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chemistry 😢🥹 > metals > Flashcards

metals Flashcards

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1
Q

describe the structure of a metal

A
  • lattice of positive ions
  • sea of delocalised electrons
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2
Q

define metallic bonding

A

the electrostatic attraction between the positive metal ions and the negative delocalised electrons

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3
Q

is metallic bonding a strong or weak attraction

A

very strong

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4
Q

what is thermal decomposition

A

a thermal decomposition reaction is when heat energy is used to break down a substance

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5
Q

what do metal carbonates decompose into

A

metal oxides and carbon dioxide
metal carbonate -> metal oxide + carbon dioxide

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6
Q

what occurs when copper carbonate is thermally decomposed

A

turns from green to black and releases co2

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7
Q

what is downward delivery

A
  • carbon dioxide is denser than air so its often collected by downward delivery
  • this means it sinks to the bottom of the tube
    -and it stays there until you need to use it
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8
Q

what are the properties of metals

A
  • high melting and boiling point
  • conduct electricity
  • malleable
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9
Q

list the metal reactivity series from low to high

A
  • Au (lowest)
  • Ag
  • Cu
  • H
  • Pb
  • Fe (middle)
  • Zn
  • C
  • Al
  • Mg
  • Ca
  • Li
  • Na
  • K (highest)
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10
Q

give the metal + water equation

A
  • metals react with cold water to form metal hydroxides and hydrogen
  • metal + water -> metal hydroxide + hydrogen
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11
Q

observations of metal + water reactions

A
  • effervescence: due to the hydrogen gas produced
  • solod disappears: due to being used up in the reaction
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12
Q

what are the metals in group 1 called and how do they react in water

A
  • alkali metals
  • they react violently in water
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13
Q

what are the reactions of Li and K in water

A
  • solid floats: it is less dense than water
  • effervescence: hydrogen gas is produced
  • solid moves: it is propelled by the effervescence across the surface
  • solid disappears: it is used up in the reaction
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14
Q

what is the group 1 reactivity series

A

Li
na
k
rb
cs
- the group 1 metals get more reactive as you go down the group

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15
Q

why do group 1 metals get more reactive as you go down the group

A

when a group 1 metal reacts it loses its outer shell electron to get a full outer shell, this happens more easily as you down the group because:
- the atoms get bigger and have more shells
- the outer electron is further from the nucleus
- the attraction between the nucleus and the outer electron is weaker

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16
Q

what is the equation for the metal + steam reactions

A

metal + steam -> metal oxide + hydrogn

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17
Q

where does the metal+steam reaction take place

A

horizontal tube

18
Q

what is the method for reacting magnesium and steam

A
  • mg + h2o -> mgO + H2
  • wet wool is heated to generate steam for the mg to react with
  • the h2 gas produced is ignited safely to destroy it
19
Q

why do metals react with cold water and steam to produce different products ?

A

steam gas more energy so bith bonds in the water molecule can break

20
Q

what is the acid + metal equation

A

acid + metal -> salt + hydrogen

21
Q

what are the observations of an acid + metal reaction

A
  • effervescence: because hydrogen gas is produced
  • the metal disappears: because its used up in the reaction
22
Q

what is a displacement reaction

A

more reactive metals can displace less reactive metals from their compounds

23
Q

observations of a displacement reaction

A
  • solid colour change
  • solution colour change
24
Q

what is an ore

A

metals found in the earths crust as compounds of oxygen and sulphur. this is because over a long time those metals have reacted with oxygen and sulphur.

25
Q

how do you extract ores

A

metals in ores need to be chemically extracted from their compounds.
how this is done depends on their reactivity

26
Q

how are native metals extracted

A

native metals dont need to be chemically extracted because they exist on their own

27
Q

how are metals extracted using electricity

A
  • metals more reactive than carbon cannot be extracted by carbon
  • electricity is used to break down their ore compounds
28
Q

how are metals extracted from their ores using carbon extraction

A
  • metals less reactive than carbon can be displaced by carbon
29
Q

what is the definition of rusting

A

a chemical process by which iron is oxidised to form rust

30
Q

what is the chemical name for rust

A

hydrated iron(III) oxide

31
Q

what does rust require to occur

A
  • oxygen
  • water
32
Q

how can rust be prevented

A

1)using barriers:
- paint
- oil
- grease
- plastic
2)sacrificial protection
-adding a block of more reactive metal e.g magnesium, this works by displacement
3) galvanising
-coating the iron in zinc

33
Q

what is the definition of an alloy

A

a mixture of a metal and one or more other elements, usually other metals or carbon

34
Q

what are an alloys characteristics

A
  • harder than pure metals
  • because the different sized atoms/ions prevent then sliding over each other
  • this means its less malleable
35
Q

how is the alloy iron used in real life

A

making steel

36
Q

how is the alloy low-carbon steel used in real life

A

ships, cars, bridges etc

37
Q

how is the alloy high-carbon steel used in real life

A

tools e.g screwdriver or knife

38
Q

how is the alloy stainless steel used in real life

A

cutlery, cooking utensils, kitchen sinks

39
Q

how is the alloy copper used in real life

A

wires, cooking pans, water pipes

40
Q

how is the alloy aluminium used in real life

A

aircraft bodies, power cables

chemistry 😢🥹 (19 decks)

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