NAME __________________________________________
PERIOD __________
DATE ___________________________
CHAPTERS 1-11 REVIEW
Write the letter for the correct answer in the blank next to each question. GOOD LUCK!
1. _____ You get a temperature reading in Fahrenheit of T = 105.3 °F. What is this temperature in
Celsius?
a. 65.23 °C
c. 26.50 °C
b. 40.72 °C
d. 76.28 °C
2. _____ You get a temperature reading in Kelvin of T = 10.11 K. What is this temperature in
Fahrenheit?
a. -441.2 °F
c. 541.6 °F
b. -262.9 °F
d. 262.9 °F
3. _____ Which of the following is correct scientific notation for 0.0923?
a. 9.023 x 102
c. 9.23 x 10-2
b. 90.23 x 10-2
d. 0.0923 x 10-2
4. _____ Which of the following is the correct standard number for 6.5723 x 10 3?
a. 6572.3
c. 0.00065723
b. 65.723
d. 65723
5. _____ What is the correct way to write the answer for 25.0/3.4 according to the rules of sig figs?
a. 7.2429
c. 7.35
b. 7
d. 7.4
6. _____ What is the correct way to write the answer for 282 + 4.323 + 2.2 according to the rules of
sig figs?
a. 289
c. 290
b. 288.523
d. 288.5
7. _____ The accepted value for the melting point of Californium (Cf) is 900 °C. You experimentally
find the melting point of Cf to be 850 °C. What is your percent error?
a. -5.6%
c. 50%
b. 5.6%
d. -0.05%
8. _____ What is 7.5 hectoliters (hL) in milliliters (mL)?
a. 750,000 mL
c. 7,500,000 mL
b. 75,000 mL
d. 0.000075 mL
9. _____ What is 2.84 miles/hour in cm/sec?
a. 7618 cm/sec
c. 127 cm/sec
b. 1.44 cm/sec
d. 0.45 cm/sec
10. _____ You are working in a pharmaceutical drug research lab and one day you find an unknown
solid at your desk with a note saying that it has a density of 7.8 g/mL. You find the mass to be 832
g. What is the volume of this unknown solid in liters (L)?
a. 1.1 L
c. 0.11 L
b. 106.7 L
d. 10.67 L
11. _____ The accepted value for the atomic radius of oxygen is 72 pm. You measure the atomic
radius of oxygen multiple times using the same instruments and get the following
measurements: 70 pm, 74 pm, 72 pm, and 73 pm. Are these measurements precise, accurate,
both, or neither?
a. Precise
c. Both
b. Accurate
d. Neither
12. _____ Who determined the charge of an electron using an oil-drop apparatus?
a. J.J. Thompson
c. Ernest Rutherford
b. John Dalton
d. Robert Millikan
13. _____ Who began the development of the modern atomic theory?
a. John Dalton
c. J. J. Thompson
b. Ernest Rutherford
d. Robert Millikan
14. _____ What is the name for particles that are the same element but have a different number of
neutrons?
a. Protons
c. Isotopes
b. Radioactive decay
d. Nucleotides
15. _____ Which of the following is NOT an indicator of a chemical change?
a. Temperature change
c. Size change
b. Color change
d. Odor change
16. _____ What type of a change is frying an egg considered?
a. Physical
c. Digestive
b. Cooking
d. Chemical
17. _____ According to the Law of Conservation of Mass when we have 22.99 g Na react completely
with 35.45 g Cl what mass of NaCl is formed?
a. 58.44 g
c. 12.46 g
b. 116.88 g
d. -12.46 g
18. _____ A 25.3 g sample of an unknown compound contains 0.8 g oxygen. What is the percent by
mass of oxygen in the compound?
a. 25.3%
c. 26.1%
b. 0.032%
d. 3.16%
19. _____ How many neutrons does Au (gold) have?
a. 79
c. 118
b. 197
d. 81
20. _____ What is the wavelength of electromagnetic radiation that has a frequency of 6.12 x 10 14
Hz?
a. 4.90 x 10-7 m
c. 4.90 x 107 m
b. 1.836 x 1023 m
d. 1.836 x 10-23 m
21. _____ What is the energy of a photon that has a frequency of 6.32 x 10 20 Hz?
a. 4.19 x 1013 J
c. 1.05 x 10-54 J
b. 4.19 x 10-13 J
d. 9.54 x 1053 J
22. _____ Which color in the section of visible light on the electromagnetic spectrum has the lowest
energy and highest frequency?
a. Blue
c. Violet
b. Orange
d. Red
23. _____ What is the noble gas electron configuration for Cobalt?
a. [Ar]4s23d7
c. [Ar]4s13d7
b. [Ar]4s23d6
d. [Ar]4d75p2
24. _____ What are the two subatomic particles found in the nucleus of an atom?
a. Electrons and neutrons
c. Electrons and protons
b. Neutrons and protons
d. Alpha particles and beta particles
25. _____ Where are valence electrons located in an atom?
a. Highest energy level
c. Lowest energy level
b. Everywhere
d. Nowhere
26. _____ What is the name for FeSO4?
a. Iron (I) sulfate
c. Iron (II) sulfide
b. Iron sulfide
d. Iron (II) sulfate
27. _____ What is the formula for hydrochloric acid?
a. HCl
c. HClO2
b. HClO
d. HClO3
28. _____ Why do elements in a group tend to have similar chemical properties?
a. They have the same number of neutrons.
b. They have the same number of valence electrons.
c. They have the same number of protons.
d. Elements in the same group don’t tend to have similar chemical properties.
29. _____ Which element has the highest electronegativity?
a. Oxygen
c. Nitrogen
b. Chlorine
d. Fluorine
30. _____ Which element is NOT needed to complete a hydrogen bond?
a. Nitrogen
c. Fluorine
b. Iron
d. Oxygen
31. _____ What are available to be lost, gained, or shared when atoms bond and form compounds?
a. Ions
c. d electrons
b. Valence electrons
d. Protons
32. _____ The equal but opposite charges present in two regions of a polar molecule create what?
a. Dipole
c. Crystal lattice
b. Electron sea
d. Ionic bond
33. _____ Out of the following, which is the strongest intermolecular force?
a. Hydrogen bond
c. Dipole-dipole force
b. Ionic bond
d. Dispersion force
34. _____ Which type of reaction occurs when two or more substances combine to form a single
compound?
a. Double replacement
c. Decomposition
b. Single replacement
d. Synthesis
35. _____ The reaction between aluminum sulfate and potassium hydroxide is an example of which
type of reaction?
a. Double replacement
c. Decomposition
b. Single replacement
d. Synthesis
36. _____ How many atoms are in 0.230 g of Pb?
a. 47.66 Pb atoms
c. 1.84 x 10-27 Pb atoms
b. 6.68 x 1020 Pb atoms
d. 47.66 x 1020 Pb atoms
37. _____ What is the molecular formula for a compound that contains 46.68% N and 53.32% O and
has a molar mass of 60.01 g/mol?
a. N2O2
c. NO
b. N2O
d. NO2
38. _____ How much O2 is needed to combust 25.0 g CH4?
a. 99.94 g O2
c. 9.99 g O2
b. 49.84 g O2
d. 800 g O2
39. _____ What is the limiting reactant when 0.656 g HCl and 0.656 g Ca(OH)2 react?
a. HCl
c. H2O
b. CaCl2
d. Ca(OH)2
40. _____ You perform an experiment and get 515.6 g of product, but in your calculations before
performing the experiment you calculated that you should have gotten 610.3 g of product. What
is your percent yield?
a. 84.48%
c. 0.84%
b. 1.18%
d. 94.70%