Chem Ch 2 Test
Multiple Choice
Identify the letter of the choice that
best completes the statement or answers the question.
____
1. The only subatomic
particle that does not carry an electric charge is the
_____.
|
a. |
proton |
c. |
electron |
|
b. |
neutron |
d. |
nucleus |
____
2. The first subatomic
particle discovered was the _____.
|
a. |
proton |
c. |
electron |
|
b. |
neutron |
d. |
nucleus |
____
3. The scientific
statement that says that compounds always have exactly the same composition by
mass is the _____.
|
a. |
atomic
theory |
c. |
law of conservation of
matter |
|
b. |
matter
hypothesis |
d. |
law of definite
proportions |
____
4. When a hypothesis is
tested by many experiments, it becomes a(n) _____.
|
a. |
scientific
law |
c. |
theory |
|
b. |
revised
hypothesis |
d. |
experimental
fact |
____
5. The atomic number of
an element whose atoms have 9 protons and 10 neutrons is
_____.
|
a. |
9 |
c. |
10 |
|
b. |
19 |
d. |
18 |
____
6. The mass number of
an element whose atoms have 12 protons and 13 neutrons is
_____.
|
a. |
12 |
c. |
25 |
|
b. |
13 |
d. |
12.5 |
____
7. One isotope of
carbon has 6 protons and 6 neutrons. The number of protons and neutrons of a
second isotope of carbon would be _____.
|
a. |
7 and 6 |
c. |
7 and 7 |
|
b. |
6 and 7 |
d. |
6 and
6 |
____
8. The correct way to
arrange the three forms of electromagnetic radiation listed below, from highest
to lowest frequency, is _____.
|
a. |
ultraviolet > visible >
infrared |
c. |
infrared > visible >
ultraviolet |
|
b. |
visible > ultraviolet >
infrared |
d. |
infrared > ultraviolet >
visible |
____
9. _____ first proposed
that matter is made up of atoms, the smallest particles of
matter.
|
a. |
Democritus |
c. |
Proust |
|
b. |
Lavoisier |
d. |
Dalton |
____
10. According to the law of
conservation of matter, if 4.0 g of hydrogen react with chlorine to produce 146
g of hydrogen chloride, how many grams of chlorine
reacted?
|
a. |
4.0 g |
c. |
146 g |
|
b. |
142 g |
d. |
150
g |
____
11. If 9.0 g of water contain
1.0 g of hydrogen, what mass of oxygen is contained in 36 g of
water?
|
a. |
4.0 g |
c. |
10.0 g |
|
b. |
8.0 g |
d. |
32
g |
____
12. Which of the following
statements is not a main point of Dalton's atomic theory?
|
a. |
All matter is made up of
atoms. |
|
b. |
Atoms are made up of smaller
particles. |
|
c. |
Atoms are
indestructible. |
|
d. |
All atoms of one element are exactly
alike, but they are different from atoms of other
elements. |
____
13. J.J. Thomson used a
cathode ray to discover the _____.
|
a. |
atom |
c. |
proton |
|
b. |
electron |
d. |
neutron |
____
14. If a scientist studies a
beam of particles, and those particles are attracted to a negatively charged
plate, the particles are most likely _____.
|
a. |
atoms |
c. |
protons |
|
b. |
electrons |
d. |
neutrons |
____
15. What is a good comparison
of the charge of an electron and the charge of a proton?
|
a. |
They are equal, but
opposite. |
c. |
They are the
same. |
|
b. |
The charge of the electron is
larger. |
d. |
The charge of the proton is
larger. |
____
16. Iodine-131 and iodine-127
are examples of _____.
|
a. |
nuclei |
c. |
isotopes |
|
b. |
isomers |
d. |
neutrons |
____
17. The discovery of isotopes
led to the discovery of _____.
|
a. |
atoms |
c. |
protons |
|
b. |
electrons |
d. |
neutrons |
____
18. The experimentation of
_____ led to the theory that the atom is a sphere of mostly empty space, with a
positively charged nucleus with electrons around it.
|
a. |
Bohr |
c. |
Rutherford |
|
b. |
Nagaoka |
d. |
Thomson |
____
19. Which of the following
are definitely in atoms of the same element?
|
a. |
3 protons, 3 neutrons and 3 protons,
4 neutrons |
|
b. |
3 protons, 3 neutrons and 4 protons,
4 neutrons |
|
c. |
4 protons, 4 neutrons and 3 protons,
4 neutrons |
|
d. |
3 protons, 4 neutrons and 4 protons,
3 neutrons |
____
20. Atomic mass units are
based on the mass of an atom of _____.
|
a. |
carbon-12 |
c. |
oxygen-16 |
|
b. |
carbon-14 |
d. |
nitrogen-14 |
____
21. The _____ is where the
electron is most likely to be found.
|
a. |
energy
level |
c. |
electron
cloud |
|
b. |
electron
orbit |
d. |
orbit |
____
22. An atom of iron contains
26 electrons. How many energy levels are needed to contain these
electrons?
|
a. |
1 |
c. |
3 |
|
b. |
2 |
d. |
4 |
____
23. The atomic number of
chlorine is 17. How many valence electrons does an atom of chlorine
have?
|
a. |
2 |
c. |
8 |
|
b. |
7 |
d. |
17 |
____
24. In a Lewis dot diagram,
the dots represent _____ in the atom.
|
a. |
all the
electrons |
c. |
the
protons |
|
b. |
the valence
electrons |
d. |
the
neutrons |
Problem
These three boxes shown in Figure 2-1 are
taken from the periodic table. They represent elements that have no known
isotopes. Use the information contained in these boxes to supply the information
requested for the atoms of each element. For atomic structure, give the number
of protons, neutrons, and electrons.
25. Beryllium:
Mass number for this atom:
Atomic structure:
26. Scandium:
Mass number for this atom:
Atomic structure:
27. Manganese: Mass number for
this atom:
Atomic structure:
The diagram in Figure 2-2 represents a
potassium atom. Answer the questions about the electron transitions that take
place in this atom.
28. How many valence
electrons does this atom have?
29. Draw a Lewis dot diagram
for this atom.
30. Suppose you wanted to
observe an emission spectrum for this atom. How would you produce such a
spectrum? Explain how this action would produce a spectrum.
31. Suppose that a potassium
atom absorbs energy that causes two electrons to move up to the fifth energy
level: one from the fourth energy level and one from the third. In terms of
emission spectra, what will happen when the electrons return to their original
levels?
32. If enough energy was
added to the atom to permit an electron to escape from the atom, which electron
would it be?
This set of data is similar to those on
which Joseph Louis Proust based his law of definite proportions in 1799. Answer
these questions about these data and their
interpretation.
|
Trial |
Nitrogen
Mass |
Oxygen
Mass |
|
101 |
13.9
g |
16.0
g |
|
102 |
25.8
g |
29.2
g |
|
103 |
19.7
g |
22.3
g |
|
104 |
31.8
g |
36.2
g |
33. Calculate the percentage
of nitrogen and oxygen for each of the four trials shown here.
34. To the nearest whole
number, the atomic masses of nitrogen and oxygen are 14 and 16, respectively.
Calculate the percentage composition of a compound made by combining one atom of
nitrogen with one atom of oxygen.
35. Assign a chemical formula
to the compound formed between one atom of nitrogen and one atom of
oxygen.