Untitled Flashcards Set

Coordinate (Dative) Covalent Bond: A type of covalent bond where one atom donates both electrons to the bond (e.g., NH₄⁺, CO).

Polar Bond: A covalent bond where electrons are unequally shared due to a difference in electronegativity, resulting in partial charges (e.g., HCl).

Nonpolar Bond: A covalent bond where electrons are equally shared, occurring in diatomic molecules or between atoms with similar electronegativities (e.g., O₂, CH₄).

Covalent Bond: A chemical bond formed by the sharing of electron pairs between atoms (e.g., H₂O, CO₂).

Ionic Bond: A bond formed by the electrostatic attraction between positively and negatively charged ions due to electron transfer (e.g., NaCl).

Polar Molecule: A molecule with an uneven distribution of charge due to polar bonds and an asymmetric shape (e.g., H₂O).

Nonpolar Molecule: A molecule with a symmetric charge distribution, even if it contains polar bonds (e.g., CO₂, CH₄).

Delocalized Electrons: Electrons that are spread over multiple atoms in a molecule or metal, common in resonance structures and metallic bonds (e.g., benzene, metals).

Resonance Structure: Different valid Lewis structures of a molecule where electrons are delocalized, often indicated by a double-headed arrow (↔) (e.g., O₃, NO₃⁻).

Diamagnetic: A substance with all paired electrons that is weakly repelled by a magnetic field (e.g., N₂).

Lone Pair: A pair of valence electrons not involved in bonding (e.g., two lone pairs on oxygen in H₂O).

Sigma (σ) Bond: A single covalent bond formed by direct head-on orbital overlap, present in all single, double, and triple bonds.

Dipole: A molecule or bond with a partial positive and partial negative charge due to uneven electron distribution (e.g., HF, H₂O).

Metallic Bond: A bond formed by a "sea" of delocalized electrons around metal cations, leading to properties like conductivity and malleability (e.g., Cu, Fe).

Triple Bond: A bond involving one sigma and two pi bonds, as seen in N₂ and C₂H₂ (ethyne).

VSEPR Theory: Valence Shell Electron Pair Repulsion theory predicts molecular shapes based on minimizing electron pair repulsions (e.g., CH₄ is tetrahedral).

Double Bond: A covalent bond consisting of one sigma and one pi bond, found in CO₂ and C₂H₄ (ethylene).

Paramagnetic: A substance with unpaired electrons that is attracted to a magnetic field (e.g., O₂).

Hybrid Orbital: A new orbital formed by the combination of atomic orbitals (e.g., sp³ in CH₄, sp² in C₂H₄).

Pi (π) Bond: A bond formed by sideways overlap of p orbitals, found in double and triple bonds