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Chemistry gcse ocr a > C4 > Flashcards

C4 Flashcards

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1
Q

Hydrogen gas test

A

Lighted splint ignites with pop

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2
Q

Oxygen gas test

A

Glowing splint relights

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3
Q

Chlorine gas test

A

Damp blue litmus paper turns red then white

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4
Q

Carbon dioxide gas test

A

Turns limewater cloudy

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5
Q

Reactivity series

A

Potassium,sodium,calcium,magnesium,aluminium,zinc,iron,tin,lead,(hydrogen),copper,silver,gold,platinum

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6
Q

Flame test

A

Nichrome wire cleaned in dilute HCl before every test, held in flame until no flame colour is produced and then dipped in solution and put in flame, colour observed

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7
Q

Lithium flame test

A

Red

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8
Q

Sodium flame test

A

Yellow

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9
Q

Potassium flame test

A

Lilac

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10
Q

Calcium flame test

A

Orange-red

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11
Q

Copper flame test

A

Green-blue

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12
Q

Hydroxide precipitate test

A

Sodium hydroxide added to form metal hydrogen precipitate

Eg- NaOH + CuX -> NaX + CuOH(precipitate)

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13
Q

Iron(II) precipitate test

A

Green

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14
Q

Iron(III) precipitate test

A

Orange-brown

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15
Q

Copper precipitate test

A

Blue

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16
Q

Calcium precipitate test

A

White

17
Q

Zinc precipitate test

A

White (dissolves in excess NaOH)

18
Q

Halide ion test

A

Dilute nitric acid and silver nitrate added to produce silver halide

19
Q

Chloride precipitate

A

White

20
Q

Bromine precipitate

A

Cream

21
Q

Iodide precipitate

A

Yellow

22
Q

Why isn’t HCl used in the halide ion test?

A

Hcl has chloride ions, which may lead to a false positive in the test

23
Q

Sulphate ion test

A

Dilute Hydrochloric acid and barium chloride to for barium sulphate (white precipitate)

24
Q

Carbonate ion test

A

Add dilute nitric acid, collect gas produced (seen by bubbles) and do carbon dioxide limewater test

25
Q

Alkali metals properties

A

Shiny, mostly solid at 20c, float on water,reactive, group 1

26
Q

Alkali metal properties (going down group)

A
  • increasing reactivity
  • decreasing melting point
  • decreasing hardness
  • increasing density
27
Q

Halogens properties

A

Non metals, reactive, forms salt when reacted with metals

28
Q

Halogen properties (going down the group)

A
  • increasing melting point
  • decreasing reactivity
  • increasing boiling point
  • increasing density
29
Q

Why does the reactivity decrease as you go down group 7 but increase as you go up group 1?

A
  • group 1 are metals, metals lose electrons on their outer shells
  • Having a shell further away from the nucleus means that the attraction of opposite charges between the nucleus and the outer electrons is weaker.This means that it is easier for the atom to lose its outer electrons.
  • this makes group 1 elements more reactive as more electron shells are present
  • group 7 are non metals , non metals lose electrons on their outer shells
  • Having a shell further away from the nucleus means that the attraction of opposite charges between the nucleus and the outer electrons is weaker.This means that it is harder for the atom to gain outer electrons.
  • this makes group 7 elements less reactive as more electron shells are present
30
Q

Fluorine

A

Pale yellow gas

31
Q

Chlorine

A

Yellow/green gas

32
Q

Bromine colour

A

Reddish-brown liquid

33
Q

Iodine

A

Shiny grey solid (sublimes to purple vapour)

34
Q

Astatine

A

Black solid

35
Q

Nobel gases properties

A

gases at room temperature, inert, group 0

36
Q

Nobel gases properties (going down group)

A
  • increasing melting point
  • increasing boiling point
  • increasing density (because density of gases at room temp remain the same but the molar mass increases)
37
Q

Transition metals properties

A

Form coloured ions,multiple oxidation states, catalysts, malleable, shiny, higher melting points and less reactive than group 1 elements, mostly form 2+ ions.

38
Q

Benefits of instrumental methods of analysis

A
  • More sensitive to smaller substances
  • Much more accurate
  • Much more quicker

Chemistry gcse ocr a (6 decks)

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