Bonding, Structure and Properties of Matter
Bonding, structure and properties of matter is the GCSE chemistry topic covering the three types of strong chemical bonding (ionic, covalent and metallic), how these bonds relate to a substance's structure, and how structure determines properties such as melting point and electrical conductivity. It also covers the states of matter and the different forms (allotropes) of carbon.
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Method
- For ionic bonding questions, describe the transfer of electrons between a metal and a non-metal atom, forming oppositely charged ions held together by strong electrostatic forces in a giant lattice.
- For covalent bonding questions, describe the sharing of pairs of electrons between non-metal atoms, and identify whether the substance forms small molecules (such as water or chlorine) or a giant covalent structure (such as diamond, graphite or silicon dioxide).
- Link structure to properties: giant structures (ionic lattices, giant covalent structures, metals) have high melting and boiling points because many strong bonds/forces must be broken; simple molecular substances have low melting and boiling points because only weak intermolecular forces between molecules need to be overcome.
- Learn when a substance conducts electricity: ionic compounds conduct only when molten or dissolved, because their ions are then free to move; metals and graphite conduct because of delocalised electrons; simple covalent substances do not conduct, as they have no free ions or electrons.
- Compare the structures of diamond (each carbon atom bonded to four others, very hard, does not conduct) and graphite (each carbon atom bonded to three others in layers, soft and slippery, conducts electricity).
- For metallic bonding, describe the structure as a lattice of positive metal ions surrounded by a sea of delocalised electrons, and use this to explain electrical conductivity and malleability.
Worked example
Explain why graphite can conduct electricity, even though diamond, which is also a form of carbon, cannot.
- Identify that in graphite, each carbon atom forms only three covalent bonds, not four.
- State that this leaves one delocalised electron per carbon atom, which is free to move.
- Explain that these delocalised electrons can move along the layers of graphite, carrying electrical charge.
- State that in diamond, every carbon atom forms four covalent bonds, so there are no delocalised electrons or free ions able to move.
- Final answer: graphite conducts electricity because of its delocalised electrons, while diamond does not conduct because all four outer electrons of each carbon atom are held in covalent bonds.
Practice questions
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Q1Name the three types of strong chemical bonding.Show answer
Answer: Ionic, covalent and metallic.
Q2State the charge on a calcium ion (Group 2).Show answer
Answer: 2+
Q3Name the giant covalent structure made of carbon in which each carbon atom is bonded to four others.Show answer
Answer: Diamond.
Q4State one reason why simple covalent substances such as chlorine have low melting points.Show answer
Answer: They have weak intermolecular forces between molecules, which need only a small amount of energy to overcome (the strong covalent bonds within each molecule are not broken).
Q5Explain why sodium chloride conducts electricity when molten but not when solid.Show answer
Answer: When solid, the ions are held in fixed positions in the lattice and cannot move; when molten, the ions are free to move and can carry electrical charge.
Q6A student says that metals conduct electricity because they contain free-moving ions. Explain why this statement is incorrect, and give the correct explanation.Show answer
Answer: Metals conduct because of delocalised (free) electrons, not free ions; the metal ions stay in fixed positions in the lattice, while the sea of delocalised electrons is free to move and carry charge.
Exam-style questions
Written in the style of a GCSE Science exam paper, with a full mark scheme.
Describe, in terms of electron transfer, how the ionic bond in magnesium oxide (MgO) is formed, including the charges on the ions produced.
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Explain why ionic compounds such as magnesium oxide have very high melting points, and why they do not conduct electricity when solid.
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A student compares two substances, X and Y. Substance X is a solid at room temperature with a very high melting point; it conducts electricity when molten or dissolved in water, but not when solid. Substance Y is a gas at room temperature with a very low boiling point and does not conduct electricity in any state. Identify the type of structure and bonding in each substance, and use the properties given to explain your reasoning.
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Free printable worksheet
Want more practice on paper? Download the bonding, structure and properties of matter worksheet pack - 23 pages of exam-style questions with a full mark scheme. One email opens every download in this browser for 14 days - no account, no card. Print it for personal and classroom use.
This topic is chapter 2 of GCSE Chemistry Workbook, the whole course as one free printable PDF.
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