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The Chemistry of Titanium 1e – Bonding and Properties Learning Intentions • To relate Melting and Boiling Point, Electrical Conductivity, Viscosity and Solubility to the structure and bonding of substances • To use information on substances to identify the bonding present Melting and Boiling Points Substance Bond broken Melting/boiling point Metal Metallic High Ionic Lattice Ionic bond High Covalent Network Covalent bond High Covalent Molecule Van der Waals forces Low • General Rule: • The stronger the bond or force that needs to be broken to get the substance to melt or boil, the higher its melting or boiling point Viscosity of Liquids • The stronger the force of attraction between molecules the greater the viscosity or thickness of the liquid Electrical Conductivity in Metals Electrical Conductivity in Ionic Liquids General rule for Electrical Conductivity • In order for something to conduct it must contain charged particles (electrons or ions) that are free to move Solubility • General Rule: • As a rule of thumb, in terms of solubility, “like dissolves like” • Ionic substances dissolve in polar solvents eg ammonium chloride in water` • Non-polar dissolve in non-polar solvents eg wax in paraffin / nail polish in acetone Polar Molecules A liquid that substances dissolves in is called a SOLVENT. Solvents can be either polar or non-polar molecules. Immiscible liquids do not mix, e.g. oil and water, however, non-polar liquids are miscible with each other. Polar solvents will usually dissolve polar molecules. Non-polar solvents will usually dissolve non-polar molecules. Water is a polar molecule so it is a polar solvent. + -+ Dissolving in Water Generally, covalent molecules are insoluble in water. However, small molecules like ethanol (C2H5OH), with a polar O-H functional group, will dissolve, + Ethanol H2O H + - Ionic Compound dissolving in water + + + - C C H H - + + + + - O H + + - + + - + + H - + + H Hydrated ions + + + - + + + - Dissolving in a non-polar solvent
