CHEM1102 Worksheet 12: Coordination Chemistry Model 1: The
... CHEM1102 Worksheet 12: Coordination Chemistry
Model 1: The oxidation number and electronic configuration of transition metal cations in
The sum of the charges of the metal cation and its ligands adds up to give the charge of the complex ion. If the
complex ion is charged, this ...
Chapter 4: Chemical Quantities and Aqueous Reactions
... 1. For the atoms in a neutral species—an isolated atom, a molecule, or a formula unit—the sum of all the
oxidation numbers is 0.
2. For the atoms in an ion, the sum of the oxidation numbers is equal to the charge on the ion.
3. In compounds, the group 1A metals all have an oxidation number of + ...
Balancing Redox Equations
... Oxidizing agent when it combines with metals.
Reducing agent when it combines with nonmetals.
Descriptive Chemistry for Midterm Exam #1
... a visible photon and move to a higher energy d-orbital from a lower energy d-orbital..
The energy gap between the d-orbitals is affected by the type of ligand. This affects the
frequencies of absorbed and reflected visible light. The compounds and complexes of a
given transition metal have different ...
Redox Review 9.1
... 4. Balance charge by adding e- as needed.
Multiply half reactions by integers so that the # of e- lost in
one reaction = # of e- gained in the other reaction.
Add the two half reactions. Simplify by canceling species
that appear on both sides of the arrow.
Check your work. Make sure that both the at ...
AP Reaction Rules
... Typically twice the number of ligands will attach as the charge on the Lewis acid
Redox: a change in the oxidation number of one or more reactants occurs as products are formed
Include single replacement, combination, and decomposition reactions
Oxidation numbers are a book-keeping idea, not the sam ...
... 2. Find a classmate to “bond” with and together
decide on the correct chemical formula (use
the oxidation numbers to help you!)
3. You will have to decide how many of each ion
you need to make a STABLE IONIC BOND.
4. Record all bonds on your Date Book (data
5. Look at the box on your paper fo ...
... b) Cr2O72- and Fe2+
c) H2O2 and MnO4¯
d) C2O42- and MnO4¯
e) S2O32- and I2
f) Cr2O72- and I¯
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.