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1
Q

Definition of 1st I.E:

Definition of 2nd I.E:

A

1st I.E: The energy required to remove 1 mole of e⁻ from 1 mole of gaseous atoms to form 1 mole of gaseous 1⁺ ions.

2nd I.E: The energy required to remove 1 mole of e⁻ from 1 mole of gaseous 1⁺ ions to form 1 mole of gaseous 2⁺ ions.

2
Q

What is the trend in Ionisation.Energy across periods? And Why?

A

▪️ Increases

Because:

N.C ⬆️

Shielding remains SAME

A.R ⬇️

Therefore, more energy required to remove e⁻

3
Q

Why does I.E drop from Be to B?

A

🔘Borons e⁻ is in a higher energy 2p orbital.

🔘 This orbital is further away from the nucleus

🔘 Little more shielding from the 2s orbital

Therefore, less energy required to remove Borons e⁻

4
Q

Why does I.E drop from N to O?

A

Electron repulsion in 2p orbital between O & B

🔘 And Shielding remains SAME!!

Therefore, it is easier to remove O’s e⁻

5
Q

What is the trend in M.P/ B.P across periods 2 & 3?

A

Increases then Decreases

Because :

(Increases): Giant Metallic –> Giant Covalent

(Decreases): Giant Covalent –> Simple Covalent

6
Q

What are the complete elemental forms of :

N
P
O
S
F/Cl/Br/I
A
N₂
P₄
O₂     
S₈    
F₂ ⁄Cl₂ ⁄Br₂ ⁄I₂
7
Q

Name the 3 types of Inter.Molecular.Forces (IMF) that apply to covalent bonding only and arrange in order of weakest first.

A

Van der Waals
Dipole-Dipole
Hydrogen Bonding

8
Q
  1. Temporary D-D force applies to?
  2. Permanent D-D force applies to?
  3. H-bonding only occurs between H:???
A
  1. Non Polar molecules e.g Cl₂ ( Cl⁺➖Cl⁻)
  2. Polar molecules e.g. HBr (H⁺➖Br⁻)
  3. H⁺➖N⁻
    H⁺➖O⁻
    H⁺➖F⁻
9
Q

Which bonding has low or high M.P/B.P? :

Covalent (Simple)
Covalent (Giant)
Ionic (Giant)
Metallic (Giant)

A

Covalent (simple) =
Low M.P/B.P

Covalent (Giant)
Ionic (Giant) = High M.P/B.P
Metallic (Giant)

10
Q

Why is Group.2 called Alkaline Earth Metals?

A

As they form compounds which are alkaline.

11
Q

What is the trend of Atomic.Radius down Group.2?

A

Atomic Radius increases as metallic ions/elements get bigger down the group.

12
Q

What is the I.E trend down Group 2?

A

I.E decreases down the group as
A.R ⬆️
Shielding ⬆️
N.C ⬆️ : But it is outweighed by the other 2 factors. Due to Larger atoms

🔴 MORE REACTIVE!!!

13
Q

Why does Reactivity Increase down Group.2?

A

Due to elements losing 2 e⁻ which becomes easier down the group due to I.E decreasing.

Therefore Reactivity increases!

14
Q

What is the trend in M.P/B.P down Group 2?

A

M.P/B.P Decreases down Group 2 due to:

▪️ metallic ions getting bigger - A.R Increases

▪️ Smaller Charge/Volume ratio - meaning e⁻s are spread out further

Therefore, there is a reduced electrostatic attraction between the metallic ions and sea of delocalised e⁻s .
So it requires less energy to break the bonds.

15
Q

Ba(s) + 2H₂O →

A

Ba(OH)₂(aq) + H₂(g)

16
Q

Mg(s) + H₂O →

A

MgO(s) + H₂(g)

17
Q

2Be(s) + O₂(g) →

A

2BeO(s)

18
Q

Be(s) + Cl₂(g) →

A

BeCl₂(s)

19
Q

How do the solubilities of Group 2 deviate down the group?

🔹SO₄²⁻
♻️CO₃²⁻
♦️OH⁻

A

SO₄²⁻ Decrease down

CO₃²⁻ Decrease down

OH⁻ Increase down

E.g. BaSO₄ = Insoluble
BaCO₃ = Insoluble

    Ba(OH)₂ = Soluble
20
Q

Group 2 Oxides can act as bases:

🔸 MgO + H₂O → ?

🔹 MgO + 2HCl → ?

♦️ Mg(OH)₂ + 2HCl → ?

A

🔸 Mg²⁺ + 2OH⁻

🔹 MgCl₂ + H₂O

♦️MgCl₂ + 2H₂O

21
Q

A strict test for group 2 SO₄²⁻ ?

A

Add HCl + BaCl₂ =

ppt forms

22
Q

Why do we add HCl to BaCl₂?

A

The acidic HCl removes any impurities and Carbonates (CO₃²⁻) that lurk around in (aq) preventing them from reacting with BaCl₂ to form other ppt which is not a true test for sulphates. !

23
Q

What are the uses for:

🔘Ca(OH)₂
🔘Mg(OH)₂
🔘BaSO₄
🔘MgSO₄

                             ?
A

✔️Ca(OH)₂ = Neutralise acidic soil

✔️Mg(OH)₂ = Indigestion remedies

✔️BaSO₄ = ‘Barium Meals’… X-Ray

✔️MgSO₄ = Epsom Salts/Mild Laxative

24
Q

Properties of Halogens-
What are + the standard states of:

🔸Fluorine ?
Chlorine ?
Bromine ?
Iodine ?

A

F₂ (g) : Pale yellow gas
Cl₂ (g) : Green gas
Br₂ (l) : Red / Brown liquid
I₂ (s) : Dark Grey solid / Purple Fumes

25
Q

What is the trend in Atomic Radius / Ionic Radius down Group 7?

A

Increases

Due to more Shielding

26
Q

What is the trend in M.P/B.P down Group 7?

A

Increases

Due to larger atoms
Which means more e⁻s
So more van der Waals between molecules which becomes stronger!

27
Q

What is the trend in Electronegativity down Group 7? And Why?

A

Decreases

▪️larger atoms : bonding e⁻s further away from nucleus

▪️More shielding between nucleus & bonding e⁻s

These 2 factors outweigh Increased N.C due to more protons.

↪️ Less attraction bet. Nucleus & bonding e⁻s.

28
Q

What is an :

Oxidising agent ?

Reducing agent ?

A

Oxidising agent =
e⁻ gainer

Reducing agent =
e⁻ loser (donor)

29
Q

Down Group 7, Reducing agents get (worse/better) and Reduce H₂SO₄ (more/less).

A

✔️Better

✔️More

30
Q

Test for halide ions -
Reactions w/ H₂SO₄:

Name the 4 reducing products of H₂SO₄ in order

A
  1. NaHSO₄
  2. SO₂
  3. S
  4. H₂S
31
Q

🅰️ NaCl/NaBr/NaI + H₂SO₄ →

A

NaHSO₄ + HCl/HBr/HI⤵️ (White Misty Fumes)

32
Q

🅱️ 2Br⁻ + H₂SO₄ + 2H⁺ →

A

Br₂ + SO₂ + 2H₂O

33
Q

© 6I⁻ + H₂SO₄ + 6H⁺ →

A

3I₂ + S + 4H₂O

34
Q

D) 8I⁻ + H₂SO₄ + 8H⁺ →

A

4I₂ + H₂S + 4H₂O

35
Q

Test for halide ions-
Using Silver Nitrate:

What do we add first before adding Acidified AgNO₃? And why?

A

🔹Add Dil. HNO₃

Because: it removes any soluble carbonates (CO₃²⁻) and hydroxides (OH⁻) –> these have the potential to react with AgNO₃ to form insoluble Ag₂CO₃ & AgOH… mixing all these ppt’s = DISASTER!!!!

36
Q
  1. AgNO₃ + F⁻ →
  2. AgNO₃ + Cl⁻ →
  3. AgNO₃ + Br⁻ →
  4. AgNO₃ + I⁻ →
A
  1. NO ppt!(as F⁻ is soluble)
  2. AgCl[White ppt] + NO₃⁻
  3. AgBr[Cream ppt] + NO₃⁻
  4. AgI [Yellow ppt] + NO₃⁻
37
Q

Which ppt dissolves in Dilute NH₃?

Cl⁻ or Br⁻ or I⁻

A

Cl⁻

38
Q

Adding Conc. NH₃ to the remaining ppt’s dissolves which halide?

Br⁻ or I⁻

A

Br⁻

39
Q

Halogen Disproportionation Reactions:

Cl₂ + H₂O ⇌

A

HClO + HCl

40
Q

In Sunlight:

2Cl₂ + 2H₂O →

A

4HCl + O₂

41
Q

Chlorination of pools:
NaClO(s) + H₂O →

Reaction w/ NaOH:
Cl₂ + 2NaOH →

A

HClO + Na⁺ + OH⁻

NaClO + NaCl + H₂O

42
Q

Disproportionation definition :

A

When a species is being oxidised and reduced at the same time in the same reaction

43
Q

Period 3 - The Elements

Na = 
Structure = 
---------------------
Mg = 
Structure = 
---------------------
Al = 
Structure = 
---------------------
Si = 
Structure = 
---------------------
P₄ = 
Structure =
---------------------
S₈ =
Structure = 
---------------------
Cl₂ = 
Structure = 
---------------------
Ar = 
Structure =
A
Na = soft METAL
Bond = Giant Metallic
---------------------
Mg = silver coloured METAL
Structure = Giant Metallic
---------------------
Al = silver coloured METAL
Structure = Giant Metallic
---------------------
Si = shiny solid NON-METAL
Structure = Giant Covalent
---------------------
P₄ = Red/White solid NON-METAL
Structure = Simple Covalent
---------------------
S₈ = Yellow Solid NON-METAL
Structure = Simple Covalent
---------------------
Cl₂ = Green gas NON-METAL
Structure = Simple Covalent
---------------------
Ar = colourless gas NON-METAL
Mono-Atomic
44
Q

Why is chlorine useful?

A

🔻Kill bacteria in water

🔻Used to make bleach (NaClO)

45
Q

How reactive is Na with water?

2Na + 2H₂O(l) →

What is the pH of the product formed?

A

Vigorous

2NaOH(aq) + H₂(g)

pH 13-14 Alkaline

46
Q

How reactive is Mg with water?

Mg + 2H₂O(l) →

What is the pH of the product formed?

A

Slow w/ cold water

Mg(OH)₂(aq) + H₂(g)

pH 10 Alkaline

47
Q

How reactive is Mg with steam?

Mg + H₂O(g) →

What is the pH of the product formed?

A

Faster w/ heat + steam

MgO(s) + H₂(g)

pH 9 Slightly Alkaline

48
Q

How does Cl react with water?

Cl₂(g) + H₂O(l) →

What is the pH of the product formed?

A

Dissolves

HClO(aq) + HCl(aq)

pH 1-2 Acid

49
Q

Period 3 reactions w/ Oxygen:

Na : Colour?
▪️2Na + ½O₂ → 
-----------------------
Mg : Colour? 
▪️Mg + ½O₂ → 
-----------------------
Al : Colour? 
▪️2Al + 1½O₂ → 
-----------------------
▪️Si + O₂ → 
-----------------------
P : Colour? 
▪️Bright White Flame
-----------------------
S : Colour? 
▪️S + O₂ →        
🔹SO₂ + ½O₂ →
A
Na - Yellow Flame 
Na₂O
-----------------------
Mg - Bright White Flame
MgO 
-----------------------
Al - Bright White Flame 
▪️Al₂O₃ (slow)
-----------------------
▪️SiO₂ (slow)
-----------------------
P - Bright White Flame
▪️P₄O₁₀
-----------------------
S - Blue Flame
▪️SO₂
🔹SO₃
50
Q

Period 3 Oxides:

Na₂O : Structure
MgO : Structure
Al₂O₃ : Structure

SiO₂ : Structure

P₄O₁₀ : Structure
SO₂ : Structure

A

Na₂O : Giant Metallic
MgO : Giant Metallic
Al₂O₃ : Giant Metallic

SiO₂ : Giant Covalent

P₄O₁₀ : Simple Covalent
SO₂ : Simple Covalent

51
Q

Na₂O : (Soluble/Insoluble)
🔸 Na₂O + H₂O → pH?

MgO : (Soluble/Insoluble)
🔸MgO + H₂O → pH?

Al₂O₃ : (Soluble/Insoluble)
🔸
SiO₂ : (Soluble/Insoluble)
🔸

P₄O₁₀ : (Soluble/Insoluble)
🔸P₄O₁₀ + 6H₂O → pH?

SO₂ : (SolubleInsoluble)
🔸 SO₂ + H₂O → pH?

SO₃ : (SolubleInsoluble)
🔸SO₃ + H₂O → pH?

A

Na₂O : (Soluble/Insoluble)
🔸 2NaOH -> pH = 14

MgO : (Soluble/Insoluble)
🔸 Mg(OH)₂ -> pH = 10

🔺Al₂O₃ :
🔴Insoluble in H₂O
🔻SiO₂ :

P₄O₁₀ : (Soluble/Insoluble)
🔸4H₃PO₄ -> pH = 0-2

SO₂ : (SolubleInsoluble)
🔸H₂SO₃ -> pH = 0-2

SO₃ : (SolubleInsoluble)
🔸H₂SO₄ -> pH= 0-2

52
Q

Definition : Amphoteric

A

Where a compound (especially a metal oxide/hydroxide) able to react both as a base and acid

53
Q

Neutralisation of period 3 Oxides:

Identify which oxides are Basic/ Amphoteric/ Acidic :

Na₂O 
MgO  
Al₂O₃  
SiO₂    
P₄O₁₀  
SO₂
A

🔵Basic Oxides ;

 1. Na₂O 
 2. MgO  

☯️Amphoteric Oxides ;
Al₂O₃

🔴Acidic Oxides ;

  1. SiO₂    
  2. P₄O₁₀
  3. SO₂
  4. SO₃
54
Q

🔵Basic Oxides ;

  1. Na₂O + H₂SO₄ →
  2. MgO + 2HCl →
A
  1. Na₂SO₄ + H₂O

2. MgCl₂ + H₂O

55
Q

☯️Amphoteric Oxides

Al₂O₃ [Acting as a Base] :
Al₂O₃ + 6HCl →

Al₂O₃ [Acting as an Acid] :
Al₂O₃ + 2NaOH + 3H₂O →

A

[Base] : 2AlCl₃ + 3H₂O

[Acid] : 2NaAl(OH)₄

         ⬇️(Notice NO Water is            
                                            produced!)
56
Q

🅰️cidic Oxides ;

  1. SiO₂ + 2NaOH →
  2. P₄O₁₀+ 12NaOH →
  3. SO₂ + 2NaOH →
    3b. + NaOH →
  4. SO₃ + 2NaOH →
A
  1. Na₂SiO₃ + H₂O
  2. 4Na₃PO₄ + 6H₂O
  3. Na₂SO₃ + H₂O
    3b. NaHSO₃
  4. Na₂SO₄ + H₂O
57
Q

Write the simplified electronic configuration for
➖Cr

➖Cu

A

Cr = [Ar] 4s¹ 3d⁵

Cu = [Ar] 4s¹ 3d¹⁰

58
Q

Write the simplified electronic configuration for

Mn

ℹ️ Mn²⁺

A

Mn = [Ar] 4s² 3d⁵

ℹ️ Mn²⁺ = [Ar] 3d⁵

59
Q

What is a Complex?

A

A molecule with a T.M ion in the middle with ligands dative covalently bonded to them

                        🙂
60
Q

What is a Ligand?

A

Molecule,Atom or ion that donates a pair of electrons to a central metal ion.

61
Q

What is a coordination number?

A

Number of Coordinate bonds

65
Q

Intro to Transition Metals -

There is a difference between D-BLOCK and TRANSITION METALS!

Define Transition Metals :

Define D-BLOCK elements :

A

T.M = elements which form STABLE IONS that have a PARTIALLY FILLED d-oribital.

D-Block = Elements that has its OUTER MOST ELECTRONS in the d-orbital

66
Q

Which 2 elements from the D-Block are not Transition.Metals?

A

Sc and Zn

67
Q

Energy absorbed can be calculated using: ?

A

∆E= hv

Energy = Planck’s Const. x frequency

68
Q

Types Of Ligands:-

Monodentate: 1 L.P
Small :
Large :

Bidentate: 2 L.P
1.
2.
3.

Multidentate:

A

[Monodentate]:
Small = H₂O₎ NH₃/OH⁻₎ CN⁻

Large = Cl⁻

[Bidentate]:

  1. Ethanedioate
  2. (en) / ethane 1,2-diamine
  3. Benzene 1,2-diol

[Multidentate]:
EDTA⁴⁻ - CHELATE EFFECT
(Haem)- found in red blood cells

69
Q

Coloured Ions -

🌗 Ligands…?… d-orbitals

Features that cause change in ∆E...
〰
〰
〰
〰
A

Ligands SPLIT d-orbitals!

〰Type of Metal
〰Type of Ligand
〰Oxidation State
〰Co-Ordination No.

70
Q

💠 Colour depends on….?

A

💠Colour depends on energy gap ∆E -> which depends on oxidation state

71
Q
OxidationNo.|Species|Col.
                      |              |
5️⃣                 |              |    
--------------------------
                      |              |
4️⃣                 |              |
-------------------------------
                      |              |
3️⃣                 |              |
-------------------------------
                      |              |
2️⃣                 |              |
A

V²⁺

OxidationNo.|Species|Col.
                      |              |
5️⃣                 |   VO₂⁺   | YELLOW🔸
--------------------------
                      |              |
4️⃣                 |  VO ²⁺   | BLUE 🔹
-------------------------------
                      |              |
3️⃣                 |  V³⁺      | GREEN💚
-------------------------------
                      |              |
2️⃣                 |              |
72
Q

Why are Transition Metal Ions Coloured?

©
©
©

A

At a certain frequency:
© e⁻ move from ground state to excited state
© Light is absorbed
© Different colour of light is transmitted

73
Q

When drawing Metal Complex Shapes, remember to:?

A

Use Dative Covalent Bonds pointing to the Central Metal Atom/[Ion]

74
Q

Complexes can show …?

A

Optical Isomerism too!

75
Q
OxidationNo.|Species|Col
5️⃣                 |              |
--------------------------
4️⃣                 |              | 
--------------------------
3️⃣                 |              |    
--------------------------
2️⃣                 |              |
A
OxidationNo.|Species|Col
5️⃣                 |  VO₂⁺   | 💛
--------------------------
4️⃣                 |  VO ²⁺  | 💙
--------------------------
3️⃣                 |      V³⁺  | 💚
--------------------------
2️⃣                 |      V²⁺ |  💜
76
Q

🐈alysis :-

Define Homogenous catalysts..

What do you form with homogenous catalysts only, during a reaction?

A

Homo. Cat. = Same phase as reactants

An INTERMEDIATE is formed in between!

77
Q

What homogenous catalyst is used in the reaction between

S₂O₈²⁻ + I⁻ ?

A

Catalyst = Fe²⁺

78
Q

Complete the equations:

  1. S₂O₈²⁻ + 2Fe²⁺ →
  2. 2Fe³⁺ + 2I⁻ →

Overall: S₂O₈²⁻ + 2I⁻ → 2SO₄²⁻ + I₂
[N.B. -The Catalyst not incl. in ionic eq]

A
  1. 2SO₄²⁻ + 2Fe³⁺

2. I₂ + 2Fe²⁺

79
Q

Define Heterogeneous Catalysts..

Name the 3 processes that use heterogeneous catalysts and name the catalysts used for each process.

A

Hetero. Cat = Different phase to reactants

🌐 Haber Process (NH₃)
- Cat. Fe(s)

🌐 Contact Process (H₂SO₄)
- Cat. V₂O₅(s)

🌐 Methanol Process
- Cat. Cr₂O₃(s)

80
Q

Haber Process:

N₂ + 3H₂ →

A

2NH₃

81
Q

Contact Process:

  1. V₂O₅ + SO₂ →
  2. V₂O₄ + ½O₂ →
        SO₃ + H₂O → H₂SO₄
A
  1. V₂O₄ + SO₃

2. V₂O₅

82
Q

Methanol Process:

CO + 2H₂ →

A

CH₃OH

83
Q

Define Autocatalysis..

  1. 2MnO₄⁻ + 5C₂O₄²⁻ + 16H⁺→
  2. 4Mn²⁺ + MnO₄⁻ + 8H⁺→
  3. 2Mn³⁺ + C₂O₄²⁻ →
A

When a PRODUCT catalyses the reaction

  1. 2Mn²⁺ + 10CO₂ + 8H₂O
  2. 5Mn³⁺ + 4H₂O
  3. 2Mn²⁺ + 2CO₂
84
Q

Redox Titrations -

  1. ?
  2. ?
  3. Calculate MOLES of chemical in burette
  4. Calculate MOLES of chemical in flask (25cm³)
  5. Work out MOLES in original soln
  6. Work out Mass/Conc. of ORIGINAL sample …… M= molxMr | C = n/v
A
  1. Write out 2 ½ equations

2. Combine to work out full IONIC EQUATION

85
Q

[Cu(H₂O)₆]²⁺ + 2OH⁻ →

A

[Cu(H₂O)₄(OH)₂] + 2H₂O

86
Q

[Cu(H₂O)₄(OH)₂] + 2NH₃ →

A

[Cu(H₂O)₄(OH)₂] + NH₄⁺

87
Q

[Cu(H₂O)₄(OH)₂] + 4NH₃ →

A

[Cu(H₂O)₂(NH₃)₄]²⁺ + 2OH⁻ + 2H₂O

88
Q

[Cu(H₂O)₆]²⁺ + CO₃²⁻

A

CuCO₃ + 6H₂O

89
Q

[Cu(H₂O)₆]²⁺ + 4HCl →

What colour solution is formed?

A

[CuCl]²⁻ + 6H₂O

Yellow Soln

90
Q

[Fe(H₂O)₆]²⁺ + 2OH⁻ →

A

[Fe(H₂O)₄(OH)₂] + 2H₂O

91
Q

[Fe(H₂O)₆]²⁺ + 2NH₃ →

A

[Fe(H₂O)₄(OH)₂] + 2NH₄⁺

92
Q

[Fe(H₂O)₆]²⁺ + CO₃²⁻ →

A

FeCO₃ + 6H₂O

93
Q

[Fe(H₂O)₆]³⁺ +3OH⁻ →

A

[Fe(H₂O)₃(OH)₃] + 3H₂O

94
Q

[Fe(H₂O)₆]³⁺ + 3NH₃ →

A

[Fe(H₂O)₃(OH)₃] + 3NH₄⁺

95
Q

2[Fe(H₂O)₆]³⁺ + 3CO₃²⁻ →

A

2[Fe(H₂O)₃(OH)₃] + 3CO₂ + 3H₂O

96
Q

[Fe(H₂O)₆]³⁺+ 4Cl⁻ →

What colour solution is formed?

A

[FeCl]⁻ + 6H₂O

Yellow Soln

97
Q

[Al(H₂O)₆]³⁺ + 3OH⁻ →

A

[Al(H₂O)₃(OH)₃] +3H₂O

98
Q

[Al(H₂O)₆]³⁺ + 3NH₃ →

A

[Al(H₂O)₃(OH)₃] + 3NH₄⁺

99
Q

[Al(H₂O)₆]³⁺ + 4OH⁻ →

A

[Al(H₂O)₂(OH)₄]⁻ + 4H₂O

100
Q

2[Al(H₂O)₆]³⁺ + 3CO₃²⁻ →

A

2[Al(H₂O)₃(OH)₃] +3CO₂ + 3H₂O