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A level chemistry > Group 2 and 7 > Flashcards

Group 2 and 7 Flashcards

1
Q

what factors affect the ionisation energies of the alkali and alkaline earth metals?

A

size of the ion and charge of the ion

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2
Q

size of the ion ….. down group 2, why

A

increases, due to more shielding and less nuclear attraction

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3
Q

group 2 metal + water

A

metal hydroxide + hydrogen

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4
Q

group 2 metal + oxygen

A

metal oxide

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5
Q

group 2 metal + chlorine

A

metal chloride

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6
Q

reactivity of group 2 metal oxides …… down the group

A

increases

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7
Q

group 2 metal oxide + water

A

metal hydroxide

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8
Q

group 2 metal oxide + acid

A

salt + water

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9
Q

group 2 metal hydroxide + acid

A

salt + water

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10
Q

solubility of group 2 metal hydroxides ….. down the group

A

increases

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11
Q

magnesium hydroxide uses

A

as a laxative or for indigestion

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12
Q

solubility of group 2 metal sulphates ……. down the group

A

decreases

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13
Q

barium sulphate uses

A

barium meal to cause contrast in x rays

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14
Q

Thermal stability

A

a measure of resistance to thermal decomposition.

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15
Q

Thermal decomposition

A

when a substance breaks down when heated.

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16
Q

Polarizing power of a cation

A

its ability to pull the electrons from the anion into the space between the ions

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17
Q

What 2 things affect polarising power?

A

size of the ion, charge density

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18
Q

how does a cation polarise a carbonate

A

distorts the carbonate ion. This weakens the C-O bond

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19
Q

thermally stability of group 2 metal carbonates …….. down the group, why?

A

increases due to decreased charge density so decreased polarisation of the carbonate ion

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20
Q

thermal decomposition of a group 2 metal carbonate forms

A

metal oxide + carbon dioxide

21
Q

fluorine properties

A

pale yellow gas at room temperature

22
Q

chlorine properties

A

pale green gas at room temperature

23
Q

bromine properties

A

brown liquid at room temperature

24
Q

iodine properties

A

black/grey solid at room temperature

25
Q

oxidising power of halogens ……. down the group, why

A

decreases, due to less nuclear attraction from shielding so harder to attract electrons to accept

26
Q

reducing power of halide ions …… down the group, why

A

increases, due to less nuclear attraction from shielding so requires less energy to donate an electron

27
Q

Disproportionation

A

the same atom is simultaneously reduced and oxidised

28
Q

Cl2 + H2O

A

HCl + HOCl

29
Q

Cl2 + NaOH (cold and dilute)

A

NaCl + NaClO + H2O

30
Q

3Cl2 + 6NaOH (hot and concentrated)

A

5NaCl + NaClO3 + 3H2O

31
Q

Li+ flame test

A

crimson

32
Q

Na+ flame test

A

Yellow

33
Q

K+ flame test

A

lilac

34
Q

Ca2+ flame test

A

red

35
Q

Ba2+ flame test

A

green

36
Q

Al3+ with NaOH

A

white ppt, dissolves in excess

37
Q

Ca2+ with NaOH

A

white ppt, does not dissolve in excess

38
Q

Mg2+ with NaOH

A

white ppt, does not dissolve in excess

39
Q

Cu2+ with NaOH

A

pale blue ppt, does not dissolve in excess

40
Q

Fe2+ with NaOH

A

pale green ppt which turns brown when left, does not dissolve in excess

41
Q

Fe3+ with NaOH

A

brown ppt, does not dissolve in excess

42
Q

what is used to clean nichrome wire for flame test

A

concentrated hydrochloric acid

43
Q

where should you hold the wire in a flame test

A

in the edge of the flame

44
Q

Cl-, Br- and I- colour ppt in silver nitrate

A

Cl- = white
Br- = cream
I-= yellow

45
Q

positive carbonate test will

A

turn limewater cloudy

46
Q

positive nitrate test will

A

turn red litmus paper blue with aluminium powder and sodium hydroxide

47
Q

sulphate test with dilute hydrochloric acid and barium sulphate will form

A

white precipitate

48
Q

why are flame test colours formed

A

heat energy excites electrons to a new energy level, a photon is released when they fall back down. This photon directly relates to the wavelength of visible light.

49
Q
A

A level chemistry (16 decks)

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