High School Science

Chemistry Unit 2: Quantum Effects and Periodic Trends

Science Core Standards

Student Learning Progressions

STANDARD II: Students will understand the relationship between energy changes in the atom specific to the movement of electrons between energy levels in an atom resulting in the emission or absorption of quantum energy. They will also understand that the emission of high-energy particles results from nuclear changes and that matter can be converted to energy during nuclear reactions. Objective 1: a. Identify the relationship between wavelength and light energy. b. Examine evidence from the lab indicating that energy is absorbed or released in discrete units when electrons move from one energy level to another. c. Correlate the energy in a photon to the color of light emitted. d. After observing spectral emissions in the lab (e.g., flame test, spectrum tubes), identify unknown elements by comparison to known emission spectra. STANDARD I: Students will understand that all matter in the universe has a common origin and is made of atoms, which have structure and can be systematically arranged on the periodic table. Objective 3: c. Identify similarities in chemical behavior of elements within a group. d. Generalize trends in reactivity of elements within a group to trends in other groups. e. Compare the properties of elements (e.g., metal, nonmetallic, metalloid) based on their position in the periodic table. STANDARD III: Students will understand chemical bonding and the relationship of the type of bonding to the chemical and physical properties of substances. Objective 1: a. Determine the number of valence electrons in atoms using the periodic table.

• Identify the relationship between wavelength and light energy. • Correlate the energy in a photon to the color of light emitted. • Identify an unknown element by comparing atomic emission spectra. • Identify the chemical behaviors of groups on the periodic table. • Compare and contrast group trends on the periodic table. • Predict and classify the physical properties of an element based on its location on the periodic table. • Determine the number of valence electrons in atoms using the periodic table.

Key Terms quantum, wavelength, emit, absorb, spectrum, energy level, photon, frequency, valence electron, metal, non-metal, metalloid, malleable, conductive, periodic table

Essentials

Extension (If Time Permits)

Eliminate

Light: waves, energy and photons • Relationship between wavelength, frequency and energy • Bohr Model: How light is emitting from an atom: electrons absorb energy, energy level transitions result in light emission. • energy absorbed and released is in “discrete” units (quanta) • Lab evidence to make connections between absorbing energy and releasing light; and using results to identify elements (flame tests and/or spectrum tubes) • • • •

Calculating wavelength, frequency and energy Photoelectric effect Heisenberg uncertainty principle Electron configuration with d and f; orbital

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