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Chemistry > period 3 > Flashcards

period 3 Flashcards

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1
Q

type of structure Na Mg Al

A

giant lattice

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2
Q

type of structure Si

A

macromolecular

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3
Q

type of structure P4 S8 Cl2

A

simple covalent molecules

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4
Q

type of structure Ar

A

mono atomic

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5
Q

type of bonding Na Mg Al

A

metallic

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6
Q

type of bonding Si P4 S8 Cl2

A

covalent

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7
Q

type of forces Na Mg Al

A

metallic bonds- attraction between positively charged metal ions and delocalised electrons in a lattice

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8
Q

type of forces Si

A

covalent- shared pair of electrons

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9
Q

type of forces P4 S8 Cl2

A

VDWs- temporary induced intermolecular forces

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10
Q

type of forces Ar

A

VDWs

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11
Q

bp and mp Na Mg Al Si

A

increasingly high

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12
Q

bp and mp P4 S8 Cl2 Ar

A

low- weak forces

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13
Q

trend across period in atomic radius

A

decreases

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14
Q

why does atomic radius decrease across period

A
  • more protons
  • electrons added to same shell so shielding is same
  • attraction between nucleus and outer electrons increases
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15
Q

trend cross period first IE

A

increases

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16
Q

why does first IE increase across period

A
  • -more protons
  • electrons added to same shell so shielding is same
  • attraction between nucleus and outer electrons increases
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17
Q

trend in electronegativity across period

A

increases

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18
Q

observations of sodium with water

A

fizzes and floats on surface

Na dissolves

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19
Q

sodium and water equation

A

Na+H2O > NaOH + 1/2H2

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20
Q

observations of magnesium with cold water

A
  • v slow reaction

- occasional bubble

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21
Q

equation magnesium and cold water

A

Mg + H2O> Mg(OH)2 + H2

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22
Q

observation magnesium with steam

A
  • white flame

- white solid

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23
Q

equation magnesium with steam

A

Mg + H2O > MgO + H2

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24
Q

why is aluminium unreactive with water

A

-resistant to further oxidation because of Al2O3 coating

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25
Q

do silicon, phosphorus and sulphur react with water

A

no

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26
Q

observations chlorine and water

A

(with universal indicator paper)

red then bleaches white

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27
Q

equation chlorine and water

A

Cl2 + H2O >< HClO + HCl

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28
Q

what is the reaction of water and chlorine an example of

A

disproportionation- chlorine simultaneously oxidised and reduced

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29
Q

does argon react with water

A

no

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30
Q

what do the period 3 elements react with oxygen to form

A

they react exothermically to form oxides, with the exception of chlorine and argon

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31
Q

observation sodium and oxygen

A
  • orange/yellow flame

- white solid

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32
Q

equation sodium and oxygen

A

4Na + O2 > 2Na2O

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33
Q

observation magnesium and oxygen

A
  • white flame

- white solid

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34
Q

equation magnesium and oxygen

A

Mg + 1/2O2 > MgO

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35
Q

observation aluminium and oxygen

A
  • unreactive due to Al2O3 coating

- fine powder- white sparkles/white solid

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36
Q

equation aluminium and oxygen

A

4Al + 3O2 > 2Al2O3

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37
Q

what kind of compounds are the metal oxides

A

basic

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38
Q

observations silicon with oxygen

A

v slow

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39
Q

equation silicon with oxygen

A

Si+ O2 > SiO2

40
Q

observations phosphorus and oxygen

A

white flames and fumes

41
Q

equation phosphorus and oxygen

A

4P + 5O2 > P4O10

42
Q

observations sulphur and oxygen

A

blue flame

choking gas

43
Q

equation sulphur and oxygen

A

S + O2 > SO2

44
Q

what kind of compounds are non metal oxides

A

acidic compounds

45
Q

what can sulphur (IV) oxide (SO2) react with oxygen to form

A

sulphur (VI) oxide (SO3)

46
Q

sulphur 4 oxide and oxygen

A

SO2 + 1/2O2> SO3

47
Q

contact process

A

SO3 + H2O > H2SO4

48
Q

why do NA20, MGO AND AL203 have high melting points

A

ionic- strong electrostatic attractions between oppositely charged ions require a lot of energy to break

49
Q

why does SiO2 have a higher melting point than P4O10

A

SiO2 macromolecular and P4O10 is simple molecular

strong covalent bonds in SiO2 require more energy to break than weak VDW forces between P4O10 molecules

50
Q

why does P4O10 have a higher melting point that SO3

A
  • P4O10 larger molecules-more electrons than SO3

- p4o10 stronger VDW forces between molecules- more energy to break

51
Q

in general, what do metal oxides from period 3 elements react with water to form

A

solutions containing hydroxide ions

52
Q

sodium oxide and water equation

A

Na2O + H2O > 2NaOH

53
Q

pH of resulting solution Na2O and H2O

A

Na2O is soluble and resulting solution has pH 11-14

54
Q

magnesium oxide and water equation

A

MgO + H2O > Mg(OH)2

55
Q

pH of resulting solution MgO and H2O

A

sparingly soluble- pH 8-10

56
Q

is Al2O3 soluble in water

A

no- pH remains 7

57
Q

what do non metal oxides of period 3 elements react with water to form

A

solutions containing H+ ions

58
Q

SiO2 and water solubility?

A

insoluble- sand

59
Q

P4O10 and water equation

A

P4O10 + 6H2O > 4H3PO4

60
Q

pH of resulting solution P4O10 and WATER

A

1-2- STRONG ACID

61
Q

SO2 and water equation

A

SO2 + H2O > H2SO3

62
Q

pH of resulting solution SO2 and water

A

2-4- weak acid

63
Q

equation SO3 and water

A

SO3 + H2O > H2SO4

64
Q

pH of resulting solution SO3

A

0-2

65
Q

examples of ionic oxides

A

Na2O and MgO

66
Q

what do ionic oxides react with acids to form and why

A

salt and water

they are basic

67
Q

equation sodium oxide and sulphuric acid

A

Na2O + H2SO4 > Na2SO4 + H2O

68
Q

equation magnesium oxide and hydrochloric acid

A

MgO + 2HCl > MgCl2 + H2O

69
Q

examples of covalent oxides

A

SiO2, P4O10, SO2, SO3

70
Q

what do covalent oxides react with aqueous alkali to form and why

A

salt and water- theyre acidic

71
Q

equation silicon oxide and sodium hydroxide

A

SiO2 + NaOH > Na2SiO3 + H2O

72
Q

equation phosphorus (v) oxide and sodium hydroxide

A

P2O5 + 6NaOH > 2Na3PO4 + 3H2O

73
Q

equation sulphur (IV) oxide and sodium hydroxide

A

SO2 + NaOH > Na2SO3 + H2O

74
Q

equation sulphur (VI) oxide and sodium hydroxide

A

SO3 + NaOH > Na2SO4 + H2O

75
Q

why does aluminium react with both acids and bases

A

its amphoteric

76
Q

equation aluminium oxide and hydrochloric acid

A

Al2O3 + 6HCl > 2AlCl3 + 3H2O

77
Q

equation aluminium oxide and nitric acid

A

Al2O3 + 6HNO3 > 2Al(NO3)3 + 3H2O

78
Q

equation aluminium oxide and sodium hydroxide

A

Al2O3 + 2NaOH + 3H2O > 2NaAl(OH)4

79
Q

what do aluminium salts form when dissolved in water

A

acidic solutions

80
Q

why do aluminium salts form acidic solutions when dissolved in water

A

the ionic lattice breaks down and the Al3+ ions become surrounded by water forming a hexaaqua ion

81
Q

hexaagua ion

A

[Al(H2O)6]3+

82
Q

how many water molecules is the Al3+ ion surrounded by

A

6

83
Q

how is each water molecule bonded to the aluminium ion

A

coordinate bond

84
Q

what does the charge on the Al3+ ion cause the electron density in the water molecule to do

A

move closer to the metal ion- water molecule polarised

85
Q

what does the Al3+ ion have enough polarising power to do

A

weaken the OH bonds in water- one of bonds breaks and a proton donated

86
Q

equation for hexaagua ion losing proton

A

[Al(H2O)6]3+ > [Al(H2O)5(OH)]2+ + H+

87
Q

what does adding a base to an aqueous solution of the hexaaqua aluminium ion produce

A

an insoluble precipitate of aluminium hydroxide

88
Q

equation for hexaaqua ion and hydroxide ion

A

[Al(H2O6)]3+ + OH- > [Al(H2O)5(OH)]2+ + H2O

89
Q

what happens to the equilibrium if you add more OH- ions to the hexaaqua aluminium ion

A

shifts to RHS to oppose change and reduce OH concentration and a new equilibrium is set up

90
Q

what new equilibrium is set up when more OH- ions are added to alumium hexaaqua ions

A

[Al(H2O)5(OH)]2+ + OH- <> [Al(H2O4)(OH2)]+ + H2O

91
Q

what final equilibrium is set up when even more OH- ions are added to aluminium hexaaqua ion

A

[Al(H2O)4(OH2)]+ + OH- <> [Al(H2O)3(OH)3] + H2O

92
Q

why is the white precipitate formed from the final equilibrium of aluminium hexaaqua ion insoluble and why does it precipitate out

A

its neutral

93
Q

overall equation for equilibrium of hexaagua ion

A

[Al(H2O)6]3+ +3OH- > [Al(H2O)3(OH3)] + 3H2O

94
Q

amphoteric

A

species that can act as an acid or base

95
Q

equation aluminium hydroxide reacting with acid

A

[Al(H2O)3(OH)3] + H+ > [Al(H2O)6]3+

simplified: Al(OH3) + H+ > Al3+ + 3H2O

96
Q

what does the white precipitate of aluminium hydroxide dissolve to form

A

colourless solution

97
Q

equation aluminium hydroxide reacting with base

A

[Al(H2O)3(OH)3] + OH- > [Al(H2O)2(OH)4]- + H2O

simplified: Al(OH)3 + OH- > Al(OH)4-

Chemistry (42 decks)

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