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Lattice Structures

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Chemistry

What’s something that ionic, covalent, and metallic bonding all have in common? One answer to this is the fact that they can all form lattice structures. Because each lattice has a structure and bonding of different types, this causes them to have different physical properties, such as differences in solubility, melting point, and conductivity, which can all be explained by their varying chemical structures.

  • Firstly, we will look at the definition of the lattice structure.
  • After that, we shall explore the types of lattice structures: ionic, covalent, and metallic.
  • Then, we will look at the characteristics of different lattices.
  • We will have a look at some examples of lattices within these sections.

A lattice is a three-dimensional arrangement of ions or atoms in a crystal.

Types Of Lattice Structures

Giant Ionic Lattice

You may remember from our articles on Bonding that Ionic Bonding occurs via the transfer of electrons from metals to non-metals. This causes metals to become charged by losing electrons, forming positively charged ions (cations). Non-metals, on the other hand, become negatively charged by gaining electrons. Ionic bonding, therefore, involves strong electrostatic forces forming between oppositely charged ions in a lattice structure.

These compounds can be arranged in giant ionic lattices called ionic crystals. They are referred to as “giant” as they are made up of large numbers of the same ions arranged in a repeating pattern.

An example of a giant ionic lattice is sodium chloride, NaCl. In the lattice of sodium chloride, the Na+ ions and Cl- ions are all attracted to each other in opposite directions. The ions are packed together in a cubic shape with the negative ions being larger in size than the positive ions.

Diagram of a giant ionic lattice of NaCl. Sahraan Khowaja, StudySmarter Originals

Covalent Lattices

Another important type of bonding is Covalent Bonding. Covalent bonding takes place between non-metals only.

Covalent bonding is the strong electrostatic attraction between two positive nuclei and the shared pair of electrons between them.

There are two types of structures that can contain covalent bonding: giant covalent structures and simple covalent structures. The difference between them is that the electrostatic attraction holding giant structures together is stronger than the electrostatic attraction holding simple structures.

Some examples of simple molecular lattices would be iodine, buckminsterfullerene (C60), and ice.

Diagram representing buckminsterfullerene (C60). Sahraan Khowaja, Studysmarter Originals

Examples of giant molecular lattices are graphite, diamond, and silicon (IV) oxide.

Shapes of the giant molecular lattices. Sahraan Khowaja, StudySmarter Originals

Metallic Lattices

When atoms of metals are closely packed together, they create a regular shape which we call a giant metallic lattice.

Within this lattice, there are free electrons in the outer shell of the metal atoms. These free electrons are also known as ‘delocalised’ electrons and they are free to drift around the structure allowing positive ions to form. This causes metallic bonding to occur.

Metallic bonding is the strong electrostatic attraction between the delocalised electrons and the positive metal ions.

An example of a metallic lattice is magnesium, and its ions have a 2+ charge.

Characteristics Of Lattices

Ionic Lattices

Giant ionic lattices have very high melting and boiling points because of the strong attraction holding the ions together.

They conduct electricity but only when they are dissolved or molten. When ionic lattices are in a solid state, their ions are fixed in position and cannot move so electricity is not conducted.

Giant ionic lattices are soluble in water and polar solvents, however, they are insoluble in non-polar solvents. Polar solvents have atoms that have a large difference in electronegativity. Non-polar solvents contain atoms with a relatively small difference in electronegativity.

Covalent Lattices

Simple covalent lattices:

Simple covalent lattices have low melting and boiling points because they have weak intermolecular forces between the molecules. Therefore, only a small amount of energy is required to break the lattice.

They do not conduct electricity in any of the states – solid, liquid, or gas as there are no ions or delocalised electrons to move around the structure and carry a charge.

Simple covalent lattices are more soluble in non-polar solvents and are insoluble in water.

Giant covalent lattices:

Giant covalent lattices have high melting and boiling points as a large amount of energy is required to break the strong bonds between the molecules.

Most of these compounds cannot conduct electricity because there are no free electrons available to carry a charge. However, graphite can conduct electricity because it has delocalised electrons.

These types of lattices are insoluble in water as they don’t contain any ions.

Metallic Lattices

Giant metallic lattices have moderately high melting and boiling points because of the strong metallic bonding.

These lattices can conduct electricity when solid or liquid as free electrons are available in both states and can drift around the structure carrying an electric charge.

They are insoluble in water due to the metallic bonds being very strong. However, they can be soluble in only liquid metals.

Lattice Structures - Key takeaways

  • A lattice is a three-dimensional arrangement of ions or atoms in a crystal.
  • Giant ionic lattices are referred to as “giant” as they are made up of large numbers of the same ions arranged in a repeated pattern.
  • Ions in a giant ionic lattice are all attracted to each other in opposite directions.
  • There are two types of covalent lattices, giant covalent lattices, and simple covalent lattices.
  • The electrostatic attraction holding giant structures together is stronger than the electrostatic attraction holding simple structures.
  • Metals form giant metallic lattice structures which consist of atoms that are closely packed together in a regular shape.

Lattice Structures

 A lattice is a three-dimensional arrangement of ions or atoms in a crystal.

Lattice structures can be used for additive manufacturing.

- Giant ionic lattices

- Covalent lattices

- Metallic lattices

An example is sodium chloride, NaCl. The ions in this structure are packed in a cubic shape. 

1. Draw a square

2. Draw an identical square offset from the first one.

3. Next, join the squares together to make a cube.

4. Then, divide the cubes into 8 smaller cubes.

5. Draw three lines through the centre of the cube,  from the centre of each face to the centre of the opposite face.

6. Add the ions, but remember the negative ions (Cl-) will be larger in size than the positive ions.

Final Lattice Structures Quiz

Question

What is a lattice? 

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Answer

A lattice is a three-dimensional arrangement of ions or atoms in a crystal.

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Question

What is the definition of covalent bonding?

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Answer

Covalent bonding is the strong electrostatic attraction between two positive nuclei and the shared pair of electrons between them.

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Question

What is the difference between giant covalent structures and simple covalent structures? 


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Answer

The difference is that the electrostatic attraction holding giant structures together is stronger than the electrostatic attraction holding simple structures.

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Question

What is the definition of metallic bonding?

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Answer

Metallic bonding is the strong electrostatic attraction between the delocalised electrons and the positive metal ions.

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Question

Do ionic lattices conduct electricity?

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Answer

They conduct electricity but only when they are dissolved or molten. When ionic lattices are in a solid state, their ions are fixed in position and so they cannot move. As a result of this, electricity is not conducted.

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Question

Why do simple covalent lattices have low melting and boiling points?

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Answer

They have weak intermolecular forces between the molecules. Therefore, only a small amount of energy is required to break the lattice.  

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Question

Why do giant covalent lattices have high melting and boiling points?

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Answer

A large amount of energy is required to break the strong covalent bonds between the molecules.

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Question

What is the arrangement of ions in a giant ionic lattice?

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Answer

The ions are packed together in a cubic shape with the negative ions being larger in size than the positive ions. 

 

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Question

Give three examples of giant molecular lattices?

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Answer

- Graphite

- Silicon (IV) oxide

- Diamond

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Question

Give three examples of simple molecular lattices?

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Answer

- Iodine 

- Buckminsterfullerene (C60)

- Ice

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Question

Are giant ionic lattices soluble?

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Answer

Giant ionic lattices are soluble in water and polar solvents, however, they are insoluble in non-polar solvents.

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Question

Are covalent lattices soluble?


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Answer

Simple covalent lattices and giant covalent lattices are both insoluble in water. 

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Question


Are metallic lattices soluble?

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Answer

Metallic lattices are insoluble in water due to the metallic bonds being very strong.

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Question

Do metallic lattices conduct electricity?

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Answer

Metallic lattices can conduct electricity when solid or liquid as free electrons are available in both states and can drift around the structure carrying an electric charge. 

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Question

Can covalent lattices conduct electricity?


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Answer

Covalent lattices cannot conduct electricity as there are no delocalised electrons to move around the structure and carry a charge.

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