Download Atomic Nucleus and Isotopes

5E Lesson Plan
Title of Lesson: The Atomic Nucleus
UFTeach Students’ Names: Melly Diaz
Teaching Date and Time: April 10th, 2014 9:20 a.m. - 10:20 a.m. (Homeroom first 20
min.)
Length of Lesson: 50 minutes
Grade / Topic: 8th Grade Physical Science – Chemistry Focus
Source of the Lesson:
http://www.princeton.edu/~achaney/tmve/wiki100k/docs/Atomic_nucleus.html
http://www.chem4kids.com/files/atom_structure.html
Appropriateness for Middle School Students: The cognitive complexity of the
benchmarks presented are in the low stage, while the lesson itself tries to push these
concepts in the moderate stage through basic applications of the concepts The lesson
will make use of this complexity through a lab activity that will tie in the multiple
concepts they learned to collectively solve problems. In collaborative groups, students
will be able to discuss their observations, which will help them gain confidence in their
results when presenting them to class. This communication is indicative of an actual
scientific community in which scientists work together to formulate conclusions.
Concepts: The concept of atomic structure and the properties of atoms are fundamental
roots in many concepts within chemistry and biological sciences. The properties of
atoms such as their atomic and mass number are important in understanding electron
configuration sequences, which also ties into bond formation between atoms to form
molecules. Ionic and covalent bonds, for example depend on the properties of the
atom’s atomic structure. . The molecules that are formed between these bonds can
furthermore have multiple properties, which affect higher-level concepts found in
sequences later within science, such as solubility and formation of proteins in biology.
Subsequently, the periodic table is organized based on basic concepts regarding the
number of protons and the charges conducted by the electron configurations in the
atoms. In physics, the basic subatomic particles, such as electrons, affects the concepts
of electricity and electron flow. Mastery of atoms, their structure, and their ability to
interact with each other are vital in application in the subjects of chemistry, biology,
physics, and fields such as engineering and medicine.
Florida State Standards (NGSSS) with Cognitive Complexity:
Benchmark
Benchmark Description
Number
Explore the scientific theory of atoms (also
known as atomic theory) by recognizing
SC.8.P.8.7
that atoms are the smallest unit of an
element and are composed of sub-atomic
particles (electrons surrounding a nucleus
containing protons and neutrons).
Cognitive
Complexity
Low
Performance Objectives: Students will be able to:
 Identify the subatomic particles that comprise an atom and its nucleus.
 Calculate the amount of subatomic particles in a given atom.
 Compare and contrast isotopes and the elements on the periodic table.
 Represent elements using the atomic symbol.
Materials List and Student Handouts
 20 copies of the lab
 20 copes of the exit and entrance ticket
 20 copies of the periodic table
 Roll of Green string
 Roll of Red string
 Roll of yellow string
 350 Purple Beads
 400 Black Beads
 Tape
 Marker
 5 Zip-lock Bags
Advance Preparations
 PowerPoint will be prepared with the engage video loaded.
 Arrive to classroom early to load PowerPoint.
 Have materials prepared and ready to be distributed before class.
 Have compatible adaptor to connect smart board and laptop.
 Print a lab sheet for each student in the class.
 Print an entrance and exit ticket for each student in the class.
 Break students into groups of 4.
Safety
 None required for this activity.
5E Lesson:
Engagement
What the Teacher Will
Do
Greet Class- Slide 1
Pass Entrance Tickets:
Slide 2
Introduce Topic
Slide 3: Play video
speaking about the
subatomic particles and
atomic nucleus.
Ask follow up questions.
Time: 12 minutes
Teacher Directions and Probing Questions Student Responses/Possible
Misconceptions
Hello everyone!
On your desks, you will find an Entrance
Ticket. Please take 3-4 minutes to
complete this to the best of your ability.
Today, our lesson is going to be about
[Question was hypothetical,
atomic structure and isotopes. Do you
and is the key question]
know what the different parts of an atom
are?
We are going to start class with a video
about basic atomic structure.
https://www.youtube.com/watch?v=lP57g
EWcisY
Can someone describe the three
Ions, Protons, and Neutrons
subatomic particles?
[Protons, Neutrons, and
Electrons]
What are the two subatomic particles that Protons and Neutrons
make up the atomic nucleus?
[Protons and Neutrons]
How do you find the atomic mass?
By counting the number of
protons
Most importantly, do electrons have any
role in the atomic nucleus?
[By adding the subatomic
particles in the atomic
nucleus]
Yes, they do.
[No, they do not!]
Excellent! Now that everyone has an
understanding of how the modern
structure of the atom and what it looks
like, let us proceed to the lab.
Exploration
Time: 25 minutes
What the Teacher Will Do Teacher Directions and Probing Questions Student Responses/Possible
Misconceptions
Slide 4 with the
So now we’re going to start the activity for
objectives.
today. You are expected to have a
Go over directions
Slide 5: (Shows student’s
names and their groups)
Pass out materials and
worksheets.
Slide 6: Shows probing
questions
thorough understanding of atomic
structure by the end of this lab!
In a few moments, you will be given a
worksheet, periodic table, and a zip-lock
bag of materials. In the bag there are
several colored strings with numbers on
them which correspond with certain
questions. Please read the directions for
each question carefully so you do not get
confused. The string necklaces represent
the nucleus of a certain atom. Black beads
are neutrons and purple beads are
protons. Who can tell me what color
beads are associated with the protons and
neutrons?
Good job. After we put everyone into
groups and before you begin the lab,
please read the background and objectives
so you can understand what you will be
doing. For the first part of the lab, you will
answer various questions that will help
you determine what element is being
represented. You will also write the atomic
symbol for each isotope. Directions for
how to write an atomic symbol are on the
lab sheet. What will you do once you
receive your lab sheet and get into your
groups?
Great! The next part of the lab is the
application and challenge questions, which
you are required to do. Your groups are
there to help you solve the problems, not
to split the work. So please make sure that
everyone in your group in participating for
each question. You will have about 20
minutes to complete the lab.
Now you will move into your groups as
you see them on the PowerPoint while we
pass out the materials and worksheets.
Please move to the assigned lab stations.
Okay, here are some questions to think
about while you do your activity and your
20 minutes begins now.
Protons are black beads and
neutrons are purple beads,
there is not a specified color.
[Protons are purple beads
and neutrons are black
beads.]
Start the lab, read the
directions.
[Read the background and
objectives.]
Probing Questions:
Warn students when there are five
minutes left.
Do you think there is a correlation with the There is no correlation.
amount of neutrons and protons? In other
words, do elements with fewer protons
[There is a correlation.
also have fewer neutrons?
Atoms with more protons
also have more neutrons,
and this makes their atomic
weight larger.]
So some elements have variants in their
There is no difference
number of neutrons. Do you think this
between the isotopes of
affects the element chemically?
different atoms.
How is the average atomic mass
significant?
[This does affect them
chemically, in fact. They can
even become radioactive
because of their instability.]
It is not significant. It is the
mass of the isotopes.
[The average atomic mass is
the mass that is seen on the
periodic table for each
element.]
Explanation
Time: 5 minutes
What the Teacher Will Do Teacher Directions and Probing Questions Student Responses/Possible
Misconceptions
Call students attention
5. 4. 3. 2. 1! Alright everyone, by now you
should have finished with your lab. Now
please move back to your seats so we may
go over your findings.
Slide 7
So, what element did everyone get for the Neon, Lithium
green string?
[Sodium]
What is the atomic number?
Atomic number 10 or 24
[atomic number is 11]
What were the atomic masses in this
20, 17, 26
particular example?
[atomic masses of 21 and 23
for the strings]
Who can come up here and write the
Nuclear Notation for the first green string?
What were the elements for the red
string?
What were the elements for the Yellow
string?
Slide 8: Application
questions.
Slide 9: Application
Questions continued
Now for the application questions.
What element has 83 protons?
11
Na
21
[ 21
]
[
Na ]
[ 11
]
Chlorine, Argon, Scandium
[Potassium, Calcium]
Aluminum, Silicon-28,
Silicon-29
[Aluminum-27, Aluminum28, and Silicon.]
Lead
An atom has an atomic number of 54.
What element is it?
[Bismuth]
Iodine
[Xenon]
Silver has a mass number of 107. It has 61
neutrons. What is its atomic number?
The atomic mass of an element is
composed of which subatomic particles?
46, 168
[47]
Protons, and Electrons
[Protons and Neutrons]
Arsenic has a mass number of 75. It has an
atomic number of 33. How many neutrons
does it have?
Tungsten has an atomic number mass of
184. It has 110 Neutrons. What is its
atomic number?
108
[42]
An element has an atomic number of 78.
What element is it?
[Gold]
Platinum
Two substances have an atomic mass of
92. However, one has 51 neutrons, and
the other has 52 neutrons. Are these the
same element? Explain in regards to the
subatomic particles.
Yes, they are elements that
are isotopes of each other.
294
[74]
[No, they are not the same
element because they have
a different number or
protons, despite having the
same mass. ]
Slide 10 Challenge
Questions.
Alright, I want to take three volunteers to
do the challenge questions on the board.
Show the operations you used to get the
final answer!
So that’s pretty much it for the lab today.
Any questions?
Elaboration
Time: 5 minutes
What the Teacher Will Do Teacher Directions and Probing Questions Student Responses/Possible
Misconceptions
Slide 11
Now let’s go more in depth into atomic
structure. So how does the atomic nucleus
actually look like?
Slide 12
The atomic nucleus is actually a tight
bundle of both the neutrons and the
protons. Most of the mass of an atom is
concentrated in the nucleus. However,
electrons are very important.
Slide 13: Picture of the
As you see, the electrons are not a part of Because they are not
Atomic Nucleus with
the atomic nucleus. This is actually
attached to the atomic
Electrons.
because electrons orbit around the atomic nucleus.
nucleus. However, they are still part of the [Because they have a very
atom. Why don’t they contribute to the
small mass.]
atomic mass?
Slide 14 – Chart of proton, Here is a chart of the masses of each
The sub atomic particles
electron, and neutron
subatomic particle. What do you notice?
have very large masses.
mass values. (use this
[All the subatomic particles
chart it’s the second
are very small; however,
image
protons and neutrons are
the largest.]
Very good! Long story short, the
subatomic particles don’t have much of a
mass to begin with. Protons and Neutrons
have very similar masses, and Electrons
are the smallest.
As you can see from the chart, the
Magnets, They don’t have a
subatomic particles have charges. What
purpose.
are these charges on the atoms of
[Bonding and creating
elements used for?
compounds.]
That’s right. The role that an electron has
Slide 14 Pass out exit
tickets
in atomic structure plays a huge factor in
chemistry, biology, and physics. Electrons
contribute to why different kinds of bonds
between elements, such as ionic and
covalent, can exist.
Now take the rest of class to complete
these exit tickets.
Evaluation
Time: 4 minutes
What the Teacher Will Do Teacher Directions and Probing Questions
Student Responses
Teachers will pass out the
1. Name the three subatomic
Exit Ticket; students will
particles of an atom. Which of the
1. Protons, Neutron,
work individually and
two are involved in the atomic
and Electrons. The
quietly until the end of
nucleus?
neutrons and protons
the period.
2. A random, unidentified element
are involved in the
has an atomic mass of 53. Is this
atomic nucleus.
Students will leave their
unique to one element? Why or
2. No, because multiple
papers on their desks
why not?
elements can have a
when the bell rings;
3. Carbon has an atomic number of 6
similar atomic mass.
teachers will collect all
and mass number of 12. What is
Elements differ in
post-assessments when
the Nuclear notation? The
their atomic number.
the bell rings. The
abbreviation for Carbon is C.
3. 23
teachers should have
4. In what subatomic particles are
Li
collected the Enter Ticket
elements different from their
11
and lab worksheet before
isotopes?
4. Isotopes of a an
handing out the Exit
5. An element has a mass number of
element vary in their
Ticket.
36 and has 20 neutrons in its atom.
number of neutrons.
What is the atomic number? How
5. Atomic number = 16,
many protons are in the atom?
Protons= 16,
Label accordingly.
Name:______________________________
Lab: What Element Am I?
Background: Elements have many different properties that set them apart from each
other. Amongst the most basic things that set them apart is their atomic structure. An
atom is the simplest unit of matter, and atoms of different elements are different from
each other.
The main difference is their atomic number, which are unique amongst each element.
The atomic number is the number of protons in each element.
The mass number is the number of protons and neutrons. Isotopes are the different
forms of an element that have a different number of neutrons, but the same number of
protons. All variations of an element, its isotopes, are represented by the Nuclear
notation which indicates mass number as a superscript and the atomic number as a
subscript.
Objective: By the end of the lab, you should be able to identify an element or isotope by
the differences in its atomic structure.
Procedure and Tips:
1. The teacher will divide you into groups.
2. You will be given materials once your groups have been situated.
3. Be careful when reading each question and handling the beads.
There are important details you do not want to mess up because
of lack of attention!
4. Keep your periodic table with you; it would be extremely difficult
to answer the questions without it.
5. Be careful with counting! Double check with your partners
to reduce error.
6. Do not split up the work between your partners. You MUST
count every set of beads for the problems.
7. Black beads are neutrons. Purple beads are protons.
Questions:
Reach into the zip-lock bag and pull out the sets of beads with
the green string. There should be two sets.
A is actually Neutrons and the Protons!
1. In the first set of green string (labeled with a 1),
a. How many Protons are there?
b. How many Neutrons are there?
c. What is the Atomic Number?
d. What is the Mass Number?
e. What is the Nuclear notation?
2. In the second set of green string (labeled with a 2),
a. How many Protons are there?
b. How many Neutrons are there?
c. What is the Atomic Number?
d. What is the Mass Number?
e. What is the Nuclear notation?
3. Identify the elements in set one and two. Are they the same elements? Are they
isotopes? Explain by elaborating on changes in the subatomic particles. Refer to
the periodic table if you need to.
Reach into the zip-lock bag and pull out the set with red string. There should be two
sets.
1. In the first set of red string, (labeled with a 1),
a. How many Protons are there?
b. How many Neutrons are there?
c. What is the Atomic Number?
d. What is the Mass Number?
e. What is the Nuclear notation?
2. In the second set of red string, (labeled with a 2),
a. How many Protons are there?
b. How many Neutrons are there?
c. What is the Atomic Number?
d. What is the Mass number?
e. What is the Nuclear notation?
3. Identify the elements in sets one and two. Are they the same elements? Are they
isotopes? Explain by elaborating on changes in the subatomic particles. Refer to
the periodic table if you need to.
Reach into the zip-lock bag and pull out the sets with the yellow string. There should
be three sets.
1. In the first set of yellow string, (Labeled with a 1),
a. How many protons are there?
b. How many neutrons are there?
c. What is the atomic number?
d. What is the mass number?
e. What is the Nuclear notation?
2. In the second set of yellow string, (Labeled with a 2),
a. How many protons are there?
b. How many neutrons are there?
c. What is the atomic number?
d. What is the mass number?
e. What is the Nuclear notation?
3. In the third set of yellow string, (Labeled with a 3),
a. How many protons are there?
b. How many neutrons are there?
c. What is the atomic number?
d. What is the mass number?
e. What is the Nuclear notation?
4. Identify the elements in the three sets. Are they the same elements? Are they
isotopes? Explain by elaborating on changes in the subatomic particles. Refer to
the periodic table if you need to.
Once done with these questions, please put all the materials back into the zip-lock
bag, go to your seats, and work on the following questions.
Application Questions
1. An atom has 83 protons. What element is it?
2. What is the atomic number of Carbon?
3. An atom has an atomic number of 54. What element is it?
4. Silver has a mass number of 107. It has 61 neutrons. What is its atomic number?
5. The atomic mass of an element is composed of which subatomic particles?
6. Arsenic has a mass number of 75. It has an atomic number of 33. How many
neutrons does it have?
7. Tungsten has an atomic number mass of 184. It has 110 Neutrons. What is its
atomic number?
8. An element has an atomic number of 78. What element is it?
9. Two substances have an atomic mass of 92. However, one has 51 neutrons, and
the other has 52 neutrons. Are these the same element? Explain in regards to
the subatomic particles.
Challenge Questions: Calculating average atomic mass. The atomic mass found on the
periodic table is actually an average of all isotopes for that element. This is calculated
based off of the percent of abundance of that isotope with the equation:
(Exact weight of isotope #1) (abundance of isotope #1) + (exact weight of
isotope #2) (abundance of isotope #2) = average atomic weight of the element.
Solve the following equations based on the formula above. Round to the hundredths
place. Remember to show your work!
If the masses of a couple of isotopes are 13.02 amu and 14 amu with percent
abundances of 21% and 79% respectively, what is the average atomic mass of the
element?
If the atomic mass of a couple of isotopes is 54.21 amu and 55.08 amu with percent
abundances of 38% and 62% respectively, what is the average atomic mass?
If the atomic mass of the isotopes are 31.04 amu, 32.91 amu, 31.58 amu, with percent
abundances of 80%, 11%, and 9% respectively, what is the average atomic mass?
Name:______________________________
Lab: What Element Am I? KEY
Background: Elements have many different properties that set them apart from each
other. Amongst the most basic things that set them apart is their atomic structure. An
atom is the simplest unit of matter, and atoms of different elements are different from
each other.
The main difference is their atomic number, which are unique amongst each element.
The atomic number is the number of protons in each element.
The mass number is the number of protons and neutrons. Isotopes are the different
forms of an element that have a different number of neutrons, but the same number of
protons. All variations of an element, its isotopes, are represented by Nuclear notation
which indicates mass number as a superscript and the atomic number as a subscript.
Objective: By the end of the lab, you should be able to identify an element or isotope by
the differences in its atomic structure.
Procedure and Tips:
8. The teacher will divide you into groups.
9. You will be given materials once your groups have been situated.
10. Be careful when reading each question and handling the beads.
There are important details you do not want to mess up because
of lack of attention!
11. Keep your periodic table with you; it would be extremely difficult
to answer the questions without it.
12. Be careful with counting! Double check with your partners
to reduce error.
13. Do not split up the work between your partners. You MUST
count every set of beads for the problems.
14. Black beads are neutrons. Purple beads are protons.
Questions:
Reach into the zip-lock bag and pull out the sets of beads with
the green string. There should be two sets.
A is actually Neutrons and the Protons!
4. In the first set of green string (labeled with a 1),
a. How many Protons are there?
i. 11
b. How many Neutrons are there?
i. 10
c. What is the Atomic Number?
i. 11
d. What is the Mass Number?
i. 21
e. What is the Nuclear notation?
i. 23
Na
11
5. In the second set of green string (labeled with a 2),
a. How many Protons are there?
i. 11
b. How many Neutrons are there?
i. 12
c. What is the Atomic Number?
i. 11
d. What is the Mass Number?
i. 23
e. What is the Nuclear notation?
6. Identify the elements in set one and two. Are they the same elements? Are they
isotopes? Explain by elaborating on changes in the subatomic particles. Refer to
the periodic table if you need to.
a. The element in both sets is Sodium. They are isotopes. They both have
the same number of protons, and thus the same atomic number.
Reach into the zip-lock bag and pull out the set with red string. There should be two
sets.
4. In the first set of red string, (labeled with a 1),
a. How many Protons are there?
i. 19
b. How many Neutrons are there?
i. 21
c. What is the Atomic Number?
i. 19
d. What is the Mass Number?
i. 40
e. What is the Nuclear notation?
i. 40
K
19
5. In the second set of red string, (labeled with a 2),
a. How many Protons are there?
i. 20
b. How many Neutrons are there?
i. 20
c. What is the Atomic Number?
i. 20
d. What is the Mass number?
i. 40
e. What is the Nuclear notation?
i. 40
Ca
20
6. Identify the elements in sets one and two. Are they the same elements? Are they
isotopes? Explain by elaborating on changes in the subatomic particles. Refer to
the periodic table if you need to.
a. The first element is Potassium, and the second is Calcium. They are not
isotopes. Potassium has an atomic number of 19, while Calcium has an
atomic number of 20, which means they have a different number of
protons.
Reach into the zip-lock bag and pull out the sets with the yellow string. There should
be three sets.
5. In the first set of yellow string, (Labeled with a 1),
a. How many protons are there?
i. 13
b. How many neutrons are there?
i. 14
c. What is the atomic number?
i. 13
d. What is the mass number?
i. 27
e. What is the Nuclear notation?
i. 27
Al
13
6. In the second set of yellow string, (Labeled with a 2),
a. How many protons are there?
i. 13
b. How many neutrons are there?
i. 15
c. What is the atomic number?
i. 13
d. What is the mass number?
i. 28
e. What is the Nuclear notation?
i. 28
Al
13
7. In the third set of yellow string, (Labeled with a 3),
a. How many protons are there?
i. 14
b. How many neutrons are there?
i. 14
c. What is the atomic number?
i. 14
d. What is the mass number?
i. 28
e. What is the Nuclear notation?
i. 28
Si
14
8. Identify the elements in the three sets. Are they the same elements? Are they
isotopes? Explain by elaborating on changes in the subatomic particles. Refer to
the periodic table if you need to.
a. Set one is Aluminum-27. Set one is Aluminum-28. Set three is Silicon.
Aluminum-27 and 28 contain a different number of neutrons, but they
are the same element because they have the same number of protons,
so, they are isotopes. Silicon has a different number of protons, so it is a
different element.
Once done with these problems, please put all the materials back into the zip-lock
bag, go to your seats, and work on the following questions.
Application Questions
1. An atom has 83 protons. What element is it?
a. Bismuth
2. What is the atomic number of Carbon?
a. 6
3. An atom has an atomic number of 54. What element is it?
a. Xenon
4. Silver has a mass number of 107. It has 61 neutrons. What is its atomic number?
a. 47
5. The atomic mass of an element is composed of which subatomic particles?
a. Protons and Neutrons
6. Arsenic has a mass number of 75. It has an atomic number of 33. How many
neutrons does it have?
a. 42
7. Tungsten has an atomic number mass of 184. It has 110 Neutrons. What is its
atomic number?
a. 74.
8. An element has an atomic number of 78. What element is it?
a. Platinum
9. Two substances have an atomic mass of 92. However, one has 51 neutrons, and
the other has 52 neutrons. Are these the same element? Explain in regards to
the subatomic particles.
a. No, they are not the same element because they have a different number
or protons, despite having the same mass.
Challenge Questions: Calculating average atomic mass. The atomic mass found on the
periodic table is actually an average of all isotopes for that element. This is calculated
based off of the percent of abundance of that isotope with the equation:
(Exact weight of isotope #1) (abundance of isotope #1) + (exact weight of
isotope #2) (abundance of isotope #2) = average atomic weight of the element.
Solve the following equations based on the formula above. Round to the hundredths
place. Remember to show your work!
If the masses of a couple of isotopes are 13.02 amu and 14 amu with percent
abundances of 21% and 79% respectively, what is the average atomic mass of the
element?
(13.02 x .21) + (14 x .79) = 13.79 amu
If the atomic mass of a couple of isotopes is 54.21 amu and 55.08 amu with percent
abundances of 38% and 62% respectively, what is the average atomic mass?
(54.21 x .38) + (55.08 x .62) = 54.74 amu
If the atomic mass of the isotopes are 31.04 amu, 32.91 amu, 31.58 amu, with percent
abundances of 80%, 11%, and 9% respectively, what is the average atomic mass?
(31.04 x .8) + (32.91 x .11) + (31.58 x .09) = 31.29 amu
Name:_______________________
Entrance Tickets
1. Name the three subatomic particles of an atom. Which of the two
are involved in the atomic nucleus?
2. A random, unidentified element has an atomic number of 53. Is this
unique to one element? Why or why not?
3. Lithium has an atomic number of 11 and mass number of 23. What is
the Nuclear notation? The abbreviation for Lithium is Li.
4. In what subatomic particles are elements similar to their isotopes.
5. An element has an atomic number of 44 and has 55 neutrons in its
atom. What is the mass number? How many protons are in the
atom? Label accordingly.
Name:_______________________
Exit Tickets
1. Name the three subatomic particles of an atom. Which of the two
are involved in the atomic nucleus?
2. A random, unidentified element has an atomic mass of 53. Is this
unique to one element? Why or why not?
3. Carbon has an atomic number of 6 and mass number of 12. What is
the Nuclear notation? The abbreviation for Carbon is C.
4. In what subatomic particles are elements different from their
isotopes?
5. An element has a mass number of 36 and has 20 neutrons in its
atom. What is the atomic number? How many protons are in the
atom? Label accordingly.
Entrance Tickets Key
1. Name the three subatomic particles of an atom. Which of the two
are involved in the atomic nucleus?
Neutrons, Protons, Electrons
The two involved in the atomic nucleus are the Neutrons and
Protons.
6. A random, unidentified element has an atomic number of 53. Is this
unique to one element? Why or why not?
Yes, because the atomic number is the number of protons, and no
two elements have the same number of protons.
2. Lithium has an atomic number of 11 and mass number of 23. What is
the Nuclear notation? The abbreviation for Lithium is Li.
23
Li
11
3. In what subatomic particles are elements similar to their isotopes.
Isotopes of an element share the same number of protons.
4. An element has an atomic number of 44 and has 55 neutrons in its
atom. What is the mass number? How many protons and electrons
are in the atom? Label accordingly.
Mass number= 99
Protons= 44
Exit Tickets
1. Name the three subatomic particles of an atom. Which of the two
are involved in the atomic nucleus?
Protons, Neutron, and Electrons
The two involved in the atomic nucleus are the Neutrons and
Protons.
2. A random, unidentified element has an atomic mass of 53. this
unique to one element? Why or why not?
No, because multiple elements can have a similar atomic mass.
Elements differ in their atomic number.
3. Carbon has an atomic number of 6 and mass number of 12. What is
the Nuclear notation? The abbreviation for Carbon is C.
12
C
6
4. In what subatomic particles are elements different from their
isotopes?
Isotopes of an element vary in their number of neutrons.
5. An element has a mass number of 36 and has 20 neutrons in its
atom. What is the atomic number? How many protons and electrons
are in the atom? Label accordingly.
Atomic number=16
Protons=16