metals and reactivity

Question 1

What are the properties of metals?

Answer 1

> they are malleable
they are ductile
they are good conductors of heat/ electricity
they have high melting and boiling points

Question 2

do metals gain or lose electrons?

Answer 2

metals lose electrons to form positive ions

Question 3

How does the reactivity of metals vary in the periodic table?

Answer 3

increases down the group and across a period

Question 4

…

Answer 4

Inert (noble metals) do not react with oxygen, water or acids

Question 5

example of noble metals

Answer 5

gold and platinum

Question 6

What is the reactivity series?

Answer 6

list of metals and some nonmetals in order of their reactivity

Question 7

What are the nonmetals, and what is their purpose?

Answer 7

hydrogen and carbon, classify more reactive and less reactive metals

Question 8

reaction of metals with oxygen

Answer 8

> most reactive metals(high in the reactivity series) react more fast with oxygen.
least reactive(lower in the reactivity series) react slower with oxygen.

Question 9

….

Answer 9

> when a metal reacts with oxygen, a metal oxide is formed which is a basic oxide..( except zinc and aluminium) they form amphoteric oxides

Question 10

What is a basic oxide and an amphoteric oxide?

Answer 10

> a basic oxide is a metal oxide
ampoteric oxide is an oxide that has both metal and non metal properties

Question 11

2Mg(s) + O2(g) → 2MgO(s).
¿What does this reaction represent?

Answer 11

magnesium is oxidised to form magnesium oxide

Question 12

4Li(s) + O₂(g) → 2Li₂O(s)
What does this reaction represent?

Answer 12

it represents lithium being oxidised

Question 13

what happens in a displacement reaction?

Answer 13

a more reactive metal displaces a less reactive metal

Question 14

reactivity series order

Answer 14

> group one metals(k,s,l)
group two metals(c,m)
carbon
zinc
iron
hydrogen
copper

Question 14

which metal can not undergo displacement reaction

Answer 14

copper

Question 15

which metals will react with dilute acids?

Answer 15

metals above hydrogen in the reactivity series

Question 16

what does the reactivity series look like in diplacement reactions

Answer 16

the more reactive metal replaces the least reactive metal from a compound

Question 17

What is a thermal decomposition reaction?

Answer 17

a type of reaction where a compound breaks down in the presence of heat (there is only one reactant)

Question 18

which compounds undergo thermal decomposition?

Answer 18

> metal hydroxides
metalcarbonates
metal nitrates

Question 19

what is an ore?

Answer 19

a rock from which a metal can be extracted

Question 20

what are common ores made up of

Answer 20

metal oxides/ sulfur

Question 21

what is iron ore

Answer 21

hematite Fe₂O₃

Question 22

what is aluminium ore

Answer 22

bauxite Al₂O₃

Question 23

what is zinc ore

Answer 23

inc blend ZnS

Question 23

what are lead and copper ores

Answer 23

> lead ore is galena PbS >copper ore is copper sulfide CuS

Question 24

What does the process of extracting a metal from its ore depend on?

Answer 24

the metals reactivity

Question 25

which method do metals less reactive than hydrogen (inert) undergo?

Answer 25

certain chemical reactions

Question 25

which method do reactive metals undergo?

Answer 25

electrolysis

Question 25

which method do metals less reactive than carbon undergo?

Answer 25

heating with carbon( reduction method)

Question 26

how do u extract a metal less reactive than carbon?

Answer 26

> the metals (zinc, iron etc..) > their metal oxides are heated with carbon, the oxygen is removed from the metal and converted to carbondioxide, carbon geins oxygen and the letal looses oxygen

Question 27

why dont all metals undergo electrolysis

Answer 27

because it is codtly since it requires alot of energy, cheaper methods are used for less reactive metals

Question 28

How do we extract copper from its ore?

Answer 28

reduction by carbon, to form copper and carbondioxide

Question 29

How do we extract iron?

Answer 29

>iron oxide Fe₂O₃, reacts with carbon to form molten iron and carbon monoxide gas CO >

Question 30

raw materials for the extraction of iron

Answer 30

>coke (mainly carbon) >hematite (iron ore) >limestone (calcium >carbonate) >air (oxygen)

Question 31

where does the extraction of iron occur?

Answer 31

in the blast furnace

Question 32

What is the main ore from which iron is extracted?

Answer 32

Hematite (Fe2O3) is the main ore from which iron is extracted.

Question 32

True or False: Iron can be extracted from its ore using only electrolysis.

Answer 32

False. Iron is primarily extracted using a blast furnace.

Question 33

Fill in the blank: The process of extracting iron from its ore involves a chemical reaction with _____ and _____ in a blast furnace.

Answer 33

carbon and oxygen

Question 34

What is the role of coke in the extraction of iron?

Answer 34

Coke acts as a reducing agent and provides the necessary heat for the reaction.

Question 35

What are the main products obtained after the reduction of iron ore in a blast furnace?

Answer 35

The main products are molten iron and carbon dioxide.

Question 36

Multiple Choice: What temperature range is typically reached in a blast furnace during the extraction of iron? A) 300-500°C B) 1000-1200°C C) 1500-2000°C

Answer 36

C) 1500-2000°C

Question 37

What is slag, and how is it formed during the iron extraction process?

Answer 37

Slag is a by-product formed from impurities in the ore and flux, which floats on top of molten iron.

Question 38

Describe the chemical equation for the reduction of iron(III) oxide using carbon.

Answer 38

The equation is: Fe2O3 + 3C → 2Fe + 3CO.

Question 39

True or False: Iron extracted from the blast furnace is 100% pure.

Answer 39

False. The iron is not pure and is known as pig iron.

Question 40

What is the purpose of limestone added to the blast furnace?

Answer 40

Limestone is added to remove impurities by forming slag.