CP Chemistry 420
December/January
UNIT 2C: ORGANIZATION OF MATTER (BONDING)
CHAPTER 6 – CHEMICAL BONDING
OBJECTIVES:
Define chemical bond.
Explain why most atoms form chemical bonds.
Describe ionic and covalent bonding.
Classify bonding type according to electronegativity differences.
State the octet rule.
Explain how to determine Lewis structures for molecules containing single bonds,
multiple bonds, or both and draw them.
List and compare the distinctive properties of ionic and covalent compounds.
Write the Lewis structure for a polyatomic ion given the identity of the atoms
combined and other appropriate information.
Describe the electron-sea model of metallic bonding, and explain why metals are good
electrical conductors.
Explain VSEPR theory.
Predict the shapes of molecules or polyatomic ions using VSEPR theory.
Describe dipole-dipole forces, hydrogen “bonding,” induced dipoles, and London
dispersion forces.
Explain what determines molecular polarity.
Mass. State Frameworks:
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.
4.2 Draw Lewis dot structures for simple molecules and ionic compounds.
4.3 Use electronegativity to explain the difference between polar and nonpolar covalent bonds.
4.4 Use valence-shell electron-pair repulsion theory (VSEPR) to predict the molecular geometry
(linear, trigonal planar, and tetrahedral) of simple molecules.
Important vocabulary:
Chemical bond
Electron-not
notation
Lewis structure
Multiple bond
Polyatomic ion
Covalent
bonding
Hydrogen
bonding
London
dispersion
force
Nonpolar
covalent bond
Single bond
Dipole
Intermolecular
force
Lone pair
Octet rule
Triple bond
Dipole-dipole
force
Ionic bonding
Metallic
bonding
Polar
Unshared pair
Double bond
Ionic
compound
Molecular
polarity
Polar-covalent
bond
VSEPR theory
STUDY GUIDE
CONTENT:
 Definition and reason for chemical bonds
 What electrons do in different bond types
 State the octet rule
 Properties of ionic v. covalent compounds
 Explanation of metallic bonding and why metals conduct electricity
 Definition of VSEPR theory and explanation
 List the different IMFs, molecules they come from, and their strength
NON-MATH SKILLS:
 Draw electron dot notation pictures
 Draw Lewis structures
 Use VSEPR theory to predict the shapes of molecules
 Predict the polarity of molecules
 Predict the IMFs between two molecules
MATH SKILLS:
 Electronegativity differences in relation to bond type