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Description
Flashcards by Maxime PANS, updated more than 1 year ago
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Created by Maxime PANS
almost 7 years ago
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| Question | Answer |
| Reactivity Series in the Group 1 | - Reactivity of Group 1 Metals Increases as You Go Down the Group - Each Outer Shell Contains Only One - Electron, When Group 1 Metals React, they will Lose One Outer Electron to Get a Full Outer Shell of Electrons - More shells as you go down due to more electrons - This Means that the Outer Electron is Further Away from the Nucleus so there are Weaker Electrostatic Forces of Attraction - This Requires Less Energy to Overcome the Electrostatic Forces of Attraction - Between the Negatively Charged - Electron and the Positively Charged Nucleus - This Allows the Electron to be Lost Easily, Making it More Reactive as You Go Down the Group |
| Reactivity Series in the Group 7 | - Reactivity of Group 7 Non - Metals Increases as You Go Up - Each Outer Shell Contains Seven - Electrons and When Group 7 Metals - React, they will Need to Gain One Outer Electron to Get a Full Outer Shell of Electrons - As You Go Up Group 7, the Number of Shells of Electrons Decreases (Period Number Decreases Up the Periodic Table) - This Means that the Outer Electrons are Closer to the Nucleus so there are Stronger Electrostatic Forces of Attraction that Attracts the Extra Electron Needed - This Allows the Electron to be Attracted More Readily, Making it More Reactive as You Go Up the Group |
| Potassium | REACTS WITH WATER REACTS WITH ACID |
| Sodium | REACTS WITH WATER REACTS WITH ACID |
| Lithium | REACTS WITH WATER REACTS WITH ACID |
| Calcium | REACTS WITH WATER REACTS WITH ACID |
| Magnesium | REACTS WITH ACID |
| Aluminium | REACTS WITH ACID |
| Zinc | REACTS WITH ACID |
| Iron | REACTS WITH ACID |
| Copper | REACTS WITH NOTHING |
| Silver | REACTS WITH NOTHING |
| Gold | REACTS WITH NOTHING |
| Reaction : Potassium with Water | Violently Melts into a Shiny Ball that Dashes Around the Surface Burns with a Lilac - Coloured Flame |
| Reaction : Sodium with Water | Very Quickly Bubbles of Gas Melts into a Shiny Ball that Dashes Around the Surface |
| Reaction : Lithium with Water | Quickly Bubbles of Gas |
| Reaction: Calcium with Water | More Slowly Bubbles of Gas White Precipitate Produced |
| Reaction: Potassium with Acid | Vigorously Bubbles of Gas Potassium Disappears |
| Reaction: Sodium with Acid | Vigorously Bubbles of Gas Sodium Disappears |
| Reaction: Lithium with Acid | Vigorously Bubbles of Gas Lithium Disappears |
| Reaction: Calcium with Acid | Vigorously Bubbles of Gas Calcium Disappears |
| Reaction: Magnesium with Acid | Quickly Bubbles of Gas Magnesium Disappears Exothermic Colourless Solution Formed |
| Reaction: Zinc with Acid | More More Slowly Bubbles of Gas Zinc Disappears Colourless Solution Formed |
| Reaction: Iron with Acid | More Slowly than Zinc Bubbles of Gas Iron Disappears Pale Green Solution Formed |
| The 4 Main Gases in the Air | Nitrogen - 78% Oxygen - 21% Argon - 0.94% Carbon Dioxide - 0.04% |
| Finding out the % by Volume of oxygen in the air using metals | 1. Place Wet Iron Fillings at the End of a Burette 2. Use a Clamp to Hold the Burette Vertically in the Trough of Water 3.Measure and Note the Starting Height of the Water Level in the Burette 4.Leave Apparatus for Several Days 5.Measure and Note the Final Height of the Water Level in the Burette |
| Equation to find out the % of oxygen | Volume of Oxygen used / Volume of Oxygen at the start |
| Explanation of Global Warming | 1.The Sun Emits Rays that Enters the Earth’s Atmosphere 2.The Heat is Emitted Back from the Earth’s Surface 3.Some Heat is Reflected Back Out into Space 4.But Some Heat is Absorbed by Greenhouse Gasses Such as Carbon Dioxide and is Trapped Within the Earth’s Atmosphere so Causes the Earth’s 5.Average Temperature to Rise as a Result |
| Consequences of Global Warming | 1.Climate Change due to Increase in Earth’s Temperature 2.Water Levels will Rise as Glaciers will Melt because of High Temperatures 3.Extinction of Species due to Inhabitable Environment 4.Migration of Species as they will Move to Areas that are More Habitable (No Droughts) 5.Spread of Diseases caused by the Cold Climate 6.Loss of Habitat due to Climate Change (Animals that Live on Glaciers) |
| Reactivity of Metals | Most Reactive Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Copper Silver Gold Least Reactive |
| Metal + Oxygen | Metal Oxide |
| Metal + Water | Metal Hydroxide + Hydrogen |
| Metal + Acid | Metal Hydroxide + Hydrogen |
| Metal Carbonate + Heat | Metal Oxide + Carbon Dioxide |
| Combustion with Hydrogen | Exothermic Water is Produced 2H2 + O2 → 2H2O |
| Combustion with Sulphur | Blue Flame Colourless Gas Produced S + O2 → SO2 |
| What is Rusting | Rusting is the Oxidation of Iron |
| Reaction of Rusting | Iron + Oxygen ----> iron (III) oxide Water 4Fe + 3O2 ----> 2Fe2O3 |
| Conditions that speed up Rusting | Water speeds up the process very much. Any form of water even water vapour. The more humid the place is the quicker an object will rust. |
| Barrier Methods | Barrier methods are ways that you can reduce the rate of reaction or temporarily stop the reaction from happening. These methods are called barrier methods. Paint ( Cars ) Oil/ Grease ( Bike Gears ) Plastic Coatings They work by sealing the iron away from the oxygen and water. This adds a protective coating that makes sure that the barrier method itself corrodes instead of the iron. |
| Galvanisation | Galvanising is a process where you apply a protective zinc coating to iron or steel to prevent it from rusting. You would charge the object a certain charge (e.g positive) and then the zinc metal coating would be oppositely charged (e.g negative) this caused a adhesive process which makes the thin layer. Certain objects have more use of galvanising than others. e.g Car than iron rods in concrete. |
| Sacrificial Protection | Sacrificial protection is a piece of more reactive metal (zinc) that protects the iron or steel. The zinc acts as a cathode It acts as a shield that will corrode itself but not allow the iron to by connecting itself directly or with a wire. |
| What are Displacement Reaction | Displacement reaction is a chemical reaction in which a more reactive element displaces a less reactive element from its compound. Both metals and nonmetals take part in displacement reactions. Example : Reaction of iron nails with copper sulphate solution. |
| What is Oxidation | Addition of Oxygen Or Removal of Hydrogen |
| What is Reduction | Addition of Hydrogen Or Removal of Oxygen |
| What is OIL RIG mean? | O xitation I s L oss of e- R eduction I s G ain of e- |
| Affects of Acid Rain | Iron corrodes Limestone buildings corrode Plants die Aquatic animals die |
| Crystalisation | 1.Evaporate some of the water to create a saturated solution (check using a glass rod, if crystals form on it, the solution is saturated) 2.Leave solution to cool so that crystals form – the salt is less soluble in cold water 3.Remove crystals by filtering , then leave to dry on a filter paper. |
| Why do we always add excess? | to ensure that the other reagent has fully reacted. The excess can be removed by filtration. |
| What does RAM stand for? | Relative Atomic Mass |
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