Download Match the person / institution with the concept / discovery

Chemistry
Unit 4
History of Atomic Theory
Review
Answer on your own paper!!!!!
Match the person / institution with the concept / discovery / conclusion / law / model.
Aristotle
Lavoisier
Proust
Boyle
Leucippus/Democritus
Rutherford
Chadwick
Millikan
Thomson
Dalton
Moseley
1.
Conducted the oil drop experiment
2.
Proposed that there were four elements
3.
Suggested that if matter was divided multiple times, eventually it would
reach a smallest, indivisible particle
4.
Measured the charge and mass of the electron.
5.
Explained the differences in atoms of different elements by claiming they
had different sizes and shapes.
6.
Explained the differences in atoms of different elements by claiming they
had different weights.
7.
Stated periodic law.
8.
Discovered the nucleus.
9.
discovered the electron.
10.
discovered the neutron.
11.
conducted the gold foil experiment.
12.
developed the nuclear model of the atom.
13.
proved the law of conservation of mass.
14.
“Father of Atomic Theory”
15.
Developed the law of constant composition.
16.
Developed the law of multiple proportions.
State the law in complete sentences using correct spelling, grammar, and punctuation.
17. Law of conservation of mass
18. Law of constant composition
19. Law of multiple proportions
20. Periodic law
Thomson’s Cathode Ray Experiment
21. What behavior of the cathode ray did Thomson witness?
a. It traveled in a straight line.
b. It bent toward the negative plate and away from the positive plate.
c. It bent toward the positive plate and away from the negative plate.
d. The behavior of the rays was erratic and could not be predicted.
22. What did he conclude from his data (observations of the rays under different conditions)?
a. All cathode rays contained negatively charged particles.
b. All substances contained the particles found in cathode rays.
c. The ratio between the mass and charge of every cathode ray particle was identical.
d. All of the above.
23. What is the name of Thomson’s atomic model?
a. Wave model
b. Planetary model
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Chemistry
Unit 4
History of Atomic Theory
Review
c. Plum pudding model
d. Nuclear model
24. Which of the following is a description of Thomson’s model?
a. Negative electrons are found around a small, dense, massive, positive nucleus
containing positive protons and neutral neutrons. The behavior of each electron is
described in terms of probabilities that are used to identify a region of space in which
there is a high probability of finding an electron of that energy.
b. Negative electrons are found outside a small, dense, massive, positively charged
nucleus, but most of the atom is empty space.
c. Negative electrons move around a small, dense, massive, positively charged nucleus
like planets orbit the sun.
d. Negative electrons are scattered through a positive mass or matrix.
25. Which of the following concepts were parts of Thomson’s model?
a. The existence of protons
b. The existence of neutrons
c. The existence of a nucleus
d. The existence of electrons
26. Which of the following was NOT discovered by Thomson’s experiments?
a. Light behaves like particles.
b. Electrons behave like waves
c. Atoms of all elements contain electrons.
d. The nucleus of the atom is positive.
Rutherford’s Gold Foil Experiment
27. What type of particles, produced by radioactive decay of uranium, was “shot” at the gold foil in
the experiment?
a. Gamma rays
b. Beta particles
c. Neutrons
d. Alpha particles
28. What were the characteristics of the particles that were “shot” at the foil?
a. Small volume, very little mass, positive charge
b. Large volume, very little mass, positive charge
c. Large volume, large mass, negative charge
d. Small volume, very little mass, negative charge
29. What behavior was observed during the experiment?
a. Most alpha particles passed directly through the gold foil with no change in their direction.
A small number of alpha particles were deflected. A very small number of alpha particles
were reflected backward.
b. Most cathode rays passed directly through the gold foil with no change in their direction. A
small number of cathode rays were deflected. A very small number of cathode rays were
reflected backward.
c. Very few cathode rays passed directly through the gold foil with no change in their
direction. Most cathode rays were deflected. A small number of cathode rays were
reflected backward.
d. Very few alpha particles passed directly through the gold foil with no change in their
direction. Most alpha particles were deflected. A small number of alpha particles were
reflected backward.
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Chemistry
Unit 4
History of Atomic Theory
Review
30. Which of the following statements are conclusions Rutherford made from the data of the gold
foil experiment?
i. Most of the atom is empty space.
ii. Neutrons are negatively charged particles found in the nucleus.
iii. Almost all of the mass of the atom is concentrated in a small, positively charged center.
iv. Protons are positively charged particles found in the nucleus.
v. Electrons orbit the nucleus like planets.
a. i, iv, v
b. iii, iv,
c. i, iii
d. i, iii, iv, v
31. What is the name of Rutherford’s atomic model?
a. Wave model
b. Planetary model
c. Plum pudding model
d. Nuclear model
32. Which of the following is a description of Rutherford’s model?
a. Negative electrons are found around a small, dense, massive, positive nucleus containing
positive protons and neutral neutrons. The behavior of each electron is described in terms
of probabilities that are used to identify a region of space in which there is a high probability
of finding an electron of that energy.
b. Negative electrons are found outside a small, dense, massive, positively charged nucleus,
but most of the atom is empty space.
c. Negative electrons move around a small, dense, massive, positively charged nucleus like
planets orbit the sun.
d. Negative electrons are scattered through a positive mass or matrix.
33. Which of the following concepts were parts of Rutherford’s model?
a. The existence of protons
b. The existence of neutrons
c. The existence of a nucleus
d. The existence of gamma rays
34. Which of the following was NOT discovered by Rutherford’s experiments?
a. Light behaves like particles.
b. Electrons behave like waves
c. Atoms of all elements contain electrons.
d. The nucleus of the atom is positive.
Short Answer Questions. Answer in complete sentences using correct spelling, grammar, and
punctuation for all questions.
35. State the two reasons that Aristotle disagreed with the concept of atoms proposed by
Leucippus and Democritus.
36. State the major concepts of Dalton’s atomic theory.
37. Sketch and label the apparatus used by Thomson in his cathode ray experiment.
38. Sketch and label the apparatus used by Rutherford in his gold foil experiment.
39. Give the location within the atom of a/an
a. Proton
b. Neutron
c. Electron
40. T/F (each statement): All atoms of the same element
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Chemistry
Unit 4
History of Atomic Theory
Review
a. Have the same number of protons
b. Have the same number of electrons
c. Have the same number of neutrons
d. Have the same mass number
e. Have the same atomic number
f. Have the same measured mass
41. Explain how isotopes of the same element can have different mass numbers.
42. Identify how often the following are on the periodic table: always, frequently, rarely, never
a. Element name
b. Element symbol
c. Atomic number
d. Mass number
e. Atomic mass
f. Isotope symbol
43. Neutral atoms must have equal numbers of
and
.
44. Complete the table:
Isotope name
Isotope
symbol
Atomic
number
Mass
number
Manganese-55
33
17
37
75
37
85
Charge
# of
protons
# of
neutrons
# of
electrons
3
20
9
4
21
10
3
18
10
0
0
11+
45. Explain the difference in atomic mass and mass number.
46. Calculate the atomic mass of the following elements
a. Sulfur Sulfur (32S: 94.93%, 31.972u; 33S: 0.76 %, 32.971u; 34S: 4.29%, 33.968u; 36S: 0.02%,
35.967 u)
b. Zinc (64Zn, 48.63%, 63.929u; 66Zn: 27.90%, 65.926u; 67Zn: 4.10%, 66.927u; 68Zn: 18.75%,
67.925u, 70Zn: 0.62%, 69.925u)
c. Oxygen (16O: 99.76 %, 15.995 u; 17O: 0.038 %, 16.999 u; 18O: 0.205 %, 17.999 u)
d. Helium (3He: 1.37 x 10-4 %, 3.016 u; 4He: ~100%, 4.003 u)
47. Write the alpha decay equation for
a. Protactinium-231
b. Americium-241
c. Einsteinium-252
d. Radium-226
48. Write the beta decay equation for
a. Hydrogen-3
b. Magnesium-28
c. Iodine-131
d. Selenium-75
49. Identify each reaction as alpha decay, beta decay, or gamma decay.
a. 21484Po  21082Pb + 42He
b. 178O*  178O + 
c. 21083Bi + 21084Po + 0-1e
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