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UNIT 6: CHEMICAL BONDING
MAIN IDEA: Atoms bond with each other by transferring or sharing valence electrons to
form compounds.
OBJECTIVES:
4.1 Explain how atoms combine to form compounds through both ionic and covalent
bonding. Predict chemical formulas based on the number of valence electrons.
 Differentiate among properties of ionic and covalent bonds.
 Define chemical bond.
 Explain why most atoms form chemical bonds.
 Describe ionic, covalent, and metallic bonding.
 Explain why most chemical bonding is neither purely ionic nor purely covalent.
4.2 Draw Lewis dot structures for simple molecules and ionic compounds.
 Differentiate between resonance structures and isomers.
4.3 Use electronegativity to explain the difference between polar and nonpolar covalent
bonds.
 Identify the type of bonding between two elements given their electronegativities.
4.4 Use valence-shell electron-pair repulsion theory (VSEPR) to predict the molecular
geometry (linear, trigonal planar, and tetrahedral) of simple molecules.
 Use models to explain the structure of a given organic or inorganic molecule.
 Identify a molecule as linear, bent, trigonal planar, trigonal pyramidal, tetrahedral,
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trigonal bipyramidal, or octahedral.
Identify the bond angles within the geometries listed above.
Use symmetry to predict the polarity of a molecule.
Distinguish between the different types of intermolecular forces and the types of
molecules that form them.
Define dipole and compare the strengths of intermolecular forces based on dipole
moments.
IMPORTANT VOCABULARY
Binary compound
Chemical bond
Chemical formula
Covalent bonding
Diatomic molecule
Dipole-dipole force
Dipole – induced dipole force
Dipole – induced dipole force
Dispersion force
Double bond
Ductility
Induced dipole
Intermolecular force
Intramolecular force
Ionic bonding
Ionic compound
Isomer
Lewis dot structure
Lone pair (unshared pair)
Malleability
Metallic bonding
Molecule
Monatomic ion
Nonpolar-covalent bond
Polar
Polar-covalent bond
Polyatomic ion
Resonance Structure
Shared pair
Single bond
Triple bond
(Un)saturated bond
Van der Waal’s force
VSEPR
STUDY GUIDE
CONTENT:
 Ionic v. polar covalent v. nonpolar covalent v. metallic bond
 Properties of ionic v. covalent compounds
 Relationship between electronegativity and bond type
 VSEPR shapes and bond angles
 Molecular polarity & Intermolecular forces
NON-MATH SKILLS:
 Predict bond type based on electronegativity
 Draw Lewis dot structures including resonance structures and isomers
 Use VSEPR to predict molecular geometries & bond angles
 Predict polarity and IMFs of molecules
MATH SKILLS:
 Electronegativity differences