Worksheet Chapter 5: Chemical Bond

1. Compare the physical properties of Magnesium chloride (MgCl2) and Tetrachloromethane (CCl4) in terms of melting point and electrical conductivity.

2. Which of the following molecules contains a double covalent bond?

3. True or False: Ionic compounds can conduct electricity in the solid state.

4. Fill in the blank: A chemical bond formed by the sharing of valence electrons between non-metal atoms is called a ________ bond.

5. Explain the formation of a dative bond in the hydroxonium ion (H3O+).

6. Magnesium (proton number = 12) reacts with Oxygen (proton number = 8) to form magnesium oxide.
(a) Write the electron arrangement for a magnesium atom and an oxygen atom.
(b) State the type of chemical bond formed and describe how the bond is formed.

7. State the three electronegative elements that can form hydrogen bonds when covalently bonded with hydrogen.

8. Explain using chemical principles why metals are good conductors of electricity and can be hammered into thin sheets without breaking (malleable).

9. True or False: Simple covalent compounds generally have low melting and boiling points because the covalent bonds within the molecules are weak.

10. Ammonia (NH3) and Methane (CH4) both have simple molecular covalent structures with similar relative molecular masses.
(a) Explain why the boiling point of Ammonia (-33 °C) is significantly higher than that of Methane (-161 °C).
(b) Explain why Ammonia is highly soluble in water, whereas Methane is insoluble.