Exam 2 Terms - Atoms, Electronic Structure, Bonding

Electrons contribute what to a solid?

bonding, electronic properties, optical properties, magnetic properties

Valence Shells

the outermost shell; determines much of the bonding

Orbital Filling

order in which bonding occurs

Orbital Bonding

order in which orbitals are filled

What are the d-shells and f-shells good for?

magnetic behavior (permanent magnets), fluorescene, and phosphorescence

Fluorescence

immediate effect

Phosphorescence

last longer

Electronegativity

ability to pull in an electron

Ionic Bonds

electron(s) are transferred between atoms, forming ions; bonding results in a cation attracting an anion (Coulombic Attraction)

What formula(s) is this?

Force of Coulombic Attraction

What formula is this?

Repulsive Force

Pauli Exclusion

each electron in an atom must have a unique combination of quantum numbers; an orbital can contain a max of two electrons only and they must have opposite spins.

Sum of Force

the net force of the attractive and repulsive forces; equilibrium bond length is where the forces equal each other and the bond is stable

Bonding Energy (U)

how much energy the ionic bond has at a particular separation distance; U = potential energy

Why is the potential energy negative/ decreasing

as the distance between ions decrease, they release potential energy

Bond Enegy

minimum bond energy, the point of equilibrium

Generalized Bonding Energies

describes how energy decreased when two ions bond

What does the red line represent?

Bond Energy

What does the red line represent?

Equilibrium Bond Length

Ionic Directionality

ionic bonds are non-directional; bond energy is independent of orientation

Ionic Fracture

atoms with repulsive forces align, leading to fracture; plastically deforming an ionic solid;