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Chemistry > Inorganic chemistry and the Periodic Table > Flashcards

Inorganic chemistry and the Periodic Table Flashcards

1
Q

What is the trend in ionisation energy for group 2?

A

Decreasing

As you descend Group 2, there are more shells of electrons, so the outer shell electron being removed is further from the nucleus + more shielded (this outweighs the increase in nuclear charge). Therefore attraction to the nucleus decreases

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1
Q

What is the trend in atomic radius in group 2 (and 1)?

A

Increasing

More shells of electrons + more shielding so electron are further away from nucleus + less tightly held therefore atom gets bigger

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2
Q

What is the trend in reactivity in group 2 (and group1)?

A

Reactivity increases/gets more vigorous
As you go down the group, the number of shells of electrons increases

  • So the outer electron being lost is further from the nucleus and more shielded (this outweighs the increased nuclear charge)
  • Therefore, the electron is more easily lost and the element is more reactive
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3
Q

What are the trends in solubility of hydroxides and sulphates for group 2?

A

Hydroxides - more soluble down the group
Sulfates - less soluble down the group

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4
Q

What is the trend in thermal stability of nitrates and carbonates?

A

As you go down group 2, the thermal stability increase
- The size of the cation increases
- So polarises the anion less

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5
Q

What is the trend in group 1 for nitrates and carbonates?

A

All group 1 nitrates decompose when strongly heated

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6
Q

What does lithium nitrate decompose to form? Why?

A

4LiNO3 → 2Li2O + 4NO2 + O2
Lithium is so strongly polarising that it causes the nitrate ion to break down

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7
Q

Why do the other group 1 nitrates melt rather than fully decompose?

A

2NaNO3 → 2NaNO2 + O2
This is because the other group 1 cations have a lower charge density so are not as strongly polarising

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8
Q

Why does only lithium carbonate decompose?

A

Li2CO3 → Li2O + CO2
Lithium is so strongly polarising that it causes the carbonate ion to break down. However other Group 1 carbonates will not decompose when heated, as the cations are not strongly polarising enough

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9
Q

What is the reaction of Group 2 metals with chlorine:

A

Metal + chlorine → metal chloride (salt)

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10
Q

What is the reaction of Group 2 metals with water:

A

Metal + water → metal hydroxide + hydrogen

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11
Q

What is the reaction of Group 2 metal oxides with water:

A

Metal oxide + water → metal hydroxide

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12
Q

What is the reaction of Group 2 metal oxides with acids:

A

Metal oxide + acid → metal salt + water

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13
Q

What is the reaction of Group 2 hydroxides with acids:

A

Metal hydroxide + acid → metal salt + water

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14
Q

Describe the method for a flame test:

A
  1. Clean a platinum or nichrome wire by heating it in a non-luminous Bunsen burner flame, dipping it into a little concentrated hydrochloric acid on a watch glass and heating it again. Continue this until the wire produces little or no colour in the flame
  2. Dip the clean wire into the acid and then into a small portion of powdered compound on a watch glass.
  3. Hold the wire so that the powdered solid is in the edge of the flame and note any colour change
  4. Observe the flame through a diffraction grating or direct vision spectroscope
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15
Q

What are the different colour of flames:

A

Calcium - Orange
Magnesium - no colour
Lithium - Crimson Red
Barium - apple green
Sodium - Yellow
Potassium - lilac

16
Q

What are the origins of colour in the flame test?

A
  • Energy provided by the flame allows an electron to be ‘excited’
  • This configuration is unstable, so the electron will return to its original energy level (relaxation)
  • Extra energy will then be emitted in the form of light
  • The difference in energy between the different electron shells determines the wavelength and therefore colour of the light emitted
17
Q

Why do some elements not have colour?

A
  • The energy provided is not sufficient to excite an outer shell electron between energy levels
  • The light emitted might have a wavelength which is not in the visible range of light
18
Q

Why do some elements not have colour?

A
  • The energy provided is not sufficient to excite an outer shell electron between energy levels
  • The light emitted might have a wavelength which is not in the visible range of light
19
Q

What are the appearances for the different halogens:

A

Chlorine - pale yellow gas
Bromine - reddish brown liquid
Iodine - grey solid/purple vapour

20
Q

What is the trend for the boiling points?

A

Down the group - boiling point increases

The London forces between the molecules of the halogen get stronger as there are more electrons/a bigger Mr. So it takes more energy to overcome them

21
Q

Explain the trend for reactivity of halogens:

A

Reactivity decreases
- Down the group, more shells of electrons therefore shielding + distance from the nucleus increase
- This outweighs the increases nuclear charge
- Therefore there is a weaker attraction of outer electron to the nucleus - so harder to gain an electron

22
Q

What is the trend for electronegativity of halogens?

A

Down the group, electronegativity decreases (harder to attract an electron)
- Distance from nucleus increases (more shells of electrons)
- Shielding increases
- These 2 factors outweigh the increased nuclear charge
- So the attraction to the nucleus is weaker

23
Q

Why is iodine a better reducing agent than bromine?

A

Iodine reduces the sulphur the furthest, so it is the best reducing agent/has the most reducing power

24
Q

What is the test for sulphate ions:

A

Add acidified barium chloride
Result = white ppt forms
(HCl added first will remove any OH- or CO32- ions that would also give a white ppt)

25
Q

What is the test for halide ions:

A

Add acidified silver nitrate
Result = Cl- = white ppt, Br- = cream ppt, I- = yellow ppt
The precipitates form because silver halides are insoluble

26
Q

Test for carbonate ions:

A

Result = effervescence (of CO2), limewater turns cloudy

27
Q

What happens when chlorine reacts with water:

A

Cl2 + H2O -> HCl + HOCl
Disproportionation

28
Q

What happens when chlorine react with cold dilute sodium hydroxide?

A

Cl2 + 2NaOH -> NaCl + NaOCl + H2O
Disproportionation

29
Q

What happens when chlorine react with hot concentrated alkali?

A

3Cl2 + 6NaOH -> NaClO3 + 5NaCl + 3H2O
Disproportionation

30
Q

What happens when hydrogen halides react with ammonia?

A

HCl + NH3 -> NH4Cl

31
Q

What happens when hydrogen halides react with water?

A

HBr + H2O -> H3O+ + Br-

32
Q

What happens when solid KCl react with concentrated sulphuric acid?

A

KCl + H2SO4 -> HCl + KHSO4
No further reaction occurs

33
Q

What happens when solid KBr halide react with concentrated sulphuric acid?

A

KBr + H2SO4 -> HBr + KHSO4
2HBr + H2SO4 -> Br2 + SO2 + 2H2O

Chemistry (22 decks)

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