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Edexcel Chemistry A level > Inorganic chemistry and periodic table > Flashcards

Inorganic chemistry and periodic table Flashcards

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1
Q

How does atomic radius change across group 2?

A

increases due to more shells of electrons.

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2
Q

How does melting point change down group 2?

A

melting point decreases

due to metallic bonding becoming weaker

reducing the electrostatic attraction between cations and delocalised electrons

due to the metal ions and delocalised electrons having a greater distance from each other.

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3
Q

How does 1st ionisation energy change across group 2?

A

decreases

Because atomic radius increases due to more shells

increased shielding.

so more repulsive force of inner shells.

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4
Q

How does reactivity of group 2 change down the group?

A

increases down the group.
because more shielding
more repulsive force by inner electrons
so easier to form cation.

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5
Q

how do group 2 metals react with oxygen?

A
  • will burn in oxygen, with Mg forming a bright white flame
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6
Q

what can be used to clean off the MgO before using in an experiment?

A

emery paper

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7
Q

give the balanced symbol equation for Mg and O

A

2Mg + O2 —-> 2MgO

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8
Q

How does Mg react with chlorine? give the equation

A

Mg + Cl2—-> MgCl2

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9
Q

How does Mg react with steam?

A

forms MgO + H2 by reacting with steam.

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10
Q

How does Mg react with warm water?

A

Forms Mg(OH) 2 + H2 through a much slower reaction

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11
Q

what pH would you expect a concentrated solution of Mg(OH)2 to be?

A

10-14

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12
Q

what would be OBSERVED when group 2 metals react with water? what is the case with calcium?

A
  • fizzing
  • metal dissolves
  • the solution heats up
  • calcium forms a white precipitate
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13
Q

How does the solubility of the hydroxides change down group 2?

A
  • increases in solubility
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14
Q

what happens to group 2 solids that are not soluble?

A

they appear as white precipitates

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15
Q

how to group 2 ionic oxides react with water?

A

form hydroxides

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16
Q

why are ionic oxides basic?

A

oxide ions accept protons to become hydroxide ions.

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17
Q

order these from most to least soluble:
Mg(OH)2
Ca(OH)2
Ba(OH)2

A

Ba(OH)2
Ca(OH)2
Mg(OH)2

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18
Q

give a use of Mg(OH)2

A

used to neutralise excess acid in the stomach to treat constipation.

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19
Q

Give uses for Ca(OH)2

A

used to neutralise acidic soils in agriculture

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20
Q

rate from most to least alkaline:
Mg(OH)2
Ca(OH)2
Ba(OH)2

A

Ba(OH)2
Ca(OH)2
Mg(OH)2

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21
Q

How does the solubility of sulfates change in group 2?

A
  • decreases
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22
Q

Explain the reaction between Ba and sulfuric acid

A

will form BaSO4 and H
reaction is slow as BaSO4 that is produced is insoluble and will only act as a barrier from further reacting.

23
Q

define thermal decomposition

A

The use of heat to break down a reactant into more than 1 product.

24
Q

How to group 2 carbonates thermally decompose?

A

Form group 2 oxides and CO2

25
Q

How does thermal stability change down group 2?

A

Becomes increasingly thermally stable.
Cations get bigger
have less of a polarising effect
distort the carbonate ion less
so less easily breaks down.
So stronger C-O bond

26
Q

How do group 1 carbonates thermally decompose?

A

do not decompose except Li.
Because they only form a 1+ charge and dont have a big enough charge to polarise the carbonate ion.

Li can because it’s ionic radius is small enough to have the polarising effect.

27
Q

outline an experiment that can be done to investigate the ease of decomposition.

A

heat known mass of carbonate in a side arm boiling tube, passing the gas through a bung and tube to limewater.

repeat with diff carbonates and same volume of limewater and same distance from bunsen burner flame.

28
Q

what is produced when group 2 Nitrates decompose?

A

NO2
Metal oxide
Oxygen

29
Q

Why do Nitrates become more stable down the group?

A

Nitrate ion has large electron cloud that can be distorted.

so since atomic radius increases down the group, charge is spread over a larger area

So the less distortion, the more stable it is since charge densities balance each other out.

30
Q

describe the method to carry out a flame test

A
  • use a nichrome wire
  • clean the nichrome wire with HCL to prevent any contamination from other metals that may mask colours
  • heat wire in bunsen burner flame
  • grind up sample
  • dip wire in it and test.
31
Q

Give the colours of the following metals:
- Lithium
- Rubidium
- Sodium
- Caesium
- Magnesium
- Strontium
- Barium
- Potassium
- Calcium

A
  • Scarlett red
  • red
  • yellow
  • blue
  • no colour (not in visible light spectra so will see orange flame)
  • red
  • apple green
  • lilac
  • brick red
32
Q

explain the occurence of flame colours

A
  • heat from the flame causes electrons to move to a higher energy level
  • since it is instable at a higher energy level, it drops down.
  • The energy emitted from this is in the form of wavelength- which if part of the visible light spectrum, can be seen.
33
Q

what is the trend in melting and boiling point for halogens? Explain

A
  • increase down the group
  • Because atomic radius increases, so have more electrons
  • meaning they have larger London forces between molecules, so more energy needed to break them.
34
Q

What is the trend in electronegativity down the group? Why?

A

Decreases
Because more electrons= larger atomic radius, so nucleus and bonding pairs attraction would be lower.

35
Q

What is the trend of reactivity down group 7? Why?

A

Decreases
Because larger atomic radius
less shielding
so attracting an electron becomes harder, so harder to form 1- ions

36
Q

how does oxidising power change down group 7?

A
  • decreases down the group
  • since harder to accept an electron
  • due to more electron shells.
  • so less attraction between nucleus and electrons
37
Q

Which ion will displace bromide and iodide.

A

chloride

38
Q

which ion will displace only iodide ions?

A

Bromide

39
Q

what is observed when potassium chloride and the following react together:

  • Chlorine
  • Bromine
  • Iodine
A
  • very pale green solution- no reaction
  • yellow solution- no reaction
  • Brown solution- no reaction
40
Q

What is observed when Potassium bromide reacts with the halides?

A

Chlorine: Chlorine displaces Bromine, so yellow solution is formed.

Bromide: No reaction, yellow solution

Iodide: brown solution no solution

41
Q

What is observed when Potassium iodide reacts with the halides?

A

Chloride: chlorine displaces, Brown solution.
Iodide: no reaction, brown
Bromide: Bromine displaces, brown solution forms.

42
Q

what colours are seen on the top layer when an organic solvent is added to the halogens?

A

Chlorine: colourless
Bromine: yellow
Iodide: purple

43
Q

What observations will be made when an organic solvent like hexane is added to the oxidation reactions of the halides?

A

Every reaction the same, except all iodide reactions will be purple except chlorine and iodine (potassium halides) as it displaces iodine.

44
Q

define disproportion reaction

A

When an element is being simultaneously oxidised and reduced.

45
Q

state the balanced equation for the reaction of chlorine with water.

A

Cl2 + H2O —> HClO + HCl

46
Q

If universal indicator is added to the solution of chlorine and water, what will be observed?

A
  • would turn red due to its acidic pH
  • then would be turn colourless due to HClO bleaching the solution.
47
Q

What are the reactions of halides with cold NaOH

What are the reactions of halides with warm NaOH

use Cl as an example

A
  • NaCl
  • HClO
  • H20

With warm:
Same products except forms NaClO3

48
Q

What is the balanced equation for NaF and H2SO4?
What are the observations?

A

NaF + H2SO$—> NaHSO4 + HF
white steamy fumes are produced of HF.

49
Q

What is the balanced equation of NaCl and H2SO4? What is observed?

A
  • NaCl + H2SO4 —-> HCl + NaHSO4

White steamy fumes of HCl seen.

50
Q

How do you test for sulfate ions

A

HCl ad Barium Chloride, forms a white ppt

51
Q

How to test for OH ions

A
  • Litmus paper will turn from red to blue as it’s an alkali, but need further tests like spectroscopy to confirm they are actually present.
52
Q

How to test for halide ions?

A
  • Nitric acid, then Silver nitrate
  • Cl forms white pp
  • I forms a yellow ppt
  • Br forms a cream ppt

Further tests- add dilute NH4- which will only redissolve Cl

Conc NH4 will redissolve Br but not I

53
Q

How to test for Carbonate ions?

A

add HCL or any dilute acid
CO2 would be produced- test with limewater.
Should turn cloudy.

54
Q

Sr, Li and Rb nitrates are all white solids. Explain how you would identify each apart from ppt reactions and decomposition reactions. No practical details are required.

A
  • On decomposition, Li and Sr would produce a brown coloured gas
  • but RbNO3 would not
  • Dissolving each in distilled water, making a solution, adding NaOH
  • a white ppt would be seen only for Sr2NO3
  • but nothing seen for LiNO3 and RbNO3

Edexcel Chemistry A level (18 decks)

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