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Chemistry > 4.1 > Flashcards

4.1 Flashcards

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1
Q

what does a group 2 element look like

A

when pure a bright silvery solid
exposed in air it appears dull as it combines with oxygen

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2
Q

what is the trend in ionization energy of group 2 metals

A

decreases down the group

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3
Q

why does ionization energy decrease down group 2

A

each quantum shell added energy of outermost electron increases
atomic radius increases so weaker force from nuclei increased shielding

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4
Q

what is the trend in group 2 elements for reactivity and why

A

increases down the group as less energy is needed to remove an electron

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5
Q

what would be observed if you burn magnesium in air

A

bright flame
formation of a white solid

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6
Q

how is barium often stored and why

A

under oil
so it cannot react with oxygen or water vapor as it is extremly reactive

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7
Q

what is the general equation for group 2 metals reacting with oxygen

A

2M(s) + O2(g) -> 2MO(s)

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8
Q

as you go down group 2 you can tell reactivity increases as they react with water because…

A

increasing effervescence

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9
Q

what is the general equation for the reaction of a group 2 metal with water

A

M(s) + 2H2O(l) -> M(OH)4(aq) + H2(g)

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10
Q

what is the trend in solubility of group 2

A

increases down the group

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11
Q

what is the trend in alkalinity of solutions formed of group 2

A

increases down the group

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12
Q

why does the trend in alkalinity of solutions formed of group 2 increase down the group

A

higher solubility therefor more OH- ions present in solution

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13
Q

what is the test for carbon dioxide

A

limewater goes cloudy
white precipitate formed

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14
Q

what do all group 2 oxides & hydroxides form when they react with acids

A

salt & water

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15
Q

what is the trend in solubility of group 2 sulfates

A

decreases down the group

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16
Q

what is the test for the presence of sulfate ions in an aqueous solution

A

add dilute nitric acid or hydrochloric acid
add solution containing barium ions
white precipitate barium sulfate formed

17
Q

why are dilute nitric acid or hydrochloric acid added in the test for sulfate ions

A

to prevent barium carbonate from forming as a white precipitate

18
Q

what is thermal stability

A

measure of the extent to which a compound decomposes when heated

19
Q

why do group 2 nitrated & carbonates have lower thermal stability than group 1

A

cation charge greater than group 1 therefor group 1 ions are less polarising so need more heating tham group 2

20
Q

what happens to group 2 nitrates & carbonates when they are heated

A

they decompose

21
Q

what do all nitrates of group 1 and 2 look like

A

white solid

22
Q

what is observed when group 1/2 nitrates decompose

A

decompose to nitrites or oxides
nitrogen dioxide (brown gas) is produced

23
Q

what do all group 1/2 carbonates look like

A

white solids

24
Q

what happens to group 1 & 2 carbonates when they are heated

A

don’t decompose
or
decompose to oxides and give off carbon dioxide

25
Q

what are the problems with flame tests

A

many compounds contain sodium impurities which will mask other colours
subjective to different levels of colour vision

26
Q

what is the flame test for lithium Li+

A

red

27
Q

what is the flame test for sodium Na+

A

yellow/orange

28
Q

what is the flame test for potassium K+

A

lilac

29
Q

what is the flame test for rubidium Rb+

A

red/purple

30
Q

what is the flame test for caesium Cs+

A

blue/violet

31
Q

what is the flame test for beryllium Be2+

A

no colour

32
Q

what is the flame test for calcium Ca2+

A

brick red

33
Q

what is the flame test for magnesium Mg2+

A

no colour

34
Q

what is the flame test for strontium Sr2+

A

crimson red

35
Q

what is the flame test for barium Ba2+

A

(apple) green

36
Q

what is the flame test for copper

A

blue/green

37
Q

what is the test for aqueous ammonium ions

A

add sodium hydroxide solution & warm
ammonia gas produced

Chemistry (46 decks)

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