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The Atom

Cornell Doodle Notes

TEACHER NOTES

These scaffolded Cornell Doodle Notes combine two effective note-taking strategies and can be used as part of the input for NGSS Disciplinary Core Idea PS1.A: Substances are made from different types of atoms, which combine with one another in various ways. Atoms form molecules that range in size from two to thousands of atoms; and each atom has a charged substructure consisting of a nucleus, which is made of protons and neutrons, surrounded by electrons. These notes cover the general definition of an atom, depict a very simplified version of the history of the atomic theory, differentiate the subatomic particles proton, neutron and electron, by their charges, masses, and locations within the atom, explain what isotopes are and how to write an element in isotopic notation (ex: Carbon-12), cover what can be learned from an element’s square on the Periodic Table, and explain how to calculate the number of neutrons in an atom. Cornell Notes are a note-taking strategy in which topic questions are written in a narrow left-hand column and definitions, explanations, and diagrams are filled in in the right-hand column. At the bottom of Cornell Notes, there is typically a section included for reflection on the lesson’s main points. See the example to the right. Doodle Notes (or Sketch Notes) are another notetaking strategy for which pictures and graphics activate the visual pathways of the brain, which helps with retention of information when compared to standard note-taking. Your visual learners will really benefit from seeing and coloring in the pictures aside the main points of the notes!

Doodle Notes is a registered trademark used with permission. See DoodleNotes.org for more details. I created a Powerpoint that goes with these notes. The Powerpoint walks the students through the lesson from the Essential Question and through all of the Topic Questions. There is a “Quick Watch” video clip included on the first slide (as well as at the top of the notes themselves) that you can use as a “hook”/intro. There are three anticipation questions that the students will answer before and after watching the video clip. At the end of the Powerpoint (as well as at the end of the notes themselves) there is a “Sum It Up” section in which students practice matching the relevant vocabulary to definitions, label a sample Periodic Table square, calculate the mass number of different atoms, and complete a chart that puts together all of the information about the subatomic particles.

See the Printing Tips on next page On the following pages, you will find 3 versions of the Cornell Doodle Notes:

KEY The KEY : pages 4-6 : All notes and “answers” are included on this version Green Circle : pages 7-9 : Use this version for your lower-level students who need more support, take more time, or who are learning English as a second language…they will have to fill in missing words Blue Square : pages 10-12 : Use this version for your mainstream students…they will have to write the topic questions and fill in some words throughout Note: the “Sum It Up” practice problems sheet is the same for both student versions. On the next page are the directions for accessing the Powerpoint for this product via Google Drive (Google Slides). This is obviously option depending on how you choose to use this in your classroom.

Here are some ways that I suggest using this resource: 1) Whole-Group lesson with differentiation : decide which students should receive which level of the notes. Hand out the notes to the students. Use the Powerpoint as a presentation and talk aloud through the lesson while the students take notes. Allow them to color/doodle further during and at the end of the lesson. 2) Differentiated Small-Group lesson : separate your students into groups by learning level. Give each student group sets of the appropriate notes for their level. Make sure each group has a device to view the presentation. Post the Powerpoint or Google Slides to your Google Classroom or other online learning platform, or email the Powerpoint version to one ‘student leader’ in each group. The students would view the Powerpoint/Slides together on one device and fill in the notes. Encourage them to add color/further notes. 3) Individual Note-Taking or Flipped Classroom : Post the Powerpoint or Google Slides presentation to your Google Classroom or other online learning platform. Hand out the appropriate-level notes to each student. Students can work at their own pace to view the presentation and complete their notes. Encourage them to add color/further notes. Thank you to these amazing artists!

Thank you very much for your purchase! If this product has met your needs, please consider leaving feedback at TeachersPayTeachers.com or feel free to email me at [email protected] with any questions or concerns! © Sunrise Science 2018

You may also be interested in my other Cornell Doodle Notes products! Click on the picture to the right!

Printing Tips! It depends how you’d like your students to use these notes. They can be printed one-sided and folded up into an interactive notebook, or you can print them double-sided and have students keep them in binders/folders. If you print them double-sided, this is what I suggest doing: o In the print settings on Adobe/Reader, keep the “Auto Orientation” button selected o Click “FLIP ON LONG EDGE” o Type in the page numbers that you’d like to print and the number of copies Printing the notes this way will avoid your students having to rotate their paper when they go to the next side. Instead, they will flip and the left and right columns will be in the same place!

Example colored notes

Google Drive Directions Below are some instructions for how to download this product and share it with your students via Google Drive. Just a note– although this is a digital resource, please know that it is for personal classroom use for only you and your students to share via email, Google Drive, or Google Classroom. Please do not upload this resource online where it can be accessed by the general public. Click on this link to access your purchase in Google!:

https://tinyurl.com/ydaytprz

When you click the link above, you’ll be taken to a screen that says “Copy Document”. Click the blue button that says “Make a Copy”. This will transfer the file to your own Google Drive account. Preferably, share this resource with your students through your Google Classroom, OR once all of your students have their own Google Drive account (drive.google.com), share the above link with them and have them make their own copy of the assignments into their own Google Drive.

Name:

_________________________________________________________________________

The atom

Class:

Analogy

Quick Just How Small is an Atom? Watch: http://tinyurl.com/lcdvfzx

______________

Date:

______________ KEY

My Guess (circle one)

Actual

If the atoms of a grapefruit were blown up to the size of blueberries, then the grapefruit would be the size of…

A basketball A school bus A large island (like Jamaica)

If an atom were blown up to the size of a football stadium, then its nucleus would be the size of…

A car

The density of an atom’s nucleus is about the same as if you stuffed which of the following into a 1 foot by | foot by | foot-sized box…

An elephant A blue whale A box store (like Target) A metropolitan city (like Chicago) Every person on Earth’s car

A soccerball

A box store (like Target) The United States The Earth

An apple A marble

A pea

The Earth A marble Every person on Earth’s car

Essential question: What important information does the Periodic Table tell us about the atoms of elements? Topic Questions:

What is an atom?

The word ‘atom’ comes from the Ancient Greek adjective ‘atomos’ which means indivisible.

The concept of an atom has changed over time. Analogies can help us understand the different models:

Billiard ball

Dalton (early 1800s)

2 What are

the subatomic particles?

The root sub means “under” or “below”

that can exist.

Protons are like the ‘fingerprint’ of the atom. Every type of atom has a unique number of protons.

Chocolate chip cookie Thomson (late 1800s)

Cherry with a pit Solar system

Rutherford (early 1900s)

nucleus

Bohr (1900s)

Particle Name

Proton

Charge

Positive (+)

Neutral (0)

Negative (-)

Symbol

p+

n0

e-

| amu

| amu

0 amu

Mass

Neutron

Electron

Cotton ball

Schrodinger, Heisenberg, Einstein, and others

1

The smallest part of a chemical element

(1900s - present)

amu = Atomic Mass Unit A tiny unit of mass used to measure the mass of subatomic particles.

© Sunrise Science 2017

KEY

Topic Questions:

3 Where are

The current atomic theory is that electrons exist in a ‘cloud’ surrounding an extremely tiny, dense nucleus. However, we often still represent the atom in the ‘Bohr’ model (like the solar system with electrons in specific orbits around the nucleus) because it makes it easier to diagram and predict atoms’ behavior.

Boron

nucleus

(where the mass is)

the subatomic particles?

electron cloud

(‘massless’ electrons moving super fast) Do

4

© Sunrise Science 2017

In a neutral (not charged) atom, there are an equal number of positive and negative particles.

Carbon - 13

Chemical Symbol A one or two letter symbol that represents the element. The first letter is always capitalized.

Element Name The elements are named using Latin and Greek word roots based on their properties, after heavenly bodies, after Gods, after places, and after scientists.

6 p+ 6 e8 n0

6 p+ 6 e7 n0

6 p+ 6 e6 n0 Carbon - 12

What does the Periodic Table tell us?

5 p+ 5 e6 n0

Atoms of the same element that have different numbers of neutrons.

What is an isotope of an atom?

5

Color the protons with your chosen color. Color the neutrons with your chosen color. Leave the electrons white.

Why are the numbers of these two particles equal?

Boron’s Subatomic Particles

The Atom

F

Fluorine

18.998

9

Carbon - 14 Atomic #

The Atomic Number is like the ‘ID’ (identity) of the element. It tells how many protons the atoms of that element contain.

Atomic Mass

The weighted average mass of all isotopes of the element.

What does this number tell you?

Mass Number

To figure out the number of neutrons in an atom’s most common isotope, R-O-U-N-D the atomic mass on the periodic table to the nearest whole number. 18.998 rounds to  19 Then, subtract the number of protons (the Atomic #). 19 subtract 9  10 Fluorine atoms have 10 neutrons

© Sunrise Science 2017

Sum it up!

KEY

Match each item with the correct statement: ___C____ 1. The smallest particle of an element that retains the properties of that element

A. PROTON

___A____ 2. A positively charged subatomic particle

B. NUCLEUS

___D____ 3. A negatively charged subatomic particle

C. ATOM

___E____ 4. A subatomic particle with no charge

D. ELECTRON

___B____ 5. The central part of an atom containing protons and neutrons

E. NEUTRON

Match each item with the correct statement: ___C____ 1. Atoms with the same number of protons but different numbers of neutrons

A. ATOMIC MASS

___B____ 2. Total number of protons and neutrons in the nucleus

B. MASS NUMBER

___A____ 3. The weighted average of the masses of the isotopes of an element

C. ISOTOPE

Label each part of the Periodic Table square:

25

Mn

Atomic Number

These are the nuclei of three different atoms. Write the isotopic notation for each (for example, Carbon – 13)

Chemical Symbol

Manganese

Element Name Atomic Mass

54.94

Boron - 12

Nitrogen - 13

Beryllium - 9

Complete the table below by referencing a periodic table. The first row has been completed as an example. Chemical Symbol

Atomic Number

Atomic Mass

Mass Number

Hyphenated Notation of Most Common Isotope

# of protons

# of electrons

# of neutrons (Show work : Mass Number – Atomic #)

Phosphorous

P

15

30.97

31

Phosphorous – 31

15

15

31 – 15 = 16

Aluminum

Al

13

26.98

27

Aluminum – 27

13

13

27 - 13 = 14

Potassium

K

19

39.10

39

Potassium – 39

19

19

39 - 19 = 20

Argon

Ar

18

39.95

40

Argon – 40

18

18

40 - 18 = 22

Lead

Pb

82

207.20

207

Lead – 207

82

82

207 - 82 = 125

Name:

_________________________________________________________________________

The atom

Class:

Analogy

Quick Just How Small is an Atom? Watch: http://tinyurl.com/lcdvfzx

______________

Date:

______________

My Guess (circle one)

Actual

If the atoms of a grapefruit were blown up to the size of blueberries, then the grapefruit would be the size of…

A basketball A school bus A large island (like Jamaica)

If an atom were blown up to the size of a football stadium, then its nucleus would be the size of…

A car

The density of an atom’s nucleus is about the same as if you stuffed which of the following into a 1 foot by | foot by | foot-sized box…

An elephant A blue whale A box store (like Target) A metropolitan city (like Chicago) Every person on Earth’s car

A soccerball

A box store (like Target) The United States The Earth

An apple A marble

A pea

Essential question: What important information does the Periodic Table tell us about the atoms of elements? Topic Questions:

What is an __________?

The word ‘atom’ comes from the Ancient Greek adjective ‘____________’ which means indivisible. The concept of an atom has changed over time. Analogies can help us understand the different ______________:

B______ ball

__________ (early 1800s)

2 What are

the ____________ particles?

Protons are like the ‘_____________’ of the atom. Every type of atom has a __________ number of protons.

C_________ chip cookie

Thomson (late __________)

C______ C_______ with a pit S_____ system ball

________________ (early 1900s)

n______

Bohr (__________)

Charge

p+

(1900s - present)

amu = A______ M___ Unit

Particle Name

Symbol The root sub means:

that can __________.

Schrodinger, Heisenberg, ______________, and others

1

The smallest part of a chemical ___________

n0

e-

A tiny unit of __________ used to measure the mass of ______________ particles.

Mass © Sunrise Science 2017

Topic Questions:

3 __________ are the subatomic particles?

The current atomic __________ is that electrons exist in a ‘cloud’ surrounding an extremely tiny, _________ nucleus. However, we often still represent the atom in the ‘________’ model (like the solar system with electrons in specific orbits around the nucleus) because it makes it easier to diagram and predict atoms’ behavior.

Boron

nucleus

(where the __________ is)

electron cloud

(‘____________’ electrons moving super ________) Do

4

© Sunrise Science 2017

C_______ - ___

Chemical Symbol A one or two __________ symbol that represents the element. The __________ letter is always capitalized.

Element Name The elements are named using Latin and Greek word roots based on their _______________, after ____________ bodies, after ___________, after places, and after ______________.

p+ en0

p+ en0

p+ en0 C_______ - ___

What does the _________________ Table tell us?

p+ en0

Atoms of the same element that have different numbers of neutrons.

What is an ____________ of an atom?

5

Color the protons with your chosen color. Color the neutrons with your chosen color. Leave the electrons white.

Why are the numbers of these two particles equal?

Boron’s Subatomic Particles

The Atom

F

Fluorine

18.998

9

C_______ - ___ Atomic #

The Atomic Number is like the ‘ID’ (____________) of the element. It tells how many ___________ the atoms of that element contain.

Atomic Mass

The weighted ______________ mass of all ____________ of the element.

What does this number tell you?

Mass _________

To figure out the number of ____________ in an atom’s most common isotope, R-O-U-N-D the atomic mass on the periodic table to the nearest __________ number. 18.998 rounds to  19 Then, _____________ the number of ____________ (the Atomic #). 19 subtract 9  _____ Fluorine atoms have _____ neutrons

© Sunrise Science 2017

Sum it up! Match each item with the correct statement: ________ 1. The smallest particle of an element that retains the properties of that element

A. PROTON

________ 2. A positively charged subatomic particle

B. NUCLEUS

________ 3. A negatively charged subatomic particle

C. ATOM

________ 4. A subatomic particle with no charge

D. ELECTRON

________ 5. The central part of an atom containing protons and neutrons

E. NEUTRON

Match each item with the correct statement: ________ 1. Atoms with the same number of protons but different numbers of neutrons

A. ATOMIC MASS

________ 2. Total number of protons and neutrons in the nucleus

B. MASS NUMBER

________ 3. The weighted average of the masses of the isotopes of an element

C. ISOTOPE

Label each part of the Periodic Table square:

These are the nuclei of three different atoms. Write the isotopic notation for each (for example, Carbon – 13)

25

Mn

Manganese

54.94

__________________

__________________

__________________

Complete the table below by referencing a periodic table. The first row has been completed as an example.

Phosphorous Aluminum Potassium Argon Lead

Chemical Symbol

Atomic Number

Atomic Mass

Mass Number

Hyphenated Notation of Most Common Isotope

# of protons

# of electrons

# of neutrons (Show work : Mass Number – Atomic #)

P

15

30.97

31

Phosphorous – 31

15

15

31 – 15 = 16

Name:

_________________________________________________________________________

The atom

Class:

Analogy

Quick Just How Small is an Atom? Watch: http://tinyurl.com/lcdvfzx

______________

Date:

______________

My Guess (circle one)

Actual

If the atoms of a grapefruit were blown up to the size of blueberries, then the grapefruit would be the size of…

A basketball A school bus A large island (like Jamaica)

If an atom were blown up to the size of a football stadium, then its nucleus would be the size of…

A car

The density of an atom’s nucleus is about the same as if you stuffed which of the following into a 1 foot by | foot by | foot-sized box…

An elephant A blue whale A box store (like Target) A metropolitan city (like Chicago) Every person on Earth’s car

A soccerball

A box store (like Target) The United States The Earth

An apple A marble

A pea

Essential question: What important information does the Periodic Table tell us about the atoms of elements? Topic Questions:

that can __________.

The word ‘atom’ comes from the Ancient _____________ adjective ‘____________’ which means indivisible. The concept of an atom has changed over time. Analogies can help us understand the different ______________: Schrodinger, Heisenberg, ______________, and others

1

The smallest part of a chemical ___________

Dalton (early 1800s)

2

Protons are . . .

Particle Name Charge Symbol The root sub means:

(1900s - present)

amu = A______ M___ Unit A tiny unit of __________ used to measure the mass of ______________ particles.

Mass © Sunrise Science 2017

Topic Questions:

3

The current atomic __________ is that electrons exist in a ‘cloud’ surrounding an extremely tiny, _________ nucleus. However, we often still represent the atom in the ‘________’ model (like the solar system with electrons in specific orbits around the nucleus) because it makes it easier to diagram and predict atoms’ behavior.

Boron

nucleus

electron cloud Do

4

Color the protons with your chosen color. Color the neutrons with your chosen color. Leave the electrons white.

C_______ - ___

© Sunrise Science 2017

p+ en0

Atoms of the same element that have different numbers of neutrons.

A one or two __________ symbol that represents the element. The __________ letter is always capitalized.

The elements are named using Latin and Greek word roots based on their _______________, after ____________ bodies, after ___________, after places, and after ______________.

p+ en0

p+ en0

p+ en0 5

Why are the numbers of these two particles equal?

Boron’s Subatomic Particles

The Atom

C_______ - ___

F

Fluorine

18.998

9

C_______ - ___

The Atomic Number is like the ‘ID’ (____________) of the element. It tells how many ___________ the atoms of that element contain.

The weighted ______________ mass of all ____________ of the element.

What does this number tell you?

To figure out the number of ____________ in an atom’s most common isotope, R-O-U-N-D the atomic mass on the periodic table to the nearest __________ number. 18.998 rounds to  19 Then, _____________ the number of ____________ (the Atomic #). 19 subtract 9  _____ Fluorine atoms have _____ neutrons

© Sunrise Science 2017

Sum it up! Match each item with the correct statement: ________ 1. The smallest particle of an element that retains the properties of that element

A. PROTON

________ 2. A positively charged subatomic particle

B. NUCLEUS

________ 3. A negatively charged subatomic particle

C. ATOM

________ 4. A subatomic particle with no charge

D. ELECTRON

________ 5. The central part of an atom containing protons and neutrons

E. NEUTRON

Match each item with the correct statement: ________ 1. Atoms with the same number of protons but different numbers of neutrons

A. ATOMIC MASS

________ 2. Total number of protons and neutrons in the nucleus

B. MASS NUMBER

________ 3. The weighted average of the masses of the isotopes of an element

C. ISOTOPE

Label each part of the Periodic Table square:

These are the nuclei of three different atoms. Write the isotopic notation for each (for example, Carbon – 13)

25

Mn

Manganese

54.94

__________________

__________________

__________________

Complete the table below by referencing a periodic table. The first row has been completed as an example.

Phosphorous Aluminum Potassium Argon Lead

Chemical Symbol

Atomic Number

Atomic Mass

Mass Number

Hyphenated Notation of Most Common Isotope

# of protons

# of electrons

# of neutrons (Show work : Mass Number – Atomic #)

P

15

30.97

31

Phosphorous – 31

15

15

31 – 15 = 16

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