ox and reduction

Question 1

what happens when an atom undergoes oxidization?

Answer 1

loses electron/has a more positive charge

Question 2

what happen to an atom when it is the reduction agent?

Answer 2

it is oxidizing/ loosing electrons

Question 3

what happens when an atom undergoes reduction?

Answer 3

gains electrons/ more negative charge

Question 4

what happen to an atom when it is the oxidation agent?

Answer 4

undergoes reductions/ gains electrons/ more negative charge

Question 5

how do you determine which atom gets priority over charge?

Answer 5

the most electronegative charge

Question 6

what oxidation state do Free elements have?

Answer 6

none/0

Question 7

what charge does monoatomic ions have?

Answer 7

the charge displayed/given to them

Question 8

what should the sum of the oxidation states add up too?

Answer 8

0/ they should cancel out unless told otherwise

Question 9

when making oxidation half-reaction which sides do the electrons go on?

Answer 9

product side

Question 10

when making reduction half-reaction which sides do the electrons go on?

Answer 10

reactant side

Question 11

when making reduction half-reaction which sides do the electrons go on?

Answer 11

reactant side

Question 12

when the two half equations add together what charge should it have?

Answer 12

o/ given charge

Question 13

skip

Answer 13

ship

Question 14

what are the steps to balancing half reactions by mass?

Answer 14

1) First balance atoms other than O and H.
2) Balance O by adding H2O to side that lacks O.
3) Balance H by adding H+ to side that lacks H.
4) Finished if in acidic solution.
5) If in basic solution, add enough OH− to neutralize the H+, rewrite H+ + OH− as H2O.
6) Add to both sides.
7) Then cancel H2O on both sides.

Question 15

what are the steps to balancing half reactions by charge?

Answer 15

1) add electrons on the product side for the oxidation agent
2) add electrons on the reactant side for the reduction agents

Question 16

when do Displacement reactions happen?

Answer 16

when a stronger reducing agent replaces a weaker reducing agent. The reactivity series below list metals from strongest to weakest reducing agent

Question 17

how do you check if something is a spontaneous reaction?

Answer 17

e(cell)=e(red) - e(oxd) needs to end up as a positive

Question 18

what is the cathode?

Answer 18

the reduction agent

Question 19

what is the anode?

Answer 19

the oxidizing agent

Question 20

on which side is the cathode put on?

Answer 20

right/ product side

Question 21

in which order is the anode presented?

Answer 21

left/ reactant side

Question 22

what is the salt bridge?

Answer 22

ions that are not contributing just helping ions flow through

Question 23

what other atom have to be in a solution in a electrochemical reaction

Answer 23

something that will return to the original charge

Question 24

what is the redox method?

Answer 24

1. Find the appropriate half-equations on the electrochemical series.
2. Identify the chemical species that are reacting.

3.The strongest oxidant (top left) will react with the 
strongest reductant (bottom right) spontaneously. This is summarised in the ‘S’ configuration of Figure1.

4.Reduction is on the top of the S and oxidation is on the bottom (hence, RED SOX).

Question 25

draw a galvanic cell reaction

Answer 25

look at phone

Question 26

what must a cell diagram contain (galvanic cell reaction)?

Answer 26

two half-cells (including half-equations, spectator ions and ion movement) an anode and a cathode (labelled with polarity) an external circuit: consisting of wires and a voltmeter an internal circuit: consisting of a salt bridge (demonstrating ion movement).

Question 27

how do you Balancing Redox Reactions by the Half-Reaction Method?

Answer 27

1In this method, the reaction is broken down into two half-reactions, one for oxidation and another for reduction. 2Each half-reaction includes electrons. Electrons go on the product side of the oxidation half-reaction—loss of electrons. Electrons go on the reactant side of the reduction half-reaction—gain of electrons. 3Each half-reaction is balanced for its atoms. Then the two half-reactions are adjusted so that the electrons lost and gained will be equal when added.

Question 28

skip

Answer 28

skip

Question 29

how do you balance a redox reaction in basic solution?

Answer 29

same as acid solution plus 1 If in basic solution, add enough OH− to neutralize the a) H+, rewrite H+ + OH− as H2O. Add to both sides. b) Then cancel H2O on both sides 4. Balance each half-reaction, with respect to charge, by adjusting the numbers of electrons. Electrons on product side for oxidation. Electrons on reactant side for reduction. 5. Balance electrons between half-reactions. 6. Add half-reactions, canceling electrons and common species. 7. Check.

Question 30

must the gas be in contact with the electrode when in a reaction?

Answer 30

yes

Question 31

how can the The cell potential at standard conditions can be found?

Answer 31

E cell = E reduction − E oxidation | . Standard electrode potentials ( E °)

Question 32

what is the formula for electromotive force (EMF)?

Answer 32

EMF = E ° reduction half-cell – E ° oxidation half-cell

Question 33

what is a galvanic cell often called?

Answer 33

primary cell

Question 34

what is a reachable battery called?

Answer 34

secondary cell

Question 35

what is a electrolyte?

Answer 35

an ionic solution that carries charge between the electrodes

Question 36

what are the key differences between an electrolytic cell and a galvanic cell.

Answer 36

1) Electrolytic cells occur in one container with a porous divider down the middle 2) Electrolytic cells use an electrolyte instead of a salt bridge. Electrolyte solution conducts the electricity. 3) Electrolytic cells use a power source to push electrons onto one of the electrodes. This is the negative electrode because it has a negative charge due to the electrons being pushed onto it. 4) Positive ions move towards the negative electrode to gain electrons. The oxidation number of the ion decreases from a positive number to zero, so it undergoes reduction. Reduction always occurs at the cathode. Therefore, reduction occurs at the negative cathode. 5) Negative ions move towards the positive electrode where they lose electrons. As the oxidation number of the ion increases from zero to a positive charge, it undergoes oxidation. Oxidation always occurs at the anode. Therefore, oxidation occurs at the positive anode. 6) The voltage required by an electrolytic cell must be greater than the EMF that the galvanic cell would generate on discharge. For example, a copper–zinc galvanic cell that produces a voltage of 1.1 V when discharging, requires more than 1.1 V to recharge

Question 37

what is the difference between galvanic cell and primary cell?

Answer 37

a primary cell is non reversible where as a galvanic cell is Spontaneous redox reactions convert the chemical energy to an electric energy