Chemistry: Bonding Concepts

Electrostatic attraction between oppositely charged ions formed by electron transfer.

Visual representation of ionic bonding that shows electron transfer and electron arrangement in ions.

Electrostatic attraction between a shared pair of electrons and the bonded atoms' nuclei.

A pair of valence electrons that is not involved in bonding and is localized on an atom.

A shared pair of electrons with both electrons originating from one atom.

Difference in electronegativity between bonded atoms causing a partial charge difference.

Attraction between positive ions and delocalized electrons in a lattice.

Measure of an atom's ability to attract shared electrons in a chemical bond.

Atoms tend to gain, lose, or share electrons to achieve a stable configuration with eight electrons in their outer shell

Electronegativity increases across a period and decreases down a group

The octet rule does not always apply, particularly for elements like Be and B, which have fewer than eight electrons in their outermost shell.

A covalent bond formed by the sharing of two pairs of electrons between two atoms

A covalent bond where electrons are unequally shared due to differences in electronegativity between the atoms.

Moving across a period, the effective nuclear charge increases, resulting in a stronger attraction between the nucleus and the bonding electrons.

Moving down a group, the distance between the nucleus and the bonding electrons increases, reducing the attraction.

A partial positive charge that develops on the atom with lower electronegativity in a polar covalent bond.

A partial negative charge that develops on the atom with higher electronegativity in a polar covalent bond.

The bond between oxygen and hydrogen in water (H2O) is polar because oxygen is more electronegative than hydrogen.

Ionic and covalent bonding are not distinct types, but rather exist on a spectrum from complete electron transfer (ionic) to equal sharing (covalent).