Electrochemistry Review Flashcards

Flashcards covering the fundamental concepts of electrochemistry including redox reactions, oxidation numbers, cell types, and thermodynamic relationships based on the lecture notes.

Electrochemical processes are oxidation-reduction reactions where chemical energy is converted to electricity or _________ energy is used to cause a nonspontaneous reaction.

electrical

Oxidation is defined as the _________ of electrons.

loss

Reduction is defined as the _________ of electrons.

gain

The oxidation number of free elements in an uncombined state, such as $Na$, $H_2$, or $P_4$, is _________.

$$0$$

In monatomic ions, the oxidation number is equal to the _________ on the ion.

charge

The oxidation number of oxygen is usually $-2$ except in peroxides like $H_2O_2$, where it is _________.

$$-1$$

The oxidation number of hydrogen is _________ when it is bonded to metals in binary compounds.

$$-1$$

According to the hierarchy rules, alkali metals always have an oxidation number of _________.

$$+1$$

In balancing redox equations, _________ is added to balance oxygen atoms.

$$H_2O$$

In balancing redox equations, _________ is added to balance hydrogen atoms in acidic solutions.

$$H^+$$

For reactions in basic solutions, _________ is added to both sides of the equation for every $H^+$ that appears.

$$OH^-$$

A _________ cell is an experimental apparatus for generating electricity through the use of a spontaneous redox reaction.

galvanic

An _________ cell uses electricity to cause a nonspontaneous redox reaction to occur.

electrolytic

In a galvanic cell, oxidation occurs at the _________.

anode

In a galvanic cell, reduction occurs at the _________.

cathode

The _________ prevents the build-up of charge between the two solutions in an electrochemical cell.

salt bridge

The standard reduction potential for the Standard Hydrogen Electrode (SHE) is _________.

$$0.00\,V$$

The standard cell potential ($E^0_{cell}$) is calculated as $E^0_{cathode} -$ _________.

$$E^0_{anode}$$

The greater the value of $E^0$, the greater the tendency for the substance to be _________.

reduced

Changing the _________ of a half-cell reaction does not change the value of $E^0$.

stoichiometric coefficients

The thermodynamic equation relating Gibbs free energy change to cell potential is $\\Delta G^0 =$_________.

-nDE0cell

The Faraday constant ($F$) is approximately _________.

$$96,500\,J/V \cdot mol$$

A reaction is spontaneous when the Gibbs free energy change ($\\Delta G$) is _________.

negative

In an electrolytic cell, the anode has a _________ charge.

positive

The electrolysis of water is a nonspontaneous process with a standard cell potential ($E^0_{cell}$) of _________.

$$-1.23\,V$$