Flashcard library · General Chemistry
Chemistry: Chemical Bonding
Master the fundamentals of chemical bonding with this essential flashcard deck! Covering key concepts from ionic and covalent bonds to molecular geometry and intermolecular forces, these cards will solidify your understanding of how atoms interact to form compounds. Perfect for reviewing core principles and preparing for exams.
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What is an ionic bond?
Electrostatic attraction between oppositely charged ions formed by electron transfer, typically metal to nonmetal.
What is a covalent bond?
Two atoms sharing one or more pairs of electrons, typically between nonmetals.
How does electronegativity difference classify a bond?
Roughly: under about 0.4 nonpolar covalent, up to about 1.7–2.0 polar covalent, larger ionic (cutoffs vary by textbook).
What is the octet rule?
Atoms tend to gain, lose or share electrons to reach eight valence electrons.
What does a Lewis structure show?
How valence electrons are arranged as bonds and lone pairs in a molecule.
What determines molecular shape in VSEPR theory?
Electron domains around the central atom spread as far apart as possible to minimize repulsion.
What geometry do three bonding domains and no lone pairs give?
Trigonal planar, with 120° bond angles, as in BF₃.
What geometry do four bonding domains and no lone pairs give?
Tetrahedral, with about 109.5° bond angles, as in CH₄.
What is hybridization?
Mixing atomic orbitals into new hybrid orbitals that match the observed bonding geometry.
How does a sigma bond differ from a pi bond?
A sigma bond is head-on overlap along the bond axis; a pi bond is side-by-side overlap of p orbitals.
How do intermolecular forces differ from covalent bonds?
They act between molecules and are much weaker than the bonds within molecules.
When does hydrogen bonding occur?
When H is bonded to N, O or F and is attracted to a lone pair on another N, O or F, as in water.
What properties do ionic compounds usually have?
High melting points, brittleness, and conductivity when molten or dissolved.
What properties do simple molecular compounds usually have?
Low melting and boiling points and poor electrical conductivity.
What is a metallic bond?
Attraction between metal cations and a sea of delocalized electrons, giving conductivity and malleability.