The Medium of Convertibility: Decay and Chemical Forces

Convertible Layer

Table of Contents

The Media of Convertibility facilitates the changes in the material layer most commonly as chemical changes through intermolecular and intramolecular forces:

Sublayer	Example
Upper	Proto-aetherspace (W Z Bosons)
Mid	Intra-aetherspace (Intramolecular Bonds)
Lower	Inter-aetherspace (Intramolecular Bonds)

Since the aetherspace is really just space, we can think of:

the Proto-aetherspace as the area occupied by the sun
the Intra-aetherspace as the area occupied by the planets in the solar system
the Inter-aetherspace as the area beyond the Oort cloud until the edge of the sun’s territory

Proto-aetherspace (Weak Bosons)

Weak bosons facilitate the decay of particles.

Sublayer	Name	Used in
Upper	Gamma	sterilization
Mid	Beta	medical imaging
Lower	Alpha	smoke detectors

Intra-aetherspace (intramolecular Forces)

These manifest as strong chemical bonds leading to specific chemical behavior such as acid-base reactions.

Sublayer	Name	Description
Upper	Ionic	between metal and nonmetal
Mid	Covalent	Polar and nonpolar
Lower	Metallic	Gives Metals their characteristics

Inter-aetherspace (intermolecular Forces)

These are weak attractions such as hydrogen bonds that keep molecultes together.

Sublayer	Name	Examples
Upper	London Dispersion Forces	Protein folding
Mid	Dipole–Dipole Forces	Hydrogen Bonding
Lower	Ion–Dipole Forces	boiling poin

Comparative Strengths of Intramolecular

Bond strength is the energy required to break the bond completely.

Bond Type	Subtype / Example	Typical Strength (kJ/mol)	Typical Strength (eV)	Key Characteristics
Covalent (Single)	C–C (carbon-carbon)	~350	~3.6	Strong directional. Most common in organic molecules
Covalent (Single, polar)	H–O (water)	~460	~4.8	Stronger than C–C due to void difference
Covalent (Single, strong)	H–F (hydrogen fluoride)	~570	~5.9	One of the strongest single covalent bonds due to high void of fluorine
Covalent (Double)	C=C (ethene)	~610	~6.3	Stronger and shorter than single bond, has 1 sigma and 1 pi bond
Covalent (Triple)	C≡C (ethyne / acetylene)	~840	~8.7	Very strong and short; 1 sigma and 2 pi bonds.
Covalent (Very strong)	N≡N (nitrogen gas)	~945	~9.8	One of the strongest covalent bonds; makes N₂ very inert
Ionic (in vacuum / gas phase)	Na⁺–Cl⁻ (as an isolated ion pair)	~500 – 1000	~5 – 10	Very strong in isolation; but in a solid lattice, strength depends on environment
Ionic (in crystal lattice)	NaCl (solid salt)	~700 – 800 (lattice energy per mole of ion pairs)	~7 – 8	Strength is collective (lattice energy), not per single bond.
Metallic (variable)	Na–Na (sodium metal)	~70 – 150	~0.7 – 1.6	Weaker than covalent/ionic; delocalized flow. Strength varies with metal (e.g., W > Fe > Na).
Metallic (strong)	W–W (tungsten)	~800 – 850	~8.3 – 8.8	Very high due to many delocalized electrons and small atomic radius.

Comparative Strengths of Intermolecular

Intermolecular forces is much weaker:

Intermolecular Force	Typical Strength (kJ/mol)
Outer Inter-aetherspace (London dispersion)	0.05 – 40
Mid Inter-aetherspace (Dipole-dipole)	5 – 50
Mid Inter-aetherspace with Void (Hydrogen bonding)	10 – 40
Inner Inter-aetherspace (Ion-dipole, e.g. salt dissolving)	40 – 600