Download File

Station 1: Parts of an Atom
PART I: Model of an Atom
Make an atom of Boron-10 by placing the correct number of subatomic
particles on the diagram. Use a different color for each subatomic
particle.
Nucleus
Key:
= protons
= neutrons
= electrons
PART II: Questions
1. Which particles make up most of the mass of the atom?
2. Most of the volume of the atom is ______ .
a. Neutrons
b. Protons
c. empty space
d. electrons
3. Most of the mass of the atom is due to __________.
I. Nucleus
IV. Electrons
II. Protons
V. Electron Cloud
III. Neutrons
a. I, II, and III
b. I and V
c. I, II, and IV
d. IV and V
4. What is the charge of the nucleus? ____________
5. What is the charge of the electron cloud? __________
6. How does the mass of an electron compare to the mass of a
proton or neutron?
7. Which two particles will always occur in the same numbers in
a neutral atom?
Station 2: Calculating Protons, Neutrons, and Electrons
An atom with a mass of 65
amu and an atomic number Copper-65
of 29
An isotope with 33 protons,
42 neutrons, and 33
Arsenic-75
electrons
An atom that contains 64
neutrons and has a mass of Indium-113
113 amu
An atom with a nucleus that
contains 80 protons and 118 Mercury-198
neutrons
An isotope that is made up
Antimony-121
of 51 electrons and 51
protons
An atom that has 72
Tin-122
neutrons and 50 electrons
Lithium-6
Helium-4
Lithium-7
Sodium-23
Station 3: Isotopes
1.
Isotopes are atoms of an element with identical chemical
properties but with different
a. numbers of protons.
b. masses.
c. numbers of electrons.
d. atomic numbers.
2.
The reason isotopes have different masses is because they
have different numbers of
a. protons
b. electrons
c. neutrons
d. energy levels
3.
Isotopes of the same element must have the same number of
a. protons
b. electrons
c. neutrons
d. energy levels
4.
The weighted average of the masses of the stable isotopes of
an element as they occur in nature is called the
a. atomic number.
b. atomic mass.
c. atomic weight.
d. mass number.
5.
The isotope shown above has ____ protons ____ electrons,
____ neutrons, and a mass number of ______.
6.
Which of the following are isotopes of each other? (There
are 2 pairs of isotopes and one that is not an isotope of any of
the others.)
I. An atom with 17 protons and 18 neutrons
II. An atom with an atomic number of 16 and 18 neutrons
III. An atom with 17 protons and 20 neutrons
IV. An atom with an atomic number of 16 and an atomic
mass of 33
V. An atom with 15 protons and 16 neutrons
_____ and _____ are isotopes of each other
_____ and _____ are isotopes of each other
Station 4: Average Atomic Mass
1. Boron has two naturally occurring isotopes with masses of
10.0129 amu (19.91% abundance) and 11.0093 amu (80.09%
abundance). Calculate the average atomic mass of boron.
2. Calculate the average atomic mass of silicon based on the
following information:
3. Bromine has two isotopes with the first having a mass of
78.918336 amu (50.69% abundance) and the second isotope
having a mass of 80.916289 amu (49.31% abundance). What is
the average atomic mass of bromine?
4. The following data was collected for an unknown element.
34.96885 amu and percent abundance of 75.77%
36.96590 amu and percent abundance of 24.23%
a. What is the average atomic mass for this element?
b. What is the identity of the element?
5. Two isotopes of potassium exist in nature: potassium-39 and
potassium-41. Potassium has an atomic mass of 39.0983 amu.
Which isotope of potassium is more abundant in nature?
Justify your answer.
Station 5: Radioactive Particles
Alpha Particles
Beta Particles
1- charge
Electron
2+ charge
No charge
Helium Nucleus
0.0055 amu
Stopped by paper,
wood, cloth, etc.
Least dangerous to
humans
Gamma Radiation
Electromagnetic
Radiation
4 amu
0 amu
Stopped by
aluminum or other
metals
Most dangerous to
humans
Stopped by lead
Label each particle that would be stopped by skin, aluminum, and lead.
1.
The mass of two protons is approximately equal to the mass of
a. an alpha particle
b. a positron
c. a beta particle
d. a neutron
2.
Compared to the mass and the penetrating power of an alpha particle, a beta particle
has
a. less mass and greater penetrating power
b. less mass and less penetrating power
c. more mass and greater penetrating power
d. more mass and less penetrating power
3.
Which particle has the least mass?
a. alpha particle
b. neutron
c. beta particle
d. proton
4.
Which of the following types of radiation is composed of particles with a
charge and mass identical to that of an electron?
a. a l p h a p a r t i c l e s
b. b e t a pa r ti c l es
c. g a m m a r a d i a t i o n
d. X - r a y s
5.
In
a.
b.
c.
d.
6.
Which of the following statements concerning the penetrating power into matter of
various types of radiation is CORRECT?
a. Alpha and beta particles penetrate equally.
b. Alpha particles penetrate deeper than beta particles.
c. Alpha particles and gamma radiation penetrate equally.
d. Gamma radiation penetrates deeper than alpha particles.
terms of subatomic particles, the composition of an alpha particle is
three neutrons and a proton.
two neutrons and two protons.
one neutron and three protons.
one neutron and two protons.
Station 6: Balancing Nuclear Equations
For each of the statements below write out the decay equation using the cards
provided. Remember that the nuclear reactions must be balanced in terms of
mass and atomic number.
1) Alpha decay of uranium-233
2) Beta decay of carbon-14
3) Beta decay of nitrogen-16
4) Alpha decay of platinum-192
5) Beta decay of phosphorus-32
6) Alpha decay of radium-226 with gamma emission
229
90
Th
14
6
C
0
1
0
1
32
15
32
16
4
2
He
14
7
N
e
192
78
e
0
1
P
S
4
2
4
2
Pt
233
92
U
16
8
O
0
0

e
188
76
Os
He
226
88
Ra
He
222
86
Rn
16
7
N
+


+
+
+
+
+




Balancing Nuclear Equations Answer Key
233U229Th  4 He
1)
92
90
2
2)
14C14 N 0e
6
7 1
16 N 0 e16O
3)
7
-1
8
192Pt 4 He188Os
4)
78
2
76
32P 0 e32S
5) 15
- 1 16
226 Ra4 He222Rn 0
6)
88
2
86
0
Station 7: Fusion vs. Fission
1. Given the balanced equation representing a nuclear reaction:
2H  3H4 He1n
1
1
2
0
Which phrase identifies and describes this reaction?
a. fission, mass converted to energy
b. fission, energy converted to mass
c. fusion, mass converted to energy
d. fusion, energy converted to mass
2. During a nuclear reaction, mass is converted into
a. Charge
b. Isomers
c. Energy
d. Volume
3. Which type of reaction releases the greatest amount of energy
per mole of reactant?
a. combustion
b. nuclear fission
c. nuclear fusion
d. oxidation-reduction
4. What type of nuclear reaction occurs in the sun?
a. nuclear fission
b. nuclear fusion
5. What type of nuclear reaction occurs in a nuclear reactor?
a. nuclear fission
b. nuclear fusion
6. Label the following illustrations as fission or fusion.
a.
b.
Station 8: Half-Life
1. After 4 half-lives have elapsed, the amount of a radioactive sample which has NOT decayed
is
a. 1/4 the original amount
b. 1/8 the original amount
c. 1/16 the original amount
d. 1/32 the original amount
2. Radioisotopes used in diagnostic medical procedures are usually
a. Radionuclides with short half-lives.
b. Radionuclides with long half-lives.
Explain your answer.
3. Are isotopes with short half-lives or long half-lives more stable? Justify your answer.
4. Use the graph to the below to answer the following questions.
a. What is the half-life of for the unknown isotope?
b. What mass of the unknown isotope will remain after 300 years?
c. How much time would it take for 20 g of the unknown isotope to decay?