Chapter 7: QA Flashcards
Name the colours for the aqueous ion, hydroxide, carbonate and oxide for group 1/2/3 metals
Aqueous ion: Colourless
Hydroxide: White solid
Carbonate: White solid
Oxide: White solid
Name the colours for the element, aqueous ion, hydroxide, carbonate and oxide for zinc
Element: Shiny grey Aqueous ion: Colourless Hydroxide: White Carbonate: White solid Oxide: Yellow when hot, white when cold
Name the colours for the element, aqueous ion, hydroxide, carbonate and oxide for lead
Element: Shiny grey Aqueous ion: Colourless Hydroxide: White Carbonate: White solid Oxide: red when hot, yellow when cold
Name the colours for the element, aqueous ion, hydroxide, carbonate and oxide for copper
Element: Pink-brown Aqueous ion: blue Hydroxide: Light blue Carbonate: Green Oxide: Black
Name the colours for the element, aqueous ion, hydroxide, carbonate and oxide for iron(ii)
Element: Shiny grey Aqueous ion: Pale green Hydroxide: dirty-green Carbonate: dirty-green solid Oxide: Black solid
Name the colours for the element, aqueous ion, hydroxide, carbonate and oxide for iron(iii) oxide
Element: Shiny grey Aqueous ion: yellow Hydroxide: Reddish-Brown Carbonate: NA Oxide: Red-brown
Name the colour of chlorine at r.t.p, in a solution as an aqueous ions, and its precipitates
r.t.p: Greenish-yellow
Solution: colourless
Aqueous ions: colourless
precipitates: white ppt
Name the colour of bromine at r.t.p, in a solution, in a solution, as an aqueous ion, and its precipitates
r.t.p: red-brown liquid
vapour: red-brown gas
solution: Orange-brown
Aqueous ion: Colourless
Precipitates: Cream ppt
Name the colour of iodine at r.t.p, as a vapour, in a solution, as an aqueous ion, and its precipitates
r.t.p: black solid
vapour: purple gas
in a solution: yellow-brown
Aqueous ion: colourless
Precipitates: yellow ppt
State what happens when carbonates are thermally decomposed
Non group 1 carbonates decompose to form a metal oxide and carbon dioxide
State what happens when hydroxides are thermally decomposed
Non group 1 hydroxides thermally decompose to form a metal oxide and water vapour
Describe the test for hydrogen
Test the gas with a lighted splint
Positive result: The lighted splint extinguishes with a ‘pop’ sound
Negative result: The splint extinguishes
Describe a test for oxygen
Test the gas with a glowing splint
Positive result: The splint rekindles
Negative result: The splint extinguishes
Describe a test for CO2
Bubble the gas through limewater
Positive result: a white ppt is formed
Negative result: no ppt is formed
Describe a test for chlorine
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
Describe a test for ammonia
Test the gas with moist red litmus paper
Positive result: the moist red litmus paper turns blue
Negative result: depends on acidity
Describe a test for sulfate and chloride ions
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
Describe a test for iodide ions
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
Describe a test for carbonate ions
Add dilute nitric acid. If carbonate ions are present, effervescence would be observed (Carbon dioxide)
Describe a test for ammonium ions
Add aqueous sodium hydroxide ad warm gently. If Ammonium ions are present, a colourless, pungent gas is evolved(Ammonia)
Describe a test for nitrate ions
Add aqueous sodium hydroxide, aluminium foil and warm gently. If nitrate ions are present, a colourless, pungent gas is evolved (Ammonia)
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
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
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
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
Since Aluminium and lead(II) ions produce identical observations when tested with aqueous NaOH or aqueous ammonia, how do we distinguish them?
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.
