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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
reaction of aluminum and oxygen
4Al (s) + 3O2 (g) → 2Al2O3 (s)
26
reaction of silicon and oxygen
Si (s) + O2 (g)→ SiO2 (s)
27
reaction of phosphorus and oxygen
4P (s) + 5O2 (g) → P4O10 (s)
28
reaction of sulfur and oxygen
S (s) + O2 (g) → SO2 (g)
29
reaction condition to produce Na2O
heated
30
reaction condition to produce MgO
heated
31
reaction condition to produce Al2O3
powdered Al
32
reaction condition to produce SiO2
powdered Si and heat strongly
33
reaction conditions to produce P4O10
heated
34
reaction condition to produce SO2
powdered S is heated
35
reaction to produce Na2O
vigorously
36
reaction to produce MgO
vigorously
37
reaction to produce Al2O3
fast
38
reaction to produce SiO2
slowly
39
reaction to produce P4O10
vigorously
40
reaction to produce SO2
gently
41
flame from Na
bright yellow flame
42
flame from Mg
bright white flame
43
flame from Al
bright white flame
44
flame from Si
bright white sparkles
45
flame from P
yellow or white flame
46
flame from S
blue flame
47
product observation from Na2O
white solid
48
product observation from MgO
white solid
49
product observation from Al2O3
white powder
50
product observation from SiO2
white powder
51
product observation from P4O10
white fumes/smoke
52
product observation from SO2
toxic fumes
53
how does sulfur form sulphur trioxide
catalyst must be used and a very high temperature 2S (s) + 3O2 (g) → 2SO3 (g)
54
what type of oxides are sodium, magnesium and aluminium oxides
ionic oxides
55
type of oxide is silicon oxide
macromolecular (giant covalent)
56
what type of oxides are phosphorus and sulfur oxides
simple molecular
57
adding water to Na2O
reacts and forms hydroxide ions in solution with a typical pH of 13 Na2O + H2O --> 2NaOH
58
adding water to MgO
slightly soluble, dissolved oxide forms a few hydroxide ions in solution, typical pH of 8 MgO + H2O --> Mg(OH)2
59
adding water to Al2O3
insoluble but amphoteric
60
adding water to SiO2
insoluble but acidic
61
adding water to P4O10
acidic recats and gives H+ ions in solution, typical pH of 1 P4O10 + 6H2O --> 4H3PO4
62
adding water to SO2
acidic, reacts and forms weak acid H2So3 with a few H+ ions in solution, typical pH of 3 SO2 + H2O --> H2SO3
63
adding water to SO3
acidic, reacts and forms string acid H2SO4 with H+ ions in solution, typical pH of 1 SO3 + H2O --> H2SO4
64
how does covalent character change across period 3
increases
65
how does ionic character change across period 3
decreases
66
reaction of Na2O with acid (HCl)
Na2O + 2HCl --> 2NaCl + H2O
67
reaction of MgO with acid (H2SO4)
MgO + H2SO4 --> MgSO4 + H2O
68
what happens when a basic ionic oxide reacts with acid
salt and water is produced (neutralisation reaction)
69
what happens when an acidic covalent oxide reacts with a base
salt and water is produced
70
SiO2 and alkali (NaOH)
SiO2 + 2NaOH --> Na2SiO3 + H2O
71
P4O10 and alkali (NaOH)
P4O10 + 12NaOH --> Na2SiO3 + H2O
72
SO2 and alkali (NaOH)
SO2 + 2NaOH --> Na2SO3 + H2O
73
SO3 and alkali (NaOH)
SO3 + 2NaOH --> Na2SO4 + H2O
74
Al2O3 and acid (H2SO4)
Al2O3 + 3H2SO4 --> Al2(SO4)3 + 3H2O
75
Al2O3 and alkali (NaOH)
Al2O3 + 2NaOH + 3H2O --> 2NaAl(OH)4

chemistry~ inorganic (7 decks)

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