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Chemistry > Chapter 8 Reactivity Trends > Flashcards

Chapter 8 Reactivity Trends Flashcards

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1
Q

What sub-shell are the outer electrons of group 2 elements in

A

S

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2
Q

What is the reaction of calcium becoming an ion

A

Ca → Ca2+ + 2e-

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3
Q

Why are group 2 elements called reducing agents

A

Group 2 element are called reducing agents because they have reduced another species. Group 2 elements are oxidised to produce 2+ ions

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4
Q

What do group 2 elements produce when they react with oxygen and what is the formula

A

Metal oxide
MO

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5
Q

What is the equation of Magnesium reacting with Oxygen

A

Mg(s) + ½O2(g) → MgO(s)

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6
Q

What are the half equations for the reaction and the Oxidation numbers:
Mg(s) + ½O2(g) → MgO(s)

A

Mg → Mg2+ + 2e-
0 → +2
Mg Oxidised

½O2 + 2e- → O2-
0 → -2 Reduced

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7
Q

What do group 2 metals react with water to produce and what is the formula

A

An alkaline hydroxide + Hydrogen Gas
M(OH)2

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8
Q

What are the observations of Group 2 elements reacting with water

A
  • Bubbling
  • Solid disappears
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9
Q

Does reactivity increase or decrease down group 2

A

Increases

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10
Q

What is the equation for the reaction of Strontium with Water

A

Sr(s) + 2H2O(l) → Sr(OH)2(aq) + H2(g)

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11
Q

In the reaction
Sr(s) + 2H2O(l) → Sr(OH)2(aq) + H2(g)
What has been oxidised and what has been reduced

A

Strontium Oxidised
Hydrogen Reduced

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12
Q

Group 2 Element + Dilute Acid →

A

Salt + Hydrogen
MASH

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13
Q

What is the equation for the reaction of Magnesium with Hydrochloric Acid

A

Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

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14
Q

In the equation of Mg With HCl
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
What is oxidised and what is reduced

A

Mg Oxidised
H Reduced

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15
Q

How many ionisation energies does the formation of a 2+ ion involve

A

2

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16
Q

What is the equation of the first ionisation energy of a group 2 element M

A

M(g) → M+(g) + e-

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17
Q

What is the equation of the second ionisation energy of a group 2 element M

A

M+(g) → M2+(g) + e-

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18
Q

Why do the ionisation energies decrease down a group

A
  • Atomic Radius Increases
  • Inner Shell Shielding increases
  • Nuclear Attraction decreases
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19
Q

Going down group 2, does the reducing ability increase or decrease

A

Increases

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20
Q

What is produced when group 2 Oxides react with water

A

hydroxide ions
alkaline solutions of the metal hydroxide

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21
Q

What is the equation of Calcium oxide with Water

A

CaO(s) + H2O(l) → Ca2+(aq) + 2OH-(aq)

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22
Q

How soluble are Group 2 Hydroxides in water

A

The Group 2 hydroxides are only slightly soluble in water

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23
Q

What happens when a solution of water and group 2 hydroxides becomes saturated

A

Any further metal and hydroxide ions will form a white precipitate

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24
Q

As you go down the group 2 hydroxides, do Solubility, Alkalinity and PH increase or decrease

A

Going down group 7
* solubility increases
* pH increases
* alkalinity increases
As solubility increases, the resulting solutions contain more OH-(aq) ions and are more alkaline

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25
Q

How is Calcium Hydroxide Ca(OH)2(a base) used in agriculture

A

is added to fields as lime by farmers to increase the pH of acidic soils in a neutralisation reaction
Ca(OH)2(s) + 2H+(aq) → Ca2+(aq) + 2H2O(l)

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26
Q

How are group 2 Bases used in medicine

A

Group 2 bases are often used as antacids for treating acid indigestion
Mg(OH)2(s) + 2HCl(aq) → MgCl2(aq) + 2H2O(l)

Magnesium and calcium carbonates are the main ingredients in indigestion tablets

27
Q

Are group 7 elements oxidising agents or reducing agents

A

oxidising agents

28
Q

What sub shells are the outer 7 electrons of group 7 elements in

A

2 are in the outer s sub-shell and 5 are in the outer p sub-shell

29
Q

What colour is chlorine solution in water

A

Pale Green

30
Q

What colour is Bromine solution in water I2(aq)

A

Orange

31
Q

What colour is Iodine solution in water I2(aq)

A

Brown

32
Q

What colour is Chlorine in a non-polar solvent

A

Pale Green

33
Q

What colour is Bromine in a non-polar solvent

A

Orange

34
Q

What colour is Iodine in a non-polar solvent

A

Purple

35
Q

What state and colour is Fluorine in at RTP

A

Pale Yellow Gas

36
Q

What state and colour is Chlorine at RTP

A

Pale Green Gas

37
Q

What state and colour is Bromine at RTP

A

Red-Brown Liquid

38
Q

What state and colour is Iodine at RTP

A

Shiny Grey - Black Solid

39
Q

What state and colour is Astatine at RTP

A

Never been seen

40
Q

Does the boiling point increase or decrease down the group 7

A

Increases

41
Q

Why does the boiling point increase going down group 7

A
  • More electrons
  • Stronger London Forces
  • More energy required to break the intermolecular forces
  • Boiling Point increases
42
Q

Does reactivity increase or decrease down group 7

A

Decreases down the group

43
Q

Why does reactiity decrease down group 7

A
  • Atomic Radius increases
  • More inner shell shielding
  • Less attraction to gain an element
  • Reactivity decreases
44
Q

Does oxidising ability increase or decrease down the group

A

Decreases

45
Q

What is Disproportionation

A

A redox reaction in which the same element is both oxidised and reduced

46
Q

What is the equation for the reaction of chlorine with water

A

Cl2(aq) + H2O(l) → HClO(aq) + HCl(aq)

47
Q

What is the reaction of chlorine with cold dilute aqueous sodium hydroxide

A

Cl2(aq) + 2NaOH(aq) → NaClO(aq) + NaCl(aq) + H2O(l)

48
Q

What is the benefit of chlorine use

A

Chlorine is beneficial in ensuring our water is safe to drink, by killing all bacteria present

49
Q

What are the risks of Chlorine Use

A

Chlorine is an extremely TOXIC gas:
* in small concentrations it is a respiratory irritant.
* in large concentrations it can be fatal.

Chlorine added to drinking water can react with organic hydrocarbons, such as methane, to form chlorinated hydrocarbons – a suspected carcinogen

50
Q

Cl2(aq) + 2Br-(aq) →

A

2Cl-(aq) + Br2(aq)

51
Q

Cl2(aq) + 2I-(aq) →

A

2Cl-(aq) + I2(aq)

52
Q

Br2(aq) + 2I-(aq) →

A

2Br-(aq) + I2(aq)

53
Q

How do you test for halide ions

A

Add aqueous silver ions to aqueous halide ions to form a precipitate of silver halide

54
Q

What is the ionic equation for testing for Halide ions

A

Ag+(aq) + X-(aq) → AgX(s)

55
Q

What colour is the precipitate formed when testing for Chloride ions
Is it soluble in Dilute NH3 or Concentrated NH3 or not at all

A

White
Soluble in dilute NH3

56
Q

What colour is the precipitate formed when testing for Bromide ions
Is it soluble in Dilute NH3 or Concentrated NH3 or not at all

A

Cream Precipitate
Soluble in concentrated NH3

57
Q

What colour is the precipitate formed when testing for Iodide ions
Is it soluble in Dilute NH3 or Concentrated NH3 or not at all

A

Yellow Precipitate
Insoluble in concentrated NH3

58
Q

How do you test for Carbonates

A

Add dilute nitric acid to a test tube containing the unknown compound
Observation - Bubbles of gas

59
Q

What is the ionic equation for a Carbonate test

A

CO32-(aq) + 2H+ → CO2(g) + H2O(l)

60
Q

How do you test for sulfates

A

Add barium nitrate to a test tube containing a solution of the unknown compound
Observation – a white precipitate (of barium sulfate) forms

61
Q

What is the ionic equation for the sulfate test

A

Ba2+(aq) + SO42-(aq) → BaSO4(s)

62
Q

What is the order you should perform the anions tests in

A
  1. Carbonate, CO32-
  2. Sulfate, SO42-
  3. Halides, Cl-, Br-, I-
63
Q

Why do you do the anion tests in this order:
1. Carbonate, CO32-
2. Sulfate, SO42-
3. Halides, Cl-, Br-, I-

A
  • If carbonate ions are present when testing for sulfate ions (addition of barium nitrate) – a white precipitate of barium carbonate, BaCO3(s), will form.
  • If carbonate ions and/or sulfate ions are present when testing for halide ions (addition of silver nitrate) – white precipitates of silver carbonate, Ag2CO3(s), and/or silver sulfate, Ag2SO4(s) will form.

Chemistry (16 decks)

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