EXPERIMENT II
REDOX ELEMENTS NITROGEN
REDOX ELEMENTS NITROGEN
I. Destination
The
objective of this experiment is that students can
study the redox reaction of
the element nitrogen in nitric acid, nitrates and ammonia salts.
II. Basic Teory
Redox (reduction / oxidation) is a
term that describes the change in oxidation number (oxidation state) of atoms in
a chemical reaction. This can be either a simple redox process such as the
oxidation of carbon to yield carbon dioxide, or the reduction of carbon by
hydrogen to yield methane (CH4), or it can be a complex processes such as
oxidation of sugar in the human body through a complicated series of electron
transfer. The term redox comes from the two concepts of reduction and
oxidation. He can be described easily as follows:
· Oxidation
describes the release of electrons
by a molecule,
atom, or ion.
·
Reduction
describes the gain of electrons by a molecule, atom, or ion.
Nitrogen (nitrum Latin, Greek nitron means "native
soda", genes means "forming") was officially discovered by
Daniel Rutherford in 1772, which called toxic air or fixed air. The knowledge
that there is a fraction of air that does not help in combustion has been known
to chemists since the end of the 18th century anymore. Nitrogen is also
assessed in a more or less the same time by Carl Wilhelm Scheele, Henry
Cavendish, and Joseph Priestley, who called it air or air burning has
flogistat. Nitrogen gas is sufficiently weak so named by Antoine Lavoisier as
azote, rather than the Greek words that mean αζωτος "lifeless". The
term has become a name to the nitrogen in the words of the French and later
evolved into other languages (Anonymous, 2009).
The element nitrogen can have multiple oxidation states, ie
+5, 0, -3, where all three oxidation states is the most common and stable among
others. There are two common nitrogen oxide acid, nitric acid (HNO3) and
nitrous acid (HNO2). Nitric acid is a strong acid as well as a strong oxidizer.
Concentrated nitric acid can oxidize almost all metals except for Au, Pt, Rh
and Ir. Nitric acid is less stable than nitric acid and tend
terdisproporsionasi into NO and HNO3
Nitrogen-free there diatmosfir (78 percent by volume). Apart
from that. The atmosphere may also contain a small amount of ammonia as a
result of decay of a substance containing nitrogen or nitric acid., Especially
after a thunderstorm. Nitrogen is also contained in the salts of sodium and
potassium nitrate. Network of all living organisms contain nitrogen compounds
in the form of the protein (Responsible Course, 2011).
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