Lecture_8-Bonding__Lewis_Structures

Ionic Bond

Transfer of valence electrons between a metal and a nonmetal to achieve noble gas electron configuration.

Covalent Bond

Sharing of valence electrons between two nonmetals to achieve noble gas electron configuration.

Lewis Structures

Diagrams that show the arrangement of valence electrons in a compound.

Electronegativity

The tendency of an atom in a bond to attract bonding electrons to itself.

Bond Dipole

A polar covalent bond that has a partial negative charged end and a partial positive charged end.

Resonance

When more than one valid Lewis structure can be drawn for a molecule.

Coulomb’s Law

The law that describes the force of attraction between two charged ions.

Valence Electrons

Electrons in the outermost shell of an atom that can participate in forming bonds.

Octet Rule

Atoms tend to gain, lose, or share electrons to achieve a full outer shell of eight electrons.

Lattice Energy

The energy released when oppositely charged ions come together to form a solid ionic compound.

Stable Arrangement

An arrangement of electrons that minimizes energy and maximizes stability, often corresponding to noble gas configurations.

Partial Charge

A charge that occurs due to the uneven distribution of electrons in a polar molecule.

Energy Savings

The energy released during the formation of ionic bonds that contributes to the stability of the compound.

Lewis Structure Motto

Whenever possible, always follow the octet rule (duet rule for hydrogen).

Exceptions to the Octet Rule

Instances where atoms may not complete an octet, such as in BH3, NO2, PCl5, and XeF4.

Bond Length

The distance between the nuclei of two bonded atoms.

Electronegativity Trend

The general trend where electronegativity increases across a period and decreases down a group.

Polar Covalent Bond

A covalent bond where the electrons are shared unequally between the atoms.

Nonpolar Covalent Bond

A covalent bond where electrons are shared equally between identical atoms.

Hydrogen Bonding

A weak bond between a hydrogen atom covalently bonded to an electronegative atom and another electronegative atom.