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N Chemistry A Level > topic 4 > Flashcards

topic 4 Flashcards

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1
Q

do atom sizes increase or decrease down the periodic table?

A

increase

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2
Q

do atom sizes increase or decrease across the periodic table?

A

decrease

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3
Q

what are 3 factors that impact ionisation energies?

A
  • nuclear radius (smaller=stronger)
  • nuclear attraction
  • # of shielding(Same as electro negativity)
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4
Q

does reactivity increase or decrease down group 2?

A

increase

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5
Q

does boiling point increase or decrease down group 2?

A

decrease

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6
Q

does boiling point increase or decrease down group 7?

A

increase

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7
Q

does reactivity increase or decrease down group 7?

A

decrease

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8
Q

G2 Metal + O2 ->

A

2MO (s)

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9
Q

G2 metal oxide + H2O ->

A

M(OH)2 (aq)

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10
Q

G2 Metal + Cl2 ->

A

MCl2 (s)

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11
Q

G2 Metal + 2H2O (l) ->

A

M(OH)2 + H2

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12
Q

Does solubility of G2 metal hydroxides increase or decrease down the group? Why?

A

increase,
because atomic radius increases so it is easier to break
1- ions
HydroxIIIIdes

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13
Q

Mg + H2O(g/steam) ->

A

MgO (s) + H2 (g)

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14
Q

Does G2 metal sulphate solubility increase or decrease down the group?

A

decrease down
Bcs 2- ions
SSSSulphate - leSSSS

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15
Q

Ba(NO3)2 (aq) + Na2SO4 (aq) ->
Barium nitrate + Sodium sulfate ->

A

BaSO4 (s) + 2 NaNO3 (aq)
Barium sulfate + Sodium nitrate

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16
Q

Ca(OH)2 (aq) + CO2 (g) ->

A

CaCO3 (s) + H2O (l)

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17
Q

what are G2 metal oxides and hydroxides used for?

A

Neutralisation reactions and agriculture

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18
Q

what is formed when brown fumes are observed?

A

NO2
Nitrogen dioxide

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19
Q

what is the definition of thermal stability?

A

How much a compound decomposes under heat

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20
Q

What are 3 factors that affect thermal stability?

A
  • ionic radius
  • outermost shell e- quantum shell
  • charge density/of cation - 2+ stronger than 1+)
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21
Q

Is a smaller ion more or less thermally stable? And why?

A

smaller = higher charge density/more polarising = less thermal stability

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22
Q

How do you know if a compound is more thermally stable than the other?

A

less decomposition = more thermally stable

23
Q

what is the procedure for flame tests?

A
  1. Nichrome wire
  2. dip in conc. HCl
  3. heat under blue bunsen flame
24
Q

what are 2 issues with flame tests?

A
  • colours are subjective
  • impurities can affect colour
25
Q

does reactivity increase or decrease down group 7? Why?

A

decrease
bcs they have more London Forces from increased e-s and protons
so more energy is needed to break stronger LFs

26
Q

What affects the electronegativity?

A
  • atomic radius
  • number of shells
27
Q

as electronegativity decreases, stability…..

A

increases

28
Q
A
29
Q

2HI + NaSO4 ->

A

NaHSO4 + HI (misty fumes)
Acid base reaction

30
Q

6 HI + H2SO4 ->

A

3 I2 + S + 4H2O
S is a yellow solid
Redox reaction

31
Q

8HI + H2SO4 ->

A

H2S + 4 I2 + 4H2O

H2S has egg smell

32
Q

CaCO3 (or decomposition of any G2 carbonates) ->

A

CaO + CO2

33
Q

What is the physical state of G1/G2 nitrates and carbonates?

A

White solid

34
Q

When brown fumes are observed after heating, what can i assume it is?

A

Nitrogen dioxide NO2

35
Q

G1 nitrates decomposition
2NaNO3(s) ->

A

2NaNO2(s) + O2 (g)

36
Q

G2 nitrate decomposition:
Be(NO3)2 (s) ->

A

BeO (s) + 2NO2 (g) + 1/2 O2 (g)

37
Q

What is the trend of G7 elements down?

A

Decreasing reactivity down
As Electronegativity decrease
Bp mp increase

38
Q

2Li (s) + Cl2 (g) ->

A

2LiCl (s)

39
Q

Ba (s) + Br2 (l) ->

A

BaBr2 (s) (white solid)

40
Q

Why are G7 ions more likely to displace those lower down the group?

A

Because they’re smaller, so incoming electron is more attracted by their protons
Smaller number of complete inner energy levels of e-, so less repulsion

41
Q

Cl2 (g) + H2O (l) ->

A

HCl (aq) + HOCl (aq)
Example of disproportionation

42
Q

What is chlorine used in water?

A

Disinfect for drinking purposes
By killing pathogens and water bourne diseases

43
Q

What is the reducing power trend down G7?

A

Increasing down
As more stabilising bcs it’s less polarising

44
Q

What is formed and their observations when sulfuric acid + sodium chloride?

A

Misty fumes
HCl formed

45
Q

What is formed and their observations when sulfuric acid + sodium bromide? (In a redox reaction)

A

Misty fumes (HBr) brown fumes (Br2)
Colourless with choking smell (SO2)

NaBr + H2SO4 → NaHSO4 + HBr

2HBr + H2SO4 → Br2 + SO2 + 2H2O

46
Q

What is formed and their observations when sulfuric acid + sodium iodide?

A

Misty fumes (HI)
Purple fumes/ black solid (iodine)
Sulfur dioxide (colourless, choking smell)
Sulfur (yellow solid)
Hydrofrm sulfide (H2S) (colourless gas with rotten egg smell)

47
Q

2 LiNO3 (decomposition)->

A

Li2O + NO2 + 3/2 O2

48
Q

NaNO3 ->

A

NaNO2 + 1/2 O2

Same for all other G1 metals except Li

49
Q

What does polarising mean?

A

ability of cation to pull the electron density of anion towards itself

50
Q

What’s the equation for chlorine reacting with cold dilute sodium hydroxide? And name the type of reaction. (2 marks)

A

Cl2 + 2OH- -> H2O + Cl- + ClO-
Disproportionation

51
Q

What’s the equation for chlorine reacting with cold dilute sodium hydroxide? And name the type of reaction. (2 marks)

A

Cl2 + 2OH- -> H2O + Cl- + ClO-
Disproportionation

52
Q

Are G1 or G2 hydroxides more soluble?

A

G1 are more soluble

53
Q

Which G2 metal does not react with water?

A

Beryllium

N Chemistry A Level (19 decks)

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