Redox Reactions Lecture Notes

These flashcards cover key concepts, definitions, and principles related to redox reactions, including oxidation states, the Daniell cell, and the Nernst equation.

What is the definition of oxidation numbers in redox reactions?

Oxidation numbers indicate the charge an atom would have in a compound if it were ionic.

What is the oxidation state of fluorine in compounds?

Fluorine always has an oxidation state of -1 in compounds except for those involving F2.

What determines the oxidation state of hydrogen?

Hydrogen usually has an oxidation state of +1, except in hydrides where it is -1.

What is the typical oxidation state of oxygen in compounds?

Oxygen typically has an oxidation state of -2, except in peroxides and fluorine compounds.

What is the difference between reduction and oxidation in redox reactions?

Reduction involves the gain of electrons and a decrease in oxidation number, while oxidation involves the loss of electrons and an increase in oxidation number.

What is a Daniell cell primarily used for in a redox reaction?

A Daniell cell converts chemical energy from a spontaneous redox reaction into electrical energy.

What happens in a galvanic cell during a redox reaction?

The oxidizing agent is reduced at the cathode, while the reducing agent is oxidized at the anode.

What is the role of a salt bridge in a galvanic cell?

A salt bridge maintains electrical neutrality by allowing the movement of ions between the two half-cells.

What is the standard reduction potential for a hydrogen half-cell?

The standard hydrogen half-cell is defined as having a reduction potential of 0 V.

What is the Nernst equation used for?

The Nernst equation calculates the cell potential at non-standard conditions, by accounting for temperature and ion concentration.