Atomic Theory Questions – Use Development of Atomic Theory to answer on separate paper.
Dalton’s Atomic Theory Quiz
1.
What year was his theory published?
2.
Which previous finding defined compounds as having consistent percent compositions?
3.
How did Dalton describe chemical reactions?
4.
How can atoms of the same element be different?
Thomson’s Atomic Theory Quiz
5. How did Thomson know that the rays came from the cathode?
6. What did Thomson conclude from cathode rays being bent by a magnet?
7. How did Thomson know cathode rays were fundamental to matter?
8. In Thomson’s model of the atom where is the positive charge?
Rutherford’s Model Quiz
9. What could Rutherford actually observe in the Gold Foil Experiment?
10. What evidence did Rutherford find to suggest that atoms have a nucleus?
11. What evidence was their that atoms are mostly empty space?
12. Where did Rutherford suggest that electrons must be found?
Bohr Model Quiz
13. What 3 natural phenomena is Bohr’s Model designed to explain? ____ _____ , _____ & _____
14. When light is absorbed electrons move between what 2 states?
15. Which way do electrons move when light is emitted?
16. What color light has the most energy?
17. Which of the following scientific laws was Dalton able to explain as due to compounds always having the same percentage composition? a. Law of Conservation of Energy b. Law of Definite Composition c. Law of Conservation of Mass d. Law of Multiple Proportions

18. Which of the following was NOT a key point of Dalton’s atomic theory? a. atoms are indivisible and indestructible. b. atoms are mostly empty space. c. atoms of an element are identical in mass. d. atoms combine in simple whole number ratios to form compounds.
19. Which of the following is NOT an update to Dalton’s atomic theory? a. Atoms are divisible and composed of smaller particles. b. Atoms can be converted into other types in a nuclear reaction. c. Atoms of an element are not identical and can differ in mass. d. Atoms of different elements are different in mass.
20. How did they know that cathode rays are not light? a. Cathode rays originated at the cathode. b. Cathode rays are attracted toward a positively charged electrode. c. Cathode rays are bent by a magnet. d. Thomson observed the same behavior of cathode-ray particles using a variety of gases in the
Crookes tubes and a variety of materials for electrodes.
21. What evidence indicated that each atom has a nucleus? a. When alpha particles are shot at gold foil some alpha particles are deflected slightly or at large angles. b. Each time an alpha particle hit this zinc sulfide coating, a flash of light was produced at the point of contact. c. Positively charged alpha particles were deflected rather than attracted by the gold nuclei.
d. Nearly all the alpha particles passed straight through as though there were no foil there.
22. How do atoms emit specific colors of light? a. The farther from the nucleus the more energy an electron has. b. Electrons tend to occupy the lowest possible energy levels. c. When excited electrons drop back down to lower energy levels it releases light of corresponding energy. d. When an electron absorbs a specific amount of energy it will be boosted to a higher energy level.
23. Who discovered the electron energy levels? a.
J.J. Thomson c. Ernest Rutherford b. Neils Bohr d. Albert Einstein
24.
What did the discoverer of the nucleus think that an atom looked like? a. Positive and negative charges are distributed evenly throughout the mass of an atom like plums in plum pudding

b. Electrons orbit the nucleus in distinct energy levels. c. Atoms consist of a small, massive, positively charged central portion surrounded mainly by empty space where electrons orbited like planets. d. Electrons occupy orbital clouds in complicated patterns around the positive nucleus.
25. Which of the following scientific laws was Dalton able to explain as due to atoms simply rearranging in a chemical reaction? a. Law of Conservation of Energy c. Law of Conservation of Mass b. Law of Definite Composition d. Law of Multiple Proportions
26. Which of the following was NOT a key point of Dalton’s atomic theory? a. atoms are indivisible and indestructible. b. atoms combine in simple whole number ratios to form compounds. c. atoms of an element are identical in mass. d. atoms have a nucleus of concentrated positive charge.
27. Which of the following is NOT an update to Dalton’s atomic theory? a. Atoms of an element are identical, particularly in mass. c. Atoms of an element are not identical and can differ in mass. d. Atoms are divisible and composed of smaller parts. b. Atoms can be converted into other types in a nuclear reaction.
28. How did they know that cathode rays have a negative charge? a. Cathode rays originated at the cathode. b. Cathode rays are attracted toward a positively charged electrode. c. Cathode rays are not light. d. Thomson observed the same behavior of cathode-ray particles using a variety of gases in the
Crookes tubes and a variety of materials for electrodes.
29. What evidence is there that atoms are mostly empty space? a. When alpha particles are shot at gold foil some alpha particles are deflected slightly or at large angles. b. Each time an alpha particle hit this zinc sulfide coating, a flash of light was produced at the point of contact. c. Positively charged alpha particles were deflected rather than attracted by the gold nuclei.
d. Nearly all the alpha particles passed straight through as though there were no foil there.
30. How do atoms absorb specific colors of light? a. The farther from the nucleus the more energy an electron has. corresponding energy. d. When an electron captures a specific amount of energy it will be boosted to a higher energy level. b. Electrons tend to occupy the lowest possible energy levels. c. When excited electrons drop back down to lower energy levels it releases light of

31. Who discovered that atoms have a nucleus? a.
J.J. Thomson c. Ernest Rutherford b.
c. Neils Bohr d. Albert Einstein
32.
What did the discoverer of the electron think that an atom looked like? a. Positive and negative charges are distributed evenly throughout the mass of an atom like plums in plum pudding. b. Electrons orbit the nucleus in distinct energy levels. c. Atoms consist of a small, massive, positively charged central portion surrounded mainly by empty space where electrons orbited like planets. d. Electrons occupy orbital clouds in complicated patterns around the positive nucleus.