Download Name Date: __ ______ Chemistry Semester I Final Exam Review

Name ______________________________
Date: __
_______
Chemistry Semester I Final Exam Review
Guide
Topics Covered
 Unit 1: Metric system, Temperature Conversions, Unit Conversions, Significant Figures, Percent
Error, Scientific Notation, Density, Dimensional Analysis with conversions, reading a graduated
cylinder, recording significant figures in the lab

Unit 2: Elements, Compounds, Pure Substances, Mixtures, Physical and Chemical Changes and
Properties, heat, specific heat

Unit 3: Groups on the Periodic table, Atomic Structure, Atoms, Ions, Isotopes, Atomic Mass,
characteristics of metals, and nonmetals, balancing nuclear reactions, half-life problems,
Identifying a pure substance, homogenous mixture, heterogenous mixture, element, and compound
through molecular diagrams.

Unit 4: Naming and writing formulas for ionic compounds, molecules, and acids, cations, anions,
polyatomic ions.

Unit 5: Percent composition, molar mass, mole conversions, empirical formulas, and molecular
formulas
UNIT 1: Scientific Measurement (Chapter 2)
1. How many sig figs are in the following numbers?
2.04
______
0.002804
______
1,230 ______
0.00989 ______
2. When adding and subtracting, the rule for sig figs is to look at the number of ___________ __________.
Calculate the following using correct sig figs: 18.345 + 4.12 = _________
21.672 – 0.5 = _________
3. When multiplying and dividing, the rule for sig figs is to look at the number of _________ _________.
Calculate the following using correct sig figs: 5.678 x 2.3 = _________
18.1 x 3 = _________
4. Put the following numbers in scientific notation: 8,923,000,000 = _________________
0.00000345 = _________________
0.00045 = ________________
5. Do the following unit conversions: 6.7dm = _______________ mm
6. How many kilometers are in 7650 milimeters? ________________
7. How many centigrams are in 8.56 decigrams? ________________
325 cL = ____________ L
8. The formula for density is: ____________
Density is the ratio of ____________ to ____________.
9. Calculate the density of an object if it has a mass of 13.2 grams and a volume of 3.4 liters.
Density = _____________
10. Calculate the mass of a piece of plastic that has a density of 3.14 g/mL and a volume of 7.2 mL.
Mass = _______________
11. Calculate the volume of an unknown substance that weighs 23.1 grams and has a density of 5.6 g/mL.
Volume = ______________
12. Perform the following temperature conversions: 967ºC = ________ K
13. Calculate the percent error:
Experimental Length = 14.1 cm
435 K = ________ ºC
Accepted Length = 14.9 cm
14. Use dimensional analysis to solve the following density problem: How many liters are 45.7 kg of bromine?
The density of bromine is 3.10g/mL.
UNIT 2: Matter and Change (Chapter 3)
15. What is a chemical change? _______________________________________________________________
Which of the following is a chemical change: ripping a piece of paper, melting ice, burning wood?
16. Give 2 examples of physical changes: _______________________________________________________
17. What is the difference between physical and chemical properties? _________________________________
______________________________________________________________________________________
Which of the following is NOT a physical property? color, boiling point, texture, density, reactivity
18. Name 2 chemical properties: _______________________
__________________________
19. What is the difference between heterogeneous and homogeneous mixtures? _________________________
_____________________________________________________________________________________
Which of the following is an example of a homogeneous mixture? copper, salsa, salt, Gatorade
20. Determine if each is a pure substance or a mixture:
sodium (Na)
______________
Kool-Aid ______________
water _______________
21. Name the 4 indicators of chemical change:
_____________________, _____________________, _____________________, ______________________
22. Define heat:
23. Define specific heat:
24. Convert the following: 38.65 cal =
J
934 J =
kcal
25. How much energy (in joules) is required to heat a piece of iron weighing 1.30g from 25.0oC to 46.0oC?
26. A 55.0g sample of a metal requires 675 J of energy to hear it from 25.0oC to 118.0oC. Calculate the specific
heat of the metal.
UNIT 3: Atomic Structure (Chapter 4)
27. Calculate the atomic mass of iron based on the following information:
Fe-56 (94.5 %)
Fe-57 (2.3 %)
Fe-59 (3.2 %)
28. The mass number is found by adding _______________ plus _________________.
29. What is the difference between a cation and an anion? (Which is positive/negative? Gained or lost e-?)
Cation: _____________________________________________________________________________
Anion: _____________________________________________________________________________
30. Nickel:
Protons = _______
Neutrons = _______
Electrons = _______
Chlorine: Protons = _______
Neutrons = _______
Electrons = _______
31. How many neutrons are in the following isotopes?
Co-60 ________
U-235 _________
32. Name 2 noble gases: ___________, ____________
W-185 ________
Name 2 halogens: ___________, ____________
33. Give 3 examples of transition metals: ___________, ___________, ___________
34. What do the numbers represent in the following symbol?
190Os
76
190 = _______________________
35. The rows on the periodic table are called ________________.
76 = _______________________
The columns on the periodic table are called ________________.
36. Write the correct charge and name for the following ions.
Example: Calcium = Ca2+ Calcium ion
Sulfur = S2- Sulfide
Lithium =
___________________
Fluorine = _____________________
Magnesium = ___________________
Nitrogen = _____________________
37. As Potassium becomes as ion, it likes to __________ (gain/lose) electrons. How many? ________
As Oxygen becomes an ion, it likes to __________ (gain/lose) electrons. How many? ________
38. Sn-120:
Protons = ________
Neutrons = ________
Electrons = ________
39. Atoms of the same element always have the same number of _____________ (protons, neutrons, electrons)
40. An isotope has 12 protons, 12 electrons, and 14 neutrons. Name the isotope using hyphen notation: _______
41. Metals are located on the
form
side of the periodic table, and tend to
. List two characteristics of metals:
42. Nonmetals are located on the
electrons to form
side of the periodic table, and tend to
. List two characteristics of nonmetals:
43. List the metalloids:
44. What are the four nuclear particles?
__________
__________
__________
__________
45. Balance the following nuclear reactions:
198
86
22
11
Rn  24 He  194
84 Po
22
Na 10 e10
Ne
U  10 e 237
93 Np
237
92
26
14
26
Si 13
Al  10 e
46. Write a balanced reaction for each nuclear reaction.
Decay of polonium-218 by alpha emission.
Decay of chlorine-32 by positron emission.
electrons to
Decay of promethium-142 by electron capture.
Decay of oxygen 18 by emission of two neutrons
47. What is half-life?
48. The half-life of phosphorous-30 is 2.5 min. If you start with 35 g of phosphorus-30, how many grams would remain
after 20.0 min?
49. The half-life of polonium-210 is 138.4 days. How many milligrams of polonium-210 remain after 415.2 days if you
start with 2.0 mg of the isotope?
50.
20.0 g of a radioactive isotope are present at 1:00 p.m., and 5.0 g remain at 2:00 p.m.
a. How many half-lives have gone by?
_________________________
b. How long is the half-life of the isotope?
_________________________
c. Predict how many grams will be left at 2:30 p.m.
_________________________
51. Know the safety rules
52. Be able to identify the various lab equipment and know their uses and know what units each measures.
Unit 4: Naming (Chapter 5)
53. What do all ionic compounds begin with?
54. Why do you have to use a roman numeral to identify some cations?
55. What do all acids begin with?
56. What do all molecules begin with?
57. Name the following compounds/molecules.
Zn3(PO3)2
__________________________________________
Co3N2
__________________________________________
S4Br7
__________________________________________
H2CO3
__________________________________________
58. Write the formula for the following compounds/molecules.
Hydrofluoric acid
_______________________
Nickel (II) chlorate
_______________________
Dicarbon pentaiodide
_______________________
Aluminum nitrate
_______________________
Unit 6 The Mole (Chapter 8)
59. What is Avogadro’s number?
60. How many things are in one mole?
61. What is the molar mass of MgCl2?
62. How many moles of SO3 are in 2.4 x 1024 molecules of SO3?
63. How many atoms of aluminum are present in a 0.275 mole sample of Al 2(CO3)3?
64. How many grams of Ba(IO3)2 are there in a 1.25 x 1022 formula unit sample of Ba(IO3)2?
65. Determine the percentage composition of sulfur in SCl2
66. Given the following percent composition data. Determine the empirical formula of the following compound.
56.8 % C
6.50 % H
28.4 % O
8.30 % N
67. The empirical formula was found to be C2H4O. What is the molecular formula if the molar mass of this
molecule is 132.16?