Exploring chemical bonding, this overview delves into covalent, ionic, and metallic bonds that form the basis of molecular and compound structures. Covalent bonds involve electron sharing between non-metals, while ionic bonds result from electron transfer between metals and non-metals, forming crystalline lattices. Metallic bonds feature a sea of delocalized electrons around metal ions, granting unique properties like malleability and conductivity. The text also examines how these bonds influence physical properties like melting points, electrical conductivity, and solubility, providing insights into the behavior of different materials.
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Covalent bonds form when non-metal atoms share electrons, resulting in molecules with unique properties
Ionic bonds occur through the transfer of electrons between metals and non-metals, resulting in crystalline structures with high melting and boiling points
Metallic bonds involve a lattice of positive metal ions surrounded by delocalized electrons, giving metals their characteristic properties
Network covalent solids have extremely high melting and boiling points due to their three-dimensional array of covalently bonded atoms
Simple molecular substances have lower melting and boiling points and are typically liquids or gases at room temperature due to weaker van der Waals forces between discrete molecules
Covalent substances generally do not conduct electricity, with network solids being exceptionally hard and durable, while simple molecular substances are typically softer and more flexible
Ionic compounds have crystalline structures with strong ionic attractions and high melting and boiling points
Ionic solids are typically hard and brittle, and can shatter when subjected to stress that aligns like-charged ions
In their solid state, ionic compounds do not conduct electricity, but when dissolved in water or melted, they can conduct electricity due to the mobility of ions, with solubility varying among different compounds
Metallic bonds allow for the movement of metal ions without breaking, resulting in the malleability and ductility of metals
Metals have moderate to high melting and boiling points and are excellent conductors of heat and electricity, but are generally insoluble in water
The delocalized electrons in metallic bonds reflect light, giving metals their characteristic shiny surface
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Covalent bond electron sharing
Covalent bonds involve sharing of electron pairs between non-metal atoms, forming molecules with single, double, or triple bonds.
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Ionic bond formation process
Ionic bonds form through electron transfer from a metal to a non-metal, creating a crystalline lattice of ions with strong electrostatic attractions.
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Metallic bond properties
Metallic bonds consist of positive metal ions in a lattice with a sea of delocalized electrons, granting metals conductivity and malleability.
