Chapter 8: Covalent Bonding

1. Chapter 8: Covalent Bonding Section 1: Molecular Compounds

2. Molecules and Molecular Compounds • Only ______ _______ exist as atoms • Ionic compounds • Electrons are ____________ • Electrostatic forces (+/-) • Similar ______________ • Molecular compounds • Electrons are _____________ • Covalent bond- atoms share same electrons • Properties ________ greatly • Ex. H2O, HCl, CO2

3. Molecules and Molecular Compounds • Molecule • Group of atoms joined by ________ _______ • Charge is _________ • Diatomic Molecule • Molecule of _______ _______ • Ex: O2, Cl2, CO

4. Molecules and Molecular Compounds • Molecular Compounds • Compound composed of _____________ • Molecules of one compound are _________ • Ex: all molecules of carbon monoxide (CO) are exactly the same • Form from 2 or more ______________ • Relatively ______ melting and boiling points • ________or _________ at room temperature

5. Ionic Compound vs. Molecular Compound Formula Unit Molecule

6. Practice Ionic Compound or Molecular Compound? • MgBr2 • C6H12O6 • High melting temperature • Gas at room temperature • Conducts electricity

7. Molecular Formulas • _________ and _________ of atoms present in a molecule of a compound • Not necessarily the ________ ______ _______ ratio • Actual number of _________ in the molecule • Examples: H2O CO No number shown, assume it means 1 1 carbon atom 1 oxygen atom Number of hydrogen atoms

8. Practice How many of each type of atom present in the the following molecular compounds? NH3 CO2 H2O2 C6H12O6 CHO

9. Molecular Formulas • Do not tell the ________ of a molecule, only the _______ and ______ of atoms. • Text pg. 215 • Ex: H2O

10. Br2, CH4, SO3, N2H2, Ne2, KBr • Do any of the above not exist? • Which of the above represent molecules? • Which of the above represent compounds? • Identify each as an Ionic Compound or Molecular Compound.