Electron Transfer Reactions

Oxidation

Oxidation

The process of combining a substance with oxygen or the removal of electrons from an atom or molecule

Reduction

The process of removing oxygen from a substance or adding electrons to an atom or molecule

Oxidation state

The oxidation state (or oxidation number) is a numerical value that represents the total number

Species

In the context of redox reactions, species refer to the different atoms, molecules, or ions taking part in the reaction, which can undergo oxidation or reduction.

oxidizing agent

A substance that causes oxidation by accepting electrons from another species, thereby being reduced in the process.

reducing agent

A substance that causes reduction by donating electrons to another species, resulting in its own oxidation.

Metals in redox reactions

are often reducing agents due to their tendency to lose electrons easily, forming positive ions

Displacement reaction

A type of redox reaction where an element displaces another in a compound, resulting in the formation of a new element and a new compound.

How does the periodic table relate to the reactivity and ease of oxidation of metals?

As you move down a group in the periodic table, metals become more reactive and oxidize more easily due to the increasing distance between the nucleus and the outer electrons, which makes it easier for them to lose electrons. This trend is influenced by factors such as atomic size, ionization energy, and electronegativity.

How does the periodic table relate to the reactivity of halogens?

As you move down the group of halogens in the periodic table, their reactivity decreases. This is due to the increasing atomic size and the shielding effect, which make it more difficult for larger atoms to attract and gain electrons.

general equation for metals and acids

metal + acid = salt + hydrogen