C5

Question 1

The reactivity series

Answer 1

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

Question 2

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

Answer 2

displace, compound

Question 3

The reactivity of metal is related to ____

Answer 3

tendency to form positive ions

Question 4

more reactive metals form positive ions faster/slower

Answer 4

faster

Question 5

reactions of metals with acids

Answer 5

metal + acid -> salt + hydrogen (MASH)

Question 6

reactions of a metal with oxygen

Answer 6

metal + oxygen -> metal oxide

Question 7

reactions of metal oxides with acids

Answer 7

metal oxide + acid -> salt + water

Question 8

reactions of metal carbonates with acids

Answer 8

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

Question 9

zinc + hydrochloride acid ->

Answer 9

zinc chloride + hydrogen

Question 10

iron + oxygen ->

Answer 10

iron oxide

Question 11

magnesium oxide + sulfuric acid ->

Answer 11

magnesium sulfate + water

Question 12

tin carbonate + hydrochloric acid ->

Answer 12

tin chloride + water + carbon dioxide

Question 13

what is oxidation?

Answer 13

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

Question 14

what is reduction?

Answer 14

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

Question 15

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

Answer 15

oxidisation

Question 16

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

Answer 16

reduction

Question 17

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

Answer 17

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

Question 18

t/f? salts are ionic compounds

Answer 18

true

Question 19

hydrochloric acid (symbol and what it reacts to make)

Answer 19

HCl, reacts to make chloride salts

Question 20

sulfuric acid (symbol and what it reacts to make)

Answer 20

H2SO4, reacts to make sulfate salts

Question 21

nitrate acid (symbol and what it reacts to make)

Answer 21

HNO3, reacts to make nitrate salts

Question 22

iron + hydrochloric acid ->

Answer 22

iron chloride + hydrogen

Question 23

zinc + sulfuric acid ->

Answer 23

zinc sulfate + hydrogen

Question 24

magnesium + nitric acid ->

Answer 24

magnesium nitrate + hydrogen

Question 25

how can soluble salts be made?

Answer 25

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

Question 26

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 _____

Answer 26

- solid metal compound - reacts - excess solid - heated - crystallise - make sure no acid remains to form an impurity in the salt product

Question 27

what apparatus is required for a titration

Answer 27

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

Question 28

titration method:

Answer 28

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

Question 29

cm^3 -> dm^3 =??

Answer 29

DIVIDE by 1000

Question 30

number of mols=

Answer 30

concentration x volume

Question 31

colour change for methyl orange:

Answer 31

yellow- red

Question 32

colour change for phenolphthalein:

Answer 32

colourless- pink

Question 33

What is an alkali

Answer 33

A base which is soluble in water

Question 34

Strong acids-

Answer 34

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

Question 35

Weak acids-

Answer 35

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

Question 36

Acidic solutions contain

Answer 36

Hydrogen, H+

Question 37

Alkalines contain-

Answer 37

Hydroxide, OH-

Question 38

Hydrochloric acid

Answer 38

HCl

Question 39

Sulfuric acid

Answer 39

H2SO4

Question 40

Nitric acid

Answer 40

HNO3

Question 41

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

Answer 41

10x

Question 42

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

Answer 42

100x

Question 43

Neutralisation

Answer 43

Occurs between an acid and base

Question 44

Alkalis are bases which

Answer 44

Are soluble in water- many bases aren't soluble in water

Question 45

Neutralisation reactions produce:

Answer 45

A salt and water

Question 46

Acids release what when they are dissolved in water?

Answer 46

H+ ions

Question 47

Calculating concentration of unknown acid from titration-

Answer 47

A. Calculate mean titre volume - from concordant results only B. Calculate mols of alkali used, then divide by mean vol

Question 48

Acidic solutions contain-

Answer 48

Hydrogen ions

Question 49

Alkali solutions contain

Answer 49

Hydroxide [OH-]

Question 50

Strong acids do what in water?

Answer 50

Fully ionise

Question 51

Strong acids can be concentrated or dilute, which depends on...

Answer 51

Amount of acid dissolved in 1cm3 of water

Question 52

Weak acids will have a higher pH (so less acidic) than a strong acid of the same...

Answer 52

Concentration

Question 53

Half equations are to show what happens to each what in terms of what?

Answer 53

Reactant,, electrons

Question 54

Fe(s) -->

Answer 54

Fe2+(aq) + 2e- - iron loses 2 electrons to form an iron ion- it's oxidised

Question 55

Cu2+(aq) + 2e- -->

Answer 55

Cu(s) Copper ions gains 2 electrons to form a Cu atom-- its reduced