HELP SO MUCH Read the following chemical equations. Reaction 1: 2KI + H2O2 → 2KOH + I2

Reaction 2: Cl2 + H2 → 2HCl

Which of the following statements is true for both the chemical equations?

I is oxidized in reaction 1 and Cl2 is oxidized in reaction 2.

I is reduced in reaction 1 and Cl2 is reduced in reaction 2.

I is oxidized in reaction 1 and Cl2 is reduced in reaction 2.

I is reduced in reaction 1 and Cl2 is oxidized in reaction 2.

I is oxidized in reaction 1 and Cl2 is reduced in reaction 2.

Explanation:

The oxidation reduction reactions are called redox reaction. These reactions are take place by gaining or losing the electrons and oxidation state of elements are changed.

Oxidation:

Oxidation involve the removal of electrons and oxidation state of atom of an element is increased.

Reduction:

Reduction involve the gain of electron and oxidation number is decreased.

Consider the following reactions.

1 =    2KI  + H₂O₂    →       2KOH + 1₂

In this reaction the oxidation state of iodine is -1 on left hand side and 0 on right hand side which means it lost the electron and gets oxidized.

2=      Cl₂ + H₂       →       2HCl

In this reaction the oxidation state of chlorine on left hand side is 0 while on right hand side its -1 thus it gets reduced.

8

explanation:

each principal energy level above the first contains one s orbital and three p orbitals. a set of three p orbitals, called the p sublevel, can hold a maximum of six electrons. therefore, the second level can contain a maximum of eight electrons - that is, two in the s orbital and 6 in the three p orbitals.

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