CHE 106 Lecture Notes - Lecture 11: Oxidation State, Fluorine, Molar Concentration

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Che 106: general chemistry- lecture 11: oxidation numbers. Elements: oxidation # of an atom in an element is 0. Monatomic ions: oxidation # of an atom in a monatomic ion equals the charge on the ion. Oxygen: the oxidation number of oxygen is -2 in most of its compounds. (an exception is h2o2 and other peroxides, where the oxidation number is -1. ) Hydrogen: the oxidation number of hydrogen is +1 in most of its compounds. Halogens: fluorine is -1 in all its compounds. The other halogens are -1 unless the other element is another halogen or oxygen. Compounds and ions: the sum of the oxidation numbers of the atoms in a neutral compound is 0. Metals tend to have positive oxidation numbers. Nonmetals tend to have negative oxidation numbers, although some are positive in certain compounds or ions. The sum of the oxidation numbers in a neutral compound is 0. What"s the ox # of fe in feso4 (aq?)

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Oxidation Numbers

The oxidation number of an element is the "charge" the element would have if all of its bonds were completely ionic; that is, if the electron pairs of each bond were transferred to the more electronegative atom.

For monatomic ions the oxidation number is simply the charge of the ion. For covalently bonded elements the oxidation number is a bookkeeping device and does not mean that the element carries an actual charge.

Determine the oxidation state for each of the elements below.

The oxidation state of chlorine in hypochlorite ion ClO- is______
The oxidation state of chlorine in chlorine pentafluoride ClF5 is_____
The oxidation state of sulfur in sulfur dioxide SO2 is_______

Oxidation states are important for keeping track of electrons in oxidation-reduction reactions. Here are some general rules to remember:

In most cases, oxygen has an oxidation state of ?2.
Group 1 and group 2 elements on the periodic table have +1 and +2 oxidation states, respectively.
In most cases, hydrogen has an oxidation state of +1.
Many elements can have more than one oxidation state. In such cases, use the other elements in the compound whose oxidation states are known to determine the oxidation state of the element that varies.

Neutral compounds

In a neutral compound, the sum of the oxidation states is zero. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In H2O, for example, each hydrogen atom has an oxidation state of +1 and each oxygen atom has an oxidation state of ?2 for a total of 2(+1)+(?2)=0.

Part A

What is the oxidation state of an individual carbon atom in CaCO3?

Express the oxidation state numerically (e.g., +1).

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Part B

What is the oxidation state of an individual nitrogen atom in HNO3?

Express the oxidation state numerically (e.g., +1).

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Ions

In an ion, the sum of the oxidation states is equal to the overall ionic charge. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In OH?, for example, the oxygen atom has an oxidation state of ?2 and the hydrogen atom has an oxidation state of +1, for a total of (?2)+(+1)=?1.

Part C

What is the oxidation state of an individual sulfur atom in SO32??

Express the oxidation state numerically (e.g., +1).

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Part D

What is the oxidation state of each individual carbon atom in C2O42??

Express the oxidation state numerically (e.g., +1).

CHE 106 Lecture Notes - Lecture 11: Oxidation State, Fluorine, Molar Concentration

CHE 106 Full Course Notes

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