Pre-IB Chemistry | Chapter 6: Chemical Bonding

Chemical Bond

a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together

Ionic Bonding

chemical bonding that results from the electrical attraction between cations and anions

Covalent Bonding

results from the sharing of electron pairs between two atoms

Nonpolar-Covalent Bond

a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge.

Polar

to have an uneven distribution of charge

Polar-Covalent Bond

A covalent bond in which the bonded atoms have an unequal attraction for the shared electrons

Molecule

a neutral group of atoms that are held together by covalent bonds

Molecular Compound

A chemical compound whose simplest units are molecules

Chemical Formula

indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts

Molecular Formula

The types and numbers of atoms combined in a single molecule of a molecular compound

Bond energy

the energy required to break a chemical bond and form neutral isolated atoms

What is the octet rule?

Chemical compounds form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level

Electron-Dot Notation

an electron configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element’s symbol

Lewis Structures

Formulas in which atomic symbols represent nuclei and inner-shell electrons, dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only on atomic symbol represent unshared electrons

Structural Formula

The kind, number, arrangement, and bonds but not the unshared pairs of the atoms in a molecule

Single Bond

A covalent bond in which one pair of electrons is shared between two atoms

Double Bond

A covalent bond in which two pairs of electrons are shared between two atoms

Triple Bond

A covalent bond in which three pairs of electrons are shared between two atoms

Properties of Double Bonds

Greater bond energies and shorter than single bonds

Properties of Triple Bonds

Stronger bond energies and shorter than double bonds

Resonance

bonding in molecules or ions that cannot be correctly represented by a single Lewis structure

Ionic Compound

composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal

Formula Unit

Simplest collection of atoms from which an ionic compound’s formula can be established

Lattice energy

The energy released when one mole of an ionic crystalline compound is formed from gaseous ions

Polyatomic Ions

A charged group of covalently bonded atoms

Metallic Bonding

The chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons

Malleability

the ability of a substance to be hammered or beaten into thin sheets

Ductility

the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire

VSEPR theory

the repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible

Hybridization

The mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energies

Hybrid orbitals

Orbitals of equal energy produced by the combination of two or more orbitals on the same atom

Intermolecular forces

forces of attraction between molecules

Dipole

created by equal but opposite charges that are separated by a short distance

Hydrogen Bonding

The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule

London dispersion forces

The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles

As atoms bond with each other, they ______.

decrease their potential energy thus creating more stable arrangements

Metallic Bonding

the overlapping of orbitals that allow outer electrons of atoms to move about freely throughout the entire lattice