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Old 07-23-2010, 12:11 PM
galexander galexander is offline
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Default Re: Official Silence About Free Energy

Originally Posted by FallaciesAbound View Post
Ah, so you are one of those that confuses "Just a theory" with "Just a hypothesis". I used to be one of those.

Actually, trees dont use capillary action to raise the water from root to leaf. This would be quite impossible, since the highest you can go with capillary action is about 30 ft. Trees use a combination of hydrostatic pressure and osmotic interchange to move the water up.

As for what creates the surface tension which drives capillary action, you should have simply googled intermolecular attraction.

London dispersion forces (Instantaneous dipole/ induced dipole)

Main article: London dispersion force
The London dispersion force otherwise known as quantum induced instantaneous polarization (one of the three types of van der Waals forces) is caused by instantaneous changes in the dipole of atoms, caused by the location of the electrons in the atoms' orbitals. The probability of an electron in an atom is given by the Schrödinger equation. When an electron is on one side of the nucleus, this side becomes slightly negative (indicated by δ-); this in turn repels electrons in neighbouring atoms, making these regions slightly positive (δ+). This induced dipole causes a brief electrostatic attraction between the two molecules. The electron immediately moves to another point and the electrostatic attraction is broken..
London Dispersion forces are typically very weak (see the comparison below) because the attractions are so quickly broken, and the charges involved are so small.[1]
[edit] Dipole-Dipole Interactions

Dipole-Dipole interactions, also called Keesom interactions after Willem Hendrik Keesom, are caused by permanent dipoles in molecules. When one atom is covalently bonded to another with a significantly different electronegativity, the electronegative atom draws the electrons in the bond nearer to itself, becoming slightly negative. Conversely, the other atom becomes slightly positive. Electrostatic forces are generated between the opposing charges and the molecules align themselves to increase the attraction (reducing potential energy).
An example of dipole-dipole interactions can be seen in hydrogen chloride:

This is not an example of hydrogen bonding (see below) because the chlorine atom is not electronegative enough.
Note that almost always the dipole-dipole interaction between two atoms is zero, because atoms rarely carry a permanent dipole, see atomic dipoles.
Often, molecules can have dipoles within them, but have no overall dipole moment. This occurs if there is symmetry within the molecule, causing the dipoles to cancel each other out. This occurs in molecules such as tetrachloromethane.
[edit] Hydrogen bonding

Main article: Hydrogen bond
Hydrogen bonds are a stronger form of dipole-dipole interactions, caused by highly electronegative atoms. They only occur between hydrogen and oxygen, fluorine or nitrogen,[2] and are the strongest intermolecular force. The high electronegativities of F, O and N create highly polar bonds with hydrogen, which leads to strong bonding between hydrogen atoms on one molecule and the lone pairs of F, O or N atoms on adjacent molecules. The high boiling point of water is an effect of the extensive hydrogen bonding between the molecules:

For quite some time it was believed that hydrogen bonding required an explanation that was different from the other intermolecular interactions. However, reliable computer calculations that became possible during the 1980s have shown that only the four effects listed above play a role, with the dipole-dipole interaction being particularly important. Since the four effects account completely for the bonding in small dimers like the water dimer, for which highly accurate calculations are feasible, it is now generally believed that no other bonding effects are operative.[citation needed]
Hydrogen bonds are found throughout nature. In water the dynamics of these bonds produce unique properties essential to all known life-forms. Hydrogen bonds, between hydrogen atoms and nitrogen atoms, of adjacent DNA base pairs generate intermolecular forces that improve binding between the strands of the molecule. Hydrophobic effects between the double-stranded DNA and the solute nucleoplasm prevail in sustaining the double-helix structure of DNA.

As for gravity, sure, you can certainly glean some energy by properly utilizing it. Hydro-electric dams for starters. But remember, the energy from those comes from the sun ultimately. Hopefully you can see how.
Thank you for blinding us with scientific detail once more.

However you forgot to tell us where the energy ultimately comes from on a molecular level for the Law of Conservation of Energy to apply.

If you can't then the energy must be 'free'.
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