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Chemistry > C5 > Flashcards

C5 Flashcards

1
Q

The reactivity series

A

Potassium, Sodium, Calcium, Magnesium, aluminium, carbon, zinc, iron, tin, lead, hydrogen, copper, silver, gold, platinum

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2
Q

a more reactive metal can ____ a less reactive metal from a ___

A

displace, compound

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3
Q

The reactivity of metal is related to ____

A

tendency to form positive ions

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4
Q

more reactive metals form positive ions faster/slower

A

faster

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5
Q

reactions of metals with acids

A

metal + acid -> salt + hydrogen (MASH)

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6
Q

reactions of a metal with oxygen

A

metal + oxygen -> metal oxide

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7
Q

reactions of metal oxides with acids

A

metal oxide + acid -> salt + water

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8
Q

reactions of metal carbonates with acids

A

metal carbonate + acid -> salt + water + carbon dioxide

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9
Q

zinc + hydrochloride acid ->

A

zinc chloride + hydrogen

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10
Q

iron + oxygen ->

A

iron oxide

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11
Q

magnesium oxide + sulfuric acid ->

A

magnesium sulfate + water

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12
Q

tin carbonate + hydrochloric acid ->

A

tin chloride + water + carbon dioxide

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13
Q

what is oxidation?

A

when a metal forms a bond with a non metal and loses its outer shell electrons

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14
Q

what is reduction?

A

when a metal is in a compound and reacts to form an element, gaining electrons

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15
Q

what is this an example of: (oxidisation/reduction)
zinc + hydrochloric acid -> zinc chloride + hydrogen

A

oxidisation

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16
Q

what is this an example of: (oxidisation/reduction)
copper oxide + carbon -> copper + carbon dioxide

A

reduction

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17
Q

Metals can be split into three groups, based on how easy it is to extract them, which are:

A
  1. the most unreactive metals are found native in the Earth’s crust
  2. Metals less reactive than carbon can be extracted from compounds by reduction with carbon. this is a special example of a displacement reaction
    (e.g. iron oxide + carbon -> iron + carbon dioxide)
  3. metals more reactive than carbon may require electrolysis to extract them. this is expensive and requires a lot of energy
18
Q

t/f? salts are ionic compounds

19
Q

hydrochloric acid (symbol and what it reacts to make)

A

HCl, reacts to make chloride salts

20
Q

sulfuric acid (symbol and what it reacts to make)

A

H2SO4, reacts to make sulfate salts

21
Q

nitrate acid (symbol and what it reacts to make)

A

HNO3, reacts to make nitrate salts

22
Q

iron + hydrochloric acid ->

A

iron chloride + hydrogen

23
Q

zinc + sulfuric acid ->

A

zinc sulfate + hydrogen

24
Q

magnesium + nitric acid ->

A

magnesium nitrate + hydrogen

25
Q

how can soluble salts be made?

A

from acids by reacting them with solid insoluble substances, such as metals, metal oxides, hydroxides or carbonates

26
Q

describe the method for the “making a names soluble salt” RP:

  1. the ____ is added to the acid until no more _____
  2. The ______ is filtered off to produce a solution of the salt
  3. the salt solution is ____ and then left to _____ to produce solid salt.
  4. An excess of the solid MUST be added to _____
A
  • solid metal compound
  • reacts
  • excess solid
  • heated
  • crystallise
  • make sure no acid remains to form an impurity in the salt product
27
Q

what apparatus is required for a titration

A

a pipette to accurately measure the volume of a reactant before transferring it to a conical flask
a burette to add small, measured volumes of one reactant to the other reactant

28
Q

titration method:

A
  1. Use the pipette and pipette filler to add a measured volume of sodium hydroxide solution to a clean conical flask.
  2. Add a few drops of indicator and put the conical flask on a white tile.
  3. Fill the burette with hydrochloric acid and note the starting volume.
  4. Slowly add the acid from the burette to the alkali in the conical flask, swirling to mix.
  5. Stop adding the acid when the end-point is reached (when the indicator first permanently changes colour). Note the final volume reading.
  6. Repeat steps 1 to 5 until
    concordant titres are obtained. More accurate results are obtained if acid is added drop by drop near to the end-point
29
Q

cm^3 -> dm^3 =??

A

DIVIDE by 1000

30
Q

number of mols=

A

concentration x volume

31
Q

colour change for methyl orange:

A

yellow- red

32
Q

colour change for phenolphthalein:

A

colourless- pink

33
Q

What is an alkali

A

A base which is soluble in water

34
Q

Strong acids-

A

Hydrochloric acid, sulfuric acid, nitrate acid– They fully ionise to release H+ ions extremely easily

35
Q

Weak acids-

A

Ethanoic acid, citric acid, carbonic acid- only partially ionise in aqueous solution, meaning some molecules split up

36
Q

Acidic solutions contain

A

Hydrogen, H+

37
Q

Alkalines contain-

A

Hydroxide, OH-

38
Q

Hydrochloric acid

39
Q

Sulfuric acid

40
Q

Nitric acid

41
Q

pH 1 has a ___ greater concentration of H+ than pH2

42
Q

pH 1 has a ____ greater concentration of H+ than pH3

Chemistry (11 decks)

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