Abc 2 Pure Crystals Research Substance

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  1. Aluminum Potassium Sulfate, 500g says:

    Lab grade chemical. Appears as white, odorless crystals having a stringent taste. Soluble in water, creating acidic solution. Non-combustible.

    Readily forms colorless cubic crystals. Click here to visit our Info & How-To Center about growing crystals.

  2. Cannabinoids says:

    Research chemicals are chemical substances used by scientists for medical and scientific research purposes. One characteristic of a research chemical is that it is for laboratory research use only. A research chemical is not intended for human or veterinary use. This distinction is required on the labels of research chemicals, and is what exempts them from regulation under parts 100-740 in Title 21 of the Code of Federal Regulations (21CFR).
    Research chemicals are fundamental in the development of novel pharmacotherapies. Common medical laboratory uses include in vivo and animal testing to determine therapeutic value, toxicology testing by contract research organizations to determine drug safety, and analysis by drug test and forensic toxicology labs for the purposes of evaluating human exposure.
    Research agrochemicals are created and evaluated to select effective substances for use in commercial off-the-shelf end-user products. Many research agrochemicals are never publicly marketed or use sequential code names, such as Nalco 247, Nalco 341, Nalco 2210, Nalco 7325, Nalco 7340, Nalco 7623, Nalco 7644, Nalco 8844, and Nalco 4WC 317 by Nalco Chemical Company.

    Cannabinoids are a class of diverse chemical compounds that activate cannabinoid receptors on cells that repress neurotransmitter release in the brain. These receptor proteins include the endocannabinoids (produced naturally in the body by humans and animals), the phytocannabinoids (found in cannabis and some other plants), and synthetic cannabinoids (manufactured chemically).
    Synthetic cannabinoids encompass a variety of distinct chemical classes: the classical cannabinoids structurally related to THC, the nonclassical cannabinoids (cannabimimetics) including the aminoalkylindoles, 1,5-diarylpyrazoles, quinolines, and arylsulphonamides, as well as eicosanoids related to the endocannabinoids.

  3. carbon says:

    Diamond and graphite are two allotropes of the same element (carbon) and the differences in their properties are a result of the way their crystal structures are arranged. Both diamond and graphite are made of pure carbon, yet they have dramatic differences in their properties. As allotropes of the same element, you might expect them to share many similarities, but that simply isn’t the case.

    At first, this question might seem odd to many people. Diamond and graphite… doesn’t sound like a particularly sensible combination. Diamond and gold, or diamond and sapphire would make more sense, right? So, why is diamond pitted in the same category with graphite – the thing that we find inside our pencils?

    Well, if you had paid attention to your Chemistry lessons in high school, you would know that there is, in fact, a very strong structural connection between the two.

    What’s the connection between the two? And why are they so different from each other?

  4. Allotropes of carbon says:

    n the world of allotropes, the carbon is nothing less than a rockstar. It has the ability to form many allotropes, thanks to its chemical structure. Its atomic number is 6, which means that it has 4 electrons in its valence shell.
    As of now, no less than 8 allotropes of carbon have been identified, and the research for discovering even more allotropes is on.

    However, out of all the known allotropes, the most popular ones are diamond and graphite. These two allotropes, which visually appear incredibly different, are still made of nothing but carbon. Although their composition is the same, they exhibit different chemical and physical properties, thanks to the arrangement of carbon atoms within them

  5. says:

    It boils down to a single factor: geometry.

    The arrangement of carbon atoms in diamond follows a tetrahedral fashion. This means that each carbon atom is attached to 4 other carbon atoms, forming strong covalent bonds.

    This crystal arrangement is energetically very favorable and imparts that characteristic strength, durability and rigidity to diamond. To scratch or break it requires a high amount of force, which makes it one of the hardest naturally-occurring materials on the planet.

    Graphite, on the other hand, has an entirely different geometric arrangement than diamond. Its carbon atoms are arranged in 2D sheets, whereas each carbon atom is bonded to three other carbon atoms to form hexagonal rings in an infinite array. Although the bonding of atoms within each individual layer is covalent and therefore quite strong (as strong as is seen in diamond), the bonding between layers is weak (Van der Waals forces).

    The result of this is that the layers slide over each and can detach from each other very easily. These weak bonds between the multiple sheets of carbon atoms make the graphite used in pencils flake off on paper, allowing you to write. In addition to being soft and slippery, graphite also has a much lower density than diamond.

    The one thing about all of this that amazes me most is how a few tweaks in the chemical structure of identical substances make them so massively different in their appearance, toughness and chemical properties!

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