Example 9.1 Using Lewis Symbols to Predict the Chemical Formula of an Ionic Compound

Transcription

1 Example 9.1 Using Lewis Symbols to Predict the Chemical Formula of an Ionic Compound For Practice 9.1 Use Lewis symbols to predict the formula for the compound that forms between magnesium and nitrogen.

2 Example 9.2 Predicting Relative Lattice Energies For Practice 9.2 Arrange the following in order of increasing magnitude of lattice energy: LiBr, KI, and CaO. For More Practice 9.2 Which compound has a lattice energy of higher magnitude, NaCl or MgCl 2?

3 Example 9.3 Classifying Bonds as Pure Covalent, Polar Covalent, or Ionic For Practice 9.3 Determine whether the bond formed between each pair of atoms is pure covalent, polar covalent, or ionic. a. I and I b. Cs and Br c. P and O

4 Example 9.4 Writing Lewis Structures For Practice 9.4 Write the Lewis structure for CO.

5 Example 9.5 Writing Lewis Structures For Practice 9.5 Write the Lewis structure for H 2 CO.

6 Example 9.6 Writing Lewis Structures for Polyatomic Ions For Practice 9.6 Write the Lewis structure for the hypochlorite ion, ClO.

7 Example 9.7 Writing Resonance Structures For Practice 9.7 Write a Lewis structure for the NO 2 ion. Include resonance structures.

8 Example 9.9 Drawing Resonance Structures For Practice 9.8 Draw the Lewis structure (including resonance structures) for diazomethane (CH 2 N 2 ).

9 Example 9.10 Writing Lewis Structures for Compounds Having Expanded Octets For Practice 9.10 Write the Lewis structure for XeF 4. For More Practice 9.10 Write the Lewis structure for H 3 PO 4. If necessary, expand the octet on any appropriate atoms to lower formal charge.

10 Example 9.11 Calculating ΔH rxn from Bond Energies For Practice 9.11 Another potential future fuel is methanol (CH 3 OH). Write a balanced equation for the combustion of gaseous methanol and use bond energies to calculate the enthalpy of combustion of methanol in kj/mol. For More Practice 9.11 Use bond energies to calculate ΔH rxn for this reaction:.

11 Example 10.1 VSEPR Theory and the Basic Shapes For Practice 10.1 Determine the molecular geometry of CCl 4.

12 Example 10.2 Predicting Molecular Geometries For Practice 10.2 Predict the molecular geometry and bond angle of ClNO.

13 Example 10.3 Predicting Molecular Geometries For Practice 10.3 Predict the molecular geometry of I 3.

14 Example 10.4 Predicting the Shape of Larger Molecules For Practice 10.4 Predict the geometry about each interior atom in acetic acid and make a sketch of the molecule.

15 Example 10.5 Determining if a Molecule Is Polar For Practice 10.5 Determine if CF 4 is polar.

16 Example 10.8 Hybridization and Bonding Scheme For More Practice 10.8 What is the hybridization of the central iodine atom in I 3?

17 Example 10.9 Bond Order For Practice 10.9 Use molecular orbital theory to predict the bond order in H 2+. Is the H 2 + bond a stronger or weaker bond than the H 2 bond?

18 Example Molecular Orbital Theory for Heteronuclear Diatomic Molecules and Ions For Practice Use molecular orbital theory to determine the bond order of NO. (Use the energy ordering of O 2.) Is the molecule paramagnetic or diamagnetic?

19 Example 11.1 Dipole Dipole Forces For Practice 11.1 Which molecules have dipole dipole forces? a. CI 4 b. CH 3 Cl c. HCI

20 Example 11.2 Hydrogen Bonding For Practice 11.2 Which has the higher boiling point, HF or HCl? Why?