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chemistry~ inorganic > Period 3 and their oxides > Flashcards

Period 3 and their oxides Flashcards

1
Q

comparison of melting points of magnesium and sodium

A

magnesium has a higher melting point as has 2+ charge so has a higher charge density

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2
Q

what is sodium metal like

A

quite a soft, silvery metal which tarnishes quickly in air

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3
Q

what is magnesium metal like

A

harder than sodium and is often seen a ribbon

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4
Q

equation for sodium reacting with water

A

2Na (s) + 2H2O (l) → 2NaOH (aq) + H2 (g)

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5
Q

how does sodium react with water

A

-vigorous, exothermic reaction
-sodium floats on surface of the water fizzing rapidly and melting as a result of the heat produced during the reaction

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6
Q

solution formed when sodium reacts with water

A

-sodium hydroxide
-pH of 13-14 so is very alkaline

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7
Q

oxidation state of sodium when it reacts with water

A

-changes form 0 in elemental state
- +1 in NaOH

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8
Q

equation of magnesium in cold water

A

Mg (s) + 2H2O (l) → Mg(OH)2 (aq) + H2 (g)

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9
Q

reaction of magnesium with cold water

A

-extremely slow reaction

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10
Q

solution formed when magnesium reacts with cold water

A

-Magnesium hydroxide forms
-pH 10 as is only partly soluble
-key component in milk of magnesia

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11
Q

oxidation state when magnesium reacts with cold water

A

-changes from 0 in elemental state
-+2 in magnesium hydroxide

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12
Q

equation for reaction of heated magnesium with steam

A

Mg (s) + H2O (g) → MgO (s) + H2 (g)

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13
Q

observations of magnesium and steam

A

-burns with a bright, white flame

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14
Q

products of hot magnesium reacting with steam

A

magnesium oxide and hydrogen gas

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15
Q

oxidation states of hot magnesium reacting with steam

A

-oxidation state changes from 0 to +2 in magnesium oxide

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16
Q

comparison of magnesium reacting with water and steam

A

-reaction with steam is much faster than reaction with cold water
-magnesium oxide and hydrogen gas are produced when reacting with steam
-magnesium hydroxide and hydrogen gas are produced when reacting with cold water

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17
Q

sodium oxide formula

A

Na2O

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18
Q

magnesium oxide formula

A

MgO

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19
Q

aluminium oxide formula

A

Al2O3

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20
Q

silicon oxide formula

A

SiO2

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21
Q

phosphorus oxide formula

A

P4O10

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22
Q

sulfur dioxide formula

A

SO2

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23
Q

reaction of sodium and oxygen

A

4Na (s) + O2 (g) → 2Na2O (s)

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24
Q

reaction of magnesium and oxygen

A

2Mg (s) + O2 (g) → 2MgO (s)

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25
Q

reaction of aluminum and oxygen

A

4Al (s) + 3O2 (g) → 2Al2O3 (s)

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26
Q

reaction of silicon and oxygen

A

Si (s) + O2 (g)→ SiO2 (s)

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27
Q

reaction of phosphorus and oxygen

A

4P (s) + 5O2 (g) → P4O10 (s)

28
Q

reaction of sulfur and oxygen

A

S (s) + O2 (g) → SO2 (g)

29
Q

reaction condition to produce Na2O

30
Q

reaction condition to produce MgO

31
Q

reaction condition to produce Al2O3

A

powdered Al

32
Q

reaction condition to produce SiO2

A

powdered Si and heat strongly

33
Q

reaction conditions to produce P4O10

34
Q

reaction condition to produce SO2

A

powdered S is heated

35
Q

reaction to produce Na2O

A

vigorously

36
Q

reaction to produce MgO

A

vigorously

37
Q

reaction to produce Al2O3

38
Q

reaction to produce SiO2

39
Q

reaction to produce P4O10

A

vigorously

40
Q

reaction to produce SO2

41
Q

flame from Na

A

bright yellow flame

42
Q

flame from Mg

A

bright white flame

43
Q

flame from Al

A

bright white flame

44
Q

flame from Si

A

bright white sparkles

45
Q

flame from P

A

yellow or white flame

46
Q

flame from S

A

blue flame

47
Q

product observation from Na2O

A

white solid

48
Q

product observation from MgO

A

white solid

49
Q

product observation from Al2O3

A

white powder

50
Q

product observation from SiO2

A

white powder

51
Q

product observation from P4O10

A

white clouds

52
Q

product observation from SO2

A

toxic fumes

53
Q

how does sulfur form sulphur trioxide

A

catalyst must be used and a very high temperature
2S (s) + 3O2 (g) → 2SO3 (g)

54
Q

what type of oxides are sodium, magnesium and aluminium oxides

A

ionic oxides

55
Q

type of oxide is silicon oxide

A

macromolecular (giant covalent)

56
Q

what type of oxides are phosphorus and sulfur oxides

A

simple molecular

57
Q

adding water to Na2O

A

reacts and forms hydroxide ions in solution with a typical pH of 13

58
Q

adding water to MgO

A

slightly soluble, dissolved oxide forms a few hydroxide ions in solution, typical pH of 8

59
Q

adding water to Al2O3

A

insoluble but amphoteric

60
Q

adding water to SiO2

A

insoluble but acidic

61
Q

adding water to P4O10

A

acidic recats and gives H+ ions in solution, typical pH of 2

62
Q

adding water to SO2

A

acidic, reacts and forms weak acid H2So3 with a few H+ ions in solution, typical pH of 3

63
Q

adding water to SO3

A

acidic, reacts and forms string acid H2SO4 with H+ ions in solution, typical pH os 1

64
Q

how does covalent character change across period 3

65
Q

how does ionic character change across period 3

chemistry~ inorganic (5 decks)

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