Redox Reactions Quiz

A chemical reaction where an element undergoes both oxidation and reduction simultaneously, resulting in the formation of products with different oxidation states.

Elements that can exhibit multiple oxidation states due to the presence of available electrons in their outer shell.

Oxidation is the process of gaining oxygen or losing electrons, while reduction is the process of losing oxygen or gaining electrons.

A reaction where a single reactant breaks down into two or more products.

In a redox reaction, the species that gains electrons is the oxidant (oxidizing agent), while the species that loses electrons is the reductant (reducing agent).

The standard hydrogen electrode (SHE) is a reference electrode used in electrochemistry, with a defined potential of 0 volts.

An anode is the electrode where oxidation occurs, while a cathode is the electrode where reduction occurs.

Elements that can exhibit only one oxidation state in their compounds, typically having a full or half-filled outermost shell.

The process of using a substance to whiten or lighten another substance. It involves the oxidation of the substance being bleached.

The ability of a substance to participate in a chemical reaction depends on its chemical properties, specifically the ability to gain or lose electrons.

Nitric acid is a strong oxidizing agent and can oxidize lead(II) oxide (PbO) to lead(II) nitrate. However, lead(IV) oxide (PbO2) is already in its highest oxidation state, so nitric acid cannot further oxidize it.

A method used to balance chemical equations by separating the overall reaction into two half-reactions: oxidation and reduction. Each half-reaction is balanced separately, then combined to give the balanced equation.

A method used to balance chemical equations by identifying the changes in oxidation numbers of reactants and products. The number of electrons lost in oxidation must equal the number gained in reduction.

The oxidation number of an element in a compound represents the hypothetical charge it would have if all bonds were ionic.

A method used to calculate the oxidation number of phosphorus in different compounds based on the rules of assigning oxidation numbers.

The sum of the oxidation numbers of all atoms in a neutral molecule is zero, while in an ion, it is equal to the charge of the ion.

The oxidation number of an atom in its elemental state is zero, regardless of the number of atoms in the molecule.

The oxidation number of alkali metals (Group 1) is always +1, and alkaline earth metals (Group 2) is always +2 in their compounds.

The oxidation number of hydrogen is always +1 in its compounds, except in metal hydrides where it is -1.

The oxidation number of oxygen is always -2 in its compounds, except in peroxides (O22-) where it is -1, and in OF2 where it is +2.

The oxidation number of halogens (Group 17) is usually -1 in their compounds, except when they are combined with a more electronegative element.

The sum of the oxidation numbers of all the atoms in a polyatomic ion is equal to the charge of the ion.

The oxidation number of an atom in a compound is the hypothetical charge it would have if all the bonding electrons were assigned to the more electronegative atom.

A chemical reaction where a substance gains oxygen or loses electrons, increasing its oxidation number.

A chemical reaction where a substance loses oxygen or gains electrons, decreasing its oxidation number.

The ability of a substance to undergo disproportionation. Elements with multiple possible oxidation states are more likely to disproportionate.

A chemical reaction where an acid and a base react to form a salt and water.

A chemical reaction where electron transfer occurs between reactants, resulting in changes in oxidation numbers.

A substance that gains electrons in a redox reaction, causing the oxidation of another substance.

The number of electrons an atom gains or loses when forming a chemical bond, indicating its relative electron charge.

The process of assigning oxidation numbers to each atom in a compound based on the hypothetical charge it would have if all bonds were ionic.

The average oxidation state of an element in a compound or ion is calculated by summing the oxidation states of all atoms of that element and dividing by the total number of atoms.

The actual oxidation state of an atom in a compound can be determined by writing the complete structural formula and considering the distribution of shared electrons.

The use of the ion-electron method to balance chemical equations involves separating the overall reaction into oxidation and reduction half-reactions, balancing each separately, and then combining them to obtain the balanced equation.