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Chemical bonds are fundamental forces that hold atoms together, forming the world's substances. There are three main types: ionic, covalent, and metallic. Ionic bonds involve electron transfer, creating charged ions that form strong, crystalline structures. Covalent bonds, including polar variations, arise from electron sharing, crucial for molecule stability and function. Metallic bonds, with delocalized electrons, give metals conductivity and malleability.
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Ionic bonds occur when electrons are transferred between atoms, resulting in the formation of positively and negatively charged ions
Covalent bonds involve the sharing of electron pairs between atoms, creating a stable balance of attractive and repulsive forces
Metallic bonds are characterized by a 'sea' of delocalized electrons surrounding a lattice of positive ions, allowing for efficient conduction of electricity and heat
Covalent bonds are formed when two atoms share one or more pairs of valence electrons, achieving a full outer electron shell and chemical stability
Single Covalent Bonds
Single covalent bonds involve the sharing of one pair of electrons between atoms
Double Covalent Bonds
Double covalent bonds involve the sharing of two pairs of electrons between atoms
Triple Covalent Bonds
Triple covalent bonds involve the sharing of three pairs of electrons between atoms
Covalent bonds have a definite orientation and shape due to the localization of shared electron pairs between bonded atoms
Polar covalent bonds occur when the sharing of electrons between atoms is unequal due to differences in electronegativity
The separation of charge in polar covalent bonds creates a dipole moment in the molecule
Polar covalent bonds play a significant role in determining physical properties such as solubility and the ability to form hydrogen bonds
Metallic bonds consist of a lattice of positively charged metal ions surrounded by a 'sea' of delocalized electrons
Conductivity
The delocalized electrons in metallic bonds allow for efficient conduction of electricity and heat in metals
Malleability and Ductility
The non-directional nature of metallic bonds allows for metals to be easily shaped and drawn into wires
Luster
The ability of delocalized electrons to absorb and re-emit light contributes to the luster of metals
00
Atoms are held together by ______ forces known as chemical bonds, which create ______ and compounds.
attractive
molecules
01
The outermost electrons, called ______ electrons, are responsible for the interactions leading to chemical bonds.
valence
02
The characteristics of substances, like ______ point and ______ conductivity, are influenced by the type of chemical bond.
melting
electrical
