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Metals Flashcards

1
Q

Where are metals found in the periodic table?

A

metals are found on the left of the table- to the left of the ladder which starts above aluminium and steps down to the right

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2
Q

List five properties of metals

A

conducts electricity and heat

shiny

malleable

ductile

some are magnetic

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3
Q

Which group is called the alkaline metals?

A

Group 1

Li

Na

K

Rb

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4
Q

What group is called the Alkaline Earth Metals?

A

Group 2

Be

Mg

Ca

Sr

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5
Q

What is special about the transistion metals?

A

They form colourful compounds

&

They often have more than one valency

Fe 2+ and Fe 3+

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6
Q

What group are called the Halogens?

A

Group 7

F

Cl

Br

I

They are all diatomic!

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7
Q

What group is called the noble gases?

A

Group 0

He

Ne

Ar

Kr

they all have a full outer shell and are inert (unreactive)

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8
Q

Name the four metals less reactive than hydrogen in the reactivity series

A

Hydrogen

Copper

Silver

Platinum

Gold- unreactive

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9
Q

Name the five metals more reactive than carbon in the reactivity series

A

potassium

sodiium

calcium

magnesium

aluminium

carbon

All these metals must be extracted using electrolysis as carbon cannot displace them as it is less reactive

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10
Q

Name the four metals between carbon and hydrogen in the reactivty series

A

Carbon

Zinc

Iron

Tin

:Lead

Hydrogen

These metals can be extracted from their ores using carbon or coke in a blast furnace

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11
Q

Why can iron be reduced or extracted from its metal ore using coke (carbon)?

A

Carbon is more reactive than iron

Carbon displaces iron

iron is reduced

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12
Q

Henry threw some copper into some hydrochloric acid. He expected to see a reaction, some fizzing, but nothing happened. explain why?

A

copper is less reactive than hydrogen

copper cannot displace hydrogen and so it does not react

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13
Q

Describe three properties of the group 1 metal sodium

A

soft - can be cut with a knife

shiny when cut but then quickly reacts and becomes dull

low melting point

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14
Q

Finish the general equation

reactive metal + water –>

A

remember the fizzing?

reactive metal + water –> metal hydroxide + hydrogen

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15
Q

What is the chemical reaction between lithium and water?

A

Li (s) + H2O(l) –> LiOH(aq) + H2(g)

Lithium hydroxide is an alkali- it will turn universal indicator blue

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16
Q

What would you observe if you put some sodium in water?

How would this compare to potassium in water?

A

For sodium

fizzing, moving around on the surface of the water

melts into a ball, metal disappears

For potassium - it is more reactive

more vigorousfizzing

moving around on the surface of the water more quickly

melts into a ball and bursts into flame (lilac in colour)

metal disappears more rapidly

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17
Q

What is the chemical reaction between sodium and water?

A

Na (s) + H2O(l) –> NaOH(aq) + H2(g)

sodium hydroxide is an alkali- it will turn universal indicator blue

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18
Q

What is the chemical reaction between potassium and water?

A

K (s) + H2O(l) –> KOH(aq) + H2(g)

potassium hydroxide is an alkali- it will turn universal indicator blue

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19
Q

How would the reaction differ between potassium and rubidium?

A

Potassium

lilac flame

Rubidium

explosive

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20
Q

What is an alloy?

A

A mixture of a metal and metal or a metal and non-metal which changes both the physical and chamical properties

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21
Q

Give three examples of an alloy

A

Brass- copper + zinc

Bronze- copper + tin

Steel- iron + carbon

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22
Q

How does the introduction of a different sized atom to a pure metal change its physical properties.

A

The smaller atoms disrupts the arrangment of the metal ions,

They no longer arrange themselves in neat rows

They do not have layers which can slide over one another

They are no longer malleable- they are harder and stronger

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23
Q

When calcium reacts with hydorchloric acid, hydrogen forms.

How can the hydrogen be collected?

A

hydrogen can be collected by downward displacement of water

OR

downward displacement of air - upside down test tube- hydrogen is less dense than air and will rise into the test tube and push the air downward

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24
Q

What are the products in this reaction?

Mg + H2O (g) –>

steam

A

Mg + H2O (g) –> MgO + H2

steam

with steam the oxide is formed-not the hydroxide!

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25
Both potassium and sodium are found in group 1 Why is potassium more reactive than sodium?
- potassium **atom is larger** - outer electrons of potassium are **further from the nucleus** - **less electrostatic attraction** between the negative outer electrons and positive nucleus - **easier to remove** the outer electron from potassium - Also, there are **more shells** between the nucleus and outer electrons in potassium - the electrons in these shells repel the outer electrons and is called **electron shielding** - easier to remove the outer electron from potassium - **potassium is more reactive for these two reasons!**
26
Complete the reaction Al + Fe2O3 --\>
Thermite reaction!! Is aluminium more reactive than iron? YES! 2Al + Fe2O3 --\> Al2O3 + 2Fe Aluminiuim is more reactive than iron aluminium displaces the iron This is a **displacement reaction**
27
Complete this general reaction metal + steam --\>
Metal + steam --\> metal oxide + hydrogen You still get hydrogen but now you have the oxide- not the hydroxide
28
What is the test for hydrogen gas?
Flaming splint you hear a squeaky pop!
29
Why does it take time for aluminium to start reacting with an acid?
aluminium forms an impermeable aluminium oxide layer. The acid must get through that layer before it comes into contact with the pure metal. This impermeable oxide layer on aluminium is an advantage- iron reacts with oxygen and rusts entirely through the metal but aluminium forms an impermeable oxide layer protecting the pure aluminium below.
30
Complete the general word equation more reactive metal + less reactive metal compound --\>
**more reactive metal** + less reactive metal compound --\> **more reactive metal** compound + less reactive metal the more reactive metal **displaces** the less reactive metal This is a **displacement reaction**
31
Complete the displacement reaction and describe what you would observe Zn + CuSO4 --\>
Is zinc more reactive than copper? Yes Zn + CuSO4 --\> ZnSO4 + Cu greysolid & blue solution --\> colourless solution & orange/pink soild
32
Below is the thermite reaction!! 2Al + Fe2O3 --\> Al2O3 + 2Fe Where is this used and is the reaction an exothermic or endothermic reaction? How do you know?
Thermite reaction is used to **connect (fuse) iron rails together on a railway**. This reaction is carried out above the seam between the two rails The reaction is **exothermic**- it releases heat rapidly and exceed the melting point of iron which melts out the bottom of the vessel and onto the seam.
33
Complete the displacement reaction and describe what you would observe Fe + ZnSO4 --\>
Is iron more reactive than zinc? No- the rion cannot displace the zinc No reaction - grey metal in colourless solution with no change to appearance
34
Complete the metal displacement reaction Ca + MgNO3 --\>
Ca + 2MgNO3 --\> Ca(NO3 )2 + 2Mg
35
Which reaction will be more vigorous and why? Mg + Fe2O3 --\> Zn + Fe2O3 --\>
The Mg and Fe reaction will be more vigorous because Mg and Fe are further apart in the reactivity series. The further apart metals are in the reactivity series the more violent their displacement reactions will be.
36
How can you use metal and acid reactions to order metals in terms of reactivity?
Place the metals in the same concentration and type of acid and compare the rate of fizzing the more vigorous the fizzing, the more reactive the metal
37
Define a metallic bond
the electrostatic attractionn between potive metal ions and the negative delocalised electrons
38
Describe the stuucture of a metal
regular arrangement of metal ions layers of metal ions surrounded by a sea of delocalised electrons
39
Why do metals have high melting points?
- many strong metallic bonds in a giant structure - requires a lot of energy to overcome
40
als
41
Are metals soluble in water or organic solvents?
No- they are not soluble in either. NOTE: reactive metals react with water but they are not soluble
42
43
Whjy do metals conduct electricity?
- metals have delocalised **electrons which are free to move** ## Footnote **and carry charge**
44
Why are metals malleable?
- metal ion layers can slide over one another - without distrubing the metallic bonds
45
Which four materials are added to a blast furnace?
iron (III) oxide limestone coke hot air
46
What are the products from a blast furnace?
iron metal carbon dioxide slag
47
Which product in a blast furnace causes a concern from the environment?
**carbon dioxide** is a **greenhouse gas** which may lead to **global warming**
48
Which reaction gets everything hot in the blast furnace?
combustion of coke C + O2 --\> CO2 exothermic!!!
49
Which reaction forms the reducing agent in the blast furnace?
C + CO2 --\> 2CO coke is added in excess so that CO is formed (carbon monoxide) carbon monoxide is the reducing agent- it reduces the iron (III) oxide
50
What is the formula for haematite?
iron (III) oxide
51
What is the name of iron ore?
Haematite
52
Complete the redox reaction which happens in the blast furnace Fe2O3 + 3CO --\>
Fe2O3 + 3CO --\> 3CO2 + 2Fe Fe has been reduced - lost oxygen C is oxidised - gained oxygen
53
Explain how the reaction below is a redox reaction- a reaction where both oxidation and reduction occurs Fe2O3 + 3CO --\> 3CO2 + 2Fe
Fe2O3 + 3CO --\> 3CO**2** + 2**Fe** Fe has been reduced - lost oxygen C is oxidised - gained oxygen
54
Which mnemonic is used to work out which elements are reduced or oxidised in a reacion?
OIL RIG OIL - oxidation is loss of electrons RIG - reduction is gain of electrons REMEMBER: if the atom has gained or lost oxygen you must speak about that and not the gain or loss of electrons
55
Why do we add limestone to a blast furnace?
To get rid of the impurity found in iron ore First- the limestone thermally decomposes to calcium oxide because the blast furnace is hot CaCO3 --\> **CaO** + CO2 The calcium oxide then reacts with the **impurity silicon dioxide** to form calcium silicate OR SLAG **CaO** + SiO2 --\> CaSiO3 SLAG The slag is less dense than the molten iron and float on top
56
Complete the thermal decomposition of calcium carbonate in a blast furnace CaCO3 --\>
Thermal decomposition means that the compound breaks apart by heating CaCO3 --\> CaO + CO2
57
Complete the reaction which forms SLAG in a blast furnace CaO + SiO2 --\>
This is a neutralisation reaction metal oxide CaO - acidic non-metal oxide SiO2 - alkaline CaO + SiO2 --\> CaSiO3 alkaline + acid --\> salt
58
What is the name of the impurity in haematite?
silicon dioxide SiO2
59
What is the chemical formula for SLAG which forms in a blast furnace/
CaSiO3
60
Why is it easy to separate SLAG from iron metal in a blast furnace?
Both are molten (melted) but the slag is less dense and floats on top of the molten iron
61
What type of reaction is this? C + O2 --\> CO2
combustion or oxidation as carbon gained oxygen
62
What type of reaction is this? CaCO3 --\> CaO + CO2
Thermal Decomposition the CaCO3 is decomposing or breaking apart
63
What is the reaction for rusting of iron?
4Fe + 3O2 + 5H2O --\> 2Fe2O3•5H2O iron needs both water and oxygen to rust! Note: salt in not needed but is a catalyst- it speeds up the reaction by lowering hte activation energy but is not used in the reaction
64
What is the chemical formula for rust?
Fe2O3
65
What is the chemical name for rust?
iron (III) oxide
66
Name three barrier methods to stop iron from rusting
paint - to stop oxygen and water getting to iron coat in plastic- to stop oxygen and water getting to iron oil or grease- to stop oxygen and water from getting to irion
67
Name two sacrificial methods to stop iron from rusting
galvanising- coating in zinc- used for buckets etc sacrificial protection with block of magnesium or zinc- used for bridges or large structures where coating in zinc is too expensive
68
What is the name of this this protection method for iron? Fe2O3 + 3Zn --\> 3ZnO + 2Fe
sacrificial protection Zn metal --\> Zn 2+ + 2e- zinc reacts and gives 2 electrons to any iron ions which have formed to reduce it back to iron metal- protecting the iron and sacrificing the zinc Fe 3+ + 3 e- --\> Fe metal
69
70
Which metal is being reduced and which one is being oxidised? How do you know? Fe2O3 + 3Zn --\> 3ZnO + 2Fe
Fe2**O**3 + 3Zn --\> 3Zn**O** + 2Fe iron is reduced as it is losing oxygen zinc is oxidised as it is gaining oxygen
71
Metal carbonates thermally decompose to form a metal oxide and carbon dioxide Which properties of carbon dioxide prevents us from collecting it by downward displacement of water and allows us to collect it by downward displacement of air?
carbon dioxide is soluble in water- if collected by downward dislacement of water the carbon dioxide would dissolve in the water carbon dioxide is more dense than air- if a tube was placed in a upright test tube the more dense carbon dioxide would fill the test tube and push the air out.
72
What is the test for carbon dioxide?
bubble though limewater limewater turns cloudy
73
What would you observe in this thermal decomposition reaction? CuCO3 --\> CuO + CO2 green black
green power moves as gas escapes the green powder turns black
74
Write the thermal decomposition reaction of Copper (II)carbonate
CuCO3 --\> CuO + CO2
75
Complete the reaction for the thermal decomposition of calcium carbonate
CaCO3 --\> CaO + CO2
76
Why can't we extract aluminium from aluminium ore using coke (carbon)
Carbon is less reactive than Aluminium it cannot displace aluminium from aluminium ore?
77
What is the name of aluminium ore?
Bauxite Al2O3
78
What method do we use for the extraction of aluminium form aluminium ore?
electrolysis
79
Define electrolysis
The decomposition of a compound using electricity
80
Why do we need to melt the aluminium ore before carying our electrolysis?
Aluminium ore is ionic, when melted the metal ions are free to move and carry charge we need electricity to pass through the molten ore for electrolysis to occur
81
What is added to aluminium oxide to make the extraction of aluminium cheaper?
Cryolite is added to the aluminium ore- this reduced the melting point of the ore Less heat is used- cheaper process
82
Why is electrolysis more expensive than using a blast furnace to extract a metal from its metal ore?
Electrolysis used both electricity and heat to extract the metal. Blast furnace only needs heat
83
Which ions are free to move when Al2O3 is melted during electrolysis
Al 3+ O 2-
84
When aluminium ore is molten the two ions which are mobile are Al 3+ O 2- Which ion will move toward the cathode? The negative electrode? Which ion eill move towards the anode? the positive electrode?
Al 3+ is positively charged and will be attracted to the cathode or negatively charge electrode O 2- is negatively charged and will be attracted to the anode or positviely charge electrode
85
Why is the entire container charge negatively in the electrolysis of aluminium ore?
The positive aluminium ions will be attracted to the bottom of the container allowing the aluminium to form there- it can then be tapped off
86
Why does aluminium oxide conduct when molten (melted) but not when it is a solid?
Aluminium oxide is ionic, when molten the ions are free to move and carry charge When in the solid form the ions are not free to move and cannot carry charge
87
Give two properties of carbon dioxide
It is soluble in water to form an acid It is more dense than air
88
Use the image below to explain why alloys are less malleable than pure metals
A pure metal will have a regular arrangement of atoms. The rows of metal atoms can slide easily over one another without disrupting the metallic bond Alloys are a mixture of metals or a metal and non-metal. This often disrupts the regular arrangement. There are no complete rows of atoms which can slide over each other. Not malleable-harder substance

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