Download VOCABULARY: Lewis Structures, bonding pairs, lone pairs

WOODLAND HILLS HIGH SCHOOL LESSON PLAN
SAS and Understanding By Design Template
Name: Dowd
Week: 11/07/11
Length of Lesson: 17 days
Course: AP Chemistry
Edline
Class website
STAGE I – DESIRED RESULTS
LESSON TOPIC:
Bonding
BIG IDEAS: (Content standards, assessment anchors, eligible content) objectives, and skill focus)
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Chemical bonding occurs as a result of attractive forces between particles.
Chemical bonding occurs as a result of attractive forces between particles.
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ESSENTIAL QUESTIONS:
What factors determine the types of chemical bonds that form between particles?
How does the distribution of electrons in atoms affect the formation of a compound?
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UNDERSTANDING GOALS (CONCEPTS): Students will understand:
The type of bonding that occurs between atoms is related to the valence electrons of those atoms.
Chemical bonding can be covalent, polar covalent, or ionic.
Lewis dot diagrams are useful for studying the structure and bonding nature atoms.
The polarity of a molecule can be determined by the distribution of electrons around the molecule.
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VOCABULARY: Lewis Structures, bonding pairs, lone pairs, resonance, formal charges, octet rule, VSEPR,
polar & nonpolar bonds/molecules, valence bond theory, hybridization, sigma & pi bonds, molecular orbital
theory, bond order, bond strength, bond length
STUDENT OBJECTIVES (COMPETENCIES/OUTCOMES): Students will be able to
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recognize the type of bonding in a compound.
 describe the role of electrons in metallic, ionic and covalent bonding
 write Lewis structures for atoms, monatomic ions, polyatomic ions. ionic compounds, and covalent
compounds
 describe and understand the value of resonance, formal charges, and the octet rule
 use the octet rule, formal charges, and resonance considerations to draw the best Lewis Structure for
polyatomic ions and covalent compounds
 identify the number and type of bonds and electron pairs in a Lewis Structure
 describe and apply VSEPR Theory to determine the molecular geometry and bond angles in a simple
molecule/polyatomic ion (or a specified atom in the molecule/ion)
 use electronegativities to determine if a bond is polar or nonpolar
 determine if a covalent molecule is polar or nonpolar
 describe the basic concepts of valence bond theory
 identify the hybridization on an atom and the angles between the orbitals
 describe the sigma and pi bonds in terms of overlapping orbitals
 describe the basic concepts of molecular orbital theory
 draw, label, and interpret energy level diagrams for homonuclear and heteronuclear diatomic molecules
involving nonmetals in the first two rows of the periodic table
 write an electron configuration for homonuclear and heteronuclear diatomic molecules involving nonmetals
in the first two rows of the periodic table
 understand and use the interrelationship between bond strength (energy), bond order, and bond length
STAGE II – ASSESSMENT EVIDENCE
PERFORMANCE TASK:
FORMATIVE ASSESSMENTS:
Class discussion
Assignments
Tests/Quizzes
Laboratory experience
Observation
Notetaking
Asking/Answering questions
Performing Lab
STAGE III – LEARNING PLAN
INSTRUCTIONAL
PROCEDURES:
MATERIALS &
RESOURCES:
Explicit Instruction
Overhead/Board
Lab material/equipment
Handouts
Content Area Reading
Presentation
Discussion
Modeling
Demonstration
Prelab
INTERVENTIONS:
Preferential seating
Cooperative work
Active Engagement
Note-taking
Partnering
Cooperative Education
Higher Level Thinking
Scaffolding
Build on prior knowledge
Build vocabulary
MINI LESSON:
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Intro to Bonding: Bond Tyes; Role of Electrons
Lewis Structures & Ionic Bonding
Covalent Bonding: Diatomic molecules; Lewis Structures; Terminology
Polyatomic molecules/ions: Intro & procedure lewis structures, atom arrangement, formal charge, resonance
VSEPR theory intro; electron pairs, geometry, angles, names
VSEPR Theory cont. : molecular geometry, bond angles, polarity, practice
Valence Bond Theory: Concept of overlap, Terminology, Overlap types, hybridization
MO Theory (H2): Concept, Terminology, Energy level diagram
MO Theory:2nd row homonuclear/heteronuclear diatomics; HF
Spectrophotometry Lab
ASSIGNMENTS:
A16.
EOC 9: 21,22,51,53,54,55,81 (Lewis Dot)
A17.
EOC 9: 57,59,61,63,65,67,88,89,96 (Lewis Dot, Resonance, Formal Charge)
A18.
EOC 10: 18,21,22,23,27,30,31,33,34 (Draw 3D models for 23,27,30) (VSEPR & Polarity)
A19.
EOC 10: 35,40,41,43,44,48,49,55,58,62,65,67,68,73 (no KK abbreviations) (VSEPR & Polarity)