Download p Atomic Structure notes packet 14_15

Academic Chemistry
UNIT 3
BASIC ATOMIC STRUCTURE
Monday
September 22
29
Notes: Isotopes and
Ions
(p. 6-7)
Tuesday
24
30
Average Atomic
Mass (p. 10)
October 1
Hwk: pg 11
Hwk: 8-9
6
Start 2nd 6 Weeks
Radioisotopes and
Nuclear Particles (p.
18)
Hwk: pg. 19
Study Guide P. 22-28
13
Wednesday
23
7
Fission and Fusion
(p. 21-22)
Read Pg. 22 and
complete P. 23
Hwk- Finish Study
Guide P. 22-28
14
Student Holiday!
Thursday
Matter and
Thermo
TEST
6 weeks
Cumulative
TEST
8
Review
Friday
26
History of the Atom
(p.3-4)
Atomic Structure
Notes (p. 2)
Hwk: pg 5
2
Lab – Average
Atomic Mass
(p.12)
3
EARLY DISMISSAL
End of
st
1 Six Weeks
Hwk: pg 13-14
Nuclear Particles
Notes (pg 15-16)
Hwk- P. 17
9
10
UNIT 3 TEST
Start Nomenclature
Unit
16
17
Hwk- Study for
the Test!
15
PSAT test
Name:
Class Period:
Test Date: Thursday 10/9/14
1
Basic Atomic Structure
WARM-UP:
Label the following items on the atom at right:
Nucleus
Electrons
Outside the Nucleus
Protons
Neutrons
Complete the following Content Frame:
Subatomic
Particle
Location
Charge
Mass
Electron
Proton
Neutron
NOTES:
•
Reading the periodic table:
•
Atomic Number: The number of _____________________________ in an atom. It
also equals the number of ___________________________ in a neutral atom.
•
Mass Number = ______________________ + _______________________
•
# of Neutrons = _____________________ – _______________________
•
Atomic Mass: The _______________________ of all naturally occurring isotopes.
•
Use the acronym “APE MAN” to help you remember the above calculations:
Atomic number = Protons = Electrons
Mass number = Atomic number + Neutrons
2
APE MAN
Democritus
Dalton
Thomson
Rutherford
Plum Pudding Model
Bohr
Electron Cloud Model
3
Dalton
What year did he publish his atomic theory?
Democritus (440 B.C.)
What did he call the tiniest piece of matter?
What did he propose?
List the postulates of his theory.
What was missing or wrong with his theory?
Rutherford
When did he make his discovery?
Thomson
When did he make his discovery?
Describe his experiment.
What subatomic particle did he discover?
Draw his model.
What TWO discoveries did he make about the atom?
His model was different from Thomson’s model by
thinking that the atom resembles our
_________________.
New Model View
What is the basis of this new model?
Bohr
When did he make his discovery?
He thought electron only traveled in _____________
paths around the nucleus.
What is the name for this model?
These electrons follow these orbits which he called
________________ _________________.
Label the model with the # of electrons in each energy
levels:
What is the name of his model?
4
Homework: Atomic Models:

Count the number of protons, neutrons, and electrons in each Model.

Use the Atomic number and the Periodic Table to determine the true identity of the element.
Element
# of
Protons
# of
Neutrons
# of
Electrons
ATOMIC #
MASS #
NAME
Symbol
Zippy
WoWie
Tigerium
4
5
6
Answer the questions below.
1.
How did you determine the name of the element?_____________________________________
2. One subatomic particle adds no mass to the atom. Which one is it?(see background)___________
3. Which subatomic particles added together equal the mass #? ____________________________
4. Using the model of an atom, as in this lab, how do you find the Atomic # of an atom? __________
__________________________________________________________________________
5. Using the model of an atom, as in this lab, how do you find the Mass # of an atom?____________
__________________________________________________________________________
6. Conclusion: Write a rule concerning how to identify an atom from its parts.
Review History of the Atom:
1. Thomson’s experiments with cathode ray tube led to the discovery of the _________________.
2. Who was the first person to suggest the idea of atoms in the fourth century B.C.?
3. Who stated that electrons do not move about an atom in definite paths but in large regions (clouds)
determined by energy?
4. Consider the following selected postulates of Dalton’s atomic theory: Circle the statement(s) below that is
(are) no longer considered to be true?
i. Each element is composed of extremely small particles called atoms.
ii. Atoms are indivisible.
iii. Atoms of a given element are identical.
iv. Atoms of different elements are different and have different properties.
5. Complete the History of the Atom Timeline
1
Date:
2
3
4
440 BC
5
1831
Inventor:
Bohr
5
6
NOTES: Isotopes and Ions
WARM-UP:
1. Complete the labels below and fill in the blanks in the statements to the right.
NOTES: Isotopes and Ions
•
Isotopes – Have the same number of __________________________ but a different number
of __________________________.
– If an atom is an isotope you name it using the element name followed by the
________________________________________.
 Ex:
–
Writing Isotope Symbols:
1. Write the atomic symbol for the element.
2. To the top left of the symbol write the mass number of the isotope.
3. Beneath that (to the bottom left of the symbol), write the atomic number of
the element.
Ex: Label the following:
Mass number
(protons + neutrons)
Element symbol
Atomic number
(protons)
Example of Isotopes:
14
𝐶
6
and
12
𝐶
6
How many protons does Carbon-14 have?
How many protons does Carbon-12 have?
How many neutrons does Carbon-14 have?
How many neutrons does Carbon-12 have?
6

Atoms as a rule are all _______________ in charge, meaning that the number of
protons and electrons in the atoms are equal.
 Ions:
Ions are __________________________________ that can only form when an atom
________________________________________________________.
Cations



Examples:
7 +
3Li
Lithium-7
Protons:
Neutrons:
Electrons:
Charge:
=
Anions



Examples:
Sulfur-32
Protons:
Neutrons:
Electrons:
Charge:
32 2- =
16S
Lab: Beanium Lab:
STATE THE PROBLEM: How can you identify an element?
BACKGROUND: Atoms are made of the subatomic particles protons, neutrons, and electrons. The
atomic number, atomic mass, name, and symbol are on the periodic table . The electrons are so small
that they add no mass to the atom. The mass # is the rounded atomic mass from the periodic table, also
determined by adding protons and neutrons.
HYPOTHESIS: (Answer the problem question above.) ____________________________________
__________________________________________________________________________________
Materials: 10 zip lock baggies, Black beans = Protons, White beans = Neutrons, Popcorn = Electrons
PROCEDURE:
1. Count the number of protons, neutrons, and electrons in the bags and record.
2. Return to your assigned seat to complete the data table and answer the questions.
7
DATA TABLE: Complete the data table and then answer the questions below.
Bag # # of
Protons
# of
Neutrons
# of
Electrons
ATOMIC
#
MASS #
NAME with mass #
Isotope
Symbol
Neutral
atom,
Isotope
or Ion
1
2
3
4
5
6
7
8
9
10
11
12
1. Which particle did you use to determine the name of the element?_________________________
2. One subatomic particle adds virtually no mass to the atom. _________________________
3. Which subatomic particles added together equal the mass #? ___________________ and
____________________
4. Using the model of an atom, as in this lab, how do you determine if an atom is the neutral version or an
ion? ______________________________________________________________
______________________________________________________________________________
5. Using the model of an atom, as in this lab, how do you determine if an atom is an Isotope?
______________________________________________________________________________
6. Conclusion: Write a rule concerning how to identify an atom from its parts.
8
Homework: Isotope, Ion and Atomic Structure
1. What subatomic particle remains the same among isotopes of the same element?
2. What subatomic particle changes among isotopes of the same element?
3. Complete the following table for the neutral atoms:
Complete
Symbol
Element name
(including mass #!)
Lead-206
Atomic
number
Mass
number
7
#
protons
#neutrons
#
electrons
82
7
Use the information below to determine if the pair of elements is a set of isotopes or different
elements. Indicate your answer in the space provided:
Isotope or different element?
1. Element D has 6 protons and 7 neutrons.
Element F has 7 protons and 7 neutrons.
2. Element J has 27 protons and 32 neutrons.
Element L has 27 protons and 33 neutrons.
3. Element X has 17 protons and 18 neutrons.
Element Y has 18 protons and 17 neutrons.
4.
14
6
X
14
7
and
X
5. Element P has an atomic number of 92 and a
mass number of 238.
Element S has 92 protons and 143 neutrons.
Use the information below to determine if the element is an ion or neutral atom. Indicate your answer in
the space provided:
Ion or neutral atom?
6. Element Z has 6 protons and 6 electrons.
7. Element N has 17 electrons and 18 protons.
8.
9. Element P has 12 protons, 12 neutrons and
10 electrons.
10. Element K has atomic # 7 and 7 electrons.
9
ISOTOPES AND AVERAGE ATOMIC MASS
•
Compare & contrast Mass Number and Atomic Mass:
Elements come in a variety of isotopes, meaning they are made up of atoms with the same atomic number but different
atomic masses. These atoms differ in the number of neutrons.
The average atomic mass is the weighted average of all the isotopes of an element.
Formula for Atomic Mass:
Practice Problems:
1. A certain element has two naturally occurring isotopes. Determine the atomic mass
given the following data and identify the element.
Isotope
Atomic Mass
Abundance
X-35
34.969 amu
75.53%
X-37
36.966 amu
24.47%
a. Show your work in calculating the average atomic mass of this isotope:
b. What element is this? (hint: compare this atomic mass to ones on the periodic table to
determine its identity!)
2. Given the following data, calculate the average atomic mass of magnesium.
Isotope
Atomic Mass
Abundance
Magnesium-24
23.985 amu
78.70%
Magnesium-25
24.986 amu
10.13%
Magnesium-26
25.983 amu
11.17%
a. Show your work in calculating the average atomic mass of Mg (Magnesium):
10
Homework - Atomic Mass Calculations:
133
132
Example: A sample of cesium is 75.0 % 55 Cs, 20.0% 55 Cs and
5.0% 134
55Cs. What is its average atomic mass?
Answer:
.750 x 133 = 99.75
.200 x 132 = 26.4
.050 x 134 = 6.70
Total = 132.85 a.m.u.
(average atomic mass)
Determine the average atomic mass of the following mixtures of isotopes.
1. 80.0%
127
53
I , 17.0%
126
53
I , 3.0%
128
53
I
_____________
2. 50.0%
197
79
Au , 50.0%
198
79
Au
_____________
.
3. 15.0%
55
26
Fe , 85.0%
56
26
Fe
_____________
.
4. 99.0%
1
1
H , 0.8%
2
1
H , 0.2%
3
1
H
_____________
.
5. 95.0%
14
7
N , 3.0%
15
7
N , 2.0%
16
7
N
_____________
.
6. 98.0%
12
6
C , 2.0%
14
6
C
_____________
.
11
LAB: Average Atomic Mass
WARM-UP:
Test Average
Quiz Average
Homework Average
74
82
84
Grading policy is that tests are worth 55%, quizzes worth 30%, and homework worth 15% of your average.
1. Look over the data before you begin the problem. Estimate this student’s average before you begin the
calculation. Will his average be closer to 74, 82, or 84?
2. Now, calculate this student’s average according to our grading policy.
LAB: AVERAGE ATOMIC MASS
Background Information: Mass number is the sum of the protons and neutrons in an atom. The electrons are so small
that they do not really contribute to the atom’s mass. Isotopes are atoms of the same element with the same number
of protons but a different number of neutrons. The mass you see on the periodic table is the average atomic mass. It
takes into account the mass of each isotope of an element and the percent abundance in nature.
Procedure:
1. Determine the average atomic mass of fictitious elements.
 Note: At each station you will see bags. Each little bag represents an atom. DO NOT OPEN THE LITTLE
BAGS!
2. Count the total number of bags (atoms) for the element.
3. Separate the bags based on isotope name (labeled on the front of the bag).
4. Count how many bags (atoms) of each isotope.
5. Calculate the percent abundance. (# atoms for each isotope/total atoms)
6. Determine the average atomic mass for the element. (Mass # of the isotope x percent abundance. Add up the
total)
7. Determine the number of protons for each element.
For Example:
Sica-11
Sica-11
Sica-12
Sica-13
Sica-13
1. There are six atoms of the element Sica.
2. I’ve separated them based on the isotope name.
12
Sica-13
3. The data table below was filled in based on the example from the previous page:
Isotope
Name
Sica-11
Sica-12
Sica-13
#3
How many
atoms of each
isotope?
2
1
3
#4
Calculate
Percent
abundance
2/6= 33%
1/6= 17%
3/6= 50%
Total atoms = 6
#5
Average Atomic Mass
11 x .33 = 3.63
12 x .17 = 2.04
13 x .50 = 6.5
Total = 3.63 +2.04 +6.5 = 12.17 amu
GATHER DATA:
Sciencetopium
Isotope Name
How many atoms
of each isotope?
Calculate Percent
abundance
Total atoms =
Tigerium
Isotope Name
How many atoms
of each isotope?
Total =
Calculate Percent
abundance
Total atoms =
Katyum
Isotope Name
How many atoms
of each isotope?
Average Atomic Mass
Average Atomic Mass
Total =
Calculate Percent
abundance
Total atoms =
Average Atomic Mass
Total =
13
Championodium
Isotope Name
How many atoms
of each isotope?
Calculate Percent
abundance
Total atoms =
Average Atomic Mass
Total =
Safarium
Isotope Name
How many atoms
of each isotope?
Calculate Percent
abundance
Total atoms =
Superdupium
Isotope Name
How many atoms
of each isotope?
Average Atomic Mass
Total =
Calculate Percent
abundance
Total atoms =
Average Atomic Mass
Total =
QUESTIONS: (look at the background info for this lab and notes on previous pages to help with these questions)
1. What is an isotope?
2. Why did you have to find the percent abundance?
3. What is the difference between a mass number and an atomic mass?
Cumulative Test Tomorrow...Study Units 1 and 2
14
Notes over Radiation
What causes nuclear decay?
Terms to know:
Radioisotopes:
Nuclear Reactions:
Radiation:
Transmutation:
Radioactive Decay:
3 Types of Radiation

alpha radiation –
__________________________________________________________________
__________________________________________________________________
o symbol :

beta radiation –
__________________________________________________________________
__________________________________________________________________
__________________________________________________________________
o Symbol:

gamma radiation –
_________________________________________________________________
__________________________________________________________________
o Symbol:
15
Types of Radiation
Property
Alpha radiation
Beta radiation
Gamma radiation
Composition
Symbol
Charge
Mass (amu)
Common Source
1/1837
Radium – 226
Carbon-14
Cobalt - 60
Penetrating
power
Shielding
Review
1. Label the following statements as alpha, beta, or gamma radiation.
____the most dangerous type of radiation
____the largest of the radiation particles
____have a positive charge
____have no mass (multiple answers)
____a helium nucleus
____cannot penetrate paper or clothes
____harmful only when ingested
16
Writing Nuclear Equations
A nuclear equation will look like this:
1.
2.
Examples: Nuclear Reactions using symbols and word equations.
1.
𝟐𝟑𝟗
𝟗𝟒𝑷𝒖
2.
𝟑𝟕
𝟏𝟗𝑲
3.
______  𝟔𝟒𝑩𝒆 +
4.
Write the equation of lead-210 undergoing alpha decay.
5.
Write the equation where lead-210 emits a beta particle.
6.
 𝟒𝟐𝑯𝒆 + ______
 _____ +
Type: ___________
Type: ___________
𝟑𝟕
𝟏𝟖𝑨𝒓
Type: ___________
𝟎
−𝟏𝒆
Show the transmutation of uranium-237 as it undergoes
alpha decay. What is the nuclide that is produced?
17
Homework Nuclear Reactions
1.
Write the nuclear decay equation for the alpha particle decay of
231
91
2.
Write the nuclear decay equation for the alpha particle decay of
146
62
3.
Write the nuclear decay equation for the beta particle decay of
152
54
Pa .
Sm .
Xe .
4. Write the nuclear decay equation for the beta particle decay of cesium-120.
5. Write the nuclear decay equation for the gamma particle decay of
142
60
Nd .
6. Which type of nuclear decay is NOT a transmutation reaction?
7. Find the missing part of the equation and label the type of transmutation (alpha, gamma or beta).
a.
b.
222
86
Rn  ____ He
4
2
Type: ______
c.
209
85
At  ____ 24He
Type: ______
d.
87
37
Rb  Sr  ____
87
38
Type: ______
14
6
C  ____  10 e
Type: ______
18
Fission and Fusion
Fission
Picture
Fusion
Picture
19
Nuclear Fission vs. Nuclear Fusion
Nuclear
f“i”s s i o n
(Spl“ i ”tting an atom into two new ones)
In nuclear fission reactions (also called radioactive decay),
a neutron is aimed at the nucleus of a large, unstable
atom, like uranium, thorium, or other radioactive
elements. The extra mass of the neutron causes the
radioactive nucleus to split apart, forming lighter
elements, free neutrons, and great quantities of energy.
This process causes convection currents that move Earth’s
tectonic plates, and generate earthquakes and volcanic
eruptions.
Nuclear Fission:






Nuclear
Source of energy in the core of the Earth that produces heat from the decay of radioactive
elements.
Produces vast quantities of energy.
Does not produce particulate air pollution like fossil fuels and coal.
Involves the splitting of harmful radioactive elements.
Loss of control leads to harmful radiation exposure.
Produces a radioactive waste product that will need to be stored.
f“u”s i o n
(combining/fusing two atoms together into one new atom)
During fusion reactions, nuclei collide and fuse, eventually forming nuclei of heavier elements and
producing enormous amounts of energy. Fusion of hydrogen to helium occurs in the sun and is the
source for all external weather related events.
Nuclear Fusion:
 Source of energy in the Sun that produces heat from the fusing of elements like hydrogen.
 Produces unsurpassed quantities of energy.
 Does not produce particulate air pollution like fossil fuels and coal.
 Does not produce a radioactive waste product that will need to be stored.
 Currently, we lack the technology to maintain reactions as a viable energy source.
20
**Write Fission or Fusion next to each of the descriptions below:**
1. Generates a large volume of solid radioactive waste.
2. Occurs in the core of the Earth.
3. The reaction occurs only at extremely high temperatures.
4. Earth’s source in internal energy. (volcanoes, plate motion, geothermal, etc.)
5. The products of this reaction are not radioactive.
6. Occurs only in the core of the Sun.
7. Earth’s source of external energy (atmosphere, oceans, weather, plants, etc.).
8. Also called radioactive decay.
9. Responsible for providing heat for the convection in the interior of the Earth.
10. A potential power source but we lack the technology to maintain the reactions so we are unable to
perform these reactions on Earth.
11. The one with a “u” in it._
12. The one with two “i’s” in it.
13. The one that sounds like “fuse”
14. The one that almost rhymes with “split.”
15. Creates enough energy for the whole Earth (inside and out)
16. Which one you love the most now .
21
and
.
Atomic Structure and Nuclear Unit 3 Test Review
TEST on
Thursday 10/9
Parts of the atom:
Learning Goals
 Describe the three subatomic particles:

protons,

neutrons

electrons.

Determine the atomic number for any element using the periodic table.

Using given information, determine one or more of the following for a neutral atom or ions.
o
Number of Protons
o
Atomic Number
o
Number of Neutrons
o
Mass Number
o
Number of Electrons
o
Complete Atomic Symbol

Identify pairs of isotopes.

Identify ions.

Calculate atomic mass.

Determine the most abundant isotope for each element based on its atomic mass.

Explain how the theory of the atom has changed over time especially from the contributions of the
following scientists.


o
Democritus
o
Dalton
o
Thomson
o
Rutherford
o
Bohr
Describe major experiments and their effects on the atomic model.
o
Thomson
o
Rutherford
Describe the current atomic model.
Example Questions
1. What quantity identifies an element?
A) atomic number
B) mass number
C) number of neutrons
D) number of valence electrons
2. Chlorine-37 can be represented as
A)
17
37
B)
37
17
C)
35
20
D)
37
35
Cl
Cl
Cl
Cl
22
3. Which isotope is the basis of the atomic mass unit (amu)?
A) hydrogen-1
B) carbon-12
C) carbon-14
D) oxygen -16
4. Which total mass is the smallest?
A) the mass of 2 electrons
B) the mass of 2 neutrons
C) the mass of 1 electron plus the mass of 1 proton
D) the mass of 1 neutron plus the mass of 1 electron
5. The diagram below represents the nucleus of an atom.
Key
Proton =
Neutron =
What are the atomic number and mass number of this atom?
A) The atomic number is 9 and the mass number is 19.
B) The atomic number is 9 and the mass number is 20.
C) The atomic number is 11 and the mass number is 19.
D) The atomic number is 11 and the mass number is 20.
6. Which represents the most abundant isotope of sodium?
A) sodium-11
B) sodium-22
C) sodium-23
D) sodium-24
7. What is the total number of electrons in a Mg ion if it loses 2 electrons?
A) 2 electrons
B) 10 electrons
C) 12 electrons
D) 14 electrons
8. Which two notations represent different isotopes of the same element?
A)
6
4
Be and 49 Be
B)
14
6
C)
6
3
D)
31
15
C and
14
7
N
Li and 36 Li
P and
32
16
S
23
9. What is the total number of neutrons in an atom of 26 Fe ?
57
A) 26 electrons
B) 31 electrons
C) 57 electrons
D) 83 electrons
10. If an element loses or gains electrons, it will form a(an)
A) Neutral atom
B) Isotope
C) Ion
D) fluorine
11. How many protons are found in an atom of fluorine?
A) 7
B) 9
C) 10
D) 19
12. Which isotope of magnesium is the most abundant?
A) magnesium-12
B) magnesium-24
C) magnesium-25
D) magnesium-26
13. In the Modern wave mechanical model of the atom, the orbitals are regions of the most probable
locations of the
A) protons
B) electrons
C) neutrons
D) positrons
14. Which scientist was the first to indicate that electrons exist in distinct energy levels?
A) Thomson
B) Rutherford
C) Millikan
D) Bohr
15. Who discovered the electron?
A) Dalton
B) Thomson
C) Rutherford
D) Bohr
24
16. Which
A)
B)
C)
D)
phrase describes an atom?
a positively charged electron cloud surrounding a positively charged nucleus
a positively charged electron cloud surrounding a negatively charged nucleus
a negatively charged electron cloud surrounding a positively charged nucleus
a negatively charged electron cloud surrounding a negatively charged nucleus
17. Complete the following table.
Complete
Symbol
41
19
23
11
Atomic
Number
Mass
Number
Protons
Neutrons
Electrons
Charge
K
12
14
30
18
Na 
-3
18. Showing all your work, calculate the atomic mass for the following element. Identify this element.
Isotope
Isotope #1
Isotope #2
Isotope #3
Mass
(amu)
27.98
28.98
29.97
Percent
Abundance
92.22%
4.69%
3.09%
19. Neon-20 accounts for 94.3% of naturally occurring neon. Neon-23 accounts for the remaining 5.7%.
Calculate the atomic mass of neon. SHOW ALL WORK!
25
20. Rutherford led to two important discoveries about the atom using his gold foil experiment. For each
observation, indicate what he was able to conclude about the atom.
A) Observation #1: Rutherford noticed that about 1 in 10,000 of the positively charged
particles was deflected. He discovered the _______________________.
B) Observation #2: Rutherford noticed that a majority of the positively charged particles
went straight through the gold foil and were not deflected. He discovered the
_______________________.
21. Complete the labels below and fill in the blanks in the statements to the right. Stop at the directions.
DIRECTIONS: Fill in the blank in each box as well as the 6 blanks below it. Use the
information provided in each box as well as the isotope name above it.
Oxygen-16
Zinc-67
Lithium-6
22. An isotope of an element has an atomic number of 8 and a mass number of 15. How many
protons, neutrons, and electrons does this atom have and which element is this?
26
23. If hydrogen has two naturally occurring isotopes, H-1 and H-2 and the atomic mass of hydrogen
is 1.0079, then which of these two isotopes of hydrogen is more abundant?
Study Guide for Nuclear Chemistry
1. What determines if an atom will be radioactive or unstable?
2. The three principle types of radioactive decay are
,
, and
Use the following answer choices for question 4-16
a. alpha particles
b. beta particles
c. gamma rays
d. alpha and beta particles
e. beta particles and gamma rays
f. all of the above
3. Described as a fast moving electron
4. Has a positive charge
5. Has no mass or atomic number
6. Changes both the mass number and atomic number in radioactive decay
7. A helium nucleus
8. Electromagnetic radiation
9. Cannot be stopped by human skin or a piece of paper
10. Largest type of radioactive decay
11. Transmutation reaction
12. Most damaging and most penetrating
13. Particle released when carbon-14 changes to nitrogen-14
14. Emission increases the stability of the nucleus
15. Not deflected by any magnetic or electrical fields
16. Write the nuclear decay equation for thorium-230 undergoing alpha decay.
17. Write the nuclear decay equation for
8
3
Li emitting a beta particle.
18. Thorium-234 can undergo beta particle production. What is the other product?
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.
19. List three positive uses of nuclear chemistry.
20. Identify the following as fission or fusion:
Label Type:_______________________
Type: ______________________
21. List properties of fusion and fission.
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