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Chemistry > 7 Group 2 & 7 > Flashcards

7 Group 2 & 7 Flashcards

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1
Q

Trend in Atomic radium down G2

A

Increases
More shells
More Dist Less Attract
More shielding

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2
Q

Trend in First IE Grp2

A

Decreases
More shielding
More shells
More distance
Less attract
Easier to remove e

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3
Q

Trend in water reactivity g2

A

Increases
more reducing power
easier to donate e due to increased Ar

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4
Q

Equation of G2 metal and water

A

Mg + 2H2O –> Mg(OH)2 + H2

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5
Q

Equation of G2 metal and steam
Explain why products form

A

Mg + H2O (g) –> MgO + H2

not stable to produce hydroxide, thermal decomposition

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5
Q

Trend in MP G2

A

Decreases
Ar inceases
Less attraction between positive metal ions and delocalised e.
Strength of metallic bonds decrease

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6
Q

Trend in solubility of G2 OH

A

Mg sparingly Ba soluble

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7
Q

Explain why Mg OH2 is sparingly soluble and not just insoluble

A

Slightly alkaline solution indicating some OH ions are dissolved in water

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8
Q

Reactions between G2 and water observations

A

Amount of precipitate formed decreases down grp, all white ppt, fizzing in all.

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9
Q

Test for Mg2+ in MgCl2

A

Add NaOH solution.
White ppt forms.

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10
Q

Explain a use of magnesium.

A

Extract titanium from titanium chloride:
TiO2 + 2Cl2 + C → TiCl4 + CO2
TiCl4 (l) + 2Mg (s) → 2MgCl2 (s) + Ti (s)

Very difficult to extract titanium from its ores (TiO2).
Initially converted to the chloride, then reduced by magnesium.

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11
Q

Use of Mg OH

A

Constipation and Antacid as its slightly alkaline and doesn’t irritate oesophagus.

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12
Q

Use of Ca OH

A

Neutralise acidic soil
Ca(OH)2 (aq) +2HCl (aq) → 2H2O (l) + CaCl2 (aq)

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13
Q

Use of calcium Oxide/ Carbonate

A

Flue gas removal
CaCO3 (s) + SO2 (g) → CaSO3 (s) + CO2 (g)
CaO (s) + SO2 (g) → CaSO3 (s)

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14
Q

Use of barium sulphate?

A

barium meals, outline gut in x rays, insoluble so safe.

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15
Q

Trend in sulphate solubility

A

decreases
Mg sol
Bas insol

16
Q

Use of barium chloride to test for sulphate ions?

A

Acidify with HCL white ppt produced.

17
Q

Na F and Cl with Sulphuric Acid
Br and I first step

A

NaCl + H2SO4 > HCl + NaHSO4

18
Q

Br and I second step with Sulphuric acid

A

H2SO4 + 2H+ + 2Br- > Br2 + SO2 + 2H2O
2HI (g) + H2SO4 (l) → I2 (g) + SO2 (g) + 2H2O (l)

19
Q

I third and fourth step with Sulphuric acid

A

6HI (g) + H2SO4 (l) → 3I2 (g) + S (s) + 4H2O (l)

8HI (g) + H2SO4 (l) → 4I2 (g) + H2S (s) + 4H2O (l)

20
Q

Test for SO42-

A
  1. Acidify with dilute HCl 2. Add BaCl
    White precipitate of BaSO4
21
Q

Test for I-

A

Acidify with dilute HNO3
2. Add AgNO3
3. (Add dilute NH3 followed by conc. NH3)

Yellow precipitate Insoluble in conc. NH3

21
Q

Test for CO32-

A

Add dilute HCl
Effervescence Gas produced turns limewater cloudy

21
Q

Test for Br-

A

Acidify with dilute HNO3
2. Add AgNO3
3. (Add dilute NH3 followed by conc. NH3)

Cream precipitate dissolves in conc. NH3 (NOT with dilute)

21
Q

Test for Cl-

A

Acidify with dilute HNO3
2. Add AgNO3
3. (Add dilute NH3 followed by conc. NH3)

White precipitate dissolves in dilute NH3

22
Q

Test for OH-

A

Damp red litmus paper
Turns from red to blue

23
Q

Test for Mg2+

A

In separate test-tubes:
* Add dilute NaOH With OH-: white precipitate

  • Add dilute H2SO4 With SO42-: nvc
24
Q

Test for Sr2+

A

In separate test-tubes:
* Add dilute NaOH With OH-: nvc

  • Add dilute H2SO4 With SO42-: white precipitate
25
Q

Test for Ca2+

A

In separate test-tubes:
* Add dilute NaOH With OH-: white precipitate/ suspension

  • Add dilute H2SO4 With SO42-: slight white precipitate
25
Q

Test for Ba2+

A

In separate test-tubes:
* Add dilute NaOH With OH-: nvc

  • Add dilute H2SO4 With SO42-: white precipitate
26
Q

Test for NH4+

A
  1. Add NaOH
  2. Heat sample
  3. Hold damp red litmus paper at test tube mouth

litmus paper will turn from red to blue.

27
Q

chlorine with water to form chloride ions and chlorate (I) ions

A

Cl2(g) + H2O(l) <-> HCl(aq) + HClO(aq)

reversible reaction, green solution formed showing presence of chlorine.

Disproportionation
(0 -> +1 in HClO)
(0-> -1 in HCl)
If Univ Ind is added, red first then bleached, protons then chlorate bleach

28
Q

reaction of chlorine with water to form chloride ions and oxygen

A

sunlight green colour fades
colourless gas is produced

2Cl2(g) + 2H2O(l) -> 4HCl(aq) + O2(g)

chlorine (0-> -1)
oxygen (-2 -> 0)

29
Q

reaction of chlorine with cold, dilute, aqueous NaOH and uses

A

Cl(g) + 2NaOH(aq) -> NaCl(aq) + NaClO(aq) + H2O(l)

  • if water replaced by NaOH, the equilibrium is destroyed as the NaOH reacts with the acids formed.
  • commercial preparation of bleach NaClO
  • the chlorate (1) may decompose to form chloride and chlorate (V)

3ClO^-(aq) -> 2Cl^-(aq) + ClO3^-(aq)

  • the reaction is slow at rtp but fast at 70˚C
  • NaClO3^-(aq) is a powerful weed killer
30
Q

Why do we use ammonia to test for halides?

A

What is used to test if a precipitate definitely contains a halide based on their ability to redissolve.

31
Q

The type of reaction involving NaCl + H2SO4

A

Acid-base

32
Q

The type of reaction involving NaI + H2SO4 then I- + H2SO4 and finally 8H+ + 8I- + H2SO4

A

Acid-base then Redox

33
Q

The type of reaction involving NaBr + H2SO4 then Br- + H2SO4

A

Acid-base then Redox

Chemistry (33 decks)

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