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Updated Mar 15, 2026

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3 pages

Cool Chemistry: How Atoms Stick Together

poppy

@poppy_wsht

Covalent, ionic, and metallic bonding are fundamental concepts in chemistry... Show more

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# Bonding

Atoms can be held together with bonds. When
bonds are formed, atoms can reach stable
electron arrangements. To reach a stable
ele

Ionic Bonding and Metallic Bonding

Definition: An ionic bond is the electrostatic force of attraction between a positively charged metal ion and a negatively charged non-metal ion.

Ionic compounds lattice structure is characterized by its ability to dissolve easily in water. When dissolved, the lattice breaks apart, and water molecules surround the separated ions.

Metallic bonding, on the other hand, occurs in pure metals and alloys. In metallic structures, the outer shell electrons of metal atoms are free to move throughout the structure.

Definition: A metallic bond is the force of attraction between free-moving (or delocalized) electrons and positive metal ions in a metal structure.

Properties of metallic bonds include:

Strong bonds leading to stable structures
High melting and boiling points
Excellent conductivity of electricity and heat due to the movement of delocalized electrons

Highlight: The delocalized electrons in metallic bonds allow metals to conduct electricity and heat efficiently, a property not shared by ionic or covalent network structures.

Comparison of Bonding Types and Their Properties

Covalent Network:
- High melting points
- Does not conduct electricity
- Very hard and difficult to break
Ionic Lattice:
- High melting points
- Conducts electricity when liquid or dissolved
- Brittle and can shatter
Metallic Lattice:
- Wide range of melting points (depending on the metal)
- Conducts electricity in solid state
- Malleable and ductile

Vocabulary: Malleable refers to the ability of a material to be hammered or pressed into shape without breaking, while ductile means the material can be drawn into a wire without breaking.

These different bonding types and structures explain why materials like diamond (covalent network), table salt (ionic lattice), and copper (metallic lattice) have such diverse properties and applications in the real world.

Covalent Bonding and Atomic Stability

Definition: A covalent bond is a bond between two non-metal elements where electrons are shared between atoms to reach a stable electron arrangement.

Covalent substances typically exist as gases or liquids at room temperature due to weak intermolecular forces. However, some covalent substances form solid structures with high melting points when they create larger molecules or covalent networks.

Example: Boron, carbon, and silicon are examples of elements that form covalent network structures, consisting of giant 3D lattices of covalently bonded atoms.

Highlight: Covalent network structures have high melting points and are solid at room temperature due to the extensive network of strong covalent bonds.

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Chemistry

•

Updated Mar 15, 2026

•

3 pages

Cool Chemistry: How Atoms Stick Together

poppy

@poppy_wsht

Covalent, ionic, and metallic bonding are fundamental concepts in chemistry that explain how atoms interact to form various substances. These different types of bonds result in distinct properties and structures of materials. Covalent bonding in non-metal elements, ionic compounds... Show more

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Ionic Bonding and Metallic Bonding

Ionic bonding occurs between metal and non-metal elements, forming compounds like sodium chloride. These compounds create a lattice structure of alternating metal and non-metal ions held together by electrostatic forces.

Definition: An ionic bond is the electrostatic force of attraction between a positively charged metal ion and a negatively charged non-metal ion.

Ionic compounds lattice structure is characterized by its ability to dissolve easily in water. When dissolved, the lattice breaks apart, and water molecules surround the separated ions.

Metallic bonding, on the other hand, occurs in pure metals and alloys. In metallic structures, the outer shell electrons of metal atoms are free to move throughout the structure.

Definition: A metallic bond is the force of attraction between free-moving (or delocalized) electrons and positive metal ions in a metal structure.

Properties of metallic bonds include:

Strong bonds leading to stable structures

High melting and boiling points

Excellent conductivity of electricity and heat due to the movement of delocalized electrons

Highlight: The delocalized electrons in metallic bonds allow metals to conduct electricity and heat efficiently, a property not shared by ionic or covalent network structures.

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Comparison of Bonding Types and Their Properties

Understanding the different types of chemical bonding is crucial for predicting and explaining the properties of various materials. Here's a comparison of covalent network, ionic lattice, and metallic lattice structures:

Covalent Network:

High melting points

Does not conduct electricity

Very hard and difficult to break

Ionic Lattice:

High melting points

Conducts electricity when liquid or dissolved

Brittle and can shatter

Metallic Lattice:

Wide range of melting points (depending on the metal)

Conducts electricity in solid state

Malleable and ductile

Vocabulary: Malleable refers to the ability of a material to be hammered or pressed into shape without breaking, while ductile means the material can be drawn into a wire without breaking.

These different bonding types and structures explain why materials like diamond (covalent network), table salt (ionic lattice), and copper (metallic lattice) have such diverse properties and applications in the real world.

Sign up to see the contentIt's free!

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Improve your grades

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Covalent Bonding and Atomic Stability

Atoms form bonds to achieve stable electron arrangements. Covalent bonding occurs between non-metal elements when atoms share electrons. This sharing creates a strong bond between the atoms, held together by the attraction between the positive nuclei and the shared electrons.

Definition: A covalent bond is a bond between two non-metal elements where electrons are shared between atoms to reach a stable electron arrangement.

Covalent substances typically exist as gases or liquids at room temperature due to weak intermolecular forces. However, some covalent substances form solid structures with high melting points when they create larger molecules or covalent networks.

Example: Boron, carbon, and silicon are examples of elements that form covalent network structures, consisting of giant 3D lattices of covalently bonded atoms.

Highlight: Covalent network structures have high melting points and are solid at room temperature due to the extensive network of strong covalent bonds.