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Chemistry > Metals > Flashcards

Metals Flashcards

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1
Q

Properties of metals

A
  • good thermal conductor
  • shiny
  • good electrical conductor
  • most are solids at room temperature
  • lustrous (can be polished
  • sonorous (make a ringing sound when it)
  • hard/strong
  • high melting and boiling points
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2
Q

Properties of non-metals

A
  • dull
  • bad thermal conductor
  • bad electrical conductor
  • most are liquids or gases at room temp
  • brittle
  • weak
  • low melt and boil pnts
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3
Q

Properties of Metallic bonding

A

– solid at room temp and pressure
- high melt and boil points
- good conductors of heat and electricity
- malleable
- ductile
- strong
- dense

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4
Q

What structure does metallic bonding create

A

Giant Metallic Lattice Structure

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5
Q

what is Metallic Bonding

A

The electrostatic force of attraction between positive metal ions and a sea of delocalized electrons

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6
Q

Why are metallic structures Malleable, Ductile, and Strong

A

The layers of metal ions are able to slide over each other so the structure will not shatter.
The metallic bonds do not break because the delocalized electrons are free to move around the structure

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7
Q

Unique characteristics of Group 1 Alkaline Metals

A
  • Soft (can be cut with a knife)
  • Low density (float on water)
  • Low melt and boil pts (Na melts into a ball in cold water)
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8
Q

Group 1 Alkaline Metal Trends: Density, Boiling Points, Reactivity

A

As you go down the group:
Density increases
Melt and Boil pts decrease
Reactivity increases

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9
Q

What happens to Potassium when added to water

A

Bursts into a lilac flame

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10
Q

What happens to Sodium when added to water

A

Melts into a ball

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11
Q

What is thermal decomposition

A

When heat energy is used to break down a substance

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12
Q

What is OIL RIG

A

Oxidisation is loss of electron (or gain of oxygen)
Reduction is gain of electrons (or loss of oxygen)

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13
Q

What is the Thermite Reaction

A

Iron(111) Oxide + Aluminium -> Aluminium Oxide + Iron

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14
Q

What is the Thermite Reaction used for

A

Welding tracks together

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15
Q

What is a REDOX reaction

A

The simultaneous reduction and oxidation of a species in a reaction

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16
Q

What is rust

A

The corrosion of iron (other metals don’t rust they corrode)

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17
Q

What is the chemical name for rust

A

Hydrated iron (lll) oxide

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18
Q

Methods of preventing Rust

A
  • Sacrificial Protection (coating in Zinc)
  • galvanising
  • Barrier methods (Coat in oil or grease or paint or plastic)
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19
Q

What needs to be present for iron to rust

A

Both oxygen and water

20
Q

what is an alloy

A

a compound consisting of a metal with at least one other element

21
Q

what is steel a mix of

A

carbon and iron

22
Q

iron + oxygen + water ->

A

hydrated iron (lll) oxide

23
Q

why does reactivity increase as you go down group 1 (alkaline metals)

A

because the atoms get bigger with more shells meaning more shielding, less attraction to the nucleus and so they are more likely to lose their outer electron

24
Q

what is the oxidising agent

A

gains electrons from other atoms (it itself reduced)

25
Q

what is the reducing agent

A

donates electrons to the other atom (it itself being oxidised)

26
Q

what is a REDOX reaction

A

when reduction and oxidation simultaneously occur

27
Q

how are unreactive metals found in the earth’s crust

A

as the uncombined element

28
Q

how are most metals extracted from the earth’s crust

A

as ores

29
Q

what is the method of extraction of a metal related to? give 2 examples

A

its position in the reactivity series
- carbon extraction for iron -
- electrolysis for aluminium -
al = more reactive than: iron

30
Q

why are alloys harder than pure metals

A

because the larger ‘other’ atoms cause an irregular pattern which doesn’t allow particles to slide over each other

31
Q

what is thermal decomposition

A

when heat energy is used to break down a substance

32
Q

equation for the thermal decomposition of a metal carbonate

A

metal carbonate -> metal oxide + carbon dioxide

33
Q

how is carbon dioxide normally collected and why

A

through downward delivery

CO2 is denser than air so it sinks to the bottom of a tube and will stay there until you want to use it

34
Q

state the reactivity series

A
35
Q

equation for when metals react with cold water

A

metal + water -> metal hydroxide + hydrogen

36
Q

what are the two observations of a reaction between metal and cold water

A
  • effervescence (hydrogen gas)
  • solid disappears
37
Q

what are the four observations of Lithium Sodium and Potassium with water

A

solid floats - it is less dense than water
effervescence - hydrogen
solid moves - effervescence propels it around
solid disappears

38
Q

what would you see when adding universal indicator in a reaction between a metal and cold water

A

turns dark blue because metal hydroxides are alkaline

39
Q

what can be observed when sodium reacts with cold water

A

solid melts

solid floats - it is less dense than water
effervescence - hydrogen
solid moves - effervescence propels it around

40
Q

what can be observed when potassium reacts with water

A

solid melts
lilac flame

solid floats - it is less dense than water
effervescence - hydrogen
solid moves - effervescence propels it around

41
Q

why are the products of reacting metals with water and steam different

A

steam has more energy so both bonds in the water molecules can break

42
Q

how are metal + steam reactions normally carried out

A
43
Q

equation for the reaction between metal and steam

A

metal +steam -> metal oxide + hydrogen

44
Q

3.5.4

A
45
Q

What are the observations when an excess of magnesium powder is added to an aqueous solution of copper (II) sulfate

A
  • pink/brown solid forms
  • solution turns colourless
46
Q

What is the meaning of exothermic

A

A reaction that gives out thermal energy

Chemistry (30 decks)

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