C5 - Flashcards in Fun Fun

What is an ore -

Rocks which contain metals at a high enough quantity whereby it is economical to extract them

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What is the Reactivity Series -

A list of metals in order of their reactivity from most to least reactive

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How is a metals reactivity determined -

Metals are each reacted with water and dilute acids to rank their reactivity

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Reactivity Series - Order

Potassium / Sodium / Calcium / Magnesium / Aluminium / Carbon / Zinc / Iron / Tin / Lead / Hydrogen / Copper / Silver / Gold

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Displacement -

A more reactive metal will displace a less reactive metal in a compound forming a new compound and isolating the other less reactive metal

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Displacement with ores -

If the metal in the ore is less reactive than carbon, displacement is carried out so that the carbon displaces the metal forming another compound and the pure metal (E.G. Copper)

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What is an Oxidation Reaction -

When oxygen atoms are gained / A reaction where electrons are lost

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What is a Reduction Reaction -

When Oxygen atoms are lost / A reaction where electrons are gained

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Half Equations -

Half Equations are used to display oxidation and reduction reactions / They show the movement of electrons in reactions

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What is considered when extracting a metal from its ore -

How easy is it to extract / Yield of valuable metal / Changing Demands

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Extracting Less reactive metals -

These metals are often found as oxides in the ground / The oxides that are less reactive than carbon are heated in the presence of carbon to displace the metal and produce carbon dioxide

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Reduction using Hydrogen -

In some cases , carbon isn't used based on the fact it can create undesirable products / Tungsten is less reactive that carbon but is displaced with hydrogen

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Metal + Acid -->

Salt + Hydrogen / This occurs as the metal is more reactive than the hydrogen in the acid and so displaces it to from a salt

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(Neutralisation Reaction) Acid + Base -->

Salt + Water

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Salts -

The salts formed are all ionic compounds / They are made from positive and negative ions attracting each other

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How to sample pure dry salt crystals -

Run a titration to find exact quantities needed / Repeat the reaction with the exact amounts needed / Crystalise the salt by slowly evaporating the water

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Acid + Carbonate -->

Salt + Carbon Dioxide + water

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What is a base -

A substance which neutralises a acid / All alkalis are bases - Not all bases are alkalis

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pH of pure water -

7

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Why do acids make aqueous solutions acidic -

When an acid is in an aqueous solution it releases H+ ions which make the solution acidic

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pH Scale -

The measure of the acidity or alkalinity of a substance ranging from 1 (Most Acidic) to 14 (Most Alkaline)

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How to measure pH -

Universal indicator / Litmus paper / pH meter

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Concentrated Acids -

Concentrated acids have more acid particles in proportion to the water molecules present / The greater the concentration of an acid , the greater its harmful effects

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Strong Acids - Examples (3)

Hydrochloric Acid / Nitric Acid / Sulfuric Acid

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Weak Acids - Examples (3)

Citric Acid / Ethanoic Acid / Carbonic Acid

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Acids - Strength

Acids only reveal their properties when in an aqueous state / Strong Acids are strong because they Ionise completely in an aqueous state

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Number of H+ ions -

Concentration of H+ ions increases by a factor of 10 (10x bigger) as you go down the pH scale

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C5

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