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Chemistry > Inorganic Chemistry > Flashcards

Inorganic Chemistry Flashcards

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1
Q

Sodium + water -

A

Sodium hydroxide + hydrogen

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2
Q

What are Halogens?

A

Elements in group 7

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3
Q

What colour of Chlorine at room temperature?

A

Green gas

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4
Q

What is the colour/state change of Bromine at room temperature?

A

Red/brown liquid - orange vapour

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5
Q

What is the colour/state change of Iodine when heated?

A

Dark grey crystalline solid - purple vapour

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6
Q

How does the atomic number of halogens increasing affect the elements?

A

Elements have darker colour and higher boiling point

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7
Q

What is a Displacement reaction?

A
  • More reactive element pushes out (displaces) a less reactive element from a compound
  • Reduction and Oxidation happens simultaneously
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8
Q

Give an Example of a Displacement Reaction using Chlorine Iodine:

A
  • Chlorine more reactive than iodine
  • Add chlorine water to potassium iodide solution
  • Chlorine react with potassium to form potassium chloride
  • Iodine displaces from salt and left in sodium, turning it brown
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9
Q

How much Nitrogen is in the air?

A

78%

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10
Q

How much Oxygen is in the air?

A

21%

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11
Q

How much Carbon Dioxide is in the air?

A

0.04%

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12
Q

How much Argon is in the air?

A

Nearly 1%

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13
Q

How can you determine the percentage of Oxygen on air?

A
  • Phosphorus in tube, attach glass syringe at either end
  • 1 syringe with air, other empty
  • Heat phosphorus - react with oxygen in air to make phosphorus oxide
  • Reacts=amount of air in syringes decreases
  • Measure starting & final volume of air using scale on syringes
  • Calculate percentage of O2 in air = difference in volume / start volume * 100
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14
Q

How do you form Magnesium Oxide?

A

Magnesium burns with bright white flame in air and white powder

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15
Q

What is the test for Hydrogen Gas?

A

Squeaky pop when burnt

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16
Q

How do you make Sulfur Dioxide?

A

Sulfur burns in air or oxygen with pale blue flame

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17
Q

What is an Example of Thermal Decomposition of Metal Carbonates?

A
  • Heat metal carbonate, get carbon dioxide & metal oxide
  • Copper(II)carbonate is green powder, decompose to form carbon dioxide and copper(II)oxide when heated
  • CuCO3 - CuO + CO2
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18
Q

What is Thermal Decomposition?

A

When substance breaks down into simpler substance when heated

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19
Q

How does Deforestation affect amount of Carbon Dioxide in atmosphere?

A

Fewer trees means less CO2 is removed from atmosphere via photosynthesis

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20
Q

How does Burning Fossil Fuels affect amount of Carbon Dioxide in atmosphere?

A

Carbon that was locked up in these fuels is being released as CO2

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21
Q

How is Increasing Carbon Dioxide linked to Climate Change?

A
  • Extra CO2 caused average temp of Earth to increase

* Global warming-climate change - cause flooding, change in rainfall patterns, rising sea levels

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22
Q

Acid + Metal -

A

Salt + Hydrogen

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23
Q

Metal + Water -

A

Metal Hydroxide + Hydrogen

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24
Q

How can you Test for how Reactive Metals are using Acid?

A
  • Reactions of different metals with dilute acids
  • More reactive = faster reaction
  • Very reactive metals (e.g. sodium) react explosively
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25
Q

How can you Test for how Reactive Metals are using Water?

A
  • Very reactive metals (e.g. potassium, sodium, lithium) react vigorously with water
  • Less reactive metals (e.g. zinc, magnesium, iron) won’t react much with cold water, react with steam
  • Copper doesn’t react with water or steam
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26
Q

What is the Reactivity series?

Please Send Lions Cats Monkeys And Crazy Zebras In To Lovely Hot Country’s Signed General Penguin

A 
Potassium
Sodium
Lithium
Calcium 
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold
Platinum
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27
Q

How do you Prevent Rusting of Iron?

A
  • Painting/coating with plastic
  • Oiling/Greasing
  • Coating of zinc - zinc oxidised instead of iron
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28
Q

Iron + Oxygen + Water -

A

Hydrated Iron(III)oxide (rust)

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29
Q

What is Rusting in Iron?

A
  • Iron In contact with oxygen and water
  • Iron corrodes and becomes flakey & soft
  • Form hydrated iron(III)oxide
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30
Q

What does Copper Oxide form when reduced and what is the Equation?

A
  • Form copper using carbon

* 2CuO + C - 2Cu + CO2

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31
Q

What is a Metal Ore?

A
  • Compound contains enough of metal to make it worthwhile extracting
  • Mote reactive metal = harder to extract from compound
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32
Q

What are the Common Properties of Iron, Aluminium and Copper?

A
  • Dense, lustrous, high melting points
  • Strong and hard to break
  • Malleable
  • Good conductors of electricity and heat energy
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33
Q

What is Iron Used for and its Main Problem?

A
  • Make gates and railings

* Corrodes easily so rusts

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34
Q

What is Aluminium used for?

A
  • Bicycle frames

* Aeroplanes

35
Q

What is Copper used for?

A
  • Electrical compounds and wiring - has low resistance so efficient at transferring electricity
  • Heating systems (underfloor heating) - speedy transfer of heat to surroundings
36
Q

How are Alloys made?

A
  • Adding other elements to the metal (metals or carbon)

* Harder than pure metals - new atoms distort layers of metal ions - difficult for them to slide over each other

37
Q

What is the pH for Acids and colour (universal indicator)?

A
  • pH 0-7

* Red - orange

38
Q

What is pH for a neutral substance and colour (universal indicator)?

A
  • pH 7

* Green

39
Q

What is pH for Alkaline’s and colour (universal indicator)?

A
  • pH 8-14

* Blue - purple

40
Q

What colour is Acid if Methyl Orange Indicator is added?

A

Red

41
Q

What colour is Alkaline if Methyl Orange Indicator is added?

A

Yellow / orange

42
Q

What colour is Acid if Litmus paper is added?

A

Red

43
Q

What colour is Alkaline if Litmus paper is added?

A

Blue

44
Q

What colour is Neutral substance if Litmus paper is added?

A

Purple

45
Q

What colour is Acid if Phenolphthalein is added?

A

Colourless

46
Q

What colour is Alkaline if Phenolphthalein is added?

A

Bright pink

47
Q

What is an Acid?

A
  • Source of Hydrogen ions (H^+)

* Proton donors

48
Q

What is a Base?

A
  • Substance that can neutralise an acid

* Proton acceptors

49
Q

What is an Alkali?

A
  • Source of hydroxide ions (OH^-)

* Soluble bases

50
Q

What is Neutralisation and its Formula?

A
  • Reaction between acid and base (alkali)

* H^+ + OH^- - H20

51
Q

Acid + Base -

A

Salt + Water

52
Q

Acid + Ammonia-

A

Ammonium Salt

53
Q

Acid + Metal Carbonate -

A

Salt + Water + Carbon Dioxide

54
Q

Acid + Metal Hydroxide-

A

Salt + Water

55
Q

Acid + Metal Oxide -

A

Salt + Water

56
Q

What is Titration used for?

A

Find out exactly how much acid is needed to neutralise a quantity of alkali (vice versa)

57
Q

How do you do a Titration?

A
  • Pipette alkali into conical flask
  • Add few drops of indicator
  • Put Acid onto burette
  • Measure volume - initial reading
  • Add acid to alkali from burette
  • Indicator changes colour when all alkali is neutralised (e.g. phenolphthalein - pink to colourless)
  • Record volume of acid to neutralise alkali
  • Repeat until concordant results
58
Q

How do you make Insoluble Salts and give and example?

A
  • Use precipitation reaction
  • Pick 2 soluble salts and react together to get insoluble salt
  • E.g. lead nitrate + magnesium sulfate = lead sulfate (insoluble)
59
Q

What Substances are Soluble?

A
  • Nitrates
  • Common Salts of sodium, potassium, ammonium
  • Common Chlorides (not silver/lead chloride)
  • Common Sulfates (not lead, barium, calcium sulfate)
60
Q

What Substances are Insoluble?

A
  • Common Carbonates (not sodium,potassium,ammonium)

* Common Hydroxides (not sodium,potassium,calcium)

61
Q

Flame test for Lithium (Li^+):

A

Bright red flame

62
Q

Flame test for Sodium (Na^+):

A

Orange flame

63
Q

Flame test for Potassium (K^+):

A

Lilac flame

64
Q

Flame test for Calcium (Ca^2+):

A

Brick red flame

65
Q

Flame test for Magnesium (Mg^2+):

A

No colour

66
Q

Flame test for Copper (Cu^2+):

A

Green flame

67
Q

How do you do the Flame Tests?

A
  • Platinum wire loop dipped in dilute HCl, hold in flame

* Dip it In sample you want to test then place in Bunsen burner

68
Q

What are Metal Hydroxides:

A
  • Insoluble

* Precipitate forms out of solution

69
Q

How can you Test for Ammonia Gas?

A
  • Damp red litmus paper

* Ammonia present = paper turn blue

70
Q

What Colour Precipitate does Chloride Ion give?

A

White precipitate

71
Q

What Colour Precipitate does Bromide Ion give?

A

Cream precipitate

72
Q

What Colour Precipitate does Iodide Ion give?

A

Yellow precipitate

73
Q

What do you use to Test for Halides?

A

Cl^-/Br^-/I^- with Nitric Acid and Silver Nitrate

74
Q

What is the Test for Carbonates?

A
  • Add dilute hydrochloric acid (HCl)

* If carbonates present = CO2 released

75
Q

What is the Test for Sulfates?

A
  • Add dilute hydrochloric acid (HCl) with barium chloride solution (BaCl2)
  • White precipitate of barium sulfate = original compound was sulfate
76
Q

What is Test for Chlorine?

A

Bleaches damp blue litmus paper, turning white

77
Q

What is Test for Oxygen?

A

Relights a glowing splint

78
Q

What is Test for Carbon Dioxide?

A

Turns limewater cloudy

79
Q

What is the Test for Hydrogen?

A

Makes a squeaky pop with lighted splint

80
Q

What is the Test to see if Water is Present?

A
  • Add anhydrous copper(II)sulfate

* If white powder turn blue - water present

81
Q

How do you make Lead Sulfate?

A
  • Add 1 spatula of lead nitrate to test tube, add water to dissolve
  • Add 1 spatula of magnesium sulfate to another test tube, add water to dissolve
  • Put both solutions into beaker, stir, lead sulfate precipitate out
  • Pour contents into filter paper, rinse contents so all magnesium nitrate gone
  • Scrape lead sulfate onto paper, dry in oven
82
Q

How do you make Soluble Salts?

A
  • Reacting acid (contains 1 ion you want in salt) with insoluble base (contains other ion you need)-usually metal oxide/hydroxide
  • Reacting acid with an alkali - titration using indicator
83
Q

How do you Make Soluble Salts using Acid and Insoluble Base?

A
  • Heat acid in water bath
  • Add base, produces soluble salt and water
  • Filter excess solid to get solution with salt and water
  • Heat solution gently, evaporate some water, cool and salt crystallises
  • Filter off solid and leave to dry
84
Q

How do you make Soluble Salts using Acid/Alkali Reactions?

A
  • Measure out acid using pipette
  • Add few drops of indicator
  • Add alkali

Chemistry (10 decks)

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