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Midterm Review: Start NOW!!!

Chemistry

Midterm Review Sheet

 

Text: Chapters 1-8; all notes, practice problems, homework

Topics:

Physical States of Matter; Heterogeneous and Homogeneous Matter

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, Dalton,  Thomson,  Millikan, Goldstein,  Rutherford , Chadwick)

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 - 9:  39 , 42, 43, 44, 61, 65

Chapter 4: Problem Solving:  pp. 103- 4:  43 , 44, 48

Chapter 5: Atomic Structure and the Periodic Table: p. 129:  33 43

Chapter 6:  Chemical Names and Formulas: pp. 166 - 7:  49 , 64

Chapter 7: Chemical Quantities (the MOLE): pp. 198 - 9: 45 , 49, 51, 55, 56, 60, 62, 66

Chapter 8: Sample test

Answers to review problems:

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 10mL

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 10 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 10 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)  8 H2O  -->   Ba(OH)+  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

 

 

 

 

 

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