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chem Flashcards

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1
Q

What are electrolytes?

A
  • ionicn compounds
    —> either molten or dissolved
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2
Q

What is electrolysis?

A

The decomposition of a compound using an electric current

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3
Q

Cathode

A
  • negatively charged electrode
  • attracts +ve charged ions
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4
Q

Anode

A
  • positively charged electrode
  • negative ions are attracted
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5
Q

What happens when ions reach an electrode?

A

They gain or lose electrons
- positive ions gain electrons from the cathode
- negative ions lose electrons at the anode

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6
Q

What forms at the cathode during electrolysis of molten salts?

A

Metal

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7
Q

What forms at the anode during electrolysis of molten salts?

A

Non-metal

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8
Q

Explain the electrolysis of acidified water

A
  • H+ ions are attracted to the cathode, gain electrons and form hydrogen gas
  • OH- ions are attracted to the anode, lose electrons and form oxygen gas
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9
Q

Explain what happens at the cathode in the electrolysis of dissolved ionic compounds

A
  • whether hydrogen or metal is produced depends on the position of the metal in the reactivity series
  • metal produced if less reactive than hydrogen
  • hydrogen produced if metal is more reactive than hydrogen
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10
Q

Reactivity series from most to least

A

Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Hydrogen
Copper
Silver
Gold

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11
Q

Example of half equations at the cathode

A

Na+ + e- —> Na

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12
Q

Example of half equations at the anode

A

2Cl- —> Cl2 + 2e-

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13
Q

Where does reduction happen?

A
  • at the cathode
  • gain of electrons
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14
Q

Where does oxidation happen?

A
  • anode
  • loss of electrons
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15
Q

Test for chlorine gas

A
  • litmus paper goes red then white
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16
Q

Testing for sulphate ions

A
  • add dilute HCL
  • add barium chloride
  • white ppt
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17
Q

How to test for metal ions

A
  • colour ppt formed when reacted with sodium hydroxide
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18
Q

Colours of Cu2+, Fe2+, Fe3+, Ca2+, Al3+ and Mg2+ metal hydroxide ppt

A
  • blue
  • green
    -brown
  • all white
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19
Q

Flame test for Li, Na, K, Ca2+, Cu2+

A
  • crimson
  • yellow orange
  • lilac
  • red orange
  • green
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20
Q

What is meant by an alloy?

A

A combination of two or more metals to combine properties

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21
Q

Electrolysis of NaCl

A

Cathode: 2H+ + 2e- —> H2

Anode: 2Cl- —> Cl2 + 2e-

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22
Q

Electrolysis of HCl

A

Cathode: 2H+ + 2e- —> H2

Anode: 2Cl- —> Cl2 + 2e-

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23
Q

Electrolysis of molten PbBr2

A

Cathode: Pb2+ + 2e- —> Pb

Anode: 2Br- —> Br2 + 2e-

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24
Q

Electroplating copper onto metals half equations

A

Anode: Cu —> Cu2+ + 2e-

Cathode: Cu2+ + 2e- —> Cu

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25
Rate equation
Reactant used or product formed ———————————————— Time
26
What is meant by an acid?
Proton donor
27
What is meant by pH?
Concentration of H+
28
What is meant by a base?
Proton acceptor
29
Rf
Distance moved by spot ———————————— Distance moved by solvent
30
How to measure rate of reaction of zinc and HCL
- inverted measuring cylinder - gas syringe - measuring loss of mass
31
How to make collisions between particles more successful
- increasing temp - adding catalyst
32
How does temp increase RoR?
- increases ke - higher frequency of collisions - greater proportion successful
33
Properties of group 1
- alkaline metals - soft - low mp - react with moist air (stored in oil) - react with water to form metal hydroxide and hydrogen - react with chlorine to produce chlorides
34
Properties of group 7
- mp and bp increase as descend group - diatomic - low bp - react with G1 metals - halogen displacement reactions
35
Describe the atom
- positively charged nucleus surrounded by negatively charged electrons - nuclear radius smaller than the atom - most of mass in nucleus
36
Size of atomic molecules from smallest to biggest
Electrons Protons Neutrons
37
Relative mass of protons, neutrons and electrons
Protons: 1 Neutrons: 1 Electrons: 0.0005 or negligible
38
How is the position of an element in the periodic table related to the arrangement of electrons?
- elements in the same group have similar outer electron configurations leading to similar chemical properties
39
How do you determine the period of an element?
Number of shells
40
How are reactions of elements related to their outer electron number?
Determined by number of outer electrons involved
41
What is a limitation of the particle model when particles are inelastic?
It does not account for varying strengths of intermolecular forces between particles which play a crucial role in chemical transitions
42
Properties of diamond
- hard, strong, high melting point - each carbon forms 4 other bonds
43
Properties of graphite
- soft and slippery - layers of graphene with each carbon bonded to 3 others - 4th electron is delocalised to form weak bonds between layers
44
Properties of fullerenes
- borderless, uncharged, no unpaired electrons - unique electronic and optical properties
45
Properties of graphene
- single carbon atom thick sheet with strength and thermal conductivity
46
How big is a nanometer in regards to atoms?
Roughly the size of 10 atoms
47
How do nanoparticles react compared to their typical sized particles?
- more reactive than normal - large SA to V ratio- more opportunity for reactions to occur
48
Difference between dilute/concentrated and strong/weak
- dilute and conc refer to amount to substance - strong and weak refer to degree of ionisation
49
As hydrogen ion concentration increases by a factor of 10, what happens to the pH value?
Decreases by a factor of one
50
Exothermic vs endothermic graph
51
What happens to the potential difference of a chemical cell?
Produces PD until all reactants are used up
52
Define Avogadros constant
The number of atoms, molecules, or ions in one mole of a substance
53
Describe Haber process
- form ammonia from hydrogen and nitrogen - iron catalyst
54
Aqueous NaCL electrolysis
- water reduced at cathode as lower reduction potential than Na - chloride ions oxidised to chlorine gas at anode
55
Aqueous CuSO4 electrolysis
- Cu2+ reduced at cathode as lower reduction potential than water - H2O oxidised at anode as easier than SO42-
56
General rules of electrolysis of aqueous ionic compounds
- cations more reactive than hydrogen will not be reduced - cations less reactive than hydrogen are reduced - anions that are halides will be oxidised to halogen gasss - anions like sulfates or nitrates will not be oxidised
57
Impact of changing temp on an exothermic reaction
Increase: equilibria shift left in endothermic direction Decrease: equilibrium shift right in exothermic direction
58
Impact of changing temp on an endothermic reaction
Increase: equilibria shift right in endothermic direction Decrease: equilibria shift left in exothermic direction
59
Impact of changing conc on equilibria
Increase in reactant conc: equilibria shift right Decrease in reactant conc: equilibria shift left Increase in product conc: equilibria shift left Decrease in product conc: equilibria shift right
60
Impact of pressure on equilibria
- depends on number of moles on each side of reaction Increase: equilibria shift to side with fewest gaseous moles Decrease: equilibria shift to side with most gaseous moles
61
Draw endo and exo graphs
62
Percentage purity equation
Mass of pure chemical ——————————— x100 Total mass of sample
63
Equation to calculate an unknown mass
Mass of known ——————— x Mr unknown Mr of known (Include relevant stoichiometry)
64
Atom economy equation
Mass of desired product ———————————— x100 Total mass of products
65
What is meant by a homologous series
A group of chemicals which have similar chemical properties and can be represented by a general formula
66
Summary of galvanic cells
- electrons flow from anode to cathode (left to right) - oxidation occurs at anode and reduction at cathode - salt bridge present to complete circuit and allow current to flow
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