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C Physical and Inorganic Chemistry > Y1 Periodicity (I) > Flashcards

Y1 Periodicity (I) Flashcards

1
Q

How does the melting point of group 2 change down the group?

A

Melting point decreases down the group
- same charge
- atoms are much larger
- specific charge is smaller as charge is more diluted
- so less energy to break bonds

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2
Q

How does the pH of group 2 hydroxides change down the group?

A

pH increases down the group
- down group 2 atoms become larger
- more OH- ions per size ratio at the top of the group
- top ofthe group are better reductants

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3
Q

Group 2 hydroxides, which are better reductants?

A

Top of the group

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4
Q

Where is atomic radius the greatest?

A

bottom left of the periodic table
- (across) less protons, less nuclear charge
- (down) more shielding, outermost electron is further from the nucleus

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5
Q

Where is ionisation energy the greatest?

A

top right of the periodic table

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6
Q

Where is electronegativity the greatest?

A

top right of the periodic table

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7
Q

Reactivity of group two down the group?

A

Increases

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8
Q

Mg + steam

A

product: MgO + H2
instead of Mg(OH)2 +H2
reacts more vigorously with steam

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9
Q

Where are group 2 hydroxides more soluble?

A

Bottom of the group

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10
Q

Where are group 2 sulfates more soluble?

A

Top of the group

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11
Q

sulfate ion test explained

A

-add BaCl2 or Ba(NO)3 aqueous
- will form a white ppt when BaSO4(s) is formed
-Problem if CO3(2-) ions are present as will form also white BaCO3(s)
-either test for carbonates with dilute nitric acid (bubble through limewater will turn limewater cloudy) or add HCl to remove with effervescence

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12
Q

Sulfate ion test

A
  • Add HCl to remove and carbonate (CO3(2-)) or sulfite (SO2(2-))impurities
    -Add barium chloride solution
  • positive test if white ppt formed
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13
Q

Cabonate ion test

A

-Add HCl (or any acid)
- effervesence produced
- bubble through limewater
-positive result if limewater turns cloudy

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14
Q

Carbonate ion + acid

A

salt + carbon dioxide + water

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15
Q

Halide ion test

A
  • Add nitric acid to remove and carbonate (CO3(2-)) or sulfite (SO2(2-))impurities
    -Add silver nitrate
    silver chloride - white ppt
    silver bromide - cream ppt
    silver iodide - yellow ppt
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16
Q

Silver nitrate test, tests for?

A

Halide ions

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17
Q

Barium chloride test, tests for?

A

Sulfates

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18
Q

Milk of magnesia is?

A

-Magnesium hydroxide Mg(OH)2
-Helps in digestion as it contains a suspension of the insoluble hydroxide (hence harmless)
-Neutralises the stomache acid and helps indigestion

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19
Q

What do you neutralise acidic soils with?

A

-Calcium hydroxide
-Ca(OH)2 + 2(H+) –> 2H20 + Ca(2+)
-H+ is acid

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20
Q

How do you neutralise flue gases?

A
  • Have CaO or CaCO3 filter beds in the flue columns
  • SO2 + CaO –> CaSO3 (IV)
  • SO2 + CaCO3 –> CaSO3 + CO2
    -the two compounds are known as lime and limestone
  • a slurry is a mixture of lime limestone and water
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21
Q

How would you describe group 2 elements?

A

Alkaline earth metals

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22
Q

kwjssn

A
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23
Q

what is calcium hydroxide known as?

A

slaked lime

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24
Q

The group two elements

A

beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).

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25
Q

What is a barium meal?

A

-Used in medicine
-a patient will swallow a cup of barium sulfate (s)
- the compund is opaque to xrays and so a structure of the persons digestive system will be able to be produced.

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26
Q

Along period 3 atomic radius…

A

Decreases
-increases proton number
-greater specific charge
-same shielding and distance from outer electron

27
Q

Along period 3 electronegativity…

A

Inreases
-smaller radius
-atom has a stronger specific charge (to attract a lone pair of electrons in a covalent bond)

28
Q

trend in ionisation energy along period 3

A

Increases
-as atomic radius decreases

29
Q

Melting point of period 3 elements

A

Silicon the greatest, Argon the lowest

30
Q

sodium flame test

A

bright yellow flame

31
Q

Magnesium flame test

A

bright white light

32
Q

Aluminium flame test

A

glowing bright white light
- oxide layer formed needs to be removed with NaOH to form aluminate Al(OH)4(-)

33
Q

Silicon flame test

A

slow burn, orange glow

34
Q

Phosphorous flame test

A

burns vigorously with pinkish white flame

35
Q

sulfur flame test

A

Blue/ lilac flame

36
Q

1) Chloride, silver nitrate test
2) add dilute ammonia
3) add conc. ammonia

A

1) white ppt (AgCl)
2) ppt redissolves
3) ppt redissolves

37
Q

1) bromide, silver nitrate test
2) add dilute ammonia
3) add conc. ammonia

A

1) cream ppt (AgBr)
2) no change
3) ppt redissolves

38
Q

1) iodide, silver nitrate test
2) add dilute ammonia
3) add conc. ammonia

A

1) yellow ppt (AgI)
2) no change
3) no change

39
Q

calcium flame test

A

brick red flame

40
Q

strontium flame test

A

red flame

41
Q

barium flame test

A

pale green flame

42
Q

copper flame test

A

green flame

43
Q

test for ammonium ions (ammonia gas)

A
  • ammonia is a base
  • will turn red litmus paper blue
    (want to produce ammonia gas faster? add NaOH)
44
Q

Group 3 oxides trend in melting point

A

MgO (Giant ionic lattice greatest charge) greatest, SO2/SO3 (simple covalent molecule) is the lowest

45
Q

In all flame tests what else is produced

A

white solid + smoky white fumes

46
Q

Titanium extraction by sodium

A
  • reduction of titanium (IV) chloride (TiCl4)
  • forms titanium and sodium chloride
  • done under inert argon gas at high temperatures
  • dilute HCl used to remove NaCl
47
Q

Titanium extraction by magnesium

A
  • reduction of titanium (IV) chloride (TiCl4)
  • forms titanium and megnesium chloride
  • done under inert argon gas at high temperatures
48
Q

Why can’t carbon be used for titanium extraction?

A

brittle titanium carbide would be produced

49
Q

Why is titanium so expensive?

A

Titanium is expensive because it is awkward to extract from its ores, rutile (TiO2)

50
Q

group 3 oxides trend in pH down the group

A

pH deacreases
- Na2O going to NaOH (pH 14)
- SO2 + H2O –> H2SO3 (IV) (pH 2-3)
- SO3 + H2O –> H2SO4(VI) (pH 0-1)

51
Q

Magnesium oxide pH

A
  • goes to magnesium hydroxide
  • pH 9
52
Q

sodium oxide pH

A

-goes to sodium hydroxide
- pH 14

53
Q

why do aluminium oxide and silicon dioxide not have a pH

A

They are insoluble as they are giant lattices

54
Q

What is the meaning of amphoteric?

A

Can act as both an acid and a base

55
Q

Phosphor oxide pH

A
  • P4O10 + 6H2O –> 4H3PO4 (pH 1)
56
Q

Sulfur dioxide and sulfur trioxide pH

A
  • SO2 + H2O –> H2SO3 (IV) (pH 2-3)
  • SO3 + H2O –> H2SO4(VI) (pH 0-1)
57
Q

Silicon dioxide + hydroxide

A

SiO2 + 2OH(-) –> SiO3(2-) +H2O

58
Q

Phosphorous oxide + hydroxide

A

P4O10 +12H2O –> 4PO4(3-) +6H2O

59
Q

Sulfur dioxide + hydroxide

A

SO2 + 2OH(-) –> SO3(2-) + H2O

60
Q

Sulfur trioxide + hydroxide

A

SO3 + 2OH(-) –> SO4(2-) + H2O

61
Q

Al2O3 and Al(OH)3 form ___________ when acting as acids

A

Aluminate ions

62
Q

Al2O3 and Al(OH)3 being amphoteric and acting as a base and acid

A
63
Q
A

C Physical and Inorganic Chemistry (15 decks)

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