group 2 Flashcards

1
Q

why are group 2 known as alkaline earth metals

A
  • they react with water to form alkalis (metal hydroxides) and hydrogen.

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2
Q

write an equation for the first ionisation energy of magnesium .

A

Mg (g) —> Mg+ (g) + e-

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3
Q

what happens to the first ionisation energy as you go down group 2? why?

A
  • decreases as number of filled electron shells increases down group —> increased shielding, increased atomic radius —> weaker force between outer electron and nucleus —> less energy needed to remove electron
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4
Q

how does reactivity with water change as you go down group 2?

A
  • increases (Mg lease —> Ba most)
  • outer electrons get further away from nucleus , reducing nuclear attraction
  • electron shielding increases, further reduces attraction between positive nucleus + outer electrons
  • outer two electrons more easily lost to form +2 ions .
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5
Q

write an equation for the reaction of Barium and water.

A
  • Ba (s) + 2H2O (l) —> Ba(OH)2 (aq) + H2 (g)
  • metal + water —> metal hydroxide + hydrogen
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6
Q

write an equation for the reaction of magnesium and steam .

A
  • Mg (S) + H2O (g) —> MgO (s) + H2 (g)
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7
Q

What’s the trend in hydroxide solubility down group 2?

A
  • Increases down the group
  • Mg(OH)2 is almost insoluble
  • Ba(OH)2 creates strong alkaline solution.
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8
Q

what’s the trend in sulphate solubility down group 2?

A
  • decreases down group
  • MgSO4 is soluble
  • BaSO4 is insoluble
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9
Q

What’s the equation when calcium oxide neutralises hydrochloric acid to form a salt and water ? (bases which neutralise acids)

A
  • CaO + 2HCl —> CaCl2 + H2O
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10
Q

what’s the trend in melting point down group 2 ? why?

A
  • decreases down group
  • because sea of delocalised electrons is further from the positive charge of the nucleus —> weaker metallic bonds/ forces of attraction which take less energy to weaken.
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11
Q

what’s the trend in atomic radius down group 2?

A
  • increases as more occupied electron shells down the group .
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12
Q

write the equation for the extraction of Titanium using Magnesium.

A
  • TiO2 + 2Cl2 + C —> TiCl4 + CO2
  • TiCl4 (l) + 2Mg (s) —> 2MgCl2 (s) + Ti (s)
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13
Q

what are flue gases ?

A
  • gases produced by power stations which are harmful to environment
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14
Q

how can CaO or CaCO3 be used to remove flue gases? write equations

A
  • CaCO3 (s) + SO2 (g) —> CaSO3 (s) + CO2 (g)
  • CaO (s) + SO2 (g) —> CaSO3 (s)
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15
Q

what is Ca(OH)2 used for ? write an equation related to one of its uses.

A
  • used to neutralise soil
  • Ca(OH)2 (aq) + 2HCl (aq) —> 2H2O (l) + CaCl2 (aq)
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16
Q

what is Mg(OH)2 used for ?

A
  • milk of magnesia - antacid to treat indisgestion, heartburn , wind etc
17
Q

what’s a use for BaSO4? why is it safe ?

A
  • in barium metals to outline gut in x-rays Ba2+ is toxic but is fine as barium sulphate is insoluble .
18
Q

how can BaCl2 be used to test for sulfate ions?

A

add your sample with HCl first to acidify the solution, then add BaCl2 . white precipitate will form if sulfate ions are present

  • Ba^2+ + SO4^2- —> BaSO4
19
Q

how are group 2 compounds neutralise acids?

A

1) as antacids = magnesium hydroxide and calcium carbonate used in indigestion tablets to neutralise excess stomach acid.

2) calcium hydroxide (slaked lime) used in farming to neutralise acidic soils