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Questions and Answers
What types of elements are present in a giant ionic lattice?
What types of elements are present in a giant ionic lattice?
A giant ionic lattice consists of a metal and a non-metal.
How does the melting point of simple molecular structures compare to giant covalent structures?
How does the melting point of simple molecular structures compare to giant covalent structures?
Simple molecular structures have a low melting point, whereas giant covalent structures have a high melting point.
Describe the conductivity of graphite and explain why it has this property.
Describe the conductivity of graphite and explain why it has this property.
Graphite conducts electricity due to the presence of delocalised electrons that can move freely.
What explains the high melting points of pure metals and alloys?
What explains the high melting points of pure metals and alloys?
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In terms of structure, how does a normal giant covalent structure differ from a giant ionic lattice?
In terms of structure, how does a normal giant covalent structure differ from a giant ionic lattice?
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Explain why simple molecular substances have low conductivity.
Explain why simple molecular substances have low conductivity.
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What characteristic of graphite's structure contributes to its unique properties, like being soft?
What characteristic of graphite's structure contributes to its unique properties, like being soft?
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How do alloys differ from pure metals in terms of structure and properties?
How do alloys differ from pure metals in terms of structure and properties?
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Study Notes
Types of Structures
- Giant Ionic Lattice: Examples include sodium chloride and calcium oxide. Made up of metal and non-metal elements. 3D lattice of ions with alternating positive and negative charges. High melting point due to strong electrostatic forces of attraction between oppositely charged ions.
- Normal Giant Covalent: Examples include diamond and silicon dioxide. Made up of non-metal and non-metal elements. Billions of atoms covalently bonded together. High melting point because covalent bonds require a lot of energy to break.
- Graphite: Made of carbon atoms arranged in hexagonal layers. Carbon atoms have delocalised electrons. High melting point.
- Simple Molecular: Examples include oxygen, water, and carbon dioxide. Made up of non-metal and non-metal elements. Billions of small molecules. Molecules are covalently bonded and held together by weak intermolecular forces. Low melting point.
- Pure Metals: Examples include iron and copper. Composed of one metallic element. Layers of positive metal ions with delocalised electrons. High melting point. High thermal conductivity as delocalised electrons carry thermal energy.
- Alloys: Examples include steel and bronze. Composed of a metal and another element. Layers of positive metal ions with atoms of different sizes mixed to form the alloy; delocalised electrons. High melting point. High thermal conductivity as delocalised electrons carry thermal energy.
Electrical Conductivity
- Giant Ionic Lattice: Conducts electricity only when molten or in solution (aq). The ions are free to move and carry charge.
- Normal Giant Covalent: Does not conduct electricity since electrons are not delocalised.
- Graphite: Conducts electricity. Delocalized electrons allow charge to move through the graphite.
- Simple Molecular: Does not conduct electricity due to the absence of delocalised electrons.
- Pure Metals: Conducts electricity well. Delocalised electrons can move throughout the metal, allowing charge to move freely.
- Alloys: Conducts electricity. Delocalised electrons can move through the metal.
Melting Points
- Giant Ionic Lattice: High melting points. Strong electrostatic forces of attraction between oppositely charged ions require a lot of energy to break.
- Normal Giant Covalent: High melting points. Strong covalent bonds require a lot of energy to break.
- Graphite: High melting point.
- Simple Molecular: Low melting points. Weak intermolecular forces require little energy to break.
- Pure Metals: High melting point.
- Alloys: High melting point.
Other Properties
- Giant Ionic Lattice: Hard and brittle. Ions can slide past one another, causing the structure to break when forces are applied.
- Normal Giant Covalent: Hard and strong. Covalent bonds give it a strong structure.
- Graphite: Soft and slippery. Layers can slide over each other. Good lubricant.
- Simple Molecular: Soft. Molecules can slide over each other. Weak intermolecular forces allow for ease of movement between molecules. Boiling points increase when molecules get larger or have stronger intermolecular forces.
- Pure Metals: Malleable and ductile. Positive ions are able to slide past each other within the structure.
- Alloys: Hard and strong due to the varying sizes of atoms, which prevents the slipping of layers seen in metals. High thermal conductivity, as delocalised electrons can carry thermal energy.
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Description
This quiz covers various types of chemical structures, including giant ionic lattices, giant covalent structures, graphite, simple molecular compounds, and pure metals. Understand the composition, properties, and examples of each type to enhance your chemistry knowledge.
