BeBr2) has which type of bond?
48. When are Roman numerals used in naming compounds?
49. Name the following compounds. Both ionic and covalent molecules are here, and
they are mixed!
A. NaOH ___________________________
B. CaO _____________________________
C. N2O _____________________________
D. N2O5 ____________________________
E. SO2 _____________________________
F. H2SO4 ___________________________
G. AgC2H3O2 _________________________
H. CuCl22H20 _______________________
50. Give the correct formula for the following:
A. Iron (III) sulfate __________________________
B. Iron (II) sulfate __________________________
C. Oxygen gas _______________________
D. Nitric Acid ______________________________
E. Lead (IV) chromate _______________________
F. Sulfur hexaflouride ________________________
G. Dinitrogen dioxide ________________________
H. Barium hydroxide _________________________
I. Magnesium sulfate heptahydrate ______________________________
J. Hydrogen gas _______________________
K. Sodium metal_______________________
Name:______________________________
Reactions and Equations
A. Coefficient
B. Reactant
C. Product
D. Balanced
E. Endothermic
F. Exothermic
G. Subscript
H. Precipitate
I. Diatomic
J. Aqueous
_____ 51. A reaction that releases heat.
_____ 52. A reaction that absorbs heat.
_____ 53. A whole number that appears before a formula in an equation.
_____ 54. A starting substance in a chemical reaction.
_____ 55. A new substance formed in a chemical reaction.
_____ 56. Equation obey the laws of conservation of mass if they’ve been properly ___.
_____ 57. A solid product.
_____ 58. A number within a formula representing the number of atoms of each element
present in the formula.
_____ 59. A solid compound dissolved in water.
_____ 60. Elements that do not exist alone!
Write out a word equation for the following equations.
61. H2SO4 + NaOH ---------------> NaSO4 + H2O
62. Ba(OH)2
+
MgCl2 ----------->
63. Why do we balance equations?
Mg(OH)2 + BaCl2
Name:______________________________
Substitute symbols and formulas for names, and then write a balanced equation for
each of the following reactions.
64. Copper combines with sulfur to form copper (I) sulfide.
65. Chlorine gas reacts with aqueous sodium bromide to form aqueous sodium chloride
and liquid bromine.
Balance the following reactions.
66. ___ WO3 + ___ H2 ___ W + ___ H2O
67. __ PdCl2 + ___ HNO3  Pd(NO3)2 + ___ HCl
68. ___ Cr + ___ O2  ___ Cr2O3
69. ___ CuS2 + ___ O2  ___ Cu + ___ SO2
Identify the type of chemical reaction shown below as synthesis (S), decomposition
(D), single replacement (SR), double replacement (DR), or combustion (C).
70.
KI + Pb(NO3)2  KNO3 + PbI2
71.
Fe + H2O  Fe2O3 + H2
72.
Ag2O  Ag + O2
73.
CH3OH + O2  CO2 + H2O
74.
S8 + O2  SO3
Name:______________________________
Given the following reactants predict the products.
75. Li + Br2 
76. NaCl 
77. Na (s) + P(s) 
78. AgNO3 + NaCl 

79. AgNO3(aq) + Cu(s) (2+)
80. H2SO4(aq) + Ca(OH) 2(aq) 
81. Ag(s) + Cu(NO3)2(aq)

82. SnF4(s) 
83. C6H14(g) + O2(g)
→
84. CaCl2(aq) + NaNO3(aq) 
85. What is the activity series, and why is it important when working with single
replacement reactions?
The Mole
86. Calculate the mass of 2.56 moles of barium phosphate.
87. Determine the number of particles in 8.20 g of potassium sulfate.
88. Determine the volume of 312 g of Bromine gas at STP.
Name:______________________________
89. Determine the percent composition for each element in Phosphorus trichloride.
90. Calculate the molecular formula of the compound whose molar mass is 60.0g and
empirical formula is CH4N.