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3.2 inorganic chemistry > 3.2.4 properties of period 3 elements and their oxides > Flashcards

3.2.4 properties of period 3 elements and their oxides Flashcards

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1
Q

write a balanced equation for the reaction of sodium with water

A

2Na(s) + 2H2O — 2NaOH (aq) + H2 (g)

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2
Q

state 3 observations from the reaction between sodium and water

A

fizzing due to H2 produced
sodium floats on water and reacts vigorously forming molten ball
phenolphthalein goes from colourless to pink

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3
Q

write a balanced equation for the reaction of magnesium and water

A

Mg(s) + 2H2O (l) — Mg(OH)2 (s) + H2(g)

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4
Q

state an observation for the reaction between water and magnesium

A

reacts very slowly with cold water so no observable reaction

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5
Q

write a balanced equation for the reaction of magnesium and steam

A

Mg(s) + H2O(g) — MgO(s) + H2(g)

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6
Q

state an observation for the reaction between magnesium and steam

A

white powder
bright white flame

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7
Q

write a balanced equation for the reaction between sodium and oxygen

A

4Na(s) + O2(g) — 2Na2O(s)

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8
Q

what is the bonding and structure of the oxide produced between sodium and oxygen?

A

giant ionic lattice
ionic bonding

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9
Q

explain the melting point of sodium oxide

A

high melting point because it requires lots of energy to overcome the strong electrostatic forces of attraction between oppositely charged ions in a lattice

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10
Q

what is an observation from the reaction between sodium and oxygen?

A

very vigorous reaction, burns with a yellow flame forming sodium oxide which is a white solid

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11
Q

write a balanced equation for the reaction between magnesium and oxygen

A

2Mg(s) + O2(g) — 2MgO(s)

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12
Q

what is the structure and bonding of the oxide produced from the reaction between magnesium and oxygen?

A

giant ionic lattice and ionic bonding

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13
Q

explain the melting point of magnesium oxide

A

high melting point because there is lots of energy required to overcome the strong electrostatic forces of attraction between oppositely charged ions held together in a lattice

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14
Q

what can be observed in the reaction between magnesium and oxygen?

A

very vigorous reaction, burns with a bright white flame forming magnesium oxide which is a white solid

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15
Q

write a balanced equation for the reaction between aluminium and oxygen

A

4Al(s) + 3O2(g) — 2Al2O3 (s)

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16
Q

what is the structure and bonding of aluminium oxide?

A

giant ionic lattice
ionic bonding

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17
Q

explain the melting point of aluminium oxide

A

high melting point so lots of energy required to overcome electrostatic forces of attraction between oppositely charged ions held together in a lattice

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18
Q

state an observation from the reaction between aluminium and oxygen

A

vigorous reaction with a bright white flame forming aluminium oxide which is a white solid

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19
Q

write a balanced equation for the reaction between silicon and oxygen

A

Si(s) + O2(g). — SiO2 (s)

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20
Q

what is the structure and bonding in silicon dioxide

A

macromolecular
covalent bonding

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21
Q

explain the melting point of silicon dioxide

A

high melting point so lots of energy required to overcome many strong covalent bonds

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22
Q

state what is observed in the reaction between silicon and oxygen

A

a slow reaction

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23
Q

write a balanced equation for the reaction between phosphorus and oxygen

A

P4(s) + 5O2 (g) — P4O10 (s)

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24
Q

what is the bonding and structure of phosphorus (v) oxide

A

simple molecular
covalent bonding

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25
Q

explain the melting point of phosphorus (v) oxide

A

low melting point since there are weak van der waals between molecules that are easy to overcome

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26
Q

state an observation for the reaction between phosphorus and oxygen

A

vigorous reaction forming masses of white fumes with a white flame

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27
Q

write a balanced equation for the reaction between sulfur and oxygen

A

s(s) + O2(g) — sO2 (g)

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28
Q

what is the structure and bonding of sulphur dioxide?

A

simple molecular
covalent bonding

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29
Q

explain the melting point of sulphur dioxide

A

low melting point because there are weak van der waals between molecules that are easy to overcome

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30
Q

state what is observed in the reaction between sulphur and oxygen

A

melts easily then burns with a blue flame forming sulphur dioxide a colourless gas with a choking smell

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31
Q

at high temperature and with a catalyst, SO3 can form from the reaction between sulphur and oxygen, write an equation

A

S(s) + 1 1/2 O2(g) — SO3(g)

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32
Q

what is the PH of the solution formed after sodium and water react?

A

12-14

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33
Q

what is the PH of the solution formed after magnesium and water react?

A

9-10

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34
Q

write a balanced equation to show the reaction between Na2O with water

A

Na2O(s) + H2O (l) — 2NaOH(aq)

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35
Q

what is the PH of the solution formed from the reaction between Na2O and water

A

12-14

36
Q

write a balanced equation to show the reaction between MgO and water

A

MgO(s) + H2O(l) — Mg(OH)2 (aq)

37
Q

what is the PH of the solution formed from the reaction between MgO and water

A

9-10

38
Q

write a balanced equation for the reaction between Al2O3 and water

A

aluminium is insoluble

39
Q

what is the PH of the solution formed from the reaction between Al2O3 and water

A

no PH change as its insoluble

40
Q

write a balanced equation for the reaction between P4O10 and water

A

p4o10(s) + 6H2O(l) — 4H3PO4(aq)

41
Q

what is the PH of the solution formed from the reaction between p4o10 and water

A

0-1

42
Q

write a balanced equation for the reaction between SO2 and water

A

silicon is insoluble in water

43
Q

what is the PH of the solution formed from the reaction between SO2 and water

A

no PH change

44
Q

what is the PH of the solution formed from the reaction between SO2 and water

A

no PH change

45
Q

write a balanced equation for the reaction between SO3 and water

A

SO3 + H2O — H2SO4

46
Q

what is the PH of the solution formed from the reaction between SO3 and water

A

0

47
Q

write an equation for a reaction between Na2O and H2SO4 and a base

A

acid : Na2O (s) + H2SO4 (aq) — Na2SO4 (aq) + H2O(l)
base : not applicable

48
Q

write an equation for the reaction between MgO and HCl and a base

A

acid : Mgo (s) + 2HCl (aq) — MgCl2 (aq) + H2O (l)
base : not applicable

49
Q

write an equation for the reaction between Al2O3 and HCl and NaOH

A

acid : Al2O3 (s) + 6HCl — 2AlCl3 + 3H2O
base : Al2O3 (s) + 2NaOH (aq) + 3H2O — 2NaAl(OH)4 (aq)

50
Q

write an equation for the reaction between p4o10 and NaOH and an acid

A

acid : no reaction
base : p4o10 (s) + 12NaOH (aq) — 4Na3PO4 (aq) + 6H2O (l)

51
Q

write an equation for the reaction between SiO2 and NaOH and an acid

A

acid : no reaction
base : SiO2 (s) + 2NaOH (aq) — Na2SiO3 (aq) + H2O (l)

52
Q

H3PO4 : write three equations, each showing the loss of an acidic hydrogen to form three anions

A

H3PO4 (aq) — H+ (aq) + H2PO4- (aq)
H3PO4 (aq) — 2H+ (aq) + HPO4 2- (aq)
H3PO4 (aq) — 3H+ (aq) + PO4 3- (aq)

53
Q

H2SO3 : write two equations each showing the loss of an acidic hydrogen to form two different anions.

A

H2SO3 (aq) — H+ (aq) + HSO3- (aq)
H2SO3 (aq) — 2H+ (aq) + SO3 2- (aq)

54
Q

H2SO4 : write two equations each showing the loss of an acidic hydrogen to form two different anions.

A

H2SO4 (aq) — H+ (aq) + HSO4 - (aq)
H2SO4 (aq) — 2H+ (aq) + SO4 2- (aq)

55
Q

what is the shape of H3PO4?

A

tetrahedral

56
Q

what is the shape of H2SO3?

A

trigonal pyramidal

57
Q

what is the shape of H2SO4?

A

tetrahedral

58
Q

predict whether the melting point of lithium oxide is higher than, the same as, or lower than the melting point of sodium oxide and explain your prediction

A

higher
because the Li+ ion is smaller than the Na+ ion so attracts O2- more strongly

59
Q

in K, what is the avg. melting point of Na2O?

A

1548

60
Q

in K, what is the avg. melting point of MgO?

A

3125

61
Q

in K, what is the avg. melting point of Al2O3?

A

2345

62
Q

in K, what is the avg. melting point of SiO2?

A

1883

63
Q

in K, what is the avg. melting point of p4o10?

A

573

64
Q

in K, what is the avg. melting point of SO2?

A

200

65
Q

in K, what is the avg. melting point of SO3?

A

290

66
Q

explain why sodium oxide forms an alkaline solution when it reacts in water

A

sodium oxide contains O2- ions which react with H2O to form OH- ions

67
Q

write an ionic equation for the reaction of phosphorus oxide with an excess of sodium hydroxide solution

A

P4O10 + 12OH- — 4PO4 3- + 6H2O

68
Q

why is phosphorus stored under water?

A

to prevent it from reacting with oxygen

69
Q

how could you distinguish between the colourless gases of SO2 and SO3?

A

dissolve in separate samples of water and test PH, more acidic solution is SO3

70
Q

predict whether the melting point of lithium oxide is higher than, the same as, or lower than the melting point of sodium oxide and explain your prediction

A

higher
Li+ ion is smaller than Na+ ion so attracts O2- more strongly

71
Q

explain why magnesium has a higher melting point than sodium

A

Mg+ has a higher charge than Na+ so attracts delocalised electrons more strongly

72
Q

other than a high melting point, give two physical properties of silicon dioxide that are characteristic of its structure and bonding

A

hard
insoluble

73
Q

phosphorus (v) oxide is known as pentoxide suggest why it is usually represented by p4o10 rather than p2o5

A

one molecule contains 4 P and 10 O

74
Q

explain why an excess of magnesium oxide can be used for neutralisation

A

MgO is sparingly soluble

75
Q

explain why the use of excess sodium hydroxide to neutralise phosphoric acid solution might lead to environmental problems

A

excess of sodium hydroxide would make the lake toxic

76
Q

suggest why sulfur dioxide forms a weakly acidic solution

A

reaction is an equilibrium

77
Q

suggest why silicon dioxide is described as an acidic oxide even though it is insoluble in water

A

SiO2 reacts with bases

78
Q

explain why the melting point of magnesium is higher than that of sodium

A

magnesium has a higher nuclear charge than sodium
it is a smaller atom meaning there is a strong attraction between the ions and delocalised electrons

79
Q

explain how metals conduct electricity

A

through a sea of delocalised electrons that flow in a given direction

80
Q

state and explain the trend in the melting points of the period 3 metals Na, Mg and Al

A

increases
nuclear charge increases
stronger attraction between cations and delocalised electrons

81
Q

in terms of atomic structure, explain why the van der waals forces in liquid argon are very weak

A

argon particles are single atoms with electrons closer to the nucleus so cannot be easily polarised

82
Q

explain why the second ionisation energy of sodium is greater than the second ionisation energy of magnesium

A

Na2+ requires loss of electron from 2p orbital

83
Q

state why more than minimum energy is not used to ionise the sample of indium

A

so more than one electron is knocked out

84
Q

explain why nickel is ductile

A

layers of ions can slide over one another

85
Q

state one reason why the first ionisation energy of rubidium is lower than the first ionisation energy of sodium

A

rubidium is a bigger atom

86
Q

state one reason why the first ionisation energy of rubidium is lower than the first ionisation energy of sodium

A

rubidium is a bigger atom

3.2 inorganic chemistry (6 decks)

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