A transfer of electrons indicates an oxidation-reduction reaction. The element losing electrons is oxidized, while the element gaining electrons is reduced.

Calcium is initially a neutral solid, but as a product has a charge of . Calcium's charge increased, meaning it must have lost electrons.

Hydrogen initially has a charge of , but as a product is a neutral diatomic gas. Hydrogen's charge decreased, meaning it must have gained electrons.

We can thus conclude that calcium was oxidized and hydrogen was reduced, indicating that electrons were transferred from calcium to hydrogen.

The charge on chlorine remains throughout the entire reaction.

Hydrogen doesn't change. Cu²⁺ doesn't change (partnered with S^2- then with SO₄^2-). Sulfur goes from S^2- and S⁶⁺(paired with 6 O^2- with a 2– charge), showing an oxidation. Nitrogen goes from N⁵⁺ to N²⁺ meaning it was reduced.

Let's break down the reaction into two separate reactions:

and

We can see that copper loses electrons, while silver gains electrons. Recall that oxidation is loss and reduction is gain, with regard to electrons. Copper is oxidized and silver is reduced.

However, this question asks for the oxidizing agent and reducing agent. Recall that the oxidizing agent is reduced, while the reducing agent is oxidized. Since copper is oxidized, it is the reducing agent. Similarly, since silver is reduced, it is the oxidizing agent.

Think "OIL RIG" Oxidation Is Loss of electrons, Reduction Is Gain of electrons. The loss and gain of electrons is what changes the charge of the atom or molecule. In redox reactions, electrons are transferred. Changing the number of protons changes the identity of the element ,which is not the case. Since chemical reactions involve valence electrons, the nucleus is unchanged.

 is converted to . Thus, an additional oxygen has been added to the original molecule, thus  was oxidized. The substance that is oxidized is also called the reducing agent because it causes the reduction of the other molecule to which the oxygen originally was bound , which is the oxidizing agent. 

An ionic equation is a chemical equation in which ionic compounds in an aqueous solution are written as dissociated ions.

A complete ionic equation shows all the ions present in the solution (which includes both the reactive and spectator ions), as the dissociated ions. The complete ionic equation for this problem's reaction is:

It is worth noting that in a complete ionic equation, it becomes readily apparent which ions are involved in the oxidation-reduction reaction, and which ions are the spectator ions (those that do not change during the reaction). For example since  and  are present on both sides of the reaction, they are spectator ions that go through the reaction unchanged. Also because the  and  are only present as dissolved ions on the reactants side of the equation and form the solid precipitate  on the product side, they are the reactive species in this chemical reaction.

The net ionic equation shows only the reactive ions in solution and the product(s) formed by them. Therefore a net ionic equation can most simply be made by looking at the complete ionic equation and omitting the spectator ions as shown below:

Net ionic equation:

In an oxidation-reduction reaction, the oxidizing agent is the reactant that accepts electrons, becoming reduced. The oxidizing or reducing agent is always the whole reagent, and is never just the atom in the reagent that is being oxidized or reduced.

 is the reagent that accepts two electrons from elemental zinc. This allows zinc to become oxidized, changing oxidation state from zero to . Copper accepts these electrons, changing from an oxidation state of to zero. As a result, we say that  is the oxidizing agent for the reaction.

Larger halogen size leads to greater acidity because of weaker H-X interactions.

Acid strength increases from left to right across a period and increases going down a group.

Acid strength of an oxy acid increases with increasing electronegativity on the halogen.