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chemistry > A1 Relating Properties To Uses And Production Of Substances > Flashcards

A1 Relating Properties To Uses And Production Of Substances Flashcards

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1
Q

Oxide

A

Any atom that is bonded with an oxygen eg carbon monoxide, magnesium oxide, ion oxide

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2
Q

Acid

A

Contains a hydrogen and dissociates in water to form hydrogen ion

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3
Q

A base

A

A substance that will react with acid to form salt and water

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4
Q

Alkali

A

A base that dissolves in water

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5
Q

Sodium hydroxide uses

A
  • To make plastics and soap
  • used as drain cleaner
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6
Q

Calcium hydroxide uses

A
  • used to raise ph of acidic soil by farmers
  • used in the treatment of acidic waste from factories that produce sulfuric acid
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7
Q

Sulfuric acid and calcium hydroxide neutralisation reaction equation

A

H2SO4 + Ca(OH)2 = CaSo4 + 2H2O

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8
Q

Magnesium hydroxide

A

To treat stomach acid indigestion

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9
Q

Amphoteric

A

Substance that can act as an acid or base in hot conditions

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10
Q

Aluminium oxide (amphoteric) uses

A
  • filler
  • paint
  • glass
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11
Q

Transition metal definition

A

A metal that forms an ion with a partially filled d subshell.

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12
Q

Name the process and catalyst (transition metal)

A

The Haber process. Fe is the catalyst

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13
Q

Transition metals function

A
  • they form coloured solutions
  • they are good catalysts as they can accept or donate electrons
  • form complex ions
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14
Q

Complex ion

A

Central atom or ion surrounded by ligands

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15
Q

Ligands

A

Substance that can donate a lone pair of electrons and form a coordinate bond eg lone pairs of electrons from oxygen donated to vanadium.

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16
Q

How catalysts happen

A
  • adsorption:reactants stick to the surface of the active site of the catalyst
  • the reactant bonds weaken
  • reaction occurs between the reactants
  • desorption: as the products form they are released from the catalyst surface
17
Q

What is the catalyst in the contact process?

A

Vanadium oxide - v2O5

18
Q

Explain why transition metals can act as catalysts

A
  • they have partially filled d subshells
  • can accept or lose electrons which means they can be oxidised or reduces
  • so it provides an alternative pathway for a reaction with a lower activation energy
19
Q

How does a catalyst lower the amount of energy needed for a reaction

A
  • adsorbs onto the surface by weakening the bonds
  • as electrons are accepted and donated back
  • this provides an alternative pathway for a reaction with lower activation energy
  • so collisions with less energy will react
20
Q

Steps in the Bayer process

A

1) bauxite ore is crushed to form grains to increase the rate of reaction
2) it is then reacted with hot sodium hydroxide under pressure (as al2o3 is amphoteric and can react with alkaline NaOH)
3) this then forms a slurry
4) alumina dissolves but iron oxide doesn’t (as al2o3 is acidic so will dissolve however iron oxide is alkaline so will not react with NaOH)
5) impurities are filtered off
6) solution is then cooled and seeded with aluminium oxide (to form smaller crystals which will grow into larger
7) aluminium hydroxide then filtered off then heated in kiln to form alumina.

21
Q

Electrolysis

A
  • decomposition of a compound using electricity
  • electrolysis can break down Ionic compounds
  • the ions must be free to move for it to work
  • ionic compounds need to be molten or dissolved
22
Q

Electrolysis for aluminium extraction

A
  • al2O3 will need to be melted first so that the ions are free to move around during electrolysis
  • as al2o3 has high melting point a lot of energy is required and is expensive to melt
  • instead it is dissolved in cryolite (al compound with lower melting point) so that the ions are free to move
  • positive aluminium ions move to the negative cathode to receive electrons (reduced to Al) al3+ + 3e- = al
  • the negative oxygen ions move to positive anode, lose electrons and are oxidised to oxygen gas 2O2- = O2 + 4e-
  • the oxygen reacts with the carbon from positive electrodes and forms carbon dioxide, so they gradually burn away. The positive electrodes need to be replaced frequently.
23
Q

Electrolysis of molten sodium chloride

A
  • the negative chloride ions move to positive anode where they lose electrons to form chlorine gas 2cl- = cl2 + 2e- (oxidation)
  • the positive sodium ions move to negative cathode where they gain electrons to form sodium na+ + e- = na
24
Q

Electrolysis of aqueous sodium chloride

A
  • negative chloride ions move to positive anode where they lose electrons to form chlorine gas 2cl- = cl2 + 2e-
  • positive hydrogen ions move to negative cathode and gain electrons to form hydrogen gas 2h+ + 2e- = h2
  • as hydrogen more reactive than sodium, Na ions react with OH- ions to form NaOH: na+ + OH- = NaOH
25
Q

Electrolysis of brine (NaCl)aq (diaphragm)

A
  • desired products cl2, h2 and NaOH
  • negative chloride ions move to anode and lose electrons to form chlorine
  • positive hydrogen ions move to negative cathode and gain electrons to form hydrogen
  • positive sodium reacts with OH- to form NaOH
  • the NaOH is contaminated by leftover NACl
26
Q

Membrane cell electrolysis of brine

A

Made of polymer which only allows positive ions to pass through it. So it would only allow Na+ not Cl-

  • Cl2 forms at positive electrode
  • h2 forms at negative electrode
  • na is less reactive than h+ so it reacts with OH- to form NaOH
  • due to the membrane the end product NaOH won’t be contaminated by cl- ions and will be pure.
27
Q

Extraction of titanium rutile- TiO2 (ore) conversion to TiCl4

A
  • rutile ore is heated with chlorine and coke at temp 1000 degrees
  • TiO2 + cl2 + C = TiCl4 + CO2
28
Q

Extraction of titanium - Refuction of titanium chloride

A
  • TiCl4 + 2Mg = Ti + 2MgCl2
    = reduction process Ti4+ + 4e- = Ti
    Or
  • TiCl4 + 2Na = Ti + 2NaCl2
29
Q

Why electrolysis is a more efficient method of extraction than the kroll process

A
  • electrolysis has less stages than the kroll process
  • less waste products
  • lower energy requirements
30
Q

The reduction of titanium chloride cannot be carried out in air. Explain why air needs to be replaced with argon gas for this reaction

A

As TiCl4 would react with oxygen in the air whereas with argon it wouldn’t as it is an inert gas.

chemistry (3 decks)

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