Bonding and structure flashcards

Bonding and structure explains how atoms join together and how the arrangement of particles determines the properties of substances. Students must understand three types of chemical bonding: ionic bonding between metals and non-metals, covalent bonding between non-metals, and metallic bonding in metals. Each bonding type produces a characteristic structure, such as giant ionic lattices, simple molecular structures, giant covalent structures, or metallic lattices. The structure of a substance directly affects its melting point, electrical conductivity, and solubility. For example, giant structures generally have high melting points, while simple molecular substances do not. Understanding how electrons are shared or transferred, and how this creates different arrangements of particles, is essential for explaining and predicting the physical properties of a wide range of materials.

1. Card 1

   What happens to electrons during ionic bonding?

   Electrons are transferred from a metal atom to a non-metal atom, forming oppositely charged ions that attract each other.

2. Card 2

   What is a giant ionic lattice?

   A regular, repeating 3D arrangement of oppositely charged ions held together by strong electrostatic forces in all directions.

3. Card 3

   Why do ionic compounds have high melting points?

   Many strong electrostatic forces between oppositely charged ions must be broken, requiring a large amount of energy.

4. Card 4

   When can ionic compounds conduct electricity?

   When molten or dissolved in water, because the ions are free to move and carry charge. Solid ionic compounds cannot conduct.

5. Card 5

   What is covalent bonding?

   A shared pair of electrons between two non-metal atoms, creating a strong attraction that holds the atoms together.

6. Card 6

   Why do simple molecular substances have low melting points?

   Only weak intermolecular forces between molecules need to be overcome, not the strong covalent bonds within each molecule.

7. Card 7

   Give two examples of giant covalent structures.

   Diamond and graphite are both giant covalent structures made entirely of carbon atoms bonded covalently throughout.

8. Card 8

   Why does graphite conduct electricity but diamond does not?

   Graphite has one delocalised electron per carbon atom that is free to move, whereas in diamond all electrons are held in covalent bonds.

9. Card 9

   What holds metal atoms together in metallic bonding?

   A lattice of positive metal ions surrounded by a sea of delocalised electrons that attract the ions strongly.

10. Card 10

    Why are metals good conductors of electricity?

    Delocalised electrons can move freely through the metallic lattice, carrying electrical charge from one place to another.

11. Card 11

    Why are metals malleable?

    Layers of metal ions can slide over each other while the delocalised electrons maintain the overall attraction, so the metal does not shatter.

12. Card 12

    What is a polymer and what type of bonding does it involve?

    A polymer is a very long chain molecule formed by many small monomers joined by covalent bonds, giving it a large relative molecular mass.

• Students often say simple molecular substances have strong bonds, confusing the strong covalent bonds inside molecules with the weak intermolecular forces between them.
• A common error is stating that ionic compounds conduct electricity when solid, forgetting that ions must be free to move for conduction to occur.
• Many students think all giant structures conduct electricity, overlooking that diamond does not because it has no free electrons.

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