oxidation and reduction in chemical reactions

Question 1

oxidation

Answer 1

when atoms lose electrons and oxidation number goes up, substances being oxidized are reactants

Question 2

reduction

Answer 2

atoms gain electrons and oxidation number goes down, substance being reduced is also a reactant

Question 3

redox reactions

Answer 3

both have oxidation and reduction happening simultaneously (at the same time) and are SINGLE replacement reactions

Question 4

metal hydride

Answer 4

metal + hydrogen, but hydrogens oxidation is -1

Question 5

half reactions

Answer 5

show half of a redox reaction, they show either the oxidation or reduction part of a redox reaction, when writing a half reaction you musts show the number of electrons gained or lost

Question 6

oxidation half reaction

Answer 6

shows an atom or ion losing electrons (show electrons on the product side)

Question 7

reduction half reaction

Answer 7

an atom or ion gaining electrons (show electrons on the reactant side)

Question 8

OIL RIG

Answer 8

oxidation is loss
reduction is gained

Question 9

TABLE J

Answer 9

metals that are more active are more oxidizable = spontaneous, those at the bottom are less oxidizable

Question 10

what does a wire do?

Answer 10

move electrons from one half cell to another and moves from a anode to cathode

Question 11

what does the salt bridge do?

Answer 11

the flow of ions between solutions in each half cell and enables redox reactions

Question 12

anode

Answer 12

oxidation happens, anode is negative in a voltaic cell, and oxidation causes the anode to get smaller (lose mass)

Question 13

cathode

Answer 13

reduction happens, cathode is positive in a voltaic cell, electrons gained = larger cathode

Question 14

where do oxidation and reduction reactions take place?

Answer 14

inside electrochemical cells

Question 15

what are the 2 type of electrochemical cells?

Answer 15

voltaic cell and electrolytic cell

Question 16

inside the voltaic cell..

Answer 16

redox reactions are spontaneous (by itself) and chemical reactions are needed to PRODUCE electricity EX a battery

Question 17

inside the electrolytic cell

Answer 17

redox reactions are non spontanneous and electricity is needed to START these chemical REACTIONS
EX: electrolysis or electroplating

Question 18

parts of a voltaic cell

Answer 18

2 half cells and electrodes

Question 19

electrodes

Answer 19

metal strips in each half cell

Question 20

2 half cells

Answer 20

containers that allow for oxidation and reduction half reactions happen

Question 21

cathode

Answer 21

reduction, cathode is positive in a voltaic cell

Question 22

voltaic cell diagram

Answer 22

show half reactions

Question 23

how do you figure out which metal is the anode and which is cathode in a diagram?

Answer 23

TABLE J, metal higher = anode because its oxidized
metal lower = cathode

Question 24

what is the flow of electrons?

Answer 24

anode to cathode

Question 25

parts of an electrolytic cell

Answer 25

1 medium, electrodes, wire, battery, and solution

Question 26

electrodes

Answer 26

anode is POSITIVE in an electrolytic cell, and a cathode is NEGATIVE

Question 27

battery

Answer 27

there needs to be electricity to force electrons to flow from anode to cathode to force a non spontaneous reaction

Question 28

electrolysis

Answer 28

electricity used to form a chemical reeaction

Question 29

solution

Answer 29

positive ion in solution = attracted to cathode (negative)
negative ion in solution = attracted to anode (positive)

Question 30

electroplating

Answer 30

example of electrolytic cell where electrolysis is used to electroplate (cover something with a different metal) onto a surface

Question 31

what is the object that gets plated?

Answer 31

a cathode (a metal) is ALWAYS CATHODE and turns (-)

Question 32

what is the anode made of?

Answer 32

whatever metal is being used for plating

Question 33

electroplating anode

Answer 33

turns (+)