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Covalent vs Metallic Bonds: How They Work in Molecules

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Avie

19/05/2023

Chemistry

Covalent and Metallic Bonding

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Covalent vs Metallic Bonds: How They Work in Molecules

Covalent and metallic bonding explores fundamental chemical bonds, explaining how atoms connect in different materials and their resulting properties.

  • Covalent bonding in molecules occurs when non-metal atoms share electron pairs
  • Properties of metallic bonding include electrical conductivity and high melting points
  • The difference between covalent and metallic bonds lies in their electron arrangement and resulting material characteristics
  • Both types of bonds are crucial in determining material properties and behavior
  • Understanding these bonds helps explain everyday material properties and applications
...

19/05/2023

31

COVALENT A covalent bond forms when two non-metal atoms share a pair of electrons. Covalent bonds are strong-a lot of energy is needed to br

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Metallic Bonding and Properties

Metallic bonding creates unique material properties that make metals essential in everyday applications. This type of bonding differs significantly from covalent bonds in structure and characteristics.

Definition: Metallic bonding involves the attraction between positive metal ions arranged in a regular lattice and a sea of delocalized electrons.

Highlight: Key properties of metals include:

  • Excellent electrical conductivity due to mobile electrons
  • High melting points resulting from strong metallic bonds
  • Malleability allowing shape changes without breaking
  • Ductility enabling formation into wires

Example: The ability of metals to conduct electricity comes from their delocalized electrons, which can freely move throughout the material.

Vocabulary: Malleable means capable of being hammered into shape, while ductile refers to the ability to be drawn into wires.

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Condensed notes on the Chemistry unit Bonding & Structure. Topics include: Metallic, Ionic & Covalent Bonding, Melting and Boiling Point, Malluablity, Solubility and Contuctivity. I hope these help!

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Subjects

Chemistry

Periodic table

Metals & non-metals

 

Chemistry

•

31

•

19 May 2023

•

2 pages

Covalent vs Metallic Bonds: How They Work in Molecules

user profile picture

Avie

@aviee

Covalent and metallic bonding explores fundamental chemical bonds, explaining how atoms connect in different materials and their resulting properties.

  • Covalent bonding in molecules occurs when non-metal atoms share electron pairs
  • Properties of metallic bondinginclude electrical conductivity and high melting... Show more
COVALENT A covalent bond forms when two non-metal atoms share a pair of electrons. Covalent bonds are strong-a lot of energy is needed to br

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Metallic Bonding and Properties

Metallic bonding creates unique material properties that make metals essential in everyday applications. This type of bonding differs significantly from covalent bonds in structure and characteristics.

Definition: Metallic bonding involves the attraction between positive metal ions arranged in a regular lattice and a sea of delocalized electrons.

Highlight: Key properties of metals include:

  • Excellent electrical conductivity due to mobile electrons
  • High melting points resulting from strong metallic bonds
  • Malleability allowing shape changes without breaking
  • Ductility enabling formation into wires

Example: The ability of metals to conduct electricity comes from their delocalized electrons, which can freely move throughout the material.

Vocabulary: Malleable means capable of being hammered into shape, while ductile refers to the ability to be drawn into wires.

COVALENT A covalent bond forms when two non-metal atoms share a pair of electrons. Covalent bonds are strong-a lot of energy is needed to br

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Understanding Covalent Bonds

Covalent bonding forms the foundation of molecular structures in non-metallic compounds. These bonds create stable molecules through electron sharing between atoms.

Definition: A covalent bond is formed when two non-metal atoms share a pair of electrons, creating a strong connection that requires significant energy to break.

Example: Common molecules featuring covalent bonds include HCl (hydrogen chloride), NH₃ (ammonia), CO₂ (carbon dioxide), and H₂O (water).

Vocabulary: A lone pair refers to electrons that aren't involved in bonding but remain associated with a specific atom.

Highlight: Structural formulae, such as CH₄ (methane) and H₂O (water), show how atoms are arranged and bonded within molecules.

Definition: A molecule consists of two or more atoms joined by covalent bonds, while diatomic molecules specifically contain two covalently bonded atoms.

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