Flashcard: Chemical Bonding Fundamentals — 24 carte

Chemical Bond — definition?

Force that holds atoms together in molecules.

Bond Formation — reason?

Atoms bond to achieve stable electron configurations.

Types of Bonds — examples?

Ionic, covalent, metallic, hydrogen bonds.

Ionic Bond — formation?

Transfer of electrons between metal and non-metal.

Covalent Bond — sharing?

Atoms share electron pairs to stabilize.

Metallic Bond — electrons?

Delocalized electrons shared among metal atoms.

Hydrogen Bond — attraction?

Weak attraction between H and F, O, N.

Lewis Theory — basis?

Electron dot structures for bonding visualization.

Octet Rule — goal?

Atoms seek 8 electrons in outer shell.

Bond Length — definition?

Distance between nuclei of bonded atoms.

VSEPR — purpose?

Predict molecular shapes based on electron pairs.

Resonance Structures — role?

Depict delocalized electrons in molecules.

Ionic Bond — ions involved?

Cations and anions attracted electrostatically.

Covalent Bond — polarity?

Depends on electronegativity difference.

Metallic Bond — properties?

Conductivity, malleability, ductility.

Hydrogen Bond — significance?

Influences water properties and biological structures.

Lewis Structures — depict?

Valence electrons and bonding patterns.

Octet Rule — exceptions?

Molecules like NO, BCl₃ violate it.

Bond Energy — indicates?

Strength of a bond; higher means stronger.

Molecular Shape — determined by?

Electron pair repulsion (VSEPR).

Resonance — effect?

Stabilizes molecules via electron delocalization.

Bond Type — transfer or sharing?

Ionic: transfer; Covalent: sharing.

Bond Characteristics — include?

Length, energy, order.

Molecular Shapes — VSEPR?

Linear, trigonal planar, tetrahedral, etc.