Laboratory Activity 5.4.1: To study the physical properties of ionic and covalent compound |
Material: » Sodium chloride » Naphthalene » Lead (II) bromide » Distilled water » Benzene |
Apparatus: » Spatula » Battery » Electric bulb » Connecting wires » Crucible » Bunsen burner » Tripod stand » Carbon rods » Glass rod » Wire gauze |
► | The animation below shows the procedures and observation of the experiment.
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► | (A) Melting point
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► | (B) Solubility
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► | (C) Volatility
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► | (D) Electrical conductivity
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► | (A) Melting point
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► | (B) Solubility
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► | (C) Volatility
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► | (D) Electrical conductivity
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► | Sodium chloride does not melt when heated because its melting point is very high. But naphthalene melts at about 8OᵒC . Sodium chloride is an ionic compound. Naphthalene is a covalent compound. | |
► | Benzene is an organic solvent. Only naphthalene dissolves in it. | |
► | Benzene evaporates quickly. | |
► | Lead (II) bromide has a lower melting point (373ᵒC) than sodium chloride(801ᵒC). Lead(II) bromide conduct electricity only in the molten state. It does not conduct electricity in the solid state. |
► | Ionic compounds are soluble in water but insoluble in organic solvents. Ionic compounds have high melting points, low volatility and can conduct electricity in the molten or aqueous states. | |
► | Covalent compounds are insoluble in water but soluble in organic solvents. Covalent compounds have low melting points, high volatility and cannot conduct electricity in all state. |
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