Chapter 1 (1.3-1.4)

Question 1

What is a simple chemical cell

Answer 1

Two different metal plates are dipped into an electrolyte and connected with connecting wires. Converts chemical energy to electrical energy.

Question 2

Simple cells: Also known as a

Answer 2

voltaic cell or galvanic cell.

Question 3

Where does A redox reaction occurs

Answer 3

in the cell that causes the flow of electrons.

Question 4

What happens in a redox reaction in a voltaic cell

Answer 4

A redox reaction occurs in the cell causing the flow of electrons.

Question 5

What happens in a simple chemical cell with Zn/Cu metals

Answer 5

The diagram shows a galvanic cell with a zinc plate and a copper plate each connected to a galvanometer. The zinc plate is submerged in a Zinc (II) sulfate solution and the copper plate is submerged in a Copper (II) sulfate solution. Both solutions are contained within a porous pot.

Question 6

What happens at the negative terminal in a voltaic cell

Answer 6

The Eº value of zinc is more negative; therefore

Question 7

The reaction that occurs at the negative terminal is

Answer 7

oxidation.

Question 8

What happens at the positive terminal in a voltaic cell

Answer 8

The Eº value of copper is more positive; therefore

Question 9

The reaction at the positive terminal is

Answer 9

reduction.

Question 10

What happens during the reduction process in a voltaic cell

Answer 10

Reduction involves receiving an electron and a decrease in oxidation number.

Question 11

What happens during the oxidation process in a voltaic cell

Answer 11

Oxidation involves the release of an electron and an increase in oxidation number.

Question 12

What is the reaction at the negative terminal (anode) of a voltaic cell

Answer 12

Zn(s) → Zn²⁺(aq) + 2e⁻.

Question 13

What is the reaction at the positive terminal (cathode) of a voltaic cell

Answer 13

Cu²⁺(aq) + 2e⁻ → Cu(s).

Question 14

Which direction do the electrons and current flow in a voltaic cell

Answer 14

Electrons flow from the negative terminal to the positive terminal while the current flows from the positive terminal to the negative terminal.

Question 15

What is the anode in a voltaic cell

Answer 15

The anode is the electrode where oxidation occurs.

Question 16

In a voltaic cell the negative terminal is also known as

Answer 16

the anode.

Question 17

What is the cathode in a voltaic cell

Answer 17

The cathode is the electrode where reduction occurs.

Question 18

In a voltaic cell the positive terminal is also known as

Answer 18

the cathode.

Question 19

What is an electrolyte

Answer 19

Substances that can conduct electricity in either the molten state or aqueous solution and undergo chemical changes.

Question 20

What is a non-electrolyte

Answer 20

Substances that cannot conduct electricity in all states.

Question 21

Electrolytes are

Answer 21

ionic compounds. acids. or alkalis that can conduct electricity when molten or in aqueous solutions due to freely moving ions.

Question 22

What is the apparatus setup for electrolysis

Answer 22

A battery is connected to a galvanometer and two electrodes submerged in an electrolyte. The battery supplies electricity

Question 23

What happens to cations in electrolysis

Answer 23

Cations move to the cathode (negatively charged electrode) where reduction occurs.

Question 24

Cation oxidation number

Answer 24

They receive electrons. causing a decrease in oxidation number.

Question 25

What happens to anions in electrolysis

Answer 25

Anions move to the anode (positively charged electrode) where oxidation occurs.

Question 26

Anions oxidation number

Answer 26

They release electrons

Question 27

What is the difference between conductors and electrolytes

Answer 27

Conductors conduct electricity in a solid or molten state without undergoing chemical changes. Electrolytes conduct electricity in a molten state or aqueous solution. decomposing into constituent elements.

Question 28

What is electrolysis

Answer 28

A process where compounds in molten state or aqueous solution decompose into their constituent elements by passing electricity through them.

Question 29

What happens during the electrolysis of molten lead(II) bromide. At the anode

Answer 29

Bromide ions (Br⁻) are oxidized to bromine gas (Br₂). 2Br⁻ → Br₂ + 2e⁻.

Question 30

What happens during the electrolysis of molten lead(II) bromide. At the cathode

Answer 30

Lead ions (Pb²⁺) are reduced to lead metal (Pb). Pb²⁺ + 2e⁻ → Pb.

Question 31

Observations

Answer 31

Brown gas (bromine) at the anode

Question 32

What factors affect the electrolysis of an aqueous solution

Answer 32

E° value. Concentration. Electrode type.

Question 33

Anions with more negative or less positive E° are

Answer 33

oxidized at the anode.

Question 34

Cations with more positive or less negative E° are

Answer 34

reduced at the cathode.

Question 35

Halide ions with higher concentrations are discharged at the

Answer 35

anode even if their E° value is more positive.

Question 36

Active electrodes (e.g. copper) release

Answer 36

metal ions instead of discharging anions at the anode.

Question 37

Electrolytic cell vs Chemical cell Electric sources

Answer 37

Electrolytic cell: Connected to an electrical source Chemical cell: Not connected to electrical sources

Question 38

Electrolytic Vs Chemical Electrodes

Answer 38

E: Usually carbon electrodes C: Different or same metals depending on the electrolyte

Question 39

Electrolytic vs Chemical Energy conversion

Answer 39

E: Electric → Chemical C: Chemical → Electric

Question 40

Electrolytic vs Chemical Oxidation location

Answer 40

E: Anode C: Negative terminal

Question 41

Electrolytic vs Chemical Reduction location

Answer 41

E: Cathode C: Positive terminal

Question 42

How is electroplating done

Answer 42

The object to be plated is the cathode. The plating metal is the anode. The electrolyte contains ions of the plating metal.

Question 43

Electroplating an iron ring with copper. At the anode

Answer 43

Cu(s) → Cu²⁺(aq) + 2e⁻.

Question 44

Electroplating an iron ring with copper. At the cathode

Answer 44

Cu²⁺(aq) + 2e⁻ → Cu(s).

Question 45

How is copper purified through electrolysis. Anode

Answer 45

Impure copper dissolves into Cu²⁺ ions and impurities fall below the anode. Cu(s) → Cu²⁺(aq) + 2e⁻.

Question 46

How is copper purified through electrolysis. Cathode

Answer 46

Cu²⁺ ions are discharged