Midterm Review: Start NOW!!!
Chemistry
Midterm Review Sheet
Text: Chapters 1-8; all notes, practice problems, homework
Topics:
Chemical and Physical Properties
Chemical and Physical Changes
Metric Prefixes
Significant Figures
Conversion factors and Dimensional Analysis
Density
Convert among Celsius, Fahrenheit, and the Kelvin temperature scale
Atomic theory ( Leucippus and Democritus,
Subatomic particles
Mass number, Atomic number, Isotope
Nuclear notation and Isotope notation
Calculate the atomic mass of an element given the percent abundance and relative atomic mass of the isotope(s)
Determine the relative mass and percent abundance of an unknown isotope given the atomic mass, the relative mass and percentage of the other isotope(s)
Organization of the Periodic Table
Ionic vs. Molecular compounds
Nomenclature
Convert among mass, representative particles, and mole of a given substance
Calculate percent composition of a substance from its chemical formula or experimental data
Derive the empirical formula of a compound from experimental data
Derive the molecular formula of a compound from experimental data
Chemical Reactions
Chemistry Review Problems
From Text
Chapter 2: Matter and Change: p. 47: 30, 32, 34, 35, 42
Chapter 3:
Scientific Measurement: p. 78 -
Chapter 4: Problem
Solving: pp. 103-
Chapter 5: Atomic Structure and the Periodic Table: p. 129: 33 – 43
Chapter 6:
Chemical Names and Formulas: pp. 166 -
Chapter 7: Chemical
Quantities (the MOLE): pp. 198 -
Chapter 8: Sample
test
Chapter 2:
30.a. heterogeneous b. heterogeneous c. homogeneous d. homogeneous e. homogeneous
32.a. element b. mixture c. mixture d. element e. mixture f. mixture
34. color change, odor change, energy absorbed or released, gas produced, precipitate forms
35. a. physical b. chemical c. chemical d. physical
42. a. physical b. physical c. physical d. physical e. chemical
Chapter 3
39. Lissa: inaccurate and imprecise; Lamont: accurate and precise; Leigh Anne: inaccurate but precise
42.a. 98.5 L b. 0.000763 cg c. 57.0 m d. 12.2 oC e. 7.50 x 10 mm f. 1.76 x 103 mL
43. a. 9.85 x 10 L b. 7.63 x 10-4 cg c. 5.70 x 10 m d. 1.22 x 10 oC e. 7.50 x 10 mm f. 1.76 x 103 mL
44. a. 43 g b. 7.3 cm2 c. 225.8 L d. 92.0 kg e. 32.4 m3 f. 104 m3
61. 12 g/cm3
65. Ge
Chapter 4
Be sure to use proper dimensional analysis setup for these problems!!!!
43.a. 1.57 s b. 4.27 x 104 mL c. 2.61 x 10 -4 mm d. 6.5 x 102 dm e. 6.42 x 10-3 kg f. 8.25 x 109 ng
44.a. 7.3 mL/s b. 78.6 mg/mm2 c. 1.54 g/cm3
48. 0.804 g/cm3
Chapter 5
33. a - d, all true
34. a. A beam of electrons (cathode ray) is deflected by an electrical field toward the positively charged plate.
b. The cathode rays were always composed of electrons regardless of the metal used in the electrodes or the gas used in the cathode ray.
35. repel
36. He did NOT expect any alpha particles (Helium nuclei) to be deflected over a large angle.
37. positive
38. number of protons = number of electrons
39. number of protons
40.a. 15 b. 42 c. 13 d. 48 e. 24 f. 82
41. atomic number (Z) = number of protons; mass number (A) = number of protons + neutrons
42. 9 19 9 10 9 F
14 29 14 15 14 Si
22 47 22 25 22 Ti
25 55 25 30 25 Mn
43. 1. mass number 2. atomic mass 3. number of neutrons 4. relative abundance
44. due to isotopes
45. 1. how many isotopes 2. atomic mass of each isotope 3. abundance of isotopes
46. weighted average of masses of all isotopes
47. (various answers)
48. Moseley: increasing atomic number; Mendeleev: increasing atomic mass
49. a. C b. La c. B, Ne, P, Br d. Hg, Br e. Bi
50. nucleus is very small and very dense
51. 5 protons and 6 neutrons in nucleus; 5 electons outside nucleus
52. 1. All atoms of the same element are not identical (due to isotopes)
2. The atom is NOT the smallest particle of matter
53. 207 amu
Chapter 6 (Review naming ALL compounds using notes, text, homework and test)
49.a. ionic b. molecular c. ionic d. molecular e. ionic f. molecular
64.a. Boron trichloride b. Dinitrogen tetrahydride c. N2O5 d. CCl4
Chapter 7
45.a. molecule (diatomic element) b. formula unit c. molecule d. atom
Use Dimensional Analysis for 49, 51, and 55!!
49. a. 1.81 x 1024 atoms Sn b. 2.41 x 1023 formula units KCl c. 4.52 x 1024 molecules SO2 d. 2.89 x 1021 formula units NaI
51.a. 60.1 g SiO2 b. 28.0 g N2 c. 107 g Fe(OH)3 d. 63.6 g Cu
55.a. 0.258 mol SiO2 b. 4.80 x 10-4 mol AgCl c. 1.12 mol Cl2 d. 0.106 mol KOH e. 5.92 mol f. 0.0200 mol Ca
56.a. 108 g C5H12 b. 547 g F2 c. 71.9 g Ca(CN)2 d. 238 g H2O2 e. 224 g NaOH f. 1.88 g Ni
60. H: 5.9 % S: 94.1 %;
62.a. 44.1 % b. 24.0 % c. 62.1 % d. 77.7 %
Chemical Reactions Sample test:
1. S 4 Ag + O2 --> 2 Ag2O
2. SR 2 Li + ZnCl2 --> Zn + 2 LiCl
3. S N2O5 + H2O --> 2 HNO3 (aq)
4. D Ba(OH)2 . 8 H2O --> Ba(OH)2 + 8 H2O
5. C C4H8 + 5 O2 --> 4 CO2 + 2 H2O
6. S 4 Na + O2 --> 2 Na2O
7. DR 3 Zn(NO3)2 + 2 Na3PO4 --> Zn3(PO4)2 + 6 NaNO3
8. SR 2 NaBr + F2 --> 2 NaF + Br2
9. DR Pb(C2H3O2)2 + 2 KCl --> PbCl2 + 2 KC2H3O2
10. D omit
11. S 2 Sr + N2 --> 2 SrN
12. C 2 C8H18 + 17 O2 --> 16 CO2 + 18 H2O
13. D omit
14. DR Mg(OH)2 --> MgO + H2O
15. SR CaCl2 + Br2 --> NR
16. DR 2 NaOH + BaBr2 --> 2 NaBr + Ba(OH)2
17. D 2 NH3 --> N2 + 3 H2
18. S 2 Al + N2 --> 2 AlN
19. SR Cu + AgNO3 --> Ag + CuNO3
20. SR Al2O3 + Fe --> NR