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NSAA > Chemistry > Flashcards

Chemistry Flashcards

1
Q

Relative mass of an electron

A

1/200

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2
Q

Using a mass spectrometer

A

…

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3
Q

Relative atomic mass

A

The average mass of one atom compared to 1/12 of the mass of one atom of carbon-12

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4
Q

Group 2

A

Alkaline earth metals

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5
Q

Going down a metal group

A

Reactivity increases

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6
Q

Going down a non-metal group

A

Reactivity decreases

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7
Q

In a chemical reaction

A

New substances are formed by the rearrangement of atoms and their electrons, but no nuclei are destroyed or created

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8
Q

Factors affecting equilibrium position

A

Concentration
Temperature
Pressure

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9
Q

Relative molar mass

A

Is this the same as relative molecular mass?

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10
Q

Avogadros number

A

Number of particles in one mole of substance

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11
Q

Grams -> moles

A

Divide grams by molar mass

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12
Q

Calculating solubility

A

…

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13
Q

Ionic bonding

A

Transfer of electrons from metals to non metals creates ions

Opposite charged ions attract

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14
Q

When to apply centrifugation

A

used for the separation of particles from a solution according to their size, shape, density and viscosity

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15
Q

When do apply dissolving

A

Separate soluble and insoluble

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16
Q

Establishing purity using chromatography

A

…

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17
Q

Why is direct current used in electrolysis

A

Means anions go to anode and cations go to cathode

If alternating current was used, it would lead to uneven disposition of the ions at the electrodes

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18
Q

At the cathode

A

Cations are reduced

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19
Q

At the anode

A

Anions are oxidised

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20
Q

Aqueous electrolysis

A

…

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21
Q

As carbon chain length increases, boiling point.

A

Increases

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22
Q

As carbon chain length increases, viscosity

A

Increases

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23
Q

As carbon chain length increases, flammability

A

Decreases

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24
Q

Alkene addition with steam (hydration)

A

Conditions:
300-600
70atm
H3PO4

alkene -> alcohol

No waste product, easy cheap - high atom economy

H+ and OH- added

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25
Q

Alcohols + sodium

A

Effervescence (hydrogen)
Mixture gets hot
Sodium dissolved
Sodium alkoxide is produced (white solid)

Test for alcohols

26
Q

Carboxylic acids

A

CnH2n+1COOH

27
Q

Metal reactivity

A

Tendency to form positive ions and the ease of extraction of the metal

28
Q

Metal extraction

A

Involved reduction processes

29
Q

Transition metals

A
  1. Able to form stable ions in different oxidation states
  2. Often form coloured compounds
  3. Often used as ionic or atomic catalysts
30
Q

Chlorine test

A

Damp blue litmus turns red and is then bleached

31
Q

Metal + NaOH

A
  1. Al3+, Ca2+, Mg2+ -> white ppt
  2. Cu2+ -> blue ppt
  3. Fe2+ -> green ppt
  4. Fe3+ -> brown ppt
32
Q

Flame tests

A

Li - crimson red
Na - yellow orange
Ca - red-orange

33
Q

Fractional distillation can be used to

A

Separate the components of air

34
Q

Origins of greenhouse gases

A

Burning fossil fuels

35
Q

Effects of greenhouse gases

A

Absorbs IR from the sun (which is absorbed and re-radiated at a lower frequency) and convert to heat energy, warming the atmosphere

36
Q

Treating water

A

With chlorine: hydrochloric and chloric (1) acid which act as disinfectants (oxidising agent)

Kills bacteria by oxidation

pH is treated by adding calcium hydroxide

37
Q

First and successive ionisation energies in group 2

A
  • decreases
  • distance from nucleus increases
  • greater shielding
38
Q

First and successive ionisation energies in period 3

A
  • increase
  • electrons are added to the same electron shell (same distance)
  • nuclear charge increases; attraction increases
  • more energy needed for removal
39
Q

Kinetic energy

40
Q

Describe the workings of a TofF spectrometer

41
Q

Electronegativity

A

The tendency of an atom to attract a shared pair of electrons

42
Q

Group 2 metals + oxygen

A 
• except Be, they all react vigorously - bright flame 
• Mg -> bright white flame 
• Ca + Sr -> red flame 
• Ba -> green flame 
Except Ba: 
• 2M + O2 -> 2MO
• Ba + O2 -> 2BaO2 (peroxide ion O22-)
43
Q

Group 2 metals + water

A

• Be does not react
• Mg reacts v slowly w/ cold water. W/ steam -> MgO + H2
• Ca, Sr and Ba react w/ cold water with increasing vigour:
-> hydroxide + hydrogen

  • Ca(OH)2 -> sparingly soluble in water; effervescence, thick white suspension
  • Sr(OH)2 -> is slightly soluble
  • Ba(OH)2 -> soluble
44
Q

Group 2 metal oxides + water

A
  • BeO mot attacked

* other hydroxides

45
Q

Group 2 hydroxide solubility

A

Solubility increases down the group

46
Q

Group 2 sulphate solubility

A

Solubility decreases down the group

47
Q

Thermal décomposition of group 2 metal carbonates

A

Metal oxide + CO2

48
Q

Cold aqueous NaOH + chlorine

A

Cl2 + 2NaOH -> NaOCl + NaCl

49
Q

Water + chlorine

50
Q

Concentrated sulphuric acid reactions

A

Chloride:

-> KHSO4 + HCl

Bromide:

  • > same as above
  • > KBr + H2SO4 -> Br2 + SO2 + 2H2O

Iodide:

  • > same as above
  • > same as above
51
Q

Reducability of halide ions

A

Iodide is the strongest reducing agent

52
Q

Atomic ratio explanations in group 1,2 and 7

53
Q

First ionisation energy explanation in groups 1,2 and 7

A

Decreases for same reason as before

54
Q

Boiling point in groups 1,2 and 7

55
Q

Melting and boiling points in periods 2 and 3

56
Q

First ionisation energy in periods 2 and 3

A

Increases for same reason as before

57
Q

Atomic radii in periods 2 and 3

58
Q

Electronegativity in periods 2 and 3

59
Q

Cycloalkanes

60
Q

Elimination

A

Removal of a small molecule for an organic molecule

E.g. ethanolic élimination of halogenoalkanes

61
Q

How does bond polarity influence reactivity

NSAA (6 decks)

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