Reducing & Oxidising Agents - Redox (5.5) Flashcards
What does an oxidising agent do?
It allows another species to lose electrons and gains the electrons and is reduced itself.
Give two examples of oxidising agent.
Potassium manganate and Potassium dichromate.
What does a reducing agent do?
It allows another species to gain electrons and provides the electrons itself, so is therefore oxidised.
Give two examples of reducing agents.
Sodium Borohydride and Lithium Hydride
The terms “oxidising agent” and “reducing agent” are absolute. True or False.
False - they are not absolute, as they act in one reaction but not in another.
Down group 1 and 2, what happens to reactivity?
It increases down the groups. (atomic radius, sheilding and electrostatic attraction).
In groups 6 and 7, what happens to reactivity?
It increases up the groups. (atomic radius, sheilding and electrostatic attraction).
Elements in groups 1 and 2 react to form positive ions. True or False?
True - they are oxidised (lose an electron)
Why does it become easier to lose an electron down groups 1 and 2?
This is due to larger radiuses and therefore increased shielding and reduced electrostatic attraction between the nucleus and outer electron (valence)
Reducing power generally increases down groups 1 and 2. True or False?
True - due to it being easy to lose an electron.
Elements in group 16 and 17 react to form positive ions. True or False?
False - they form negative ions and are reduced (gain an electron).
Why does it become harder to gain an electron as you go down groups 16 and 17?
There are larger radiuses, increased shielding, and reduced electrostatic attraction between nucleus and incoming electron.
Does oxidising power generally decrease down groups 16 and 17?
Yes, it does. ( you’re right ;))
