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Inorganic Flashcards

1
Q

test for sulfate ions

A
  • add dilute HCl
  • add barium chloride
  • white precipitate shows presence
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2
Q

Aluminium oxide + sodium hydroxide

A

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

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3
Q

magnesium ions + dilute NaOH

A

white precipitate

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4
Q

Phosphorus + oxygen

A

P4(s) + 5O2(g) = P4O10 (s)
Phosphorus (V) oxide

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5
Q

magnesium + oxygen

A

Mg(s) + 1/2O2 (g) = MgO(s)
Magnesium oxide

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6
Q

barium ions + dilute NaOH

A

no change

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7
Q

Aluminium oxide + sulfuric acid

A

Al2O3 + 3H2SO4 = Al2(SO4)3 + 3H2O

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8
Q

Phosphorus oxide + sodium hydroxide

A

P4O10 + 12NaOH = 4Na3PO4 + 6H2O

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9
Q

Silicon + oxygen

A

Si(s) + O2(g) = SiO2
Silicon dioxide

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10
Q

period 3 oxides + water (pH)

A

Na2O + H2O = 2NaOH (12-14)
MgO + H2O = Mg(OH)2 (9-10)

Phosphoric (V) acid (0-2)

P4O10 + 6H2O = 4H3PO4
……..H3PO4 = 3H+ + PO4 3-

Sulfuric (IV) acid (0-2)
SO2 + H2O = H2SO3
……..H2SO3 = 2H+ + SO3 2-

Sulfuric (VI) acid (0-2)
SO3 + H2O = H2SO4
…….. H2SO4 = 2H+ + SO4 2-

Silicon dioxide is insoluble in water, but forms salts when reacted with bases = acidic.

Aluminium oxide is also insoluble in water , however can react with bases and acids to form salts (amphoteric)

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11
Q

use of magnesium hydroxide

A

antacid - helps indigestion

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12
Q

solubility of group 2 compound (singly charged negative ion)

A

increases down the group

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13
Q

test for hydroxides

A
  • drop red litmus paper into solution
  • if present, paper turns blue
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14
Q

Which period 3 elements react well in air

A

More reactive metals (Na, Mg)
Non metals (P, S)

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15
Q

flame test for strontium ions

A

red

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16
Q

how to test for halide ions

A
  • add dilute nitric acid
  • add a few drops of silver nitrate
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17
Q

Sulfur + oxygen

A

S(s) + O2(g) = SO2(g)

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18
Q

test for carbon dioxide

A
  • bubble through limewater
  • will turn cloudy if positive
19
Q

use of calcium hydroxide

A

neutralises agricultural soil

20
Q

use of barium sulfate

21
Q

magnesium + steam

A

faster reaction
Mg(s) + H2O(g) = MgO(s) + H2(g)

22
Q

sodium + oxygen

A

2Na(s) + 1/2 O2(g) = Na2O(s)
sodium oxide

23
Q

aluminium + oxygen

A

2Al(s) + 1.5 O2(g) = Al2O3(s)
Aluminium oxide

24
Q

magnesium + cold water

A

slow reaction
weakly alkaline as mag hydroxide is not very soluble
Mg(s) + 2H2O(l) = Mg(OH)2(aq) + H2(g)

25
sodium + cold water
vigorous reaction highly alkaline as NaOH is extremely soluble 2Na(s) + 2H2O(g) = 2NaOH(aq) + H2(g)
26
Sulfur trioxide + sodium hydroxide
SO3 + 2NaOH = Na2SO4 + H2O
27
28
Structure of period 3 oxides
Na2O - Ionic MgO - Ionic Al2O3 - ionic SiO2 - Giant covalent P4O10 - Simple covalent SO2 - simple covalent
29
precipitates of halide ions with silver nitrate solution
flouride - no precipitate chloride - white bromide - cream iodide - yellow
30
explain the trend in melting points of period 3 oxides
Na2O - lower than MgO since it only forms 1+ ions, not 2+ = lower charge . Al2O3 - lower than expected due to less difference in electronegativity (partially covalent) SiO2 - higher than other non-metals as it is a giant macromolecular structure. Stronger covalent bonds P4O10 and SO2 have relatively low melting points since they only have VDW forces which take little energy to break.
31
Sulfur dioxide + sodium hydroxide
SO2 + 2NaOH = Na2SO3 + H2O
32
test for ammonium ions
- add dilute NaOH solution - gently heat - test using damp red litmus paper (turns blue)
33
Silicon dioxide + sodium hydroxide
SiO2 + 2NaOH = Na2SiO3 + H2O
34
Which period 3 elements react slowly in air
Al , Si
35
test for carbonates
- add dilute hydrochloric acid - carbon dioxide formed (bubbles) - test for this by bubbling through limewater
36
sodium oxide + hydrochloric acid
Na2O + 2HCl = 2NaCl + H2O
37
flame test for calcium ion
brick red
38
solubility of group 2 compound (doubly charged negative ion)
decreases down the group
39
strontium ions + dilute NaOH
slight white precipitate
40
Magnesium oxide + sulfuric acid
MgO + H2SO4 = MgSO4 + H2O
41
flame test for barium ions
pale green
42
calcium ions + dilute NaOH
slight white precipitate
43
solubility of silver halide precipitates in ammonia
chloride - dilute ammonia bromide - conc ammonia iodide - insoluble

CHEM (10 decks)

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