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Chemistry > Chapter 7: QA > Flashcards

Chapter 7: QA Flashcards

1
Q

Name the colours for the aqueous ion, hydroxide, carbonate and oxide for group 1/2/3 metals

A

Aqueous ion: Colourless
Hydroxide: White solid
Carbonate: White solid
Oxide: White solid

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2
Q

Name the colours for the element, aqueous ion, hydroxide, carbonate and oxide for zinc

A 
Element: Shiny grey
Aqueous ion: Colourless
Hydroxide: White
Carbonate: White solid
Oxide: Yellow when hot, white when cold
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3
Q

Name the colours for the element, aqueous ion, hydroxide, carbonate and oxide for lead

A 
Element: Shiny grey
Aqueous ion: Colourless
Hydroxide: White
Carbonate: White solid
Oxide: red when hot, yellow when cold
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4
Q

Name the colours for the element, aqueous ion, hydroxide, carbonate and oxide for copper

A 
Element: Pink-brown
Aqueous ion: blue
Hydroxide: Light blue
Carbonate: Green
Oxide: Black
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5
Q

Name the colours for the element, aqueous ion, hydroxide, carbonate and oxide for iron(ii)

A 
Element: Shiny grey
Aqueous ion: Pale green
Hydroxide: dirty-green
Carbonate: dirty-green solid
Oxide: Black solid
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6
Q

Name the colours for the element, aqueous ion, hydroxide, carbonate and oxide for iron(iii) oxide

A 
Element: Shiny grey
Aqueous ion: yellow
Hydroxide: Reddish-Brown
Carbonate: NA
Oxide: Red-brown
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7
Q

Name the colour of chlorine at r.t.p, in a solution as an aqueous ions, and its precipitates

A

r.t.p: Greenish-yellow
Solution: colourless
Aqueous ions: colourless
precipitates: white ppt

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8
Q

Name the colour of bromine at r.t.p, in a solution, in a solution, as an aqueous ion, and its precipitates

A

r.t.p: red-brown liquid
vapour: red-brown gas
solution: Orange-brown
Aqueous ion: Colourless
Precipitates: Cream ppt

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9
Q

Name the colour of iodine at r.t.p, as a vapour, in a solution, as an aqueous ion, and its precipitates

A

r.t.p: black solid
vapour: purple gas
in a solution: yellow-brown
Aqueous ion: colourless
Precipitates: yellow ppt

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10
Q

State what happens when carbonates are thermally decomposed

A

Non group 1 carbonates decompose to form a metal oxide and carbon dioxide

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11
Q

State what happens when hydroxides are thermally decomposed

A

Non group 1 hydroxides thermally decompose to form a metal oxide and water vapour

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12
Q

Describe the test for hydrogen

A

Test the gas with a lighted splint
Positive result: The lighted splint extinguishes with a ‘pop’ sound
Negative result: The splint extinguishes

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13
Q

Describe a test for oxygen

A

Test the gas with a glowing splint
Positive result: The splint rekindles
Negative result: The splint extinguishes

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14
Q

Describe a test for CO2

A

Bubble the gas through limewater
Positive result: a white ppt is formed
Negative result: no ppt is formed

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15
Q

Describe a test for chlorine

A

test the gas with moist blue litmus paper
Positive result: the moist blue litmus paper turns red and then white
Negative result: depends on acidity

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15
Q

Describe a test for ammonia

A

Test the gas with moist red litmus paper
Positive result: the moist red litmus paper turns blue
Negative result: depends on acidity

16
Q

Describe a test for sulfate and chloride ions

A

To a sample of unknown solution, add dilute nitric acid, followed by aqueous silver nitrate./barium nitrate. If chloride/sulfate ions are present, a white ppt will form

17
Q

Describe a test for iodide ions

A

To a sample of unknown solution, add dilute nitric acid followed by aqueous silver nitrate. If iodide ions are present, a yellow ppt will form

18
Q

Describe a test for carbonate ions

A

Add dilute nitric acid. If carbonate ions are present, effervescence would be observed (Carbon dioxide)

19
Q

Describe a test for ammonium ions

A

Add aqueous sodium hydroxide ad warm gently. If Ammonium ions are present, a colourless, pungent gas is evolved(Ammonia)

20
Q

Describe a test for nitrate ions

A

Add aqueous sodium hydroxide, aluminium foil and warm gently. If nitrate ions are present, a colourless, pungent gas is evolved (Ammonia)

21
Q

State the observations for Aluminium ions, lead(II) ions, Zinc, copper(ii) ions, iron(II) ions, Iron(III) ions, calcium ions when a few drops of NaOH is added and when excess NaOH is added

A

Aluminium - A white ppt forms which dissolves in excess in NaOH, forming a colourless solution
Lead(II) - A white ppt forms which dissolves in excess NaOH, forming a colourless solution
Zinc - A white ppt forms which dissolves in excess NaOH, forming a colourless solution
Copper(ii) - A light blue ppt forms which is insoluble in excess NaOH
Fe(II) - A green ppt forms which is insoluble in excess NaOH
Fe(III) - A red-brown ppt forms which is insoluble in excess NaOH
Calcium - A white ppt forms which is insoluble in excess NaOH

22
Q

State the observations for Aluminium ions, lead(II) ions, Zinc, copper(ii) ions, iron(II) ions, Iron(III) ions, calcium ions when a few drops of NH3 is added and when excess NH3 is added

A

Aluminium - A white ppt forms which is insoluble in excess NH3
Lead(II) - A white ppt forms which is insoluble in excess NH3
Zinc - A white ppt forms which dissolves in excess NH3, forming a colourless solution
Copper(II) - A light blue ppt forms which is insoluble in excess NH3
Iron(II) - A green ppt forms which is insoluble in excess NH3
Iron(III) - A red-brown ppt forms which is insoluble in excess NH3
Calcium - no ppt forms

23
Q

Since Aluminium and lead(II) ions produce identical observations when tested with aqueous NaOH or aqueous ammonia, how do we distinguish them?

A

A third test is carried out by adding either aqueous sulphate, chloride, or iodide ions, which would form a ppt in the presence of lead(II) ions, but not in the presence of aluminium ions.

Chemistry (7 decks)

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