Group 7 - Halogens and Redox Flashcards

1
Q

Define oxidation and an oxidising agent

A

The process of electron loss

Accepts electrons (itself is reduced) allowing other substances to be oxidised

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2
Q

Define reduction and a reducing agent

A

The process of electron gain

Donates electrons (itself is oxidised) allowing other substances to be reduced

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3
Q

Diatomic and uncombined elements have oxidation states of ?

A

0

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4
Q

Combined oxygen has an oxidation state of?

A

-2

Unless with peroxides where it is -1

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5
Q

Combined hydrogen has an oxidation state of?

A

+1

Except metal hydrides where its -1

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6
Q

Combined fluorine always has an oxidation state of?

A

-1

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7
Q

Increasing oxidation state numbers signify?

A

Oxidation

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8
Q

Decreasing oxidation states indicate?

A

Reduction

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9
Q

Define electronegativity?

A

The power of an atom to withdraw electron density to itself in a covalent bond

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10
Q

Describe and explain the trend in electronegativity down group 7?

A

Decreases down the group

Atoms get larger down the group meaning the outer electrons are further from the nucleus. Increased shielding.
Weaker attraction between nucleus and outer electrons.

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11
Q

Describe and explain the trends in boiling points down G7

A

Melting and boiling points increase

Larger atoms have more electrons and therefore the VDW forces between molecules are stronger.

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12
Q

Colour and physical state of fluorine

A

Yellow
Gas

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13
Q

Colour and physical state of chlorine

A

Green
Gas

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14
Q

Colour and physical state of bromine

A

Red/brown
Liquid

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15
Q

Colour and physical state of iodine

A

Grey
Solid

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16
Q

Describe and explain the trend in oxidising ability of halogens down G7

A

Oxidising ability decreases

When halogens react they gain an electron so as the atoms become larger down the group. The force of attraction between the nucleus and outer electrons is weaker. Therefore, its harder for the halogen to gain an electrons and react.

Generally a halogen will displace a halide from solution if the halide is below it in the PT

17
Q

What is disproportionation?

A

When an element is both oxidised and reduced

18
Q

What are chlorate ions used for?

Pros and cons

A

Killing bacteria

Pros:
Kills pathogenic microorganisms
Prevents growth of algae which eliminates bad tastes and smells

Cons:
Chlorine gas irritates the respiratory system
Liquid chlorine can cause severe chemical burns
Can react with organic compounds in water to form carcinogenic chlorinated hydrocarbons

19
Q

Describe the trend in the reducing ability of halide ions down group 7

A

Reducing power increases

The larger the ion the more easily it can lose and electron as the outer electrons are further away from the nucleus and there is a greater shielding affect.

20
Q

How can the reactions of sodium halides with sulfuric acid reflect the reducing power of the halides?

A

Sodium chloride reacts with H2SO4 to form NaHSO4 and HCl gas.
This is not a redox reaction as the cl- is not a strong enough reducing agent to reduce the sulfur. (Oxidation state remains the same)

Sodium Bromide reacts with H2SO4 in 2 ways:
1. A similar acid base reaction to NaCl
2. -> SO2 + H2O + Br2 - Here the Br- ions are strong enough reducing agents to reduce the sulfuric acid to sulfur dioxide. Redox reaction

Sodium Iodide reacts with H2SO4 similarly as before in a acid base reaction but also can further reduce H2SO4 to H2S (smells of bad eggs)

21
Q

How do you test for Halide Ions?

A

Add dilute nitric acid to remove other ions.

Then add silver nitrate solution

F- = no ppt
Cl- = white ppt
Br- = cream ppt
I- = yellow ppt

To be extra sure you can test by adding ammonia solution.

Cl- ppt will dissolve in dilute ammonia
Br- ppt will dissolve in conc ammonia
I- ppt will not dissolve in **conc ammonia

22
Q

Reaction of chlorine with water?

And in sunlight?

A

Cl2(g) + 4H2O(l) ⇋ HClO(aq) + HCl(aq)

Disproportionation occurs

2Cl2(g) + 2H2O(l) -> 4HCl (aq) + O2(g)

23
Q

Reaction of chlorine and sodium hydroxide

What is the household name for the product?

A

Cl2(g) + 2NaOH(aq) -> NaClO(aq) + NaCl(aq) +H2O(l)

Disproportionation occurs