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261 Cards in this Set
- Front
- Back
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Halogens are ........ molecules? Halogens are bonded by ? |
Diatomic Single Covalent bond |
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What is the appearance of these halogens at room temp? Fluorine Chlorine Bromine Iodine |
F - pale yellow gas Cl - Green gas Br - dark red volatile liquid I - grey solid |
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Name 4 of the trends as you go down the group of halogens? |
•Become Darker
•Melting & boiling points increase
•Change from gas to liquid to solid at Room Temp.
•Become less volatile |
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What is the property that has no trend for the halogens |
Their Solubility in water |
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Where are Halogens most soluble? |
In Organic Solvents, Hexane ; Cyclohexane |
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What is the most reactive halogen? |
Fluorine |
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Why are smaller halogens more reactive than larger halogens |
Because the nucleus in a smaller halogen is closer to the outer shell. Meaning less nuclear shielding occurs so the positive attraction is stronger to be able to attract an extra electron |
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If a Solution of chlorine reacts with potassium iodide ions. What is produced? What is the colour change? What is the oxidising agent? |
• Potassium Chloride and Iodine • Pale Green > Brown • Chlorine, each atom gains an electron. So it is said to be reduced |
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How do displacement reactions work? What type of a reaction is it? |
• The more reactive halogen displaces a less reactive halogen from a compound. • A Redox Reaction |
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How do u test for Halide ions? |
Add Silver solution and a coloured precipitate will be formed. |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What coloured precipitates are formed from Halide ions?
• Chlorine • Bromine • Iodine |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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Oxidation states tell us... |
How many electrons have been lost or gained compared to an unreacted element |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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Oxidation states tell us... |
How many electrons have been lost or gained compared to an unreacted element |
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Oxidation States are useful for... |
• Naming Inorganic Compounds • Identifying Oxidising & Reducing Agents • Balancing Redox Reactions |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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Oxidation states tell us... |
How many electrons have been lost or gained compared to an unreacted element |
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Oxidation States are useful for... |
• Naming Inorganic Compounds • Identifying Oxidising & Reducing Agents • Balancing Redox Reactions |
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What is the Oxidation State of? PO4^-3 |
Oxygen= -2 x 4 = -8 P-8 = 3 P = 5 |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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Oxidation states tell us... |
How many electrons have been lost or gained compared to an unreacted element |
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Oxidation States are useful for... |
• Naming Inorganic Compounds • Identifying Oxidising & Reducing Agents • Balancing Redox Reactions |
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What is the Oxidation State of? PO4^-3 |
Oxygen= -2 x 4 = -8 P-8 = 3 P = 5 |
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Name the two versions of Sodium Nitrate? NaNO3 & NaNO2? |
NaNO3- Na = +1 N = +5 O3 = -6 Sodium Nitrate (V) NaNO2 Na = +1 N = +3 O2 = -4 Sodium Nitrate (III) |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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What is Electrolysis? |
The movement of ions therefore it can't take place with a solid |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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Oxidation states tell us... |
How many electrons have been lost or gained compared to an unreacted element |
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Oxidation States are useful for... |
• Naming Inorganic Compounds • Identifying Oxidising & Reducing Agents • Balancing Redox Reactions |
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What is the Oxidation State of? PO4^-3 |
Oxygen= -2 x 4 = -8 P-8 = 3 P = 5 |
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Name the two versions of Sodium Nitrate? NaNO3 & NaNO2? |
NaNO3- Na = +1 N = +5 O3 = -6 Sodium Nitrate (V) NaNO2 Na = +1 N = +3 O2 = -4 Sodium Nitrate (III) |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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What is Electrolysis? |
The movement of ions therefore it can't take place with a solid |
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What moves to the cathode in electrolysis? What moves to the anode in electrolysis? And what happens at each electrode? |
Cations/ Pos. ions move to the cathode to gain electrons (reduced) Anions/ Neg. ions move to the anode to lose electrons (oxidised) |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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Oxidation states tell us... |
How many electrons have been lost or gained compared to an unreacted element |
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Oxidation States are useful for... |
• Naming Inorganic Compounds • Identifying Oxidising & Reducing Agents • Balancing Redox Reactions |
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What is the Oxidation State of? PO4^-3 |
Oxygen= -2 x 4 = -8 P-8 = 3 P = 5 |
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Name the two versions of Sodium Nitrate? NaNO3 & NaNO2? |
NaNO3- Na = +1 N = +5 O3 = -6 Sodium Nitrate (V) NaNO2 Na = +1 N = +3 O2 = -4 Sodium Nitrate (III) |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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What is Electrolysis? |
The movement of ions therefore it can't take place with a solid |
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What moves to the cathode in electrolysis? What moves to the anode in electrolysis? |
Cations/ Pos. ions move to the cathode to gain electrons (reduced) Anions/ Neg. ions move to the anode to lose electrons (oxidised) |
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What happens when PbBr2 (molten lead bromide) is electrolysed? |
•At the anode bromide ions lose electrons and are oxidised •At the cathode lead ions gain electrons and are reduced |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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Oxidation states tell us... |
How many electrons have been lost or gained compared to an unreacted element |
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Oxidation States are useful for... |
• Naming Inorganic Compounds • Identifying Oxidising & Reducing Agents • Balancing Redox Reactions |
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What is the Oxidation State of? PO4^-3 |
Oxygen= -2 x 4 = -8 P-8 = 3 P = 5 |
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Name the two versions of Sodium Nitrate? NaNO3 & NaNO2? |
NaNO3- Na = +1 N = +5 O3 = -6 Sodium Nitrate (V) NaNO2 Na = +1 N = +3 O2 = -4 Sodium Nitrate (III) |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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What is Electrolysis? |
The movement of ions therefore it can't take place with a solid |
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What moves to the cathode in electrolysis? What moves to the anode in electrolysis? |
Cations/ Pos. ions move to the cathode to gain electrons (reduced) Anions/ Neg. ions move to the anode to lose electrons (oxidised) |
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What happens when PbBr2 (molten lead bromide) is electrolysed? |
•At the anode bromide ions lose electrons and are oxidised •At the cathode lead ions gain electrons and are reduced |
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What impurities are made by the electrolysis of lead bromide |
Molten Lead metal at the bottom of the container |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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Oxidation states tell us... |
How many electrons have been lost or gained compared to an unreacted element |
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Oxidation States are useful for... |
• Naming Inorganic Compounds • Identifying Oxidising & Reducing Agents • Balancing Redox Reactions |
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What is the Oxidation State of? PO4^-3 |
Oxygen= -2 x 4 = -8 P-8 = 3 P = 5 |
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Name the two versions of Sodium Nitrate? NaNO3 & NaNO2? |
NaNO3- Na = +1 N = +5 O3 = -6 Sodium Nitrate (V) NaNO2 Na = +1 N = +3 O2 = -4 Sodium Nitrate (III) |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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What is Electrolysis? |
The movement of ions therefore it can't take place with a solid |
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What moves to the cathode in electrolysis? What moves to the anode in electrolysis? |
Cations/ Pos. ions move to the cathode to gain electrons (reduced) Anions/ Neg. ions move to the anode to lose electrons (oxidised) |
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What happens when PbBr2 (molten lead bromide) is electrolysed? |
•At the anode bromide ions lose electrons and are oxidised •At the cathode lead ions gain electrons and are reduced |
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What impurities are made by the electrolysis of lead bromide |
Molten Lead metal at the bottom of the container |
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What are electrodes made of? And Why? |
Graphite & Platinum Because they are inert/unreactive |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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Oxidation states tell us... |
How many electrons have been lost or gained compared to an unreacted element |
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Oxidation States are useful for... |
• Naming Inorganic Compounds • Identifying Oxidising & Reducing Agents • Balancing Redox Reactions |
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What is the Oxidation State of? PO4^-3 |
Oxygen= -2 x 4 = -8 P-8 = 3 P = 5 |
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Name the two versions of Sodium Nitrate? NaNO3 & NaNO2? |
NaNO3- Na = +1 N = +5 O3 = -6 Sodium Nitrate (V) NaNO2 Na = +1 N = +3 O2 = -4 Sodium Nitrate (III) |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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What is Electrolysis? |
The movement of ions therefore it can't take place with a solid |
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What moves to the cathode in electrolysis? What moves to the anode in electrolysis? |
Cations/ Pos. ions move to the cathode to gain electrons (reduced) Anions/ Neg. ions move to the anode to lose electrons (oxidised) |
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What happens when PbBr2 (molten lead bromide) is electrolysed? |
•At the anode bromide ions lose electrons and are oxidised •At the cathode lead ions gain electrons and are reduced |
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What impurities are made by the electrolysis of lead bromide |
Molten Lead metal at the bottom of the container |
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What are electrodes made of? And Why? |
Graphite & Platinum Because they are inert/unreactive |
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What are the usual products for the electrolysis of a molten salt? |
At the Cathode: A metal At the Anode: A Non-Metal ; apart from Hydrogen. |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What have variable Oxidation numbers? |
Transition Metals |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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Oxidation states tell us... |
How many electrons have been lost or gained compared to an unreacted element |
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Oxidation States are useful for... |
• Naming Inorganic Compounds • Identifying Oxidising & Reducing Agents • Balancing Redox Reactions |
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What is the Oxidation State of? PO4^-3 |
Oxygen= -2 x 4 = -8 P-8 = 3 P = 5 |
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Name the two versions of Sodium Nitrate? NaNO3 & NaNO2? |
NaNO3- Na = +1 N = +5 O3 = -6 Sodium Nitrate (V) NaNO2 Na = +1 N = +3 O2 = -4 Sodium Nitrate (III) |
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What coloured precipitates are formed from Halide ions? • Chlorine • Bromine • Iodine |
Silver Chloride- White Silver Bromide- Cream Silver Iodide- Pale Yellow |
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What is Electrolysis? |
The movement of ions therefore it can't take place with a solid |
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What moves to the cathode in electrolysis? What moves to the anode in electrolysis? |
Cations/ Pos. ions move to the cathode to gain electrons (reduced) Anions/ Neg. ions move to the anode to lose electrons (oxidised) |
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What happens when PbBr2 (molten lead bromide) is electrolysed? |
•At the anode bromide ions lose electrons and are oxidised •At the cathode lead ions gain electrons and are reduced |
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What impurities are made by the electrolysis of lead bromide |
Molten Lead metal at the bottom of the container |
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What are electrodes made of? And Why? |
Graphite & Platinum Because they are inert/unreactive |
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What are the usual products for the electrolysis of a molten salt? |
At the Cathode: A metal At the Anode: A Non-Metal ; apart from Hydrogen. |
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The Electrolysis of water produces what at each electrode? |
Water is reduced at the cathode: Hydrogen given off and (OH) ions are made
Water is oxidised at the anode: Oxygen is given off and H+ ions are made |
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Oxidation is... |
• A reaction involving the loss of electrons • The gain of oxygen • Increase in oxidation number state • Loss of Hydrogen |
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Reduction is... |
•A reaction involving the gain of electrons • Loss of Oxygen • Decrease in Oxidation state • Gain of Hydrogen |
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What is the oxidation number of something in its elemental state? |
0 |
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What moves to the cathode in electrolysis? What moves to the anode in electrolysis? And what happens at each electrode |
Cations/ Pos. ions move to the cathode to gain electrons (reduced) Anions/ Neg. ions move to the anode to lose electrons (oxidised) |
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What is the Oxidation Number of.... Fluorine Group 1 Oxygen Group 2 Chlorine Hydrogen |
F = -1 G1= +1 O = -2 G2 = +2 Cl = -1 H = +1 |
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Oxidation states tell us... |
How many electrons have been lost or gained compared to an unreacted element |
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Oxidation States are useful for... |
• Naming Inorganic Compounds • Identifying Oxidising & Reducing Agents • Balancing Redox Reactions |
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What are the usual products at each electrode for the electrolysis of a molten salt? |
At the Cathode: A metal At the Anode: A Non-Metal ; apart from Hydrogen. |
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Name the two versions of Sodium Nitrate? NaNO3 & NaNO2? |
NaNO3- Na = +1 N = +5 O3 = -6 Sodium Nitrate (V) NaNO2 Na = +1 N = +3 O2 = -4 Sodium Nitrate (III) |
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Electrolysis of Solutions: At the cathode there will be....
Products at the cathode are.... |
1) Metal ions from the salt & water the salt is dissolved in
2) Less Reactive Metals are plated on the cathode (Copper) • Reactive Metals remain as ions and Hydrogen is produced by the reduction of water. |
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Electrolysis of Solutions: At the cathode there will be....
Products at the cathode are.... |
1) Metal ions from the salt & water the salt is dissolved in
2) Less Reactive Metals are plated on the cathode (Copper) • Reactive Metals remain as ions and Hydrogen is produced by the reduction of water. |
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Electrolysis of solutions: At the Anode there will be....
Products at the Anode are.... |
1) There will be Neg. ions from the salt & the water the salt is dissolved in.
2) Halogen is produced by the halide ions as they are more likely to be oxidised than water. (EG: fluorine & bromine) •Other Neg. ions, allow water to be oxidised and oxygen produced. (EG: Nitrates & Sulfates ) |
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Electrolysis of Solutions: At the cathode there will be....
Products at the cathode are.... |
1) Metal ions from the salt & water the salt is dissolved in
2) Less Reactive Metals are plated on the cathode (Copper) • Reactive Metals remain as ions and Hydrogen is produced by the reduction of water. |
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Electrolysis of solutions: At the Anode there will be....
Products at the Anode are.... |
1) There will be Neg. ions from the salt & the water the salt is dissolved in.
2) Halogen is produced by the halide ions as they are more likely to be oxidised than water. (EG: fluorine & bromine) •Other Neg. ions, allow water to be oxidised and oxygen produced. (EG: Nitrates & Sulfates ) |
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What happens to the anode and the cathode of Electrolysis involving Copper electrodes in Copper sulfate solution? |
The anode loses mass because the copper atoms turn to ions in the solution The Cathode gains Copper as it is deposited so that the concentration of solution remains constant |
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Equilibrium is...
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Established in a closed system when molecules enter and leave at the same rate |
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Equilibrium is...
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Established in a closed system when molecules enter and leave at the same rate |
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Dynamic equilibrium is.... |
•The rate of the forward reaction is equal to the backwards reaction. •It is a reversible change •The concentrations of reactants & products stay constant |
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Equilibrium is...
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Established in a closed system when molecules enter and leave at the same rate |
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Dynamic equilibrium is.... |
•The rate of the forward reaction is equal to the backwards reaction. •It is a reversible change •The concentrations of reactants & products stay constant |
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How does the colour of the reaction develop between hydrogen and iodine? |
• Purple colour originally given off by iodine becomes paler as the forward reaction occurs.
• The depth of purple colour will stay constant when equilibrium is reached |
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At equilibrium the concentration of reactants and products don't need to be the same. Give an example of this... |
Hydrogen + iodine > Hydrogen iodide |
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At equilibrium the concentration of reactants and products don't need to be the same. Give an example of this... |
Hydrogen + iodine > Hydrogen iodide |
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Kc is what ? |
Equilibrium Constant |
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At equilibrium the concentration of reactants and products don't need to be the same. Give an example of this... |
Hydrogen + iodine > Hydrogen iodide |
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Kc is what ? |
Equilibrium Constant |
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Equilibrium Constant:
Kc = ............./............... |
Products / Reactants |
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If Kc > 0 what does it mean? |
The position of equilibrium is towards the products |
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If Kc > 0 what does it mean? |
The position of equilibrium is towards the products |
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What do we have to do to work out the units of Kc? |
Sub mol/dm^3 in the equation for each reactant and product |
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State Le Chatalier's Principle |
It states that if a system is at equilibrium and a change is made to any of the conditions then the system responds to counteract the change as much as possible |
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State Le Chatalier's Principle |
It states that if a system is at equilibrium and a change is made to any of the conditions then the system responds to counteract the change as much as possible |
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How do Catalysts affect equilibrium position? |
Catalysts don't affect the position of equilibrium. They only affect the speed of attainment of equilibrium |
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How does temp. affect the equilibrium in an.... Exothermic reaction
Endothermic reaction |
Exo- If temp. is increased less product is formed • If temp. is reduced more product is formed.
Endo- If temp. is increased more product is formed • If temp. is reduced less product is formed. |
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How does temp. affect the equilibrium in an.... Exothermic reaction
Endothermic reaction |
Exo- If temp. is increased less product is formed • If temp. is reduced more product is formed.
Endo- If temp. is increased more product is formed • If temp. is reduced less product is formed. |
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How does concentration affect the position of equilibrium? |
If the concentration of reactants is increased more product is formed. If the concentration of the products is increased the less product formed the more reactant there are. |
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How does pressure affect equilibrium? |
If the pressure of gas is increased then the position of equilibrium will move in the direction where there are less gas moles to reduce pressure again. |
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Kc is affected by..... Kc is not affected by..... |
• Temperature • Conc. & Pressure so long as equilibrium is allowed to be established |
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What is chlorine? What does it irritate? What happens if it is inhaled at concentrations above 40ppm |
• A toxic gas, detectable by smell at 1ppm • It irritates the eyes, skin &a respiratory system. • It reacts in the lungs to form HCl, damages lung tissue, essentially causes drowning as liquid floods the lungs |
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What is chlorine? What does it irritate? What happens if it is inhaled at concentrations above 40ppm |
• A toxic gas, detectable by smell at 1ppm • It irritates the eyes, skin &a respiratory system. • It reacts in the lungs to form HCl, damages lung tissue, essentially causes drowning as liquid floods the lungs |
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How is Chlorine transported? & Why this way? |
• As a liquid • Because more can be stored in a fixed volume as a liquid under pressure than as a gas |
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What is chlorine? What does it irritate? What happens if it is inhaled at concentrations above 40ppm |
• A toxic gas, detectable by smell at 1ppm • It irritates the eyes, skin &a respiratory system. • It reacts in the lungs to form HCl, damages lung tissue, essentially causes drowning as liquid floods the lungs |
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How is Chlorine transported? & Why this way? |
• As a liquid • Because more can be stored in a fixed volume as a liquid under pressure than as a gas |
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What safety features are taken to prevent chlorine causing havoc? |
• Tanks have pressure release devices, to release some chlorine as a gas in order to vent the tank. • Inside of the tank kept dry because if it reacted with water then it would form corrosive acids • An excess flow valve needed in case chlorine leaving the tank exceeds a predetermined value |
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What is chlorine? What does it irritate? What happens if it is inhaled at concentrations above 40ppm |
• A toxic gas, detectable by smell at 1ppm • It irritates the eyes, skin &a respiratory system. • It reacts in the lungs to form HCl, damages lung tissue, essentially causes drowning as liquid floods the lungs |
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How is Chlorine transported? & Why this way? |
• As a liquid • Because more can be stored in a fixed volume as a liquid under pressure than as a gas |
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What safety features are taken to prevent chlorine causing havoc? |
• Tanks have pressure release devices, to release some chlorine as a gas in order to vent the tank. • Inside of the tank kept dry because if it reacted with water then it would form corrosive acids • An excess flow valve needed in case chlorine leaving the tank exceeds a predetermined value |
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A method used to check if Chlorine is leaking? |
Use a stick with cloth soaked in conc. ammonia solution over the end. If chlorine was leaking a white cloud of Ammonium Chloride would be seen |
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What is chlorine? What does it irritate? What happens if it is inhaled at concentrations above 40ppm |
• A toxic gas, detectable by smell at 1ppm • It irritates the eyes, skin &a respiratory system. • It reacts in the lungs to form HCl, damages lung tissue, essentially causes drowning as liquid floods the lungs |
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How is Chlorine transported? & Why this way? |
• As a liquid • Because more can be stored in a fixed volume as a liquid under pressure than as a gas |
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What safety features are taken to prevent chlorine causing havoc? |
• Tanks have pressure release devices, to release some chlorine as a gas in order to vent the tank. • Inside of the tank kept dry because if it reacted with water then it would form corrosive acids • An excess flow valve needed in case chlorine leaving the tank exceeds a predetermined value |
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A method used to check if Chlorine is leaking? |
Use a stick with cloth soaked in conc. ammonia solution over the end. If chlorine was leaking a white cloud of Ammonium Chloride would be seen |
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Two uses of Chlorine are? |
• Water treatment, where it is added to kill bacteria • Household Bleach to remove stains from clothing |
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What is chlorine? What does it irritate? What happens if it is inhaled at concentrations above 40ppm |
• A toxic gas, detectable by smell at 1ppm • It irritates the eyes, skin &a respiratory system. • It reacts in the lungs to form HCl, damages lung tissue, essentially causes drowning as liquid floods the lungs |
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How is Chlorine transported? & Why this way? |
• As a liquid • Because more can be stored in a fixed volume as a liquid under pressure than as a gas |
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What safety features are taken to prevent chlorine causing havoc? |
• Tanks have pressure release devices, to release some chlorine as a gas in order to vent the tank. • Inside of the tank kept dry because if it reacted with water then it would form corrosive acids • An excess flow valve needed in case chlorine leaving the tank exceeds a predetermined value |
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A method used to check if Chlorine is leaking? |
Use a stick with cloth soaked in conc. ammonia solution over the end. If chlorine was leaking a white cloud of Ammonium Chloride would be seen |
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Two uses of Chlorine are? |
• Water treatment, where it is added to kill bacteria • Household Bleach to remove stains from clothing |
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What is the equation to make bleach using chlorine? |
Cl2 + 2NaOH > 2NaClO + H2 Sodium Chlorate ^ |
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What is the equation to make bleach using chlorine? |
Cl2 + 2NaOH > 2NaClO + H2 Sodium Chlorate ^ |
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How much % of NaClO is used in Household Bleach products? |
5% |
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What is the equation to make bleach using chlorine? |
Cl2 + 2NaOH > 2NaClO + H2 Sodium Chlorate ^ |
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How much % of NaClO is used in Household Bleach products? |
5% |
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How do you determine the accurate concentration of NaClO? |
Iodine-Thiosulfate Titration Redox Titration |
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What is the equation to make bleach using chlorine? |
Cl2 + 2NaOH > 2NaClO + H2 Sodium Chlorate ^ |
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How much % of NaClO is used in Household Bleach products? |
5% |
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How do you determine the accurate concentration of NaClO? |
Iodine-Thiosulfate Titration Redox Titration |
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What are iodine-thiosulfate Titrations used for... |
To find the conc. of a chemical that is a strong enough oxidising agent to oxidise iodide ions. |
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What is the equation to make bleach using chlorine? |
Cl2 + 2NaOH > 2NaClO + H2 Sodium Chlorate ^ |
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How much % of NaClO is used in Household Bleach products? |
5% |
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How do you determine the accurate concentration of NaClO? |
Iodine-Thiosulfate Titration Redox Titration |
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What are iodine-thiosulfate Titrations used for... |
To find the conc. of a chemical that is a strong enough oxidising agent to oxidise iodide ions. |
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In Case of Bleach, excess iodide ions are added to chlorate ions. What colour is shown? |
Iodine, Chlorine ions & water are produced. Showing a brown colour |
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How can the iodine be titrated? What is the colour change? How is the end point of this titration identified? |
• Using thiosulfate ions • Brown > Pale Yellow • Using Starch solution, when the final trace of Blue/Black colour is no longer visible. |
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How can the iodine be titrated? What is the colour change? How is the end point of this titration identified? |
• Using thiosulfate ions • Brown > Pale Yellow • Using Starch solution, when the final trace of Blue/Black colour is no longer visible. |
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What is Atom Economy ? |
It's the % of reactant atoms ending up as the desired product |
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The Equation for atom economy is..... |
Relative Formula Mass of desired product --------------------------------- x100 Relative formula mass of all reactants used |
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The Equation for atom economy is..... |
Relative Formula Mass of desired product --------------------------------- x100 Relative formula mass of all reactants used |
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Fluorine Atoms have the greatest tendency to be ........
Making them great .............. agents |
Reduced / gain electrons
Oxidising Agents |
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The Equation for atom economy is..... |
Relative Formula Mass of desired product --------------------------------- x100 Relative formula mass of all reactants used |
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Fluorine Atoms have the greatest tendency to be ........
Making them great .............. agents |
Reduced / gain electrons
Oxidising Agents |
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What is made when Sodium Fluoride & Sodium Chloride react with Conc. Acid.
What is produced when they meet moist air? |
Hydrogen Fluoride Hydrogen Chloride
White Fumes as tiny droplets of HCl are made |
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The Equation for atom economy is..... |
Relative Formula Mass of desired product --------------------------------- x100 Relative formula mass of all reactants used |
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Fluorine Atoms have the greatest tendency to be ........
Making them great .............. agents |
Reduced / gain electrons
Oxidising Agents |
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What is made when Sodium Fluoride & Sodium Chloride react with Conc. Acid.
What is produced when they meet moist air? |
Hydrogen Fluoride Hydrogen Chloride
White Fumes as tiny droplets of HCl are made |
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What is made when Sodium Bromide reacts with Conc. sulfuric acid.
However what extra product is produced and why? |
•Hydrogen Bromide
•Sulfur Dioxide because Bromide ions are strong enough reducing agents to reduce the sulfuric acid. |
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The Equation for atom economy is..... |
Relative Formula Mass of desired product --------------------------------- x100 Relative formula mass of all reactants used |
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All Hydrogen Halides react with Ammonia to make....
What happens when a glass rod dipped in Conc. Ammonia Solution is placed in a Hydrogen Halide? |
Salts
A white cloud of Ammonium Halide |
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What happens when hydrogen halides react with H2SO4 and why? |
HF & HCl- Don't react HBr- Makes sulphur dioxide HI- Makes Hydrogen sulfide |
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What is made when Sodium Bromide reacts with Conc. sulfuric acid.
However what extra product is produced and why? |
•Hydrogen Bromide
•Sulfur Dioxide because Bromide ions are strong enough reducing agents to reduce the sulfuric acid. |
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What is made when Sodium Fluoride & Sodium Chloride react with Conc. Acid.
What is produced when they meet moist air? |
Hydrogen Fluoride Hydrogen Chloride
White Fumes as tiny droplets of HCl are made |
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What is made when Sodium Bromide reacts with Conc. sulfuric acid.
However what extra product is produced and why? |
•Hydrogen Bromide
•Sulfur Dioxide because Bromide ions are strong enough reducing agents to reduce the sulfuric acid. |
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Sodium Iodide added to conc. sulfuric acid produces what? |
Hydrogen Iodide & Hydrogen sulfide gas
H2S formed because Iodide ions are even stronger reducing agents. |
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How do u make each hydrogen halide in a lab? Hydrogen chloride Hydrogen Bromide Hydrogen Iodide |
• Conc. H2SO4 + NaCl to make HCl • Conc. Phosphoric acid is used to make HBr and HI • Because unlike H2SO4 the phosphoric acid will not be reduced so a pure hydrogen halide will be formed. |
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What happens to the thermal stability of Hydrogen Halides. |
• Decreases as you go down G7 • Bond strength between hydrogen-halogen decreases as you go down G7 |
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Are Hydrogen Halides broken down by heating in the lab? |
• Hydrogen Fluoride & Chloride isn't broken down into separate elements • HBr is strongly heated, some brown Br gas is made • HI if a red hot needle is plunged into it then purple gaseous iodine is made. |
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Why are very soluble hydrogen halides acidic? What is the exception? |
• There is almost 100% dissociation • Apart from HF |
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What do all acidic solutions have? |
H+ (aq) ions or H3O+ ions |
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Why was the Deacon Process developed? |
To counter the problem of HCl being produced by the demand of alkalis |
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Why was the Deacon Process developed? |
To counter the problem of HCl being produced by the demand of alkalis |
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What does the process involve? |
HCl mixing with oxygen and being passed over a catalyst |
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Why was the Deacon Process developed? |
To counter the problem of HCl being produced by the demand of alkalis |
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What does the process involve? |
HCl mixing with oxygen and being passed over a catalyst |
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What are the products of the process? Why was one of them a useful product? |
• Chlorine and Steam • Chlorine in demand for bleaching paper & fabrics |
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In theory how is the best yield obtained? However why are compromises made in chemical plants? |
•Best yield obtained using high pressure, low temp. & excess oxygen • compromise made based on the rate of reaction, the cost & the safety |
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How has the process been developed to work in the present day? |
To produce pure chlorine whilst operating at low temp. & low cost |
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What is the products of the process used for? |
• The chlorine is used as feedstock • The HCl produced can be turned in Hydrochloric acid Or • Recycled through the process again being used as chlorine in step 1 |
