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Nuclear Chemistry Part 2: Fusion and Fission | Crash Course Chemistry #39

Classroom Resource Information

Title:

Nuclear Chemistry Part 2: Fusion and Fission | Crash Course Chemistry #39

URL:

https://aptv.pbslearningmedia.org/resource/04b58bc6-4c33-474e-868a-ad97c16529b1/nuclear-chemistry-part-2-fusion-and-fission-crash-course-chemistry-39/

Content Source:

PBS

Type:

Audio/Video

Overview:

Continuing our look at nuclear chemistry, Hank takes this episode to talk about fusion and fission. What they mean, how they work, their positives, negatives, and dangers. He also discusses e=mc2, mass defect, and applications of fission and fusion in the real world.

Content Standard(s):

Science
SC2015 (2015)
Grade: 9-12
Chemistry

2 ) Develop and use models of atomic nuclei to explain why the abundance-weighted average of isotopes of an element yields the published atomic mass.

NAEP Framework

NAEP Statement::
P12.4: In a neutral atom, the positively charged nucleus is surrounded by the same number of negatively charged electrons. Atoms of an element whose nuclei have different numbers of neutrons are called isotopes.

Unpacked Content

Scientific And Engineering Practices:

Developing and Using Models

Crosscutting Concepts: Scale, Proportion, and Quantity

Disciplinary Core Idea: Matter and Its Interactions

Evidence Of Student Attainment:

Students:

Identify isotopes of elements.
Develop a model that relates the published atomic mass of an element on the periodic table to the abundance of that element's isotopes.
Use the model to determine the most common isotopic form of an element in nature.

Teacher Vocabulary:

Atomic mass
Isotopes
Abundance
Weighted average
Nucleus
Protons
Neutrons
Macroscopic level
Atomic/ molecular/ particulate level

Knowledge:

Students know:

Each atom has a charge substructure that consists of a nucleus, which is made of protons and neutrons, surrounded by electrons.
The majority of an atom's mass comes from the protons and neutrons in the nucleus.
Electrons have a very small mass, so they are not typically included in atomic mass calculations.
Atoms of an element can have different masses, and we call those atoms isotopes.
Isotopes of a given element have the same number of protons, but different number of neutrons.
Most elements exist in nature in isotopic form.

Skills:

Students are able to:

Develop a model based on evidence to illustrate the relationship between the structure of the atom and the average atomic mass of an element.
Use the model to make predictions.
Calculate weighted averages.
Determine the most common isotopic form of an element in nature.

Understanding:

Students understand that:

Models can be computational or mathematical.
The published atomic mass of an element is a weighted average of all known isotopes of that element.
Macroscopic patterns are related to the nature of atomic/ molecular/ particulate level structure.

AMSTI Resources:

ASIM Module:
Calculating Average Atomic Mass Coinium Isotopes of Atoms, Coinium Isotopes of Atoms

Tags:

chemistry, emc2, fission, fusion, mass defect, nuclear

License Type:

Custom Permission Type
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This resource provided by:

Author:

Stephanie Carver

ALEX Classroom Resource

Nuclear Chemistry Part 2: Fusion and Fission | Crash Course Chemistry #39