Naming Ionic Compounds with Transition Metals
... Rules for naming ionic compounds
with transition metals:
1. The name of the metal ALWAYS comes first:
The metal’s name is as it is on the periodic table
Identify the metals charge with Roman Numerals
2. The name of the nonmetal ALWAYS comes second.
Change the ending of the nonmetal to “ide”
... Common Oxidation Numbers:
a) Any element = 0
b) H (in compounds) = +1
c) O (in compounds) = −2
d) Any monoatomic ion = its charge
Electrochemistry Oxidation – Reduction and Oxidation Numbers
... Chemists have devised a useful bookkeeping method
to determine if electron transfer is involved in a
chemical reaction. It is referred to as the oxidation
If an atom loses electrons, it is oxidized.
If an atom gains electrons, it is reduced.
The oxidation state or equivalently, the oxi ...
Oxidation-Reduction (Redox) Reactions
... comparing the oxidation number of an atom before
and after reaction allows us to determine whether
the atom has gained or lost electrons
convenient way to keep track of electrons in a
Exam 2 Review - Iowa State University
... 3. Certain elements almost always have the same oxidation number.
a. Group 1A elements = +1
b. Group 2A elements = +2
c. Group 3A elements = +3
d. F, Cl, Br, I = -1 in binary compounds with metals
e. H = +1 (-1 in metallic hydrides)
f. O = -2
4. The sum of oxidation numbers of all atoms in a compoun ...
Rules and Clues for Determining Oxidation Number
... F: Always –1, except F2
O: Almost always –2 (exceptions: cmpds. w/ O-O or O-F bonds)
Alkali metals: Always +1 (except pure metal (0))
Alkaline earths: Always +2 (except pure metal (0))
H: +1 when bonded to main group (C, O, N, halide groups)
-1 when bonded to metals
5. Ranges of oxidation states for ...
AP Chapter Five Outline
... Oxidation numbers compare the charge of an uncombined atom with
its actual charge in a compound. All neutral atoms have an equal
number of protons and electrons and thus have no net charge.
Oxidation numbers of atoms in molecular compound are assigned as
though electrons were completely transfer ...
The oxidation state, often called the oxidation number, is an indicator of the degree of oxidation (loss of electrons) of an atom in a chemical compound. Conceptually, the oxidation state, which may be positive, negative or zero, is the hypothetical charge that an atom would have if all bonds to atoms of different elements were 100% ionic, with no covalent component. This is never exactly true for real bonds.The term ""oxidation"" was first used by Lavoisier to mean reaction of a substance with oxygen. Much later, it was realized that the substance on being oxidized loses electrons, and the use of the term ""oxidation"" was extended to include other reactions in which electrons are lost.Oxidation states are typically represented by small integers. In some cases, the average oxidation state of an element is a fraction, such as 8/3 for iron in magnetite (Fe3O4). The highest known oxidation state is reported to be +9 in the cation IrO+4, while the lowest known oxidation state is −5 for boron, gallium, indium, and thallium. The possibility of +9 and +10 oxidation states in platinum group elements, especially iridium(IX) and platinum(X), has been discussed by Kiselev and Tretiyakov.The increase in oxidation state of an atom through a chemical reaction is known as an oxidation; a decrease in oxidation state is known as a reduction. Such reactions involve the formal transfer of electrons, a net gain in electrons being a reduction and a net loss of electrons being an oxidation. For pure elements, the oxidation state is zero.There are various methods for determining oxidation states/numbers.In inorganic nomenclature the oxidation state is determined and expressed as an oxidation number represented by a Roman numeral placed after the element name.In coordination chemistry, oxidation number is defined differently from oxidation state.