Electrolysis Flashcards

1
Q

An electric current is

A

A flow of electrons or ions

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2
Q

Covalent compounds - conduct electricity?

A

NO- because the electrons are shared so are fixed in a certain position and are not able to move freely and conduct electricity.

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3
Q

Ionic compounds - conduct electricity?

A

NOT when solid because the ions aren’t free to move

YES when molten or in solution because the ions can move freely

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4
Q

Electrolysis is

A

A chemical change caused by passing on electric current through a compound that is either molten or in solution

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5
Q

An Electrolyte is

A

A substance that undergoes electrolysis. Covalent compounds AREN’T because they don’t contain ions

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6
Q

Anode

A

Positive electrode

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7
Q

Cathode

A

Negative electrode

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8
Q

PANC

A

Positive Anode Negative Cathode

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9
Q

Charges of common positive ions (cations) - 1+

A
H+
Na+
Ag+
K+
Li+
NH4+
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10
Q

Charges of common positive ions (cations) - 2+

A
Ba2+
Ca2+
Cu2+
Mg2+
Zn2+
Pb2+
Fe2+
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11
Q

Charges of common positive ions (cations) - 3+

A

Fe3+

Al3+

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12
Q

Testing for cations (Flame tests)

A
-Dip a platinum wire in Hydrochloric Acid and then into the solid, then into flame
Li+       Red flame
Na+      Strong orange flame
K+        Lilac flame
Ca2+    Brick red flame
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13
Q

Testing for cations (Precipitation reactions)

A

-Add sodium hydroxide solution to the solution containing:

NH4+, Ammonia = No precipitate is formed but there will be a strong smell and when heated will turn damp litmus blue -ALKALINE
Cu2+, Copper = Blue precipitate (Copper ll hydroxide)
Fe2+, Iron ll = Green precipitate (Iron ll hydroxide)
Fe3+, Iron lll = Orange- brown precipitate (Iron lll hydroxide)

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14
Q

Charges of common negative ions (anions) - 1-

A
Cl-
Br-
F-
I-
HCO3-
OH-
NO3-
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15
Q

Charges of common negative ions (anions) - 2-

A

O2-
S2-
SO42-
CO32-

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16
Q

Testing for anions (Chlorine, Bromine + Iodine)

A

-Add enough dilute nitric acid to make your solution (in water) acidic and then add sliver nitrate solution

Cl- = white precipitate (silver chloride)
Br- = pale cream precipitate (silver bromide)
I- = yellow precipitate (silver iodide)
17
Q

Testing for anions (Sulfates)

A

-Add enough dilute hydrochloric acid to make your solution (in water) acidic and then add barium chloride solution

SO42- = white precipitate (barium sulfate)

18
Q

Testing for anions (Carbonates)

A

-Add dilute nitric acid and look for bubbles of gas produced and collect, test for Carbon Dioxide

CO32- = bubbles of CO2

19
Q

Half equations at cathode

A

Cu2+(aq) + 2e- –> Cu(s)

20
Q

Half equations at anode

A

2I-(aq) –> I2(aq) + 2e-

21
Q

OILRIG

A
Oxidisation
Is
Loss of electrons
Reduction
Is
Gain of electrons
22
Q

Reducing agent

A

Substance that reduces something else (gives it electrons)

23
Q

Oxidising agent

A

Substance that oxidises something else (takes its electrons)

24
Q

Redox reaction

A

Where both oxidisation and reduction occur