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CGP GCSE Chem
> ~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~ > Flashcards
~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~~ Flashcards
Study These Flashcards
CGP GCSE Chem
(233 decks)
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The Three States of Matter - Solid, Liquid and Gas
Substances Can Change from One State to Another
Diffusion is the Movement of Particles Through a Liquid or Gas
Potassium Manganate(VII) and Water
Ammonia and Hydrogen Chloride
Bromine Gas and Air
The Nucleus
The Electrons
Number of Electrons Equals Number of Protons
Atomic Number and Mass Number Describe an Atom
Molecules are Groups of Atoms
Elements Consist of One Type of Atom Only
Compounds are Chemically Bonded
Mixtures are Easily Separated - Not Like Compounds
Filtration is Used to Separate an Insoluble Solid from a Liquid
Crystallisation is Used to Separate a Soluble Solid from a Solution
You Can Use Filtration and Crystallisation to Separate Rock Salt
You Need to Know How to Do Paper Chromatography
How Chromatography Separates Mixtures...
Chromatography Can Help You to Identify Dyes
Simple Distillation is Used to Separate Out Solutions
Fractional Distillation is Used to Separate a Mixture of Liquids
The Periodic Table is a Table of All Known Elements
Elements in a Group Have the Same Number of Outer Electrons
Electron Shell Rules:
Follow the Rules to Work Out Electronic Configurations
Ionic Bonding - Transfer of Electrons
A Shell with Just One Electron is Well Keen to Get Rid...
A Nearly Full Shell is Well Keen to Get That Extra Electron...
Groups 1, 2, 6 and 7 are Most Likely to Form Ions
Ionic Compounds All Form in a Similar Way
Giant Ionic Structures Have High Melting and Boiling Points
A Covalent Bond is a Shared Pair of Electrons
Hydrogen, H2
Chlorine, Cl2
Hydrogen Chloride, HCI
Ammonia, NH3
Nitrogen, N2
Water, H20
Oxygen, O2
Carbon Dioxide, CO2
Methane, CH4
Ethane, C2H6
Ethene, C2H4
Simple Molecular Substances
Giant Covalent Structures
Diamond
Graphite
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Equations Show the Reactants and Products of a Reaction
Symbol Equations Need to Be Balanced
Method: Balance just ONE type of atom at a time
Isotopes are the Same Except for an Extra Neutron or Two
Relative Atomic Mass Takes All Stable Isotopes into Account
Relative Formula Mass, Mr
Finding the Empirical Formula (from Masses of Percentages)
The Empirical Formula isn’t Always the Same as the Molecular Formula
The Three Important Steps - Not to be Missed...
Percentage Yield Compares Actual and Theoretical Yield
‘The Mole’ is Simply the Name Given to a Certain Number
Nice Easy Formula for Finding the Number of Moles in a Given Mass:
Salts Can be Anhydrous or Hydrated
You Can Calculate How Much Water of Crystallisation a Salt Contains
Avogadro’s Law - One Mole of Any Gas Occupies 24 dm3
You Can Calculate Volumes in Reactions If You Know the Masses
Concentration is the ‘Amount of Stuff’ per Unit Volume
Concentration = No. of Moles / Volume
Converting Moles per dm3 to Grams per dm3
Electric Current is a Flow of Electrons or Ions
Ionic Compounds Only Conduct Electricity when Molten or in Solution
Covalent Compounds Don't Conduct Electricity
Metals are Held Together by Metallic Bonding
Metals are Good Conductors of Electricity and Heat
Most Metals are Malleable
Electrolysis is Used to Make New Substances
Electrolytes are Liquids that Conduct Electricity
In Molten Ionic Compounds There’s Only One Source of Ions
Electrolysis of Aqueous Solutions is a Bit More Complicated
Sulfuric Acid:
Sodium Chloride:
Copper(III) Sulfate:
No. Of Electrons Transferred Increases with Time and Current
Coulombs and Faradays are Amounts of Electricity
One Mole of Product Needs ‘n’ Moles of Electrons
Use These Steps in Calculations
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Periods
Groups
The Elements can be Classified as Metals or Non-Metals
Group 0 Elements are All Inert, Colourless Gases
Group 1 Elements All React in a Similar Way with Water
Group 1 Elements Become More Reactive Down the Group
Atoms Lose Electrons More Easily Down the Group
Halogen - Seven Letters - Group 7
Hydrogen Chloride Gas Dissociates in Water...
...but Not in Methylbenzene
More Reactive Halogens will Displace Less Reactive Ones
Halogen Displacement Reactions Involve Transfer of Electrons
Acid + Metal -> Salt + Hydrogen
The Name of the Salt Depends on the Metal and Acid Used
Metals Also React with Water
The Reactivity Series - How Well a Metal Reacts
A More Reactive Metal Displaces a Less Reactive Metal
Iron and Steel Corrode to Make Rust
There are Two Main Ways to Prevent Rusting
The Atmosphere is Mostly Nitrogen and Oxygen
You can Investigate the Proportion of Oxygen in the Atmosphere Using Copper
You can Investigate the Proportion of Oxygen in the Atmosphere Using Iron or Phosphorus
You Can Make O2 in the Lab
When you Burn Something it Reacts with Oxygen in Air
Magnesium
Carbon
Sulfur
You Can Collect Gases in a Test Tube
Dilute Acid reacts with Calcium Carbonate to Produce Carbon Dioxide
The Thermal Decomposition of Metal Carbonates Also Produces CO2
CO2 is used in Fizzy Drinks and Fire Extinguishers
Carbon Dioxide is a Greenhouse Gas
Increasing Carbon Dioxide is Linked to Climate Change
Flame Tests Identify Metals Ions
Some Metals Form a Coloured Precipitate with NaOH
‘Ammonium Compound + NaOH’ Gives off (Stinky) Ammonia
Hydrochloric Acid Can Help Detect Carbonates
Test for Sulfates with HCI and Barium Chloride
Test for Halides (Cl-, Brx, l-) with Nitric Acid and Silver Nitrate
There are Tests for 5 Common Gases
Wet Copper(II) Sulfate is Blue - Dry Copper(II) Sulfate is White
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Alkanes are Hydrocarbons
MethAne Formula: CH4
EthAne Formula: C2H6
PropAne Formula: C3H8
ButAne Formula: C4H10
PentAne Formula: C5H12
Alkanes are a Homologous Series
Complete Combustion Happens When There’s Plenty of Oxygen
Incomplete Combustion of Alkanes is NOT Safe
Halogens React with Alkanes to make Haloalkanes
Alkenes Have a C=C Double Bond
EthEne Formula: C2H4
PropEne Formula: C3H6
ButEne Formula: C4H8
Halogens React with Alkanes, Forming Haloalkanes
Ethanol Can Be Produced from Ethene and Steam
Ethanol Can Also be Produced by Fermentation
Both Methods have Advantages and Disadvantages...
Ethanol can be Dehydrated to Form Ethene
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The pH Scale Goes from 0 to 14
An Indicator is Just a Dye That Changes Colour
Acids can be Neutralised by Bases (or Alkalis)
Acids react with Metal Oxides to make Salt + Water...
... and with Metal Carbonates to give Salt + Water + Carbon Dioxide
Salts can be Soluble or Insoluble
Making Soluble Salts Using Acids and Insoluble Bases
Making Soluble Salts Using an Alkali
Making Insoluble Salts - Precipitation Reactions
Titrations are Used to Find about Concentrations
The Calculation - Work Out the Number of Moles
Reactions Can Go at All Sorts of Different Rates
The Rate of a Reaction Depends on Four Things:
Typical Graphs for Rate of Reaction
Three Ways to Measure the Speed of a Reaction
Precipitation
Change in Mass (Usually Gas Given Off)
The Volume of Gas Given Off
Reaction of Hydrochloric Acid and Marble Chips
This graph shows the effect of using finer particles of solid
Reaction of Magnesium Metal with Dilute HCl
This graph shows the effect of using more concentrated acid solutions
Sodium Thiosulfate and HCl Produce a Cloudy Precipitate
The Decomposition of Hydrogen Peroxide
More Collisions Increases the Rate of Reaction
Higher Temperatures
Higher Concentration (or PRESSURE)
Larger Surface Area
Catalysts
Faster Collisions Increase the Rate of Reaction
Energy Must Always be Supplied to Break Bonds
In an Exothermic Reaction, Energy is Given Out
In an Endothermic Reaction, Energy is Taken In
The Change in Energy is Called the Enthalpy Change
Energy Level Diagrams Show if it’s Exo- or Endo- thermic
The Activation Energy is Lowered by Catalysts
Bond Energy - The Amount of Energy in a Bond
Example: The Formation of HCl
You can find out Enthalpy Changes using Calorimetry
Calorimetry - Dissolving, Displacement and Neutralisation Reactions
Calorimetry - Combustion
Calculate the Heat Energy Transferred
Calculate the Molar Enthalpy Change
Reversible Reaction
Reversible Reactions Will Reach Dynamic Equilibrium
Changing Temperature and Pressure Can Get You More Product
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Most Metals are Found in Ores
Metals Often have to be Separated from their Oxides
Methods of Extraction and Linked to the Order of Reactivity
Electrolysis Removes Aluminium from Its Ore
Cryolite is Used to Lower the Temperature (and Costs)
Electrolysis - Turning IONS into the Atoms You Want
Electrolysis is Expensive - It’s All That Electricity...
The Raw Materials are Iron Ore, Coke and Limestone
Reducing the Iron Ore to Iron:
Removing the Impurities:
Iron and Aluminium have some Properties in Common
The Uses of Iron Depend on Its Properties
And so do the Uses of Aluminium
Crude Oil is Separated into Different Hydrocarbon Fractions
Burning Fuels Can Produce Pollutants
Carbon Monoxide is Produced by Incomplete Combustion
Sulfur Dioxide and Nitrogen Oxides Come from Burning Fuel
Acid Rain is Caused by Sulfur Dioxide and Nitrogen Oxides
Cracking - Splitting Up Long-Chain Hydrocarbons
Conditions for Cracking: Heat, Plus a Catalyst
Addition Polymers are Made Under High Pressure
Polymers can be Shown Using Repeating Units
Polymers can be Made by Condensation Polymerisation
Polymers Have Lots of Uses
Most Polymers are Hard to Get Rid Of
Nitrogen and Hydrogen are Needed to Make Ammonia
The Reaction is Reversible, So There’s a Compromise to be Made:
Ammonia is Used to Make Nitric Acid and Ammonium Nitrate Fertiliser
The Contact Process is Used to Make Sulfuric Acid
A Catalyst is Important When Making SO3
Modern Industry Uses Loads of Sulfuric Acid
Electrolysis of Salt gives Hydrogen, Chlorine and NaOH
The Half-Equations - Make Sure the Electrons Balance
Chlorine
Sodium Hydroxide
Hydrogen
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