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Description
Flashcards by Malachy Moran-Tun, updated more than 1 year ago
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Created by Malachy Moran-Tun
almost 3 years ago
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| Question | Answer |
| What is Ionic Bonding? | Transfer of Electrons Between a Metal and a Non-Metal |
| Why are Ionic Bonds Strongly Attracted to Each-other? | The Electrostatic Forces of Attraction hold the Ions Together |
| What are Group 1 Elements also known as? | Alkali Metals |
| How many Outer Electrons do Group 1 Metals have? | One outer electron |
| What Physical Properties do Group 1 Metals have? | > Low melting and boiling points (compared with other metals) > Very soft - can be cut with a knife |
| Why do Group 1 Metals NOT form Covalent Bonds? | > Form ionic compounds > Loose the outer electron very easily > Outer electron CANNOT be shared |
| Why are Group 1 Metals So Reactive? | > Easy to loose the outer electron > Loosing the outer electron forms a stable electronic structure (1⁺ ion) |
| How and Why does Reactivity Change as you do Down Group 1? | > Reactivity increases > Outer electron is more easily lost > Electron is further from the nucleus > Electrostatic shielding from shells > Less attraction to the nucleus > Less energy required to remove electron |
| What is the General Word Equation for Reactions with Water and Alkali Metals? | Alkali Metal + Water → Alkali Metal Hydroxide + Hydrogen |
| Why do Alkali Metals from Alkali in Water? | They produce hydroxides which contain OH⁻ ions |
| What happens when Lithium Reacts with Water? | > Bubbles Fiercely on Water Surface > 2Li(s) + 2H₂O(l) → 2LiOH(aq) + H₂(g) |
| What happens when Sodium Reacts with Water? | > Melts into a ball and fizzes as it moves around on the surface > 2Na(s) + 2H₂O(l) → 2NaOH(aq) + H₂(g) |
| What happens when Potassium Reacts with Water? | > Reacts very rapidly and bursts into a lilac flame as it flies about the surface > 2K(s) + 2H₂O(l) → 2KOH(aq) + H₂(g) |
| What are Group 7 Elements also known as? | Halogens |
| How many Outer Electrons do Group 7 Elements have? | Seven outer electrons |
| What type of Molecule do Halogens (Naturally) Exist as? | Diatomic Molecules (e.g. Cl₂, Br₂, I₂ etc.) |
| Why do Halogens Exist as Diatomic Molecules? | Share one pair of electrons in a covalent bond to give both atoms a full outer shell |
| How do the Melting and Boiling Points Change going Down Group 7? | Increase (Fluorine lowest → Iodine highest) |
| What Colour and State are the Following at Room Temperature? > Fluorine > Chlorine > Bromine > Iodine | > Fluorine - Yellow Gas > Chlorine - Green Gas > Bromine - Orange Liquid > Iodine - Grey Solid |
| What is the Chemical Test for Chlorine? | Damp blue litmus paper turns red then bleaches white |
| How and Why does Reactivity Change as you do Down Group 7? | > Reactivity decreases > Electron is harder to attract > Outer shell is further from the nucleus > Electrostatic shielding from shells > Less attraction to the nucleus > Less energy available to attract electron |
| What is the General Word Equation for Reactions with Metals and Halogens? | Halogen + Metal → Metal Halide (Salt) |
| What is the General Word Equation for Reactions with Hydrogen and Halogens? | Halogen + Hydrogen → Hydrogen Halide |
| What happens when Hydrogen Halides Dissolve in Water? | Form acidic solutions (e.g. HCl forms Hydrochloric Acid) |
| What happens if a More Reactive Halogen Reacts with a Halogen Compound? | More reactive halogen displaces the less reactive one |
| Why are Halogen Displacement Reactions Redox? | > Halogen Gains Electrons (Reduction) > Halide Ions Loose Electrons (Oxidation) |
| What are Group 0 Elements also known as? | Noble Gases |
| How many Outer Electrons do Group 0 Metals have? | Full Outer Shell (2, 8, 8 for first 3 periods) |
| What are the Physical and Chemical Properties of Group 0 Elements? | > Colourless Gases (at room temp.) > Monatomic (exist as single atoms) > Extremely unreactive (almost inert) > Non-Flammable > Low Melting / Boiling Points > Low Densities |
| Why are Group 0 Elements Inert? | They have a full outer shell of electrons so they don't gain / loose / share electrons easily |
| What are some Uses of Noble Gases? | > (All) Provide an Inert Atmosphere > Argon used in Filament Lamps (non-flammable) > Argon and Helium Protect Metals during Welding > Helium used in Airships and Party Balloons (Low-Density) |
| What happens to Melting / Boiling Points / Density as you go Down Group 0? | > Melting / Boiling Points Increase > Density Increases |
| What is the Rate of Reaction? | How Fast a Reaction Happens |
| How do Reactions Occur? | Particles collide with enough energy to react |
| What is the Minimum Amount of Energy for a Reaction to Occur Called? | The Activation Energy |
| How do you Increase the Rate of Reaction (generally)? | Increase the Frequency of Collisions or Increase the Energy of Collisions (so they're more successful) |
| How do you Calculate the Rate of Reaction? | Rate = Amount of Product Formed ÷ Time or Rate = Amount of Reactant Used ÷ Time |
| How do you Increase Rate of Reaction by Changing the Surface Area and why? | > Increasing the surface area to volume ratio > Usually done by decreasing size of pieces (powdering them etc.) but overall volume is the same > There is more surface for collisions to occur > Collisions occur more frequently - faster rate of reaction |
| How do you Increase Rate of Reaction by Changing the Concentration and why? | > Increasing the concentration > There are more reacting particles in the same volume > Collisions occur more frequently - faster rate of reaction |
| How do you Increase Rate of Reaction by Changing the Temperature and why? | > Increasing the temperature > Reactant particles have more energy > More kinetic energy means particles move faster > Particles moving faster collide more frequently - faster rate of reaction > Particles with more energy successfully react more frequently - faster rate of reaction |
| How do you Increase Rate of Reaction by Changing the Pressure and why? | > Increase the pressure > Same number of particles in a lower volume > Collisions occur more frequently - faster rate of reaction |
| How could you Test Rates of Reaction? | > Measure how quickly a precipitate forms (if applicable) > Measure a change in mass (usually by gas being given off) > Measure a volume of gas given off |
| How would you Test Rates of Reaction by using a Precipitate being Formed? | > Put a piece of paper with an X below the flask > Mix the two solutions > Time how long it takes for the X to "disappear" > Result is Subjective |
| How would you Test Rates of Reaction by using the Change in Mass? | > Place the flask on scales > Mix the two solutions > Bung the flask with cotton wool (for safety) > Measure how quickly the mass decreases |
| How would you Test Rates of Reaction by using the Volume of Gas? | > Mix the two solutions > Bung the flask with either a gas syringe or upside-down measuring cylinder filled with water > Measure the volume against the time elapsed > Faster the volume increases, the faster the reaction |
| When plotting Rates of Reaction on a Graph, how do you determine the Rate? | The gradient |
| How do you calculate Gradient? | Curved line: Draw a tangent off a specific point then Straight line: Gradient = Δy ÷ Δx (Δ = change in) |
| What do Catalysts do? | Increase the Rate of Reaction without being Chemically Changed or Used Up |
| How do Catalysts Work? | Decrease the Activation Energy needed for a Reaction to Occur by providing an Alternative Reaction Pathway |
| What are Enzymes and Where are they Found? | Biological Catalysts found in Living Cells / Organisms |
| What is an Exothermic Reaction? | A reaction which gives out energy to the surroundings - rise in temperature of the surroundings |
| What is an Endothermic Reaction? | A reaction which takes in energy from the surroundings - fall in temperature of the surroundings |
| What is a Reaction Profile? | A Graph which shows the Energy Levels of Reactants and Products in a Reaction |
| How do you tell if a Reaction is Exothermic on a Reaction Profile | > Products have a Lower Energy than the Reactants > Difference in Height Represents the Energy Given Out |
| How do you tell if a Reaction is Endothermic on a Reaction Profile | > Products have a Higher Energy than the Reactants > Difference in Height Represents the Energy Taken In |
| On a Reaction Profile, what is the Activation Energy? | Energy Difference between the Reactants and the Peak of the Curve |
| Which of the Following Reactions are Exothermic, Endothermic or Both (depending on the elements): > Dissolving Salts > Neutralisation > Displacement > Precipitation | > Dissolving Salts - Both > Neutralisation - Both (usually Exo) > Displacement - Exothermic > Precipitation - Exothermic |
| Is Breaking Chemical Bonds Endothermic or Exothermic | Endothermic; it requires energy |
| Is Forming Chemical Bonds Endothermic or Exothermic | Exothermic; it releases energy |
| How do you Calculate Overall Energy Change? | Overall Energy Change = Energy Required to Break Bonds - Energy Released by Forming Bonds (Example in Revision Guide) |
| What is a Hydrocarbon? | A molecule that contains Carbon and Hydrogen ONLY |
| What is a Homologous Series? | A family of molecules which have the same general formula and share chemical properties |
| What is the General Formula for Alkanes? | CₙH₂ₙ₊₂ |
| What are the first 6 Alkanes and their Formulæ? | Methane - CH₄ Ethane - C₂H₆ Propane - C₃H₈ Butane - C₄H₁₀ Methylbutane* - C₅H₁₂ Cyclohexane - C₆H₁₂ *aka pentane |
| Why are the Physical Properties Different in Alkanes / Hydrocarbons? | The intermolecular forces are stronger between bigger molecules, which hold the chains of atoms together |
| Why do Longer Hydrocarbons have Higher Boiling Points? | > Intermolecular forces break easier in SMALLER molecules > There is still another place where the force is strong enough to hold in in place > Bonds are harder to break so boiling point is higher |
| Why are Shorter Hydrocarbons Easier to Ignite? | > Shorter hydrocarbons have lower boiling points > The gas molecules mix with oxygen in the air to produce a combustible gas mixture > If the mixture comes in contact with a spark, it will ignite |
| Why are Longer Hydrocarbons more Viscous? | > Viscosity is how easily a substance flows > Stronger force between hydrocarbon molecules > Harder for the liquid to flow - higher viscosity |
| What does it mean if a Molecule is Saturated? | All the atoms have formed bonds with as many other atoms as they can |
| What's the Difference between Alkanes and Alkenes? | Alkanes - Saturated, they have all single bonds Alkenes - Unsaturated, they have a double bond |
| What is Cracking? | Chemical reaction in which large alkane molecules are split into smaller alkanes and alkenes |
| What are the First Three Alkenes and their Formulæ? | Ethene - C₂H₄ Propene - C₃H₆ Butene - C₄H₈ |
| What is the Test for Alkenes? | > Add orange bromine water > If the colour remains, it is an alkane > If the solution becomes colourless, it is an alkene |
| How does the Test for Alkenes with Bromine Water Work? | > When an alkene reacts with bromine, the double bond breaks > At the same time, the atoms in the bromine molecule break apart > The bromine atoms are "added" to the broken ethene molecule (an addition reaction) |
| What do Hydrocarbons (alkanes and alkenes) form in Full Combustion Reactions? | Carbon Dioxide (CO₂) and Water (H₂O) |
| Why must Tests for Ions be Unique? | So only one ion can be identified |
| What Colour do the Following Ions Produce under a Flame? Lithium (Li⁺) Sodium (Na⁺) Potassium (K⁺) Calcium (Ca²⁺) Copper (Cu²⁺) | Lithium (Li⁺) - (Crimson) Red Sodium (Na⁺) - Yellow Potassium (K⁺) - Lilac Calcium (Ca²⁺) - Orange-Red Copper (Cu²⁺) - Blue-Green |
| What Colour do the Following Ions Produce when Reacted with Sodium Hydroxide (NaOH)? Aluminium (Al³⁺) Calcium (Ca²⁺) Copper(II) (Cu²⁺) Iron(II) (Fe²⁺) Iron(III) (Fe³⁺) Magnesium (Mg²⁺) | Aluminium (Al³⁺) - White Calcium (Ca²⁺) - White Copper(II) (Cu²⁺) - Blue Iron(II) (Fe²⁺) - Green Iron(III) (Fe³⁺) - Brown Magnesium (Mg²⁺) - White |
| How do you Test for Ammonium Ions (NH₄⁺) with Sodium Hydroxide (NaOH)? | Reaction of NH₄⁺ and NaOH produce ammonia gas, which turns a moistened, red litmus paper blue |
| What is Flame Photometry? | An instrumental method which allows you to identify flame colours from ions |
| How can you measure the Concentration of an Ion using Flame Photometry? | The intensity of a measured wavelength indicates the concentration of that ion |
| What are the Advantages of Flame Photometry? | > Very sensitive - can detect small amounts of substances > Very fast - tests can be automated > Very accurate - tests eliminate human error > Works for mixtures - the accuracy allows for multiple ions to be detected and cross-referenced |
| What Colour Precipitate do the Following Ions Produce when Reacted with Silver Nitrate (AgNO₃)? Chloride (Cl⁻) Bromide (Br⁻) Iodide (I⁻) | Chloride (Cl⁻) - White Bromide (Br⁻) - Cream Iodide (I⁻) - Yellow |
| What is the Test for Carbonate Ions (CO₃²⁻)? | > Add dilute hydrochloric acid > Bubble any gas produced through limewater > If limewater turns cloudy, CO₃²⁻ ions are present (since there is CO₂ gas) |
| What is the Test for Sulfate Ions (SO₄²⁻)? | > Add dilute hydrochloric acid > Add barium chloride solution > White precipitate will form is SO₄²⁻ is present |
| What are Nanoparticles? | Tiny particles consisting of only a few hundred atoms |
| What is the Size of Nanoparticles | 1 - 100 nanometres 1 nanometre = 1 × 10⁻⁹m ... like m'dick- what |
| What Properties of Nanoparticles make them Useful? | > Small Size > Large Surface Area : Volume Ratio |
| What are some Examples of the Uses of Nanoparticles? | > Titanium Dioxide - absorbs UV radiation and is also near-invisible > SA:V ratio make them good Catalysts - stain-resistant clothes are often treated with nanoparticulate to catalyse dirt > Nanomedicine - tiny fullerenes are absorbed more easily into the body > Lubricants > Tiny electrical circuits - such as ones in computers' chips and more |
| What are some Risks of Using Nanoparticles? | > Small size may pose hazards to human health > They can be breathed in or pass through cell membranes easily > The SA:V ratios could make them catalyse harmful reactions > They could easily carry toxic substances bound to them |
| wow you're done- nerd | lol that's so gay |
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