Ch. 2 Review Textbook Questions
P. 52
1) How long ago were Greek philosophers thinking about the nature of matter and
its composition?
2) How were Greek philosophers similar to modern scientists?
3) How were Greek philosophers different from modern scientists?
P. 53-54
4) What was Democritus’s “atomic theory of matter”?
5) What did Lavoisier measure that led to the Law of Conservation of Matter?
6) What did Proust measure that led to the Law of Definite Proportions?
7) What idea in Dalton’s Atomic Theory would explain the Law of Conservation of
Mass?
8) What idea in Dalton’s Atomic Theory would explain the Law of Definite
Proportions?
P. 59
9) How is a “scientific law” different from a “scientific theory”?
10) What do both a “scientific law” and a “scientific theory” have in common?
11) In the 4th paragraph of this page, a sentence states that “theories explain laws”.
Provide one example supporting this statement.
12) What has to be done before a hypothesis can be formed?
13) What has to be done before a theory or a law can be formed?
P. 61-65
14) What is the charge of an electron?
15) What is the charge of a proton?
16) What is the charge of a neutron?
17) What is the book’s definition of an “isotope” in P. 62?
18) There are 2 atoms that are isotopes of one another. What subatomic particle do
they have equal numbers of?
19) There are 2 atoms that are isotopes of one another. What subatomic particle do
they have different numbers of?
20) How does the mass of a proton relate to the mass of a neutron?
21) Describe Rutherford’s Gold Foil Experiment in a couple sentences.
22) What data led Rutherford to propose that the atom has a nucleus?
23) What is a “nucleus”?
P. 66
24) What does the “atomic number” tell you about an atom?
25) What does the “mass number” tell you about an atom?
26) Write an isotope symbol for each of the 2 isotopes in Figure 2.11.
P. 74
27) What is an “emission spectrum”?
28) How many lines are in an emission spectrum of hydrogen?
29) What did Bohr suggest about electrons based on these emission spectrums?
P. 77-78
30) What is an “electron cloud”?
31) What is a “valence electron”?
32) How many valence electrons does hydrogen have?
33) How many valence electrons does oxygen have?
34) How many valence electrons do atoms in Group 2 have?
P. 79
35) Describe a “Lewis Dot Diagram”.
36) Draw the “Lewis Dot Diagram” of oxygen.
37) What do the dots around the O in oxygen’s Lewis Dot Diagram represent?
38) What would you predict the Lewis Dot Diagram of P to be? Explain your
prediction.
Back to P. 54:
39) What is Dalton’s 1st Point in his Atomic Theory?
40) Is this point still believed to be 100% correct? If no, explain why.
41) What is Dalton’s 2nd Point in his Atomic Theory?
42) Is this point still believed to be 100% correct? If no, explain why.
43) What is Dalton’s 3rd Point in his Atomic Theory?
44) Is this point still believed to be 100% correct? If no, explain why.
P. 50
45) In the sentence “Because of its unique properties, it makes life on Earth
possible.”, what is the word “it” referring to?
P. 51
Read “Launch Lab”. One sentence says, “In trying to determine the structure of the
atom, chemists had a similar experience.”
46) What did scientists have a similar experience to?
47) Why was scientist’s experience similar to that described above?
Ch. 2 Study Guide
Differenciate between a hypothesis, scientific law, and scientific theory.
How have experiments led to changes in the atomic theory?
Reference Dalton’s reliance on the Laws of Conservation of Mass and Definite
Proportions
Reference Thomson’s Cathode Ray Tube Experiments
Reference Rutherford’s Gold Foil Experiments
Reference Bohr’s experiments with emission spectra
Describe the structure of the atom (nucleus, electron cloud, energy levels, protons,
neutrons, and electrons)
Relative mass, charge, and location of each subatomic particle.
Identify the atomic number, mass number, and number of all 3 subatomic particles
given an isotope symbol of any neutral atom.
Or identify the isotope symbol given the # of subatomic particles.
Given the Isotope symbol (or atomic number and mass number) of any neutral
atom: