For each of the following oxidation-reduction reactions, identify which element is oxidized and which is reduced.

a. Mg ( s ) + Br 2 ( l ) → MgBr 2 ( s )    b. 2Na ( s ) + S ( s ) → Na 2 S ( s )    c. CO 2 ( g ) + H 2 ( g ) → CO ( g ) + H 2 O ( g )    d. 6K ( s ) + N2 ( g ) → 2K 3 N ( s )

Interpretation:

The element being oxidized and reduced in the given reaction should be determined.

Concept Introduction:

The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.

The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.

Given:

Mg(s) + Br2(l) → MgBr2(s)

The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.

While determining the oxidation state of compound, the element with greater electronegativity is assigned with negative value of oxidation state which is equal to the charge as an anion in ionic compounds and element whose oxidation states are fixed are assigned. For compounds with no charge, the sum of oxidation states is zero

Interpretation:

The element being oxidized and reduced in the given reaction should be determined.

Concept Introduction:

The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.

The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.

Interpretation:

The element being oxidized and reduced in the given reaction should be determined.

Concept Introduction:

The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.

The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.

Interpretation:

The element being oxidized and reduced in the given reaction should be determined.

Concept Introduction:

The oxidation state is defined as the charge(s) that an atom would have when electron(s) were transferred completely from a molecule or ion.

The element being oxidized is the one whose oxidation increases in the reaction whereas the reduced element is the one whose oxidation number decreases in the reaction.