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Chemistry IGCSE > Metals FOR NOW!!! > Flashcards

Metals FOR NOW!!! Flashcards

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1
Q

What is the bonding of metals described?

A

Cations and delocalized electrons held together with delocalized electrons.

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2
Q

What is the structure of a metallic bond?

A

Lattice of cations surrounded by delocalized electrons.

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3
Q

What is an alloy?

A

A mixture containing at least one metal.

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4
Q

What are the charectaristics of alloys and are those charectaristics from mixtures or coumpounds?

A
  • Easy to seperate (mixture)
  • No fixed ratio (mixture)
  • Rnge of melting points (mixtures)
  • Two elements bonded (compund)
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5
Q

What do alloys change?

A
  • Reactivity
  • Malleablility
  • Melting point
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6
Q

Why is it easy to replace a metal ion in a metalic bond with a different one of the same charge?

A

Because the electrons in a metallic bond are always moving, which causes bonds to re-arrange.

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7
Q

What is the malleability of mettalic bonds (one type of ionic element)?

A

They are malleable because the ions can move without breaking metallic bonds.

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8
Q

How malleable are pure metals?

A

Pure metals are malleable. The layers can easily slide over eachother.

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9
Q

How malleable are alloys?

A

They are less malleable than pure metals because they have differently sized atoms/ions which caus ethe layers to not be able to slife over eachother as easily. This is because regular lattice is disrupted.

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10
Q

How do metals get a full outer energy level?

A

They react by losing electrons to form cations.

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11
Q

What defines a more reactive chemical?

A

The less energy required to lose electrons.

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12
Q

Why is energy needed for metals to achieve a full outer energy level?

A

The energy is neede to break the electrostatic forces between outer electrons and the nucleus.

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13
Q

What are the reactivity rules from most important to least?

A
  1. No. of electrons lost/excluding Ag (more = more enregy)
  2. No. of occupied energy levels/distance between nucleus and outer energy levels (more = less energy)
  3. No. of protons/atomic number (more = more energy)
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14
Q

What metals react with water?

A
  • Group 1
  • Ca
  • Sr
  • Ba
  • Ra
  • Mg (reacts but very slowly)
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15
Q

Metal +water =>

A

metal hydroxide + hydrogen

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16
Q

What is the defenition of dispacement?

A

A more reactive element replaces a less ractive element from its compound form (compound + metal).

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17
Q

How does displacement work?

A

The more reactive element loses an electron and bonds to the compund (the electron is transferred).

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18
Q

What observations can be present in a displacement reaction?

A
  • Temp. increase (greater difference in reactivity => higher temp).
  • Solid changes color.
  • Solution changes color.
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19
Q
A
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20
Q

Why are displacement reactions used?

A

To determine the order of reactivity because they give a posotive/negative result.

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21
Q

What is the defenition of extraction?

A

Obtaining a pure element/metal from a compound.

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22
Q

Why are there not many pure metals naturally?

A

Because pure metals react with O2/H2O over time to from compunds.

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23
Q

What is the reactivity series?

A
  1. K
  2. Na
  3. Li
  4. Ca
  5. Mg
  6. Al
  7. Zn
  8. Fe
  9. Cu
  10. Ag
  11. Au
24
Q

Group the reactivity series into how you extract them.

A
  • K, Na, Li, Ca, Mg, Al = electrolysis
  • Zn, Fe = Displacement wit carbon
  • Cu, Ag = Decomposition
  • Au = No extraction needed
25
Q

Metal + steam (hot water) =>

A

Metal oxide + hydrogen

26
Q

How is the experiment for metal + steam set up?

A
27
Q

What are the observations of Mg + H2O?

A
  • Bursts with white flame
  • Produces white solid
28
Q

What chameicals don’t ract with steam at all?

A
  • Cu
  • Ag
  • Au
29
Q

What are the observations of Zn + H2O?

A
  • Produces white solid (ZnO), but is yellow when hot.
  • Burns with blue flame
  • Glows red
30
Q

What are the observations of Fe + H2O?

A
  • Produces orange/brown solid
  • NOT DONE WITH FLASHCAD
31
Q

Why do we use carbon for displacement (reactivity series).

A
  1. Abundnat
  2. Produces a gaseoous oxide (easy to seperate)
32
Q

Why does the metal oxide need to be a liquid in electrolysis?

A

Because it needs to conduct and since it is ionic, it needs to be a liquid for this to occure. High mpt :(

33
Q

Draw a diagram of electrolysis.

A
34
Q

What goes to the cathode?

A

The anion (+ ion)

35
Q

What goes to the anode?

A

The cation (- ion)

36
Q

What is the defenition of an iron ore?

A

Haematite or iron (III) oxide (orange/brown)/siliconeoxide (sand)

37
Q

What is the overall reaction of the extrction of Fe?

A

2Fe2O3(s) + 3C(s) => 3CO2(g) + 4Fe(s)

38
Q

What is bad about the extraction of Fe?

A
  • Climate change
  • Acid rain
39
Q

What does acid rain imapct?

A
  • Trees
  • Fish
  • Limestone buildings
40
Q

What is the firts reaction for the extraction of Fe and the observations?

A

C + O => CO2
* Combustion
* Exothermic => releases heat (2000 degrease celcius)

41
Q

Wha the is the second reaction for the extraction of Fe and the observations?

A

CO2 + C => 2CO (g) carbonmonoxide (toxic)

42
Q

What is the third reaction for the extraction of for the extraction of Fe and the observations?

A

3CO(g) + Fe2O3 (s) => 2Fe (l) + 3CO2
* Fe is contaminated with SiO2 and will cause it to become brittle.

43
Q

What is the equation for removing impurities from Fe?

A

CaCO3 limestone = 2000°C =decomposes=>CaO + CO2 :(

CaO base + SiO2 =neutralisation=> CaSiOcalciumsilicate (less dense than SiO2

44
Q

Draw a diagram of the aparatus that extracts Fe and how it works.

A
O2 cannot reach Fe / Calciumsilicate is less dense than SiO2
45
Q

Corrosion

A

The reaction of metals to from compounds causing their properties to change.

46
Q

Metal + oxygen

A

=> Metal oxide

47
Q

Metal + water

A

=> Metal hydroxide + hydrogen

48
Q

Metal + acid

A

=> Salt + hydrogen

49
Q

Iron + oxygen

A

=> hydrated iron (III) oxide
rust

50
Q

What is the symbol for rust?

A

Fe3 . xH2O

51
Q

When iron rusts, does the rust form a protective layer on the iron?

A

NO! The oxygen and water can still enter the iron underneath and can still react.

52
Q

What are the ways of protecting Fe?

A
  1. Covering Fe with paint, oil or another metal<= best option
  2. Sacrificial protection => cover in a more reactive metak that recats instead of iron. All metals except for Zn (galvanising) are more reactive thatn Fe
53
Q

What will happen to iron in a test tube with water air.

A

Rust

54
Q

What will happen to iron in a test tube with boiled water and oil?

A

No rust because the oxygen is removed and the oil prevents any more from entering.

55
Q

What will happen to iron in a test tube with air and CaCl2? Also what is CaCl2?

A

No rust because CaCl2 is anhydrous and removes the water.

56
Q

What will happen to iron in a test tube with water and salt air (WaCl)

A

Rusts a lot because salt air is a catalyst for rusting.

57
Q
A

Chemistry IGCSE (12 decks)

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