AP®︎ Chemistry: Topic 2.1 Flashcards

An atom's ability to attract shared electrons in a chemical bond.

Increases across a period and decreases down a group because of charge and distance effects.

Attraction increases with larger charges and shorter distances between oppositely charged particles.

Outermost electrons that participate in bonding and determine many chemical properties.

Electrons are shared nearly equally between atoms with similar electronegativities.

Electrons are shared unequally between atoms with different electronegativities.

Delta positive and delta negative charges caused by unequal electron distribution in a bond.

A separation of charge in a bond caused by unequal electron sharing.

Polar bonds have some ionic character, so bonding ranges continuously from covalent to ionic.

Electrostatic attraction between cations and anions, usually formed after electron transfer.

Cations are positively charged ions; anions are negatively charged ions.

A repeating three-dimensional arrangement of ions in an ionic solid.

Usually brittle, high-melting solids that conduct electricity when molten or dissolved.

Conductive, malleable, ductile, and lustrous because mobile electrons move through the solid.

Metal plus nonmetal is usually ionic; two nonmetals are usually covalent; metals are metallic.

About 0 to 0.4 is nonpolar covalent, 0.4 to 1.7 polar covalent, above 1.7 often ionic.

Observed properties classify bonding more reliably than electronegativity difference alone.

A bond treated as effectively nonpolar because the electronegativity difference is very small.

Attraction between metal cations and mobile valence electrons spread throughout the solid.