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2.76 MB | 87 pages

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2.76 MB | 87 pages

This is a student-centered, active learning lesson without lecture or notetaking!

C.6.A: The student is expected to understand the experimental design and conclusions used in the development of modern atomic theory,…

C.6.E: Express the arrangement of electrons in atoms through electron configurations …

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This guided inquiry lesson enables students to construct their own understanding of the Quantum model of the atom, as well as how to contruct the electron configuration, noble gas electron configuration, and orbital notation of an element. Students are able to actively learn the material without lecture or note taking.

• Students identify the differences between the Bohr model of the atom and the Quantum model of the atom by comparing illustrations of the two models.

• Students identify the shape and electron composition of s and p orbitals by comparing illustrations of several s and p orbitals.

• Students use orbital cutouts to learn how to properly fill s and p orbitals with electrons. They also learn how the Aufbau Principle determines the order that orbitals are filled. Students then practice properly filling pictures of s and p orbitals for different elements.

• Students compare the picture of filled s and p orbitals to the electron configuration of an element and discover how an electron configuration describes the distribution of electrons in the Quantum model of the atom. Students then practice writing electron configurations from pictures of filled orbitals.

• Students compare the electron configuration of an element to its orbital notation and discover how an orbital notation describes the distrubution of electrons in the Quantum model of the atom. Students also learn how Hund’s rule and the Pauli Exclusion Principle are used when drawing orbital notations. Students then practice drawing orbital notations containing s and p orbitals from electron configurations.

• Students use the orbital notations of d and f orbitals to identify the maximum of electrons that can fill d and f orbitals.

Students physically “walk” a periodic table and learn how to use the periodic table to determine the order of orbital filling.

Students physically “walk” a periodic table and learn how to use the periodic table to write the noble gas electron configurations.

Students use a set of task cards to practice writing electron configurations, noble gas electron configurations, and orbital notations.

Students are provided with student study sheets summarizing all of the important concepts and vocabulary in this lesson.

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• Remembering: Explain the following terms: orbital, electron cloud, suborbital, Aufbau Principle, Hund’s Rule, Pauli Exclusion Principle, electron configuration, orbital notation, noble gas electron configuration.

• Understanding: Characterize s, p, d, and f orbitals in terms of their shape (s and p only), number of suborbitals, and maximum number of electrons.

• Applying: Demonstrate how to use patterns in the periodic table to determine the order of orbital filling.

• Analyzing: Differentiate between the Bohr model of the atom and the Quantum model of the atom.

• Evaluating: Discuss the relationship between electron configurations, noble gas electron configurations, orbital notations, and the periodic table.

• Creating: Use the Aufbau Principle, Hund’s Rule, the Pauli Exclusion Principle, and periodic table to construct the electron configuration, noble gas electron configuration, and orbital notation of an element.

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• Cover page (1 page)

• Guided inquiry lesson (14 pages)

• Handouts (3 page)

• Orbital cutouts (1 page)

• Task Cards – 6 versions (24 pages)

• Task Card Answer Sheet (1 page)

• Student study sheets (2 pages)

• Teacher notes (2 pages)

• Guided inquiry lesson with suggested answers (14 pages)

• Task card answers (6 pages

• Periodic Table Squares (19 pages)

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• Please go to your

• Look for the

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Kendo's Chemistry Store

Total Pages

87

Answer Key

Included

Teaching Duration

1 hour

$5.00

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