Metals

Question 1

metallic bonding

Answer 1

the electrostatic force of attraction between positively charged ions and delocalised electrons (electrons that are free to move)

Question 2

ore

Answer 2

a naturally occurring solid material from which a metal or valuable mineral can be extracted, and which contains a relatively high proportion of the metal, making extraction profitable and worthwhile

Question 3

mineral

Answer 3

a solid, naturally occurring inorganic substance

Question 4

native

Answer 4

metals found pure (uncombined as elements) in their metallic form in nature and which are unreactive elements

Question 5

reactivity series - group A metals

Answer 5

• mercury, silver, gold
• least reactive metals, found uncombined in the Earth’s crust as an element or ore
• extracted from their ore using heat alone

Question 6

reactivity series - group B metals

Answer 6

• zinc, iron, tin, lead, copper
• moderately reactive metals
• extracted from their ore by heating with carbon or carbon monoxide
• C / CO oxidised to form CO₂ forcing metal to be reduced
• C / CO must be more reactive than metal being reduced

Question 7

reactivity series - group B metals - equation

Answer 7

metal oxide + carbon / carbon monoxide ➡️ metal + carbon dioxide

Question 8

reactivity series - group C metals

Answer 8

• potassium, sodium, calcium, magnesium, aluminium
• very reactive metals
• extracted from their ore using electrolysis
• positive ions gain electrons (are reduced) at the negative electrode
• negative ions lose electrons (are oxidised) at the positive electrode

Question 9

reactivity series - group C metals - why must a DC supply be used?

Answer 9

so that the same reaction occurs at the same electrode all the time, meaning that the products can be identified

Question 10

reduction

Answer 10

the removal of oxygen / the gain of electrons

Question 11

oxidation

Answer 11

the addition of oxygen / the loss of electrons

Question 12

oil rig 🏗

Answer 12

• oxidation is loss (of electrons)

* reduction is gain (of electrons)

Question 13

metal + water ➡️

Answer 13

metal hydroxide + hydrogen

Question 14

metal + oxygen ➡️

Answer 14

metal oxide

Question 15

metal + acid ➡️

Answer 15

salt + hydrogen

Question 16

displacement reactions rule

Answer 16

the metal which is higher in the electrochemical series will displace a metal lower in the series from its compounds in solution

Question 17

half cell

Answer 17

a metal in solution of its own ions

Question 18

electrolyte

Answer 18

an electrically conducting solution containing ions

Question 19

ion bridge examples

Answer 19

• folded filter paper soaked in salt water
• glass u-tube containing potassium chloride solution / gel
• string soaked in salt water
• a porous plug in the middle of a u-tube (the solutions for each half cell go in either side of the plug)

Question 20

electrochemical cell voltage rule

Answer 20

the further apart the metals are in the ECS the greater the voltage produced

Question 21

electrochemical series

Answer 21

a measure of how easily a metal atom loses electrons to form positive ions in solution

Question 22

simple cell

Answer 22

made by linking two metals with an electrolyte

Question 23

electrochemical cell

Answer 23

the arrangement of two metals connected by wires to a meter with a wet filter paper placed between them

Question 24

ion bridge

Answer 24

completes the circuit because it allows ions to move, carrying the current between the two halves of the cell