Understand the concept of oxidation states and explain why the oxidation state of an element is zero. Deduce the oxidation states of an atom in an ion or a compound, including the examples of hydrogen in metal hydrides (-1) and oxygen in peroxides (-1). Utilize oxidation numbers in the naming of compounds. Understand and use the terms: oxidation number and oxidation state.
Explain that oxidation and reduction can be described in terms of electron transfer, change in oxidation state, oxygen gain/loss or hydrogen loss/gain. Identify the oxidized and reduced species and the oxidizing and reducing agents in a chemical reaction.
Deduce redox half-equations and equations in acidic or neutral solutions.
Predict the relative ease of oxidation of metals. Predict the relative ease of reduction of halogens. Interpret data regarding metal and metal ion reactions.
Recall that oxidation occur at the anode and reduction occurs at the cathode in electrochemical cells. Identify electrodes as anode and cathode, and identify their signs/polarities in voltaic cells and electrolytic cells, based on the type of reaction occurring at the electrode.
Recall that a primary (voltaic) cell is an electrochemical cell that converts energy from spontaneous redox reactions to electrical energy. Explain the direction of electron flow from anode to cathode in the external circuit, and ion movement across the salt bridge. Construction of primary cells including: half-cells containing metal/metal ion, anode, cathode, electric circuit, salt bridge.
Understandthat secondary (rechargeable) cells involve redox reactions that can be reversed using electrical energy. Deduce the reactions of the charging process from given electrode reactions for discharge, and vice versa.
Recall that an electrolytic cell is an electrochemical cell that converts electrical energy to chemical energy by bringing about non-spontaneous reactions. Explain how current is conducted in an electrolytic cell. Deduce the products of the electrolysis of a molten salt. Construct electrolytic cells including: a DC power source, an anode, a cathode, and the electrolyte.
Deduce equations to show changes in the functional groups during oxidation of primary and secondary alcohols, including the two-step reaction in the oxidation of primary alcohols. Explain the experimental set-up for distillation and reflux. The names and formulas of specific oxidizing agents, and the mechanisms of oxidation, will not be assessed.
Deduce equations to show reduction of carboxylic acids to primary alcohols via the aldehyde, and reduction of ketones to secondary alcohols. Include the role of hydride ions in the reduction reaction. The names and formulas of specific reducing agents, and the mechanisms of reduction, will not be assessed.
Recall that the reduction of unsaturated compounds by the addition of hydrogen lowers the degree of unsaturation. Deduce the products of the reactions of hydrogen with alkenes and alkynes.