9150284
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| Question | Answer |
| Newlands and then Mendeleev attempted to... | classify the elements by arranging them in order of the atomic weights. - This list can be arranged in a table so elements with similar properties are in columns/groups |
| It's called a periodic table because... | Similar properties occur at regular intervals |
| The early periodic table was incomplete and some elements were placed in inappropriate groups if the strict order of atomic weight was followed. Mendeleev did what to solve this? | He left gaps for elements that hadn't been found |
| What discovery changed how the periodic table was constructed? | That of protons, neutrons and electrons! Then all elements were in the appropriate groups... |
| The modern periodic table can also be seen as an arrangement of the elements in terms of? | Their electronic structures |
| Group 1 metals have: - a low density - react with ____ to form ionic compounds that form a metal ion (with +1 charge) - The compounds are _____ solids which form _____ solutions in water - They react with ___ to form hydrogen - Form _____ that dissolve in water to give ____ solutions | 1) NON-METALS 2) WHITE 3) COLOURLESS 4) WATER 5) HYDROXIDES 6) ALKALINE |
| In Group 1 the further down an element is ...? (2 points) The ____ its melting and boiling point. | The more reactive the elements get The LOWER its melting and boiling point |
| Compared with G1 elements, transitions metals are: | - Stronger and harder - Higher melting points (EXCEPT for mercury that annoying element) - Higher DENSITIES |
| Transitions metals are much less reactive and don't react that vigorously with oxygen and water as G1 elements True or False? | TRUE |
| Sing the 3 further praises of the transition metals | 1) Form coloured compounds 2) Have ions with different charges 3) Useful as catalysts |
| Elements in Group 7 (halogens) react with ______ to form IONIC compounds in which the ____ ion carries a charge of ___ | 1) METALS 2) HALIDE 3) MINUS ONE |
| In Group 7 the further down you go: | 1) The LESS REACTIVE the element 2) The HIGHER its melting pt and boiling pt |
| A ___ reactive halogen can displace a ___ reactive halogen in an ___ solution of its salt | 1) MORE 2) LESS 3) AQUEOUS below is how you would start such a displacement. Can you predict which tests tube will show displacement? The answer is: Tube 2 and 3 (from left) |
| Trends in reactivity in the periodic table can be explained cause the higher the energy level, the less easily... | electrons are gained |
| Name some commercial water softeners and advantages/disadvantages | Ion exchange water softener - Sodium ions could be bad for your health (HBP) - Costs money to keep topped up - Could be saving money because less soap is wasted - Can add products to washing machine/kettle to protect from scale - Filter jugs - But softening water could be bad for your health |
| Soft water readily forms a lather with soap. Hard water reacts with soap to form ____ so more soap is needed to form lather. _____ detergents do not form scum. | 1) SCUM 2) SOAPLESS |
| Temporary hard water is softened by boiling. Permanent hard water remains hard when boiled. TRUE OR FALSE? | TRUE |
| Temporary hard water contains HCO3- ions (hydrogencarbonate) which ____ on heating into _____ ions. These react with calcium or magnesium ions to form _____. | 1) DECOMPOSE 2) CARBONATE 3) PRECIPITATES |
| Using hard water can ____ costs and temporary hard water can reduce the _____ of kettles and heating systems because it produces ____ when heated | 1) reduce 2) efficiency 3) scale |
| Hard water can be softened by: 1) adding sodium carbonate (washing soda) - ____ with calcium or magnesium ions to form ______ 2) ion exchange resins which contain ____ or sodium ions which replace the calcium and magnesium ions | 1) which reacts 2) precipitate of calcium and magnesium carbonate 3) hydrogen |
| Water of the correct quality is produced by? Human beings need water of the correct quality for LIFE which has sufficiently low levels of _____ | 1) Choosing an appropriate source 2) Passing the water through filter beds to remove any solids 3) STERILISING with CHLORINE 4) Dissolved salts and microbes |
| Water filters containing carbon, silver and ion exchange resins can... | improve taste and quality of water by removing dissolved substances from tap water |
| Arguments for adding fluoride to water | - Improves dental health - Almost no health effects except fluorosis - Can protect against some types of heart disease linked with tooth decay bacteria - Only added in tiny amounts |
| Arguments against adding fluoride | - People should choose - Fluorosis - Not big benefit - Could affect brain e.g. cause learning difficulties - Can't control people's intakes so can become unsafe |
| The relative amounts of energy released when substances ___ can be measured by what? What can this method be used to compare? | 1) ARE BURNED 2) SIMPLE CALORIMETRY 3) Amount of energy released by fuels and foods |
| How can we calculate the amount of energy released or absorbed by a chemical reaction in solution? What type of reactions can you use this method for? | Mix the reagents together in an insulated container Measure the temperature change You can use this method for reactions of solids with water or for NEUTRALISATION reactions |
| Describe the energy level diagrams for exothermic and endothermic. How would you change it if you had to add activation energy? | EXOTHERMIC Reactants have more energy Give out a lot of energy to the surroundings (-ΔH) Products have less energy so are drawn lower ENDOTHERMIC the opposite of exothermic |
| In a chemical reaction energy must be supplied to ___ bonds and is released to ____ bonds. How do you calculate ΔH? | 1) BREAK 2) FORM ΔH = sum of bonds broken – sum of bonds made |
| Energy released to form bonds is greater than energy needed to break existing bonds in an EXOTHERMIC reaction Energy needed to break existing bonds is greater than energy released to form new ones True or false? | We form bonds for products (release energy) We break bonds of the reactants (we need energy for this) TRUE |
| Energy level diagram for catalyst | |
| Hydrogen can be ___ as a fuel in combustion ____. It can also be used in _____ that produce electricity to power vehicles. The equation for hydrogen combustion: | 1) burned 2) engines 3) fuel cells hydrogen + oxygen --> water |
| Flames test are used to identify ____. The metals that can be identified with these are ____. Describe the flame colour for each. | 1) METAL IONS 2) Lithium - Crimson Potassium - Lilac Calcium - Red Sodium - Yellow Barium - Green |
| Name the ions that form white precipitates with SODIUM HYDROXIDE ions Of them, ____ precipitate dissolves in excess sodium hydroxide solution | 1) Aluminium, calcium and magnesium 2) ALUMINUM HYDROXIDE |
| Copper(II), iron(II) and iron(III) What precipitates do they form with sodium hydroxide solution? | Copper(II) forms blue precipitate Iron(II) forms a green one Iron(III) forms brown |
| Carbonates react with dilute ___ to form ______ turning limewater cloudy because of the calcium carbonate white precipitate. | 1) ACIDS 2) CARBON DIOXIDE |
| Halide ions in solution produce ____ with ___ nitrate solution in the presence of dilute ____ acid. The ions and their precipitate colours are...? | 1) PRECIPITATES 2) SILVER 3) NITRIC (Silver) bromide --> cream chloride --> white iodide --> yellow |
| Sulfate ions in solution produce a white precipitate with barium chloride solution in the presence of dilute HYDROCHLORIC ACID TRUE OR FALSE? | TRUE |
| Describe a titration | 1) Unknown concentration of solution in flask 2) Measure volume of solution using pipette 3) Indicator in flask 4) Solution of known concentration in burette 5) White tile under flask 6) Add acid/alkali drop-wise 7) Swirl the mixture and check for colour change (neutralisation) end point 8) Volume of known solution added is recorded |
| The raw materials for the Haber process are | Nitrogen (from the air) Hydrogen (from natural gas or other sources) |
| The ___ gases are passed over ____ of __ at a high temperature (about ___*C) and a high pressure (about ___ atmospheres) What's the word equation? The ammonia ____ and is removed on c___. The remaining hydrogen and ____ are ____. | 1) PURIFIED 2) CATALYST 3) IRON 4) 450 5) 200 6) liquefies 7) cooling 8) nitrogen 9) recycled nitrogen + hydrogen <-> ammonia |
| When a reversible reaction occurs in a closed system when is equilibrium reached | When the reactions occur at exactly the same rate in each direction |
| The relative amounts of all the reacting substances at equilibrium depend on the conditions of the ___ | REACTION |
| If the temperature is raised how is the yield in endo/exo reactions affected? | The yield from the ENDOTHERMIC reaction increases and the yield from the EXOTHERMIC REACTION decreases |
| If the temperature is lowered, yield from the endothermic reaction DECREASES and yield from the exothermic reaction INCREASES true or false | true |
| In ____ reactions, an increase in pressure will favour the reaction that produces the least number of ____ as shown by the symbol equation | 1) GASEOUS 2) MOLECULES |
| Importance of equilibrium in Haber process | These factors, together with reaction rates, are important when determining the optimum conditions in industrial processes |
| Social and economic pros and cons of uses of alcohols | Alcohols SOCIAL 1) Death and illness 2) Days lost at work ECONOMIC 1) Big income from taxes for government and drinks companies 2) Costs a lot of money to police alcohol-related crimes and costs NHS a lot of money |
| Same as last flashcard but for carboxylic acids and esters | SOCIAL 1) Ethanol can be used as biofuel. Biodiesel (made from plant oils which are esters). When processed these break down into carboxylic acids. Reacted with methanol/ethnaol to make esters used as biodiesel. 2) Land could be used for food crops 3) Land for biodiesel farms made by deforestation - harmful to environment but we need an alternative to crude oil, so there's little choice |
| Methanol, ethanol and propanol | - First 3 members of a homologous series of alcohols - Dissolve in water to form a neutral solution - React with sodium to produce HYDROGEN - BURN in air - Are used as FUELS and SOLVENTS - Ethanol is the main alcohol in alcoholic drinks |
| Ethanol can be oxidised to ___ by chemical oxidising agents or microbial action. Ethanoic acid is the main acid in ____. | 1) ETHANOIC ACID 2) VINEGAR |
| Carboxylic acids | - dissolve in WATER to form ACIDIC solutions - react with carbonates to produce CARBON DIOXIDE - react with ALCOHOLS in the presence of an ACID CATALYST to produce esters - don't ionise completely when dissolved in WATER and so are WEAK ACIDS - Aqueous solutions of WEAK ACIDS have a higher pH value than aqueous solutions of STRONG ACIDS with the same concentration |
| Esters (like ethyl ethanoate) Functional group? Uses? | Ethyl ethanoate is an ester produced from ethanol and ethanoic acid. -COO- They are volatile compounds with distinctive smells and are used with perfumes and flavourings |
| Social, environmental, economic consequences of using fuels | SOCIAL - May not be convenient to use hydrogen as not many filling stations - H Might not be able to match performance with petrol ENVIRONMENTAL - Global warming - Pollution - May need to use alternative fuel sources e.g. hydrogen which don't contribbute to global warming - Supplying hydrogen could be bad for the environment because use electrolysis (which burns fossil fuels) ECONOMIC - Safety and storage is an issue with fuels like hydrogen - Price of hydrogen might be higher |
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