Hey Matt, a little help?

[aneaglesangel]

I've got a couple of haunts that seem to have some of the same properties. I set Gabby on the chemical possibilities here and what she gave me as information makes me think these substances can act as a "battery" for paranormal activity. I'm wondering, do you have the capabilities to test some soil and water for me? If so, how do I go about getting the soil and water samples for you? Do I need a specific amount of water and soil to be able to test it? Let me know, for the similarities in these two cases and the fact that the contaminations seem very similar to me. Thanks so much for your help! Hugs!

[aneaglesangel]

This is information sent to me by Gabby, the team Analyst. By what I'm reading here, I think these substances have a high potential for creating energy that spirits can use. And so, fuel a haunting in my eyes. I'd love for you, Matt to go over this. I sort of think I have an understanding of these substances, but any input would be greatly appreciated! Yes, my poor little mind never stops, LOL!

The following information is on PCB's, Mercury and Cadmium. These substances have been found to be in existence at two locations of some incredibly active haunts I've investigated recently. I'm putting our Researcher/Case Manager on the rest of the haunts that I've found to be active. I'll let you know if I find more correlations between haunts and contaminants as time goes by!

A dielectric is an electrical insulator that may be polarized by an applied electric field. When a dielectric is placed in an electric field, electric charges do not flow through the material, as in a conductor, but only slightly shift from their average equilibrium positions causing dielectric polarization. Because of dielectric polarization, positive charges are displaced toward the field and negative charges shift in the opposite direction. This creates an internal electric field that partly compensates the external field inside the dielectric.[1] If a dielectric is composed of weakly bonded molecules, those molecules not only become polarized, but also reorient so that their symmetry axis aligns to the field.[2]
Although the term "insulator" refers to a low degree of electrical conduction, the term "dielectric" is typically used to describe materials with a high polarizability. The latter is expressed by a number called the dielectric constant. A common, yet notable example of a dielectric is the electrically insulating material between the metallic plates of a capacitor. The polarization of the dielectric by the applied electric field increases the capacitor's capacitance.[2]
The study of dielectric properties is concerned with the storage and dissipation of electric and magnetic energy in materials.[3] It is important to explain various phenomena in electronics, optics, and solid-state physics.

So to some degree it is possible that PCBs could energize.

Main article: Isotopes of cadmium
Naturally occurring cadmium is composed of 8 isotopes. For two of them, natural radioactivity was observed, and three others are predicted to be radioactive but their decay is not observed, due to extremely long half-life times. The two natural radioactive isotopes are 113Cd (beta decay, half-life is 7.7 × 1015 years) and 116Cd (two-neutrino double beta decay, half-life is 2.9 × 1019 years). The other three are 106Cd, 108Cd (double electron capture), and 114Cd (double beta decay); only lower limits on their half-life times have been set. At least three isotopes - 110Cd, 111Cd, and 112Cd - are stable. Among the isotopes absent in natural cadmium, the most long-lived are 109Cd with a half-life of 462.6 days, and 115Cd with a half-life of 53.46 hours. All of the remaining radioactive isotopes have half-lives that are less than 2.5 hours, and the majority of these have half-lives that are less than 5 minutes. This element also has 8 known meta states, with the most stable being 113mCd (t½ = 14.1 years), 115mCd (t½ = 44.6 days), and 117mCd (t½ = 3.36 hours).
The known isotopes of cadmium range in atomic mass from 94.950 u (95Cd) to 131.946 u (132Cd). For isotopes lighter than 112 u, the primary decay mode is electron capture and the dominant decay product is element 47 (silver). Heavier isotopes decay mostly through beta emission producing element 49 (indium).
One isotope of cadmium, 113Cd, absorbs neutrons with very high probability if they have an energy below the cadmium cut-off and transmits them readily otherwise. The cadmium cut-off is about 0.5 eV.[6] Neutrons with energy below the cutoff are deemed slow neutrons, distinguishing them from intermediate and fast neutrons.
Cadmium is created via the long S-process in low-medium mass stars (.6 -> 10 solar masses), lasting thousands of years to do. It requires a silver atom to capture a neutron and then undergo beta decay.[citation needed]



Mercury dissolves to form amalgams with gold, zinc and many other metals. Because iron is an exception, iron flasks have been traditionally used to trade mercury. Other metals that do not form amalgams with mercury include tantalum, tungsten and platinum. When heated, mercury also reacts with oxygen in air to form mercury oxide, which then can be decomposed by further heating to higher temperatures.[7]
Since it is below hydrogen in the reactivity series of metals, mercury does not react with most acids, such as dilute sulfuric acid, though oxidizing acids such as concentrated sulfuric acid and nitric acid or aqua regia dissolve it to give sulfate, nitrate, and chloride salts. Like silver, mercury reacts with atmospheric hydrogen sulfide. Mercury even reacts with solid sulfur flakes, which are used in mercury spill kits to absorb mercury vapors (spill kits also use activated carbon and powdered zinc).[7]
Some important mercury salts include:

* Mercury(I) chloride (calomel) is sometimes still used in medicine, acousto-optical filters and as a standard in electrochemistry;[8]
* Mercury(II) chloride is a very corrosive, easily sublimating and poisonous substance;[4]
* Mercury fulminate, (a detonator widely used in explosives);[4]
* Mercury(II) oxide, the main oxide of mercury;
* Mercury(II) sulfide (found naturally as the ore cinnabar, or vermilion which is a high-grade paint pigment);[4]
* Mercury(II) selenide, Mercury(II) telluride, Mercury cadmium telluride and mercury zinc telluride are semiconductors and infrared detector materials.[9]

In these compounds, mercury displays two oxidation states: +1 and +2. The +1 state oxidation involves the dimeric cation, Hg2+2. Solutions of Hg2+2 are in equilibrium with Hg2+ and metallic mercury:

Hg2+ + Hg is in equilibrium with Hg2+2

This equilibrium causes solutions of Hg2+2 to have a small amount of Hg2+ present. Consuming the Hg2+ by another reaction, such as complexation with strong ligands or precipitation of an insoluble salt, will cause all the Hg2+2 to fully disproportionate to Hg2+ and elemental mercury.[10]
Besides Hg2+2, mercury also forms other mercury polycations such as Hg2+3.[11]
Higher oxidation states of mercury were confirmed in September 2007, with the synthesis of mercury(IV) fluoride (HgF4) using matrix isolation techniques.[12]
Laboratory tests have found that an electrical discharge causes the noble gases to combine with mercury vapor. These compounds are held together with van der Waals forces and result in Hg·Ne, Hg·Ar, Hg·Kr, and Hg·Xe (see exciplex). Organic mercury compounds are also important. Methylmercury is a dangerous compound that is widely found as a pollutant in water bodies and streams.[13]