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a-level chemistry > Groups 1, 2 > Flashcards

Groups 1, 2 Flashcards

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1
Q

name the three physical properties of group two elements

A
  • ionisation energy
  • atomic radius
  • reactivity
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2
Q

how does ionisation energy change down group two and why

A
  • ionisation energy decreases down group two
  • greater atomic radius, increased shielding, easier to lose an electron
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3
Q

how does reactivity change down group two and why

A
  • reactivity increases down group two
  • increased electron shielding and atomic radius, outer (valence) electron easier to lose, reactions can occur more easily
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4
Q

how does atomic radius change down group two and why

A
  • atomic radius increases
  • additional electron shells
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5
Q

what type of reaction is a metal + water

A

redox reaction

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6
Q

metal + water ->

A

metal hydroxide + hydrogen

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7
Q

what kind of solution is a metal hydroxide

A

an alkaline solution

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8
Q

general equation for reaction of group 2 metals with water

A

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

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9
Q

how is a reaction with water different to one with steam

A
  • steam produces a metal oxide and hydrogen
  • reaction with steam is faster because it has more energy
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10
Q

metal + steam ->

A

metal oxide (white powder) + hydrogen

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11
Q

general equation for reaction of group 2 metal and steam

A

M(s) + H2O(g) -> MO(s) + H2

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12
Q

metal + chlorine gas ->

A

metal chloride (white precipitate)

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13
Q

general equation for reaction of group 2 metal + chlorine gas

A

M(s) + Cl2(g) -> MCl2(s)

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14
Q

how does reactions with chlorine gas change down group two

A
  • it becomes more vigorous down group 2
  • because metals more reactive
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15
Q

metal + oxygen ->

A

metal oxide

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16
Q

general equation for group 2 metal + oxygen in normal conditions

A

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

17
Q

which two group two metals dont fit the general pattern of reaction with oxygen

A

strontium and barium

18
Q

strontium/barium + oxygen ->

A

metal peroxide

19
Q

when do strontium and barium become peroxides

A

when reacting with excess oxygen and heat energy

20
Q

(with excess oxygen and heat energy)
M(s) + O2(g) ->

A

MO2

21
Q

which group 2 metals react

A

Mg-Ba

22
Q

general equation for reactions of metal oxides and water

A

MO(s) + H2O(l) -> M(OH)2(aq)

23
Q

general equation for reactions of metal oxides and dilute hydrochloric acid

A

MO(s) + 2HCl(aq) -> MCl2(aq) + H2O(l)

24
Q

general equations for metal hydroxides in water

A

—————H2O(l)——————
M(OH)2(s) ——-> M(OH)2(aq)

25
Q

general equation for reactions of metal hydroxides and dilute hydrochloric acid

A

M(OH)2(aq) + 2HCl(aq) –> MCl2(aq) + 2H2O(l)

26
Q

how does solubility of metal hydroxides change down group two

A
  • solubility increases down group two
  • (magnesium hydroxide least soluble)
27
Q

real life uses of magnesium hydroxide

A
  • antiacid (neutralises acids in the body)
  • neutralises acidic soil
28
Q

how does solubility of metal sulfates change down group two

A
  • solubility decreases down group two
  • (barium sulfate least soluble)
29
Q

real life uses of barium sulfate

A
  • used in medicine as ‘barium metals’ (allows internal organs and tissues to be imaged)
  • usually toxic, but cannot be absorbed into the bloodstream so safe
30
Q

how does thermal decomposition occur

A

when substances are heated in aerobic conditions

31
Q

thermal decomposition of a group 2 metal carbonate produces

A

metal oxide (white powder) + carbon dioxide

32
Q

general equation for thermal decomposition of group 2 metal carbonates

A

MCO3(s) –> MO(s) + CO2(g)

33
Q

group 2 metal nitrates undergo thermal decomposition to form

A

metal oxide + nitrogen dioxide + oxygen

34
Q

general equation for thermal decomposition of group 2 metal nitrates

A

2M(NO3)2(s) —> 2MO(s) + 4NO2)g) + O2(g)

35
Q

what group 1 metal carbonate and nitrate acts the same as group 2

A

lithium

36
Q

thermal decomposition of group 1 metal carbonates

A
  • wont decompose upon heating as they require extremely high temperatures to do so
37
Q

group 1 metal nitrates undergo thermal decomposition to produce

A

metal nitrite + oxygen

38
Q

general equation for thermal decomposition of group one metal nitrates (excluding lithium)

A

2MNO3(s) –> 2MNO2(s) + O2(g)

39
Q

describe and explain the trend in thermal stability for group 1 and 2 nitrates and carbonates

A
  • become more thermal stable down the group
  • down group, ionic radius increases (-smaller ions at top have a higher charge density)
  • higher charge density
  • polarise more
  • distorts anion
  • weakens c-o bond /n-o bond
  • less thermally stable

a-level chemistry (21 decks)

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