WATER NEWS

• Hydrogen Electrons Valence
• Hydrogen Electrons Protons
• Hydrogen Electrons Per Shell
• Hydrogen Electrons Neutrons
• Hydrogen Mass Number

A molecule of hydrogen is the simplest possible molecule. It consists of two protons and two electrons held together by electrostatic forces. Like atomic hydrogen, the assemblage can exist in a number of energy levels. Ortho-hydrogen and para-hydrogen. Two types of molecular hydrogen (ortho and para) are known. Ionised hydrogen is very common in nebula in outer space where the electrons have been stripped off the hydrogen atoms by intense UV light and are very easily. Hydrogen is an essential for life, the universe and just about everything. Life, in fact, is multiply dependent on it. Without hydrogen we wouldn't have the Sun to give us heat and light. There would be no useful organic compounds to form the building blocks of life. And that most essential substance for life's existence, water, would not exist.

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An orbital structure is the space in an atom that’s occupied by an electron. But when describing these super-microscopic properties of matter, scientists have had to rely on wave functions — a. HYDROGEN IS THE universe's simplest atom: a single electron orbiting a single proton. In a fuel cell, incoming hydrogen gas is separated by a catalyst at the anode into protons and electrons.

Hydrogen Electrons Valence

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Hydrogen: What’s the difference between H, H2, H+, H- and OH- ?

Distinguishing between these different forms of Hydrogen can be confusing to those of us who flunked high school chemistry. Here is an attempt at clarification.

H = Atomic Hydrogen
Atomic hydrogen is number 1 on the Periodic Table of Elements. It consists of one proton and one unpaired electron which means that it is a free radical.
However an atom of hydrogen rarely exists on its own because its unpaired electron eagerly seeks to join up with another electron.

The molecular form of hydrogen is more common.

H₂ = Molecular Hydrogen

H₂ is a gas which forms when two hydrogen atoms bond together and become a hydrogen molecule. H2 is also called molecular hydrogen.It consists of two protons and two electrons. Consequently it is the most common form of Hydrogen because it is stable with a neutral charge. H2 is not a free radical. It is the antioxidant in ‘hydrogen-rich’ water.

H2 is the smallest molecule in the universe. That means it can go where nothing else can …including into your mitochondria which are the powerhouses of your cells. Hydrogen gas cannot be kept in plastic because it will pass right through the walls of the container.

H⁺ = Proton

When the Hydrogen atom loses an electron all that is left is a proton. It becomes the positively charged hydrogen ion known as H⁺. This is the form of Hydrogen that produces the ATP enzyme that powers our cells and mitochondria.

The H⁺ hydrogen ion is the basis of the pH scale.

H:^– = Hydride

Hydride is a hydrogen atom which has an extra electron. This means that it is a negatively charged ion, or anion. That is why Hydride ion (H-) has the minus sign distinguishing it from a regular Hydrogen atom (H). The two dots after the H means that this ion has two electrons instead of just one. The extra electron means that H- is not a free radical however it is not stable because this form of hydrogen is a very strong base (extremely alkaline) which reacts with water to produce hydroxide (OH^–and molecular hydrogen (H₂).

H:^– + H₂O –> H₂O + OH^–

Hydride (H:^– ) also reacts with metals to form chemical compounds which are reducing agents.

OH^– = Hydroxide ion

Hydroxide (OH–) is also known as the hydroxyl ion. When water dissociates or comes apart into its component parts it forms OH^– (hydroxide ions) and H₃O⁺ (hydronium ions).
2H₂O ⇆ OH^– and H₃O⁺

This reaction is reversible. The hydroxide ion also reacts with the hydronium ion (H3O+) to become two water molecules.

The Hydroxide ion (OH^– ) is a base (alkaline). The Hydroxide ion is not a free radical or an antioxidant. Dissolved molecular hydrogen gas (H2) is the antioxidant in ‘hydrogen-rich’ water.

Hydroxide (OH^–) is sometimes confused with the hydroxyl radical (OH^•). The dot to the upper right of the OH indicates an unpaired electron which means that Hydroxyl is a free radical, actually one of the most reactive oxygen radicals. Hydroxide and Hydroxl are two entirely different species. It is important to not confuse them.

H₃O⁺ = Hydronium ion

A water molecule (H₂0) plus a hydrogen ion (H⁺) becomes a hydronium ion (H₃O⁺). The H⁺ ion is a lone proton with a powerful charge. It does not exist on its own in an aqueous solution because it is immediately attracted to the unshared electrons in the oxygen atom of H₂O. The result is Hydronium (H₃O⁺). This process is reversible. Two water molecules can disassociate to form hydronium plus hydroxide.
2H₂O ⇆ OH^– and H₃O⁺
Experiments indicate that the proton (H⁺) is very promiscuous. It changes from one H₂O partner to another many times per second creating a new H₃O⁺ ion as it moves.

pH = Potential of Hydrogen

pH stands for potential of Hydrogen and is actually a measurement of the concentration of hydrogen ions (H+) in a solution. Water breaks down (dissociates) into protons (H⁺) and hydroxides (OH^–). This reaction is reversible.

H₂O ⇆ H⁺ and OH^–
2H₂O ⇆ OH^– and H₃O⁺

pH indicates whether water is acidic, neutral, or alkaline. More H⁺ = more acidic. Less H⁺ = more alkaline.

Because H+ immediately associates with H₂O to form H₃O⁺ (Hydronium), pH can also be said to be a measurement of the concentration of H₃O⁺ in a solution.

The pH scale is logarithmic. Increasing by 1 on the pH scale results in a 10 times decrease in the hydronium ion concentration and increasing by 3 on the pH scale results in a 1,000 times decrease in the hydronium ion concentration.

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This is easily the most important use of the terms oxidation and reduction at A' level.

Definitions

• Oxidation is loss of electrons.

• Reduction is gain of electrons.

It is essential that you remember these definitions. There is a very easy way to do this. As long as you remember that you are talking about electron transfer:

A simple example

The equation shows a simple redox reaction which can obviously be described in terms of oxygen transfer.

Copper(II) oxide and magnesium oxide are both ionic. The metals obviously aren't. If you rewrite this as an ionic equation, it turns out that the oxide ions are spectator ions and you are left with:

A last comment on oxidising and reducing agents

Hydrogen Electrons Protons

If you look at the equation above, the magnesium is reducing the copper(II) ions by giving them electrons to neutralise the charge. Magnesium is a reducing agent.

Looking at it the other way round, the copper(II) ions are removing electrons from the magnesium to create the magnesium ions. The copper(II) ions are acting as an oxidising agent.

Warning!

This is potentially very confusing if you try to learn both what oxidation and reduction mean in terms of electron transfer, and also learn definitions of oxidising and reducing agents in the same terms.

Personally, I would recommend that you work it out if you need it. The argument (going on inside your head) would go like this if you wanted to know, for example, what an oxidising agent did in terms of electrons:

• An oxidising agent oxidises something else.

• Oxidation is loss of electrons (OIL RIG).

• That means that an oxidising agent takes electrons from that other substance.

• So an oxidising agent must gain electrons.

Hydrogen Electrons Per Shell

Or you could think it out like this:

Hydrogen Electrons Neutrons

• An oxidising agent oxidises something else.

• That means that the oxidising agent must be being reduced.

• Reduction is gain of electrons (OIL RIG).

• So an oxidising agent must gain electrons.

Hydrogen Mass Number

Understanding is a lot safer than thoughtless learning!