1
Q
How many outer electrons does oxygen have?
A
6
2
Q
How many more electrons does oxygen need?
A
2 to complete their outer shell
3
Q
What does the oxygen atom do in oxygen gas?
A
Share two pages of electrons with another
4
Q
What does this form?
A
A double covalent bond
5
Q
What does this look like?
A
O=O
6
Q
Page 13
A
Ok
CGP GCSE Chem
flashcards
Decks in class (233)
# Cards
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The Three States of Matter - Solid, Liquid and Gas16
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Substances Can Change from One State to Another12
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Diffusion is the Movement of Particles Through a Liquid or Gas2
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Potassium Manganate(VII) and Water5
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Ammonia and Hydrogen Chloride8
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Bromine Gas and Air5
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The Nucleus5
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The Electrons8
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Number of Electrons Equals Number of Protons4
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Atomic Number and Mass Number Describe an Atom7
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Molecules are Groups of Atoms3
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Elements Consist of One Type of Atom Only4
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Compounds are Chemically Bonded6
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Mixtures are Easily Separated - Not Like Compounds6
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Filtration is Used to Separate an Insoluble Solid from a Liquid5
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Crystallisation is Used to Separate a Soluble Solid from a Solution6
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You Can Use Filtration and Crystallisation to Separate Rock Salt10
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You Need to Know How to Do Paper Chromatography9
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How Chromatography Separates Mixtures...3
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Chromatography Can Help You to Identify Dyes4
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Simple Distillation is Used to Separate Out Solutions8
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Fractional Distillation is Used to Separate a Mixture of Liquids9
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The Periodic Table is a Table of All Known Elements13
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Elements in a Group Have the Same Number of Outer Electrons6
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Electron Shell Rules:7
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Follow the Rules to Work Out Electronic Configurations2
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Ionic Bonding - Transfer of Electrons5
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A Shell with Just One Electron is Well Keen to Get Rid...4
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A Nearly Full Shell is Well Keen to Get That Extra Electron...6
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Groups 1, 2, 6 and 7 are Most Likely to Form Ions10
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Ionic Compounds All Form in a Similar Way7
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Giant Ionic Structures Have High Melting and Boiling Points7
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A Covalent Bond is a Shared Pair of Electrons5
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Hydrogen, H24
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Chlorine, Cl23
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Hydrogen Chloride, HCI2
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Ammonia, NH34
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Nitrogen, N24
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Water, H204
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Oxygen, O26
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Carbon Dioxide, CO25
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Methane, CH43
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Ethane, C2H63
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Ethene, C2H44
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Simple Molecular Substances6
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Giant Covalent Structures6
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Diamond5
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Graphite5
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Equations Show the Reactants and Products of a Reaction7
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Symbol Equations Need to Be Balanced3
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Method: Balance just ONE type of atom at a time4
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Isotopes are the Same Except for an Extra Neutron or Two6
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Relative Atomic Mass Takes All Stable Isotopes into Account8
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Relative Formula Mass, Mr3
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Finding the Empirical Formula (from Masses of Percentages)7
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The Empirical Formula isn’t Always the Same as the Molecular Formula4
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The Three Important Steps - Not to be Missed...7
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Percentage Yield Compares Actual and Theoretical Yield7
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‘The Mole’ is Simply the Name Given to a Certain Number6
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Nice Easy Formula for Finding the Number of Moles in a Given Mass:1
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Salts Can be Anhydrous or Hydrated6
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You Can Calculate How Much Water of Crystallisation a Salt Contains5
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Avogadro’s Law - One Mole of Any Gas Occupies 24 dm35
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You Can Calculate Volumes in Reactions If You Know the Masses3
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Concentration is the ‘Amount of Stuff’ per Unit Volume4
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Concentration = No. of Moles / Volume2
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Converting Moles per dm3 to Grams per dm33
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Electric Current is a Flow of Electrons or Ions4
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Ionic Compounds Only Conduct Electricity when Molten or in Solution5
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Covalent Compounds Don't Conduct Electricity3
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Metals are Held Together by Metallic Bonding3
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Metals are Good Conductors of Electricity and Heat1
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Most Metals are Malleable2
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Electrolysis is Used to Make New Substances7
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Electrolytes are Liquids that Conduct Electricity4
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In Molten Ionic Compounds There’s Only One Source of Ions15
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Electrolysis of Aqueous Solutions is a Bit More Complicated5
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Sulfuric Acid:8
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Sodium Chloride:8
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Copper(III) Sulfate:8
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No. Of Electrons Transferred Increases with Time and Current3
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Coulombs and Faradays are Amounts of Electricity4
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One Mole of Product Needs ‘n’ Moles of Electrons4
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Use These Steps in Calculations5
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Periods3
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Groups5
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The Elements can be Classified as Metals or Non-Metals9
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Group 0 Elements are All Inert, Colourless Gases5
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Group 1 Elements All React in a Similar Way with Water8
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Group 1 Elements Become More Reactive Down the Group8
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Atoms Lose Electrons More Easily Down the Group5
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Halogen - Seven Letters - Group 78
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Hydrogen Chloride Gas Dissociates in Water...6
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...but Not in Methylbenzene3
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More Reactive Halogens will Displace Less Reactive Ones11
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Halogen Displacement Reactions Involve Transfer of Electrons8
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Acid + Metal -> Salt + Hydrogen9
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The Name of the Salt Depends on the Metal and Acid Used5
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Metals Also React with Water6
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The Reactivity Series - How Well a Metal Reacts5
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A More Reactive Metal Displaces a Less Reactive Metal8
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Iron and Steel Corrode to Make Rust5
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There are Two Main Ways to Prevent Rusting6
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The Atmosphere is Mostly Nitrogen and Oxygen1
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You can Investigate the Proportion of Oxygen in the Atmosphere Using Copper7
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You can Investigate the Proportion of Oxygen in the Atmosphere Using Iron or Phosphorus11
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You Can Make O2 in the Lab10
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When you Burn Something it Reacts with Oxygen in Air3
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Magnesium4
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Carbon5
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Sulfur5
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You Can Collect Gases in a Test Tube7
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Dilute Acid reacts with Calcium Carbonate to Produce Carbon Dioxide5
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The Thermal Decomposition of Metal Carbonates Also Produces CO27
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CO2 is used in Fizzy Drinks and Fire Extinguishers10
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Carbon Dioxide is a Greenhouse Gas5
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Increasing Carbon Dioxide is Linked to Climate Change3
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Flame Tests Identify Metals Ions7
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Some Metals Form a Coloured Precipitate with NaOH7
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‘Ammonium Compound + NaOH’ Gives off (Stinky) Ammonia6
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Hydrochloric Acid Can Help Detect Carbonates6
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Test for Sulfates with HCI and Barium Chloride5
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Test for Halides (Cl-, Brx, l-) with Nitric Acid and Silver Nitrate9
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There are Tests for 5 Common Gases5
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Wet Copper(II) Sulfate is Blue - Dry Copper(II) Sulfate is White9
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Alkanes are Hydrocarbons4
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MethAne Formula: CH41
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EthAne Formula: C2H61
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PropAne Formula: C3H81
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ButAne Formula: C4H101
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PentAne Formula: C5H121
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Alkanes are a Homologous Series8
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Complete Combustion Happens When There’s Plenty of Oxygen4
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Incomplete Combustion of Alkanes is NOT Safe5
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Halogens React with Alkanes to make Haloalkanes5
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Alkenes Have a C=C Double Bond4
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EthEne Formula: C2H41
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PropEne Formula: C3H61
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ButEne Formula: C4H84
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Halogens React with Alkanes, Forming Haloalkanes8
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Ethanol Can Be Produced from Ethene and Steam8
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Ethanol Can Also be Produced by Fermentation5
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Both Methods have Advantages and Disadvantages...8
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Ethanol can be Dehydrated to Form Ethene5
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The pH Scale Goes from 0 to 148
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An Indicator is Just a Dye That Changes Colour6
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Acids can be Neutralised by Bases (or Alkalis)7
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Acids react with Metal Oxides to make Salt + Water...9
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... and with Metal Carbonates to give Salt + Water + Carbon Dioxide5
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Salts can be Soluble or Insoluble6
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Making Soluble Salts Using Acids and Insoluble Bases6
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Making Soluble Salts Using an Alkali5
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Making Insoluble Salts - Precipitation Reactions3
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Titrations are Used to Find about Concentrations13
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The Calculation - Work Out the Number of Moles4
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Reactions Can Go at All Sorts of Different Rates3
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The Rate of a Reaction Depends on Four Things:4
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Typical Graphs for Rate of Reaction8
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Three Ways to Measure the Speed of a Reaction3
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Precipitation5
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Change in Mass (Usually Gas Given Off)6
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The Volume of Gas Given Off5
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Reaction of Hydrochloric Acid and Marble Chips7
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This graph shows the effect of using finer particles of solid4
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Reaction of Magnesium Metal with Dilute HCl4
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This graph shows the effect of using more concentrated acid solutions7
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Sodium Thiosulfate and HCl Produce a Cloudy Precipitate12
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The Decomposition of Hydrogen Peroxide9
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More Collisions Increases the Rate of Reaction2
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Higher Temperatures2
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Higher Concentration (or PRESSURE)3
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Larger Surface Area2
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Catalysts2
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Faster Collisions Increase the Rate of Reaction6
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Energy Must Always be Supplied to Break Bonds3
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In an Exothermic Reaction, Energy is Given Out2
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In an Endothermic Reaction, Energy is Taken In2
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The Change in Energy is Called the Enthalpy Change6
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Energy Level Diagrams Show if it’s Exo- or Endo- thermic12
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The Activation Energy is Lowered by Catalysts5
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Bond Energy - The Amount of Energy in a Bond5
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Example: The Formation of HCl3
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You can find out Enthalpy Changes using Calorimetry1
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Calorimetry - Dissolving, Displacement and Neutralisation Reactions5
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Calorimetry - Combustion11
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Calculate the Heat Energy Transferred5
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Calculate the Molar Enthalpy Change4
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Reversible Reaction6
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Reversible Reactions Will Reach Dynamic Equilibrium6
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Changing Temperature and Pressure Can Get You More Product8
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Most Metals are Found in Ores6
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Metals Often have to be Separated from their Oxides5
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Methods of Extraction and Linked to the Order of Reactivity8
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Electrolysis Removes Aluminium from Its Ore4
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Cryolite is Used to Lower the Temperature (and Costs)5
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Electrolysis - Turning IONS into the Atoms You Want8
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Electrolysis is Expensive - It’s All That Electricity...3
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The Raw Materials are Iron Ore, Coke and Limestone3
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Reducing the Iron Ore to Iron:6
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Removing the Impurities:5
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Iron and Aluminium have some Properties in Common5
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The Uses of Iron Depend on Its Properties7
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And so do the Uses of Aluminium5
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Crude Oil is Separated into Different Hydrocarbon Fractions19
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Burning Fuels Can Produce Pollutants2
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Carbon Monoxide is Produced by Incomplete Combustion3
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Sulfur Dioxide and Nitrogen Oxides Come from Burning Fuel4
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Acid Rain is Caused by Sulfur Dioxide and Nitrogen Oxides12
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Cracking - Splitting Up Long-Chain Hydrocarbons7
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Conditions for Cracking: Heat, Plus a Catalyst10
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Addition Polymers are Made Under High Pressure3
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Polymers can be Shown Using Repeating Units7
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Polymers can be Made by Condensation Polymerisation5
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Polymers Have Lots of Uses6
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Most Polymers are Hard to Get Rid Of5
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Nitrogen and Hydrogen are Needed to Make Ammonia6
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The Reaction is Reversible, So There’s a Compromise to be Made:10
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Ammonia is Used to Make Nitric Acid and Ammonium Nitrate Fertiliser6
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The Contact Process is Used to Make Sulfuric Acid4
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A Catalyst is Important When Making SO31
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Modern Industry Uses Loads of Sulfuric Acid4
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Electrolysis of Salt gives Hydrogen, Chlorine and NaOH6
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The Half-Equations - Make Sure the Electrons Balance3
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Chlorine2
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Sodium Hydroxide3
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Hydrogen2
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