1. Atom Structure Data Information
P.O.G.I.L
Atom Structure Data Information
Atom are the smallest unit of matter that make up everything!
Atoms are made of 3 subatomic particles.
Atoms are made of protons, neutrons and electrons.
Protons are located in the nucleus which is located in the center of the atom.
Protons have a ‘+1’ charge (much like a battery has a + charge on it).
Protons have a mass of 1 amu = (21)×10-27 kg. = kg.
Neutrons are located in the nucleus which is located in the center of the atom.
Neutrons are neutral, they have no charge (like a dead battery).
Neutrons has a mass of 1 amu = (21)×10-27 kg. = kg.
Electrons are located in the clouds of the atoms. The word “cloud” represents the layers, i.e. orbits, of the electrons as the whiz around the atom’s nucleus. . Only 2 electrons on the first shell (cloud). Only 8 electrons on the second shell (cloud) and only 8 electrons on the 3rd shell(cloud). This rule only pertains to the 1st 18 elements on the periodic table.
Electrons have a charge of ‘-1’ (much like a battery has a – charge at one end).
Electrons mass is thousands of times smaller than protons and neutrons so we say it has no mass although it really does. The mass is just soo small that it just doesn’t count. Imagine a dog has fleas. If you weigh the mass of the dog say it is 20 kg. Now add some fleas to the dog. Did the mass of the dog really change enough to count? This is why we ‘say’ electrons have no mass.
Isotopes are atoms of the same element that contain equal numbers of protons but different numbers of neutrons in their nucleus.
Isotopes are atoms of the same element that have different atomic masses.
Ions are atoms with a charge. The atom has lost or gained electrons therefore protons do not equal electrons.
Amu – atomic mass unit

2. APE MAN Pneumonic note: APE MAN Pees in the middle!
A – Atomic Number P – Protons E – Electrons M – Mass Number N - Neutrons
How to use APE MAN A
= P
= E M
- A
------
= # Neutrons
Example: How to use APE MAN (for a neutral atom) read the fine print! A
= P = 2 protons
= E = 2 electrons
M mass number
- A
= # Neutrons = 2 Neutrons

3. Protons 37 48 1 31 38 3 Start Time: End time: Explore:
1. What is an atom made of?
2. What are the 3 subatomic particles?
3. Where are the protons located?
4. What is the mass of the Proton?
5. What is the unit that is used for mass?
6. What is the charge of a proton?
Understand:
7. Create your own understanding of what an proton is:
8. Where on the periodic table do I look to find the number of protons of an atom?
9. I have 5 protons, who am I?
Definition:
10. Define proton:
11. Which subatomic particle determines the element of the atom?
Analyze:
12. Describe the location of the proton:
13. What is the total number of protons in a cadmium, Cd, atom that has a mass of 112?
14. In the early 1900s many scientist thought that an atom consisted of a positive substance with negative charges scattered throughout the substance. Then Earnest Rutherford completed an experiment that changed the concept of the atom. His discovery led to the understanding that an atom consists mostly of empty space with – a. protons orbiting a dense nucleus made of electrons and neutrons b. electrons orbiting a dense nucleus made of protons and neutrons.
c. neutrons and protons orbiting a cloud of electrons
d. electrons and protons orbiting a cloud of neutrons
15. How many protons are in an atom of hafnium, Hf, with a mass of 178?
16. Describe the location and the charge of a proton.
17. Using the atom model, determine the element:
18: Using the data chart, determine the atom:
Protons
Team roles
Team Member
Scientist: read questions, keep track of time, make sure all participate
Engineer: Talks to instructor, speaks for the team
Mechanic: Get materials, records answers
Technology: look up information on internet, share results found
Who am I
Number of protons
Number of Neutrons
Number of Valence Electrons 37 48 1 31 38 3

4. Neutrons Start Time: End time: Explore: 1. What is an atom made of?
2. What are the 3 subatomic particles?
3. Where are the neutrons located?
4. What is the mass of the Neutron?
5. What is the unit that is used for mass?
6. What is the charge of a neutron?
Understand:
7. Create your own understanding of what a neutron is:
8. Where on the periodic table do I look to find the number of neutrons of an atom?
9. I have an atomic mass of 4 who am I? How many neutrons do I have?
Can an element have different number of neutrons? What are they called?
Definition:
11. Define neutron:
12. If I add the mass of the proton with the mass of the neutron, what do I get?
Analyze:
13. Describe the location of the neutron:
14. How many neutrons are in this atom?
15. What is the mass of the nucleus?
16. What did you have to add together to find the mass of the nucleus?
17. What is located in the nucleus?
18. What is the charge of the nucleus?
19. How do you determine the charge of the nucleus?
20. Using APE MAN, determine the # of neutrons in a Carbon Atom with a mass of 12:
21. Using APE MAN, determine the # of neutrons in a Carbon Atom with a mass of 14:
22. What is the only subatomic particle that is different between Carbon 12 and Carbon 14? What are these called?
Neutrons

5. Electrons Start Time: End time: Explore: What is an atom made of?
What are the 3 subatomic particles?
Where are the electrons located?
What is the mass of the electron?
What is the unit that is used for mass?
What is the charge of an electron?
Understand:
6. Create your own understanding of what an electron is:
7. Where on the periodic table do I look to find the number of electrons of a atom?
8. Can the number of electrons change for an atom, why or why not?
Definition:
9. Define electrons:
Analysis:
11. How many electrons are on this atom?
12. How can you tell?
13. What is the charge of the cloud?
14. Use APE MAN to determine the number of electrons for a Fluorine Atom:
What is the charge of this Fluorine atom? (Hint: Protons-Electrons)
16. If Fluorine had 1 more electron, what would its charge be now?
Team Reflection Use of time:
1. What were the group’s greatest strengths? What indications were there that the team worked together? What frustrated your group the most? What could the group do to improve in the team?
Electrons
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