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Chemistry · Unit 1 · Properties and structure of materials · Compounds and mixtures

Explain the properties of ionic compounds by modelling ionic bonding as ions arranged in a crystalline lattice structure with strong electrostatic forces of attraction between oppositely charged ions.

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Question 1

Sodium chloride (NaCl) has a melting point of 801 °C, while molecular iodine (I\(_{2}\)) has a melting point of 114 °C. Explain why sodium chloride has a significantly higher melting point than iodine.

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Question 2

Sodium chloride (NaCl) has a melting point of 801 °C, while magnesium oxide (MgO) has a melting point of 2852 °C. Which statement correctly explains why MgO has a higher melting point than NaCl?

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Question 3

Sodium chloride \((\text{NaCl})\) has a melting point of \(801\,^{\circ}\text{C}\). Explain why sodium chloride has such a high melting point in terms of its structure and bonding.

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More in Compounds and mixtures

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Explain the properties of covalent compounds by modelling covalent bonding as the sharing of an electron pair in the region between two nuclei with a strong electrostatic force of attraction between both nuclei.
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Identify that pure substances have distinct measurable properties (e.g. melting and boiling point, reactivity, strength, density) and mixtures have properties dependent on the identity and relative amounts of the substances that make them up.
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