This chemistry course uses the Science & Engineering Practices and Crosscutting Concepts from the Michigan Science Standards to explore topics including Structure of the Atom, Matter & the Periodic Table, Energy & Reactions, and Environmental Chemistry.
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A1. A course overview and syllabus are included in the online course
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A2. Minimum computer skills and digital literacy skills expected of the learner are clearly stated.*
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B1. The online course objectives or competencies are measurable and clearly state what the learner will be able to demonstrate as a result of successfully completing the course.*
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B3. The online course content is aligned with accepted state and/or other accepted content standards, where applicable.*
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C7. The online course provides regular opportunities for learner-learner interaction.
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F5. The course provides the necessary technical functionality to score and record assessments and calculate earned course points or grades.*
Protons are positively charged subatomic particles that have mass of 1 amu and are located in the nucleus
Neutrons are neutral subatomic particles that have mass of 1 amu and are located in the nucleus
Electrons are negatively charged subatomic particles that have a mass that is negligible mass relative to protons and neutrons. Electrons are located in the electron cloud surrounding the nucleus
Atomic theories have changed over time since the initial Greek/Dalton model as new experimental evidence is produced
The number of protons determines the element
The number of neutrons and protons determine the mass (isotopes)
The balance of electrons to protons determines the charge (ions)
The structure of the atom is determined by the attractive and repulsive forces of the subatomic particles
Even though protons all have a positive change, strong force holds the protons together in the nucleus
Unit 2:
Nuclear fission is a nuclear reaction in which a heavy nucleus splits spontaneously or on impact with another particle, with the release of energy
Nuclear fusion is a nuclear reaction in which atomic nuclei of low atomic number fuse to form a heavier nucleus with the release of energy. This process happens in stars.
Radioactive decay is the process by which an unstable atomic nucleus loses energy by emitting radiation (alpha, beta, gamma) to form a new isotope or element
The total number of neutrons and protons does not change in a nuclear process (nuclear equations)
Within a sample, the number of atoms that will decay can be predicted based on element and the amount of time (graph reading)
The amount of energy released in a nuclear reaction is much larger than the energy released in chemical reactions
Electrons exist at different energy levels
When electrons move up energy levels, they absorb energy
When electrons move down energy levels, they release energy as light (fluorescence)
Light behaves as both a wave and a particle (wavelength, frequency, photons)
The periodic table orders elements horizontally by the number of protons in the atom’s nucleus and places those with similar chemical properties in columns due to the same number of valence electrons.
The location on the periodic table and the electronegativity difference between atoms determines the type of bonds atoms will form
Unit 3:
Use lewis dot structures to predict what elements will bond ionically and covalently.
Explain the energy changes that occur when two atoms approach each other and form a bond (this repeats in the DCI below)
Covalent bonds occur between nonmetal atoms and involved a sharing of electrons (modeled using Lewis Dot Structures)
Ionic bonds occur between metals and nonmetals and involve electrons transferring to the nonmetal elements.
Metallic Bonds exist as a delocalization of charge
Unit 4:
Create a model of electrical forces as atoms approach one another and bond (ie, covalent bonding PE graph vs. helium attraction)
Atomic radius influences IMFAs and chemical bonds (larger atoms have larger internuclear distance when attracted)
As atoms move closer and a bond is created, energy is transferred (released) to the surroundings.
Bond strength is greater than intermolecular forces of attraction
Any time two atoms form a strong chemical bond or two molecules form a weak LDF attraction, chemical energy is converted into other forms of energy
Atoms and molecules can be attracted to each other through intermolecular forces of attraction (IMFAs) and include LDFs, dipole-dipole, and hydrogen bonds
The strength of attraction between neighboring representative particles determines states of matter at room temperature
Create a model of electrical forces as atoms approach one another (PE graph or some other form)
Predict when and describe why a bond will form
Molecules form specific three dimensional shapes based on the bonded electrons and lone pairs on the central atom. This determines molecular polarity.
Molecular polarity is an uneven distribution of electrons as they move through space
Bond polarity is based on electronegativity differences. This leads to polar molecules with positive and negative regions.
Instructor will provide daily, live instruction and also a mix of independent and on demand learning options, in a structured, virtual classroom setting. Students are expected to regularly check school email, reply accordingly, and schedule meetings with instructors, as needed, during on demand time.