1) Based on your understanding the metallic bonding and metallic solids answer the following:

a) Aluminium has a boiling point of 2519^oC, while zinc boils at 907^oC. Explain the difference in boiling points between these two metals.

b) Which metal, scandium (Sc) or yttrium (Y) would you expect to have the higher boiling point? Briefly, explain your choice.

2) Given the following data and your understanding of ionic bonding, answer the questions below:

Ionic radii: Na¹⁺ = 95 pm Mg²⁺ = 65 pm Ca²⁺ = 99 pm

Ionic radii: F^1- = 136 pm Cl^1- = 181 pm

a) Sodium fluoride boils at 1704^oC while magnesium fluoride boils at 2227^oC. Explain the difference in boiling points between these two ionic crystals.

b) Magnesium chloride and calcium chloride each have a different solubility in water at 20^oC. Which of these two salts would you expect to have the higher solubility? Briefly explain your choice.

1) Identify the type of orbital hybridization being used by the highlighted atom in each of the following molecules/ions:

a) the "C" in HCN b) the "N" in NO₃^1- c) the "B" in BCl₃

2) Consider the following acetone molecule: CH₃ -CO -CH₃

According to the valence bond theory and orbital hybridization, account for every bond in the molecule in terms of the orbital hybridization used by each atom, the orbital overlap involved and the resulting bond type (sigma/pi) formed.

1a) Draw the Lewis Diagrams for the following molecules or ions:

i) IO₄^1- ii) SO₃ iii) ClF₃ iv) ClO₃^1- v) TeCl₄

1b) Which, if any, of these particles would be considered "resonance structures"?

1c) Using the VSEPR Theory, state the expected shape of each particle.

1d) Consider the three neutral molecules, which, if any, would be polar?

1e) State the bond angle around the central atom in particles (i) and (ii)?

1f) State the type of orbital hybridization that is being used by the following atoms:

i) the sulphur in SO₃ ii) the tellurium in TeCl₄

1) Consider the following pairs of compounds, indicate which of the pair would have the higher boiling point and briefly explain your answer.

a) C₃H₈ vs C₆H₁₄ b) CH₃OH vs CH₃Cl c) CO₂ vs SO₂

2) If carbon and silicon are in the same chemical family, explain why carbon dioxide is a gas at room temperature but silicon dioxide is an extremely hard solid that melts at 1722^oC.

3) You have three solids and wish to classify them as either ionic, molecular or network. Suggest an experimental procedure and the observations that would allow you to distinguish between these three types of solids.