Chemical bonding is crucial for atoms to form molecules and compounds, seeking stability by achieving a full valence shell. The text delves into covalent, ionic, and metallic bonds, each with unique properties and roles in molecular and crystal structures. Covalent bonds involve shared electron pairs, ionic bonds result from electron transfer forming charged ions, and metallic bonds are due to delocalized electrons. Factors like electron configuration, bond order, and ionic radii affect bond strength, distinguishing them from weaker intermolecular forces.
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Covalent bonds involve the sharing of electron pairs between atoms to fulfill the octet rule
Ionic bonds form when electrons are transferred between a metal and nonmetal, creating ions held together by electrostatic forces
Metallic bonds feature a collective sharing of electrons among metal atoms, resulting in properties such as conductivity and malleability
Covalent bond strength is influenced by bond order, atom size, and electronegativity difference
Ionic bond strength is affected by ionic charges and radii
Metallic bond strength is determined by the number of delocalized electrons and properties of metal ions
Chemical bonds are strong interactions that hold atoms together within molecules or crystal lattices
Intermolecular forces are weaker attractions between molecules
Hydrogen bonds are the strongest type of intermolecular force, but still weaker than chemical bonds
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Definition of Chemical Bonding
Process where atoms combine to form molecules/compounds via attraction.
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Octet Rule Guiding Principle
Atoms fill valence shell with 8 electrons to resemble noble gases for stability.
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Types of Chemical Bonds
Covalent: sharing electrons. Ionic: transferring electrons. Metallic: pooling electrons.
