Starter quiz
- Why do atoms form bonds?
- To increase their energy.
- To decrease their temperature.
- To attain a stable electron configuration. ✓
- To increase their size.
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- Match the type of bonding to its description:
- covalent⇔Electrons are shared between atoms. ✓
- ionic⇔Electrons are transferred, so charged ions, not atoms, are bonded. ✓
- metallic⇔Electrons are delocalised among a lattice of metal ions. ✓
- What type of bonding can be found between non–metal atoms?
- covalent ✓
- ionic
- metallic
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- From the diagrams below, select the image depicting a substance with ionic bonding.
A
B ✓
C
- What is a key characteristic of metallic bonding?
- The sharing of electron pairs equally between atoms.
- The complete transfer of electrons between atoms to form charged ions.
- The pooling of electrons in a 'sea' around a network of ions. ✓
- The presence of a dipole moment due to unequal electron sharing.
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- Which of the following substances would you expect to conduct electricity when solid?
- sodium chloride
- iron ✓
- carbon dioxide
- graphite ✓
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Exit quiz
- Match the following terms to the correct definition.
- bonding⇔A force of attraction between atoms or ions that holds them together. ✓
- property⇔A characteristic of a substance describing how it appears and behaves. ✓
- charge carrier⇔Particles that enable electrical conductivity. ✓
- structure⇔The arrangement of particles in a substance. ✓
- The two types of structure are simple and ______.
- 'giant' ✓
- Which of the following terms can be used to describe substances that have a full outer shell of electrons?
- inert ✓
- reactive
- stable ✓
- unstable
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- Why do simple molecular substances have low boiling points?
- The covalent bonds between the atoms are weak.
- The forces of attraction between molecules are weak. ✓
- The ionic bonds between the ions are weak.
- The intramolecular bonds between the atoms are weak.
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- The presence of which of the following allows conductivity in a substance?
- delocalised electrons ✓
- free–moving ions ✓
- a full outer shell of electrons
- ions in fixed positions
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- Match the following structures to the type of bonding.
- covalent⇔simple or giant molecular structures ✓
- ionic⇔giant lattice structure ✓
- metallic⇔layers of positive ions in a 'sea' of delocalised electrons ✓
Worksheet
Presentation
Video
Lesson Details
Key learning points
- There are three different types of bonding (covalent, ionic, metallic).
- There are only two types of structure (simple and giant).
- The type of bonding and structure are what lead to properties of substances.
- Melting/boiling points are linked to intermolecular forces (simple) and bond strength (giant).
- Conductivity is linked to whether there are free moving charge carriers.
Common misconception
Ionic substances are binary compounds. Bonding and structure are the same thing. Only bonding influences properties.
As well as multiple ions in ionic substances, there can be polyatomic ions too. Bonding informs structure, and bonding and structure together influences properties.
Keywords
Bonding - Refers to the force of attraction between atoms or ions that hold them together.
Force of attraction - Refers to any force that causes two or more substances to come together.
Structure - Structures in chemistry are determined by the type of bonding and arrangement of atoms or ions.
Property - A feature or characteristic of a substance that can be used to classify it, or describe how it behaves.
Charge carrier - Particles that enable electrical conductivity, such as delocalised electrons or free–moving ions.