In a hexagonal close-packed (HCP) structure, there are 6 atoms per unit cell.

In a hexagonal close-packed (HCP) structure, the coordination number is 12, as each atom is in contact with 12 others.

Increasing the concentration of a reactant will shift the equilibrium position to the right, favoring the formation of products.

According to Le Chatelier's principle, increasing the concentration of products will shift the equilibrium to the left, favoring the formation of reactants.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right to produce more products.

According to Le Chatelier's principle, if the concentration of reactants is increased, the equilibrium will shift to the right to produce more products.

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants.

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants.

The slowest step in a reaction mechanism that determines the overall rate of the reaction is called the rate-determining step.

For a first-order reaction, the rate is directly proportional to the concentration of the reactant, so doubling the concentration doubles the rate.

For a first-order reaction, the rate is directly proportional to the concentration of reactants, so doubling the concentration doubles the rate.

An increase in oxidation number indicates that the element is losing electrons, which means it is being oxidized.

A decrease in oxidation state indicates that the element has gained electrons, which means it is reduced.

A decrease in oxidation state indicates that the element has gained electrons, which is defined as reduction.

A decrease in oxidation state indicates that the element is gaining electrons, which means it is being reduced.

If the oxidation state of an element decreases, it is gaining electrons, which is known as reduction.

An increase in the oxidation state of an element indicates that it has lost electrons, which means it is oxidized.

The substance that gains electrons in a redox reaction is called the oxidizing agent.

The oxidation state of the reducing agent decreases as it loses electrons during the reaction.

Reduction is defined as the gain of electrons, which decreases the oxidation state of the element.

In a reversible process, the work done is always maximum compared to irreversible processes.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.

Increasing the temperature of an exothermic reaction shifts the equilibrium to the left (towards the reactants), while for an endothermic reaction, it shifts to the right (towards the products).

If the forward reaction is exothermic, the reverse reaction must be endothermic, as it absorbs heat.

In a simple cubic lattice, there is 1 atom effectively present in one unit cell, as each corner atom contributes 1/8th of an atom to the unit cell.

In a simple cubic lattice, there is 1 atom per unit cell (1/8 atom from each of the 8 corners).

In an electrochemical cell, oxidation occurs at the anode.

In electrolysis, oxidation occurs at the anode.

Selectivity in adsorption refers to the preference of an adsorbent for one gas over another, which can be crucial in separation processes.

Adsorption refers to the process where molecules adhere to the surface of a solid or liquid, forming a film.