Download North Haven Public Schools Curriculum

North Haven Public Schools Curriculum
Unit Title/ focus: Chemical Bonding and VSEPR Theory
Textbook: Prentice Hall Chemistry – Chap. 7, 8
Designer Names (s): Larry Fabianski, Marc Horowitz, Julie Nichols
Subject Area: Chemistry L2/L3
Grade Level: 10, 11, 12
Estimated Amount of Instructional Time: 3 weeks
Connecticut State Standards
Chemical Bonds
Biological, chemical and physical properties of matter result from the ability of atoms to form bonds from
electrostatic forces between electrons and protons and between atoms and molecules.
 Atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by
exchanging electrons to form ionic bonds.
 Chemical bonds between atoms in molecules such as H2, CH4, NH3, H2CCH2, N2, Cl2, and many
large biological molecules are covalent.
 Salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by
electrostatic attraction.
 The atoms and molecules in liquids move in a random pattern relative to one another because the
intermolecular forces are too weak to hold the atoms or molecules in a solid form.
 Lewis dot structures can provide models of atoms and molecules.
 The shape of simple molecules and their polarity can be predicted from Lewis dot structures.
 Electronegativity and ionization energy are related to bond formation.
 Solids and liquids held together by Van der Waals forces or hydrogen bonds are affected by
volatility and boiling/melting point temperatures.
Big Ideas
Enduring Understandings
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Atoms of metallic elements tend to lose their valence electrons achieving a complete outer octet.
Atoms of non-metallic elements tend to gain electrons achieving a complete outer octet.
Changes in the number of valance electrons result in a charged atom (cation, anion).
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The valance electrons of netal atoms can be modeled as a sea of electrons resulting in a compact
and orderly pattern.
Molecular bonding involves the sharing of electrons while ionic bonding involves the transfer of
electrons to complete the outer octet.
Lewis dot structures provide models of atoms and molecules.
VSEPR theory is used to predict the shapes of molecular compounds.
Intermolecluar forces are used to determine states of matter.
Essential Questions
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Why do atoms combine to form bonds?
How do ionic and covalent bonds differ in formation and properties?
How does VSEPR shape affect the polarity of a molecule?
What holds molecules together in solids and liquids?
What Students Should Know and Be Able to Do
(Skills and Knowledge)
Prerequisite Concepts/Skills
Students will…
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Be able to name and write formulas for compounds.
Be able to recognize whether a compound is ionic or covalent.
Classify metals and non-metals.
Determine the number of valence electrons.
Knowledge
Students will…
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Understand hybridization and VSEPR theory.
Understand the effect of polarity on the characteristics of a compound.
Skills
Students will…
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Be able to use Lewis structures and VSEPR theory to predict the shape and polarity of a molecule.
Be able to identify the main contributing intermolecular force between molecules.
Vocabulary
valence electrons
anion
octet rule
diatomic molecule
triple covalent bond
VSEPR theory
bent
trigonal planar
intermolecular forces
hydrogen bonds
ionic bond
covalent bond
Lewis dot diagram
single covalent bond
polar covalent bond
dipole (polarity)
tetrahedral
hybrid orbitals
dipole interactions
cation
metallic bond
unshared electron pair
double covalent bond
nonpolar covalent bond
linear
pyramidal
resonance
dispersion forces
Pacing Guide
Unit 6: Chemical Bonding and VSEPR theory – 8 blocks
 Ionic Bonding – 1 block
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Covalent Bonding – 2 blocks
o Lewis Structures
o VSEPR theory
o Polarity
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Intermolecular Forces – 1 block
o H-bonding, Dipole-Dipole, Dispersion Forces
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LABS: Molecular Formulas/Geometry lab (1 block)
Chromatography Laboratory (1 block)
Assessment Evidence
Required Assessments:
Two quiz
End of Unit Test
Supplemental Assessments:
Lab reports
Lab activities: Molecular Formulas/Geometry lab
Chromatography Laboratory