- Consider the following substances:
|lead (II) bromide
- (a) Name the substance(s) that conduct electricity in the solid state.
- (b) Name the substance(s) that conduct electricity both in the liquid
state (i.e. when molten) and in aqueous solution. Explain.
- (c) Name the substance(s) that do not conduct electricity themselves
but form conducting liquids when dissolved in water. Explain.
- (d) Name the substance(s) that do not conduct electricity. Explain.
- Take a look at the properties of two bromine-containing compounds:
- hydrogen bromide, HBr,
- sodium bromide, NaBr.
- (a) The difference in conductivities of these two compounds can be
explained in terms of bonding. Describe the bonding in these two compounds.
- (b) Explain the difference in electrical conductivity for NaBr in the
solid state and in the liquid state.
- (c) Explain the difference in electrical conductivity for HBr in aqueous
solution and in the solid and liquid states.
- (d) Write the chemical equation which describes the behaviour of HBr
in aqueous solution.
- Describe the trends in the electronegativities of the elements across a
row and down a column of the periodic table.
- Which element in the periodic table has the largest electronegativity?
- Which element in the periodic table has the smallest electronegativity?
- Arrange the following elements in order of decreasing electronegativity.
- (a) Mg, Al, P, O, K
- (b) C, Si, Ga, O, Ca
- (b) P, As, Cl, S, Mg
- Explain why CO2 has no dipole moment.
- Explain why H2O is a polar molecule.
- Explain why I2 is a nonpolar covalent compound.
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