1. A Covalent bonding B Polar covalent bonding C Metallic bonding D Hydrogen bonding E Ionic bonding F London dispersion forces

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1 Higher (National 6) Unit 1: Chemical changes and structure 1c Bonding and structure Problem sheets 1. A Covalent bonding B Polar covalent bonding C Metallic bonding D Hydrogen bonding E Ionic bonding F London dispersion forces Which box (or boxes) show(s) the type of bonding or force that: a. is responsible for the low boiling point of the Noble gases (1 box)? b. exists between molecules (2 boxes)? c. could be considered as intermediate between ionic and covalent bonding in the bonding continuum (1 box)? d. allows electrons a lot of movement (1 box)? e. is present in (i) brass, (ii) hydrogen chloride and (iii) ammonia (NH3)? 2. Calcium oxide and lithium chloride both form ionic lattices. Suggest a reason why the boiling point of calcium oxide (2850 C) should be much higher than that of lithium chloride (610 C). Hint: write the ionic formulae for each 3. The melting points of the dioxides of elements from group (IV) of the periodic table are: Dioxide Carbon (CO2) Silicon (SiO2) Germanium Tin (SnO2) (GeO2) Melting Point ( C) a. Explain in terms of structure why there is such a large difference between the melting point of CO2 and the other oxides? b. Sketch the structure of the first two oxides in the table, then add the labels where appropriate: covalent bond, London dispersion force, covalent network 4. A C6H6 B C2H5OH C NH3 D HBr E Cu Which box (or boxes) show(s) a substance which: a. Is non-polar? b. Will probably dissolve in non-polar solvents, e.g. hexane? c. Will probably dissolve in a polar solvent, e.g. water? d. Will have hydrogen bonds? 5. Both butane (BP 272K) and propanol (BP 370K) have similar molecular mass. Why is the boiling point of propanol so much higher?

2 6. Lithium iodide is quite soluble in non-polar solvents. a. What does this indicate about the type of bonding and structure in lithium iodide? b. Would lithium fluoride be soluble in non-polar solvents? Hint: Check the difference in electronegativities. 7. The elements Na to Ar make up the 3 rd period of the Periodic Table. a. Copy and complete the following table: Element Melting point ( C) Bonds or forces broken at melting point Sodium 98 Metallic Silicon 1410 Phosphorus 44 b. Name the two elements in the 3 rd period which form the compound with the greatest degree of ionic character. 8. Tin iodide can be prepared directly from its elements. Excess tin is heated for about an hour with iodine dissolved in tetrachloromethane (CCl4). Tetrachloromethane, which has a boiling point of 77 C, acts as a solvent for both the iodine and for the tin iodide that is formed. When the reaction is complete, the excess tin is removed. On cooling the remaining solution, orange crystals of tin iodide appear. a. Why is a condenser used when melting the reaction mixture? b. Give two pieces of evidence from the method of preparation that suggests tin iodide is a covalent molecular compound.

3 Exam type questions ( ) London dispersion forces

4 10. Hydrogen and fluorine can react explosively to form hydrogen fluoride gas. The boiling point of hydrogen fluoride, HF, is much higher than the boiling point of fluorine, F2. H-F Boiling point: 19.5 C F-F Boiling point: -188 C Explain fully why the boiling point of hydrogen fluoride is much higher than the boiling point of fluorine. In your answer you should mention the intermolecular forces (Van der Waals) involved and how they arise. 11. The structures below show molecules that contain chlorine atoms. Explain clearly why trichloromethane is more soluble in water than tetrachloromethane. Your answer should include the names of the intermolecular forces (Van der Waals) involved. 12. Liquid hydrogen sulphide has a boiling point of -60 C. Explain clearly why hydrogen sulphide is a gas at room temperature. In your answer you should mention the intermolecular forces (Van der Waals) involved and how they arise.

5 Unit 1: Chemical changes and structure Bonding and structure Ink exercise 1. Use the table below to answer the questions that follow. A IBr B CCl 4 C IF D NaCl E C 6 H 14 a. Which two molecules are non-polar? b. Which substance conducts in the molten state? c. Name three substances you would expect to dissolve in water d. Two molecules have London Dispersion forces between the molecules. Name one (4) 2. Explain each of the following: a. Silicon dioxide has a much higher melting point than carbon dioxide. b. Propanol and butane have almost the same molecular mass bur propanol has a boiling point 97 o C and butane 0.5 o C. c. Potassium chloride dissolves in water but not in hexane d. Ice is less dense than water. (4) 3. Name the three forms of carbon. (1) 4. Magnesium chloride and aluminium chloride could be expected to have similar properties as both are metal and non-metal compounds. On heating aluminium chloride changes from a solid to a gas at the relatively low temperature of 180 o C, but magnesium chloride does not melt until 1417 o C. Molten aluminium chloride is an insulator of electricity and magnesium chloride a conductor. a. State the type of bonding in aluminium chloride and magnesium chloride. b. Explain your answers to (a) c. Which of the two compounds would you expect to be soluble in water? (5) [12]

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