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AS Level Chemistry > 10. CHEMICAL PERIODICITY > Flashcards

10. CHEMICAL PERIODICITY Flashcards

1
Q

Colour of flame when Na reacts with O2

A

yellow

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2
Q

Colour of flame when Mg reacts with O2

A

white

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3
Q

Product formed when Na reacts with O2

A

white solid Na2O

white solid Na2O2

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4
Q

Product formed when Mg reacts with O2

A

white solid MgO

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5
Q

Reaction of Na with O2

A
  • vigorous reaction

- produces white solid Na2O only

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6
Q

Reaction of Mg with O2

A
  • vigorous reaction

- produces white solid MgO only

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7
Q

Product of reaction of Si with O2

A

SiO2

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8
Q

Colour of flame when Si reacts with O2

A

pale blue flame

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9
Q

Reaction speed of Si with O2

A

slow

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10
Q

Reaction speed of P with O2

A

vigorous

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11
Q

Product of reaction of P with O2

A

P4O10 and P4O6

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12
Q

Colour of flame when P reacts with O2

A

white or yellow flame

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13
Q

Observation when P reacts with O2

A
  • white or yellow flame

- clouds of white P4O10 formed

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14
Q

Colour of flame when S reacts with O2

A

blue flame

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15
Q

Product when S reacts with O2

A

colourless fumes of SO2

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16
Q

Reaction speed when S reacts with O2

A

gentle reaction

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17
Q

Colour of flame when powdered Al reacts with O2

A

white

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18
Q

Product of reaction when Al reacts with O2

A

Al2O3

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19
Q

Reaction of Cl2 with O2

A
  • does not react directly

- has several oxides

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20
Q

Product of reaction of Na with Cl2

A

solid NaCl

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21
Q

Product of reaction of Mg with Cl2

A

solid MgCl2

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22
Q

Product of reaction of Al with Cl2

A

solid Al2Cl6

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23
Q

Product of reaction of Si with Cl2

A

colourless volatile liquid SiCl4 (not giant structure)

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24
Q

Product of reaction of P4 with Cl2

A
  • liquid PCl5 in excess chlorine
  • PCl3 in less chlorine
  • PCl4 has an expanded octet
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25
Q

Chlorides of sulfur

A

SCl2 and S2Cl2

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26
Q

Observation when Na reacts with Cl2

A
  • yellow flame

- white solid produced

27
Q

Observation when Mg reacts with Cl2

A
  • white flame

- white solid produced

28
Q

When does Al2Cl6 exist

A

at low temperatures

29
Q

When does AlCl3 exist

A

at high temperatures

30
Q

Types of phosphorus

A
  • white phosphorus (P4)

- red phosphorus (P)

31
Q

Observations when Na reacts with H2O

A
  • vigorous reaction
  • floats
  • melts
  • moves in circles
  • white solid disappears
  • gas produced
32
Q

Product when Na reacts with H2O

A

alkaline solution of pH 14 NaOH and H2 gas

33
Q

Product when Mg reacts with liquid H2O

A

weakly alkaline solution of pH 11 Mg(OH)2 and H2 gas

- slow reaction

34
Q

Why is Na(OH) more alkaline than Mg(OH)2

A
  • magnesium hydroxide is only slightly soluble in water while sodium hydroxide is completely soluble in water
  • a lower concentration of OH- ions enter the solution
35
Q

Product when Mg reacts with steam

A

MgO and H2

- vigorous reaction

36
Q

Why do all Period 3 elements exist in positive oxidation states in their oxides

A

because oxygen is more electronegative than any of the Period 3 elements

37
Q

Why are MgO and Mg(OH)2 used in indigestion remedies

A

they neutralise excess acid in the stomach

38
Q

Reactions of Al2O3

A

ACID
- forms aluminium sulfate Al2(SO4)3
HOT CONCENTRATED ALKALI
- forms sodium tetrahydroxoaluminate NaAl(OH)4

39
Q

Reaction of SiO2

A

HOT CONCENTRATED ALKALI
- forms Na2SiO3 (sodium silicate)

behaves as an acidic salt

40
Q

Why does SiO2 not react with water

A

water cannot break down its giant molecular structure

41
Q

Reaction of P4O10 with water

A

forms acidic solution of H3PO4 (phosphoric acid)

42
Q

Reaction of SO2 and SO3 with water

A

SO2 –> H2SO2 (sulfurous acid)

SO3 –> H2SO4 (sulfuric acid)

43
Q

What happens to the electronegativity going across a period

44
Q

Why does electronegativity increase across a period

A
  • the electrons are more strongly attracted to the nucleus

- by the increasing positive nuclear charge

45
Q

When does ionic bonding happen

A

the greater the difference in the electronegativity of the atoms, the more likely it is that the compound will have ionic bonding

46
Q

Use of magnesium oxide

A

used to line the inside of furnaces

47
Q

Use of Al2O3 and SiO2

A
  • make ceramics

- provide electrical insulation

48
Q

How do the oxides of sodium and magnesium form alkaline solutions in water

A

the O2- turns into (OH)- by acting like a base and accepting a proton from H+

49
Q

What happens when NaCl is added to water

A
  • polar water molecules are attracted to the ions
  • so dissolve the chlorides by breaking down the giant ionic structure
  • solution formed contains Na+ and Cl- ions surrounded by water molecules (hydrated ions)
50
Q

Products of reaction of SiCl4 with H2O

A

SiO2 and HCl gas

  • SiO2 does not react with water (off-white precipitate)
  • some of the HCl dissolves in water, leaving an acidic solution
51
Q

Observations when SiCl4 reacts with H2O

A
  • white fumes of HCl produced

- off-white precipitate of SiO2

52
Q

Name of reaction of SiCl4 and PCl5 with water

A

Hydrolysis

53
Q

Products of reaction of PCl5 with water

A
  • acidic solution of H3PO4

- HCl gas. some of the gas dissolves to give an acidic solution

54
Q

Observations when PCl5 reacts with H2O

A
  • white fumes of HCl gas
55
Q

General observations of NaCl and MgCl2 with water

A
  • white solid dissolves to form less colour

- alkaline solution produced

56
Q

General observations of Al to S chlorides with water

A
  • white fumes of HCl produced

- acidic solution formed

57
Q

How does Al2Cl6 form a solution with pH 3

A
  • when added to water, the dimers are broken down and Al and Cl ions enter the solution
  • the Al3+ causes a water atom surrounding it to lose an H+ ion, thus turning the solution acidic
58
Q

What provides evidence for the ionic and covalent bonding of Al2O3

A

it reacts with both acids (which is typical of ionic oxides) and alkalis (which is typical of covalent oxides)

59
Q

Observations when phosphorus reacts with chlorine

A
  • green colour of chlorine disappears
  • white flame
  • white solid formed
  • solid melts
60
Q

What is the name of H3PO4

A

phosphoric(v) acid

61
Q

What is the name of K2Cr2O7

A

potassium dichromate(VII)

62
Q

What is the name of KMnO4

A

potassium manganate(VII)

63
Q

Physical properties of ceramics such as aluminium oxide and silicon dioxide

A
  • high melting/boiling/sublimation point

- electrical/thermal insulator

64
Q

Common brown gases

A
  • bromine

- NO2

AS Level Chemistry (6 decks)

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