Cmc chapter 20

Chapter Menu Electrochemistry Section 20.1 Voltaic Cells Section 20.2 Batteries Section 20.3 Electrolysis Exit Click a hyperlink or folder tab to view the corresponding slides.

Section 20-1 Section 20.1 Voltaic Cells ,[object Object],oxidation: the loss of electrons from the atoms of a substance; increases an atom’s oxidation number ,[object Object],[object Object],reduction: the gain of electrons by the atoms of a substance; decreases the atom’s oxidation number

Section 20-1 Section 20.1 Voltaic Cells (cont.) salt bridge electrochemical cell voltaic cell half-cell In voltaic cells, oxidation takes place at the anode, yielding electrons that flow to the cathode, where reduction occurs. anode cathode reduction potential standard hydrogen electrode

Section 20-1 Redox in Electrochemistry ,[object Object],[object Object]

Section 20-1 Redox in Electrochemistry (cont.)

Section 20-1 Redox in Electrochemistry (cont.) ,[object Object],[object Object]

Section 20-1 Redox in Electrochemistry (cont.) ,[object Object]

Section 20-1 Chemistry of Voltaic Cells ,[object Object],[object Object],[object Object]

Section 20-1 Chemistry of Voltaic Cells (cont.) ,[object Object],[object Object],[object Object]

Section 20-1 Calculating Electrochemical Cell Potentials ,[object Object],[object Object]

Section 20-1 Calculating Electrochemical Cell Potentials (cont.) ,[object Object]

Section 20-1 Calculating Electrochemical Cell Potentials (cont.)

Section 20-1 Calculating Electrochemical Cell Potentials (cont.) ,[object Object],[object Object]

Section 20-1 Use Standard Reduction Potentials ,[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 20-1 Section 20.1 Assessment In electrochemistry, the site where oxidation occurs is called ____. A. electrode B. anode C. cathode D. ion

[object Object],[object Object],[object Object],[object Object],Section 20-1 Section 20.1 Assessment The standard potential of a voltaic cell is the difference between the: A. electrode voltage B. standard reduction potential of the cell and hydrogen C. standard reduction potentials of the half-cell reactions D. half-cell reactions and the salt bridge

Section 20-2 Section 20.2 Batteries ,[object Object],reversible reaction: a reaction that can take place in both the forward and reverse directions ,[object Object],[object Object],[object Object]

Section 20-2 Section 20.2 Batteries (cont.) battery dry cell primary battery secondary battery Batteries are voltaic cells that use spontaneous reactions to provide energy for a variety of purposes. fuel cell corrosion galvanization

Section 20-2 Dry Cells ,[object Object]

Section 20-2 Dry Cells (cont.) ,[object Object],[object Object],[object Object]

Section 20-2 Dry Cells (cont.) ,[object Object],[object Object]

Section 20-2 Dry Cells (cont.) ,[object Object]

Section 20-2 Lead-Acid Storage Battery ,[object Object],[object Object],[object Object],[object Object]

Section 20-2 Lithium Batteries ,[object Object],[object Object]

Section 20-2 Fuel Cells ,[object Object]

Section 20-2 Fuel Cells (cont.) ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Section 20-2 Corrosion ,[object Object],[object Object],[object Object],[object Object]

Section 20-2 Corrosion (cont.) ,[object Object],[object Object],[object Object],[object Object]

Section 20-2 Corrosion (cont.)

Section 20-2 Corrosion (cont.) ,[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 20-2 Section 20.2 Assessment Which type of battery has a reversible spontaneous reaction? A. alkaline battery B. secondary battery C. primary battery D. zinc-carbon battery

[object Object],[object Object],[object Object],[object Object],Section 20-2 Section 20.2 Assessment Which is NOT a method of preventing corrosion? A. painting B. galvanization C. coating with electrolytes D. sacrificial anode

Section 20-3 Section 20.3 Electrolysis ,[object Object],redox reaction: an oxidation-reduction reaction electrolysis electrolytic cell ,[object Object],[object Object],In electrolysis, a power source causes nonspontaneous reactions to occur in electrochemical cells.

Section 20-3 Reversing Redox Reactions ,[object Object],[object Object]

Section 20-3 Applications of Electrolysis ,[object Object]

Section 20-3 Applications of Electrolysis (cont.) ,[object Object]

Section 20-3 Applications of Electrolysis (cont.) ,[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 20-3 Section 20.3 Assessment Which of the following is NOT a product of electrolysis of brine? A. Chlorine gas B. Hydrogen gas C. Sodium hydroxide solution D. Sodium metal

[object Object],[object Object],[object Object],[object Object],Section 20-3 Section 20.3 Assessment What is required to drive a nonspontaneous reaction in an electrolytic cell? A. electrodes B. additional ions C. an energy source D. an electrolyte

Resources Menu Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion

Study Guide 1 Section 20.1 Voltaic Cells Key Concepts ,[object Object],[object Object],[object Object]

Study Guide 1 Section 20.1 Voltaic Cells (cont.) Key Concepts ,[object Object]

Study Guide 2 Section 20.2 Batteries Key Concepts ,[object Object],[object Object],[object Object],[object Object]

Study Guide 3 Section 20.3 Electrolysis Key Concepts ,[object Object],[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 1 A salt bridge is used for what? A. electrolysis B. allowing ions to move from one half-cell to the other C. increasing the reduction potential D. linking multiple voltaic cells together

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 2 Batteries that can be used more than once are also called ____. A. primary batteries B. secondary batteries C. tertiary batteries D. fuel cells

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 3 Corrosion is loss of metal by what mechanism? A. electrolysis B. galvanization C. oxidation-reduction reaction D. salt bridge

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 4 Electrolysis of H 2 O results in what products? A. H + and OH – B. H 2 O 2 and O 2 C. NaOH and H 2 D. H 2 and O 2

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 5 Which of the following is NOT a dry-cell? A. a car battery B. a silver battery C. a zinc-carbon battery D. an alkaline battery

[object Object],[object Object],[object Object],[object Object],STP 1 Which is NOT a characteristic of an acid? A. sour taste B. conduct electricity in solution C. reactivity with some metals D. slippery feel

[object Object],[object Object],[object Object],[object Object],STP 2 Which metal has the lowest standard reduction potential? A. Sodium B. Magnesium C. Lithium D. Silver

[object Object],[object Object],[object Object],[object Object],STP 3 Which statement is NOT true about batteries? A. Batteries are composed of two half-cells. B. Secondary batteries are also known as storage batteries. C. Redox reactions in zinc-carbon batteries are easily reversible. D. Batteries are compact forms of voltaic cells.

[object Object],[object Object],[object Object],[object Object],STP 4 Which of the following is the equation used to calculate a cell potential? A. E 0 cell = E 0 oxidation – E 0 reduction B. E 0 cell = E 0 reduction – E 0 oxidation C. E 0 cell = E 0 reduction + E 0 oxidation D. E 0 cell = E 0 reduction x E 0 oxidation

[object Object],[object Object],[object Object],[object Object],STP 5 Which is NOT an example of a sacrificial anode? A. magnesium B. aluminum C. iron D. titanium

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Cmc chapter 20

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Cmc chapter 20