Which of the following reactions of calcium compounds is or...

Which of the following reactions of calcium compounds is or are redox reactions? a. $\mathrm{CaCO}_{3}(s) \rightarrow \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)$ b. $\mathrm{CaO}(s)+\mathrm{SO}_{2}(g) \rightarrow \mathrm{CaSO}_{3}(s)$ c. $\mathrm{CaCl}_{2}(s) \rightarrow \mathrm{Ca}(s)+\mathrm{Cl}_{2}(g)$ d. $3 \mathrm{Ca}(s)+\mathrm{N}_{2}(g) \rightarrow \mathrm{Ca}_{3} \mathrm{N}_{2}(s)$

Which of the following reactions of calcium compounds is or are redox reactions?
a. $\mathrm{CaCO}_{3}(s) \rightarrow \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)$
b. $\mathrm{CaO}(s)+\mathrm{SO}_{2}(g) \rightarrow \mathrm{CaSO}_{3}(s)$
c. $\mathrm{CaCl}_{2}(s) \rightarrow \mathrm{Ca}(s)+\mathrm{Cl}_{2}(g)$
d. $3 \mathrm{Ca}(s)+\mathrm{N}_{2}(g) \rightarrow \mathrm{Ca}_{3} \mathrm{N}_{2}(s)$

Key Concepts

Redox Reaction

A redox reaction, short for reduction-oxidation reaction, is one in which electrons are transferred between species. This involves one substance being oxidized (losing electrons) while another is reduced (gaining electrons). Such reactions are characterized by changes in the oxidation states of the elements involved.

Oxidation States

The concept of oxidation states (or oxidation numbers) is a way to keep track of electron transfer in chemical reactions. By assigning oxidation states to atoms, one can determine whether a change in electron count has occurred, which is essential for identifying redox reactions.

Oxidizing and Reducing Agents

In a redox process, the oxidizing agent is the species that accepts electrons and is reduced, while the reducing agent is the species that donates electrons and is oxidized. Understanding these agents is crucial for analyzing and predicting the course of redox reactions.

Reaction Type Analysis

Evaluating whether a reaction is a redox process involves analyzing the changes in oxidation states of the elements in the reactants and products. This analytical approach differentiates redox reactions from other types of reactions where electron transfer does not occur.

Transcript

00:01 Okay, let's look at an equation.

00:03 And in this equation, let's determine if this is a redox equation for calcium.

00:09 How would we know that? well, first of all, we know that a redox equation means that, or a reaction is that there's going to be a change in oxidation state.

00:18 So we need to decide if, in fact, there is a change in oxidation state for calcium in this reaction.

00:24 And how do we know that? well, let's look at the first part of this problem, which right here.

00:31 Calcium carbonate.

00:32 Carbonate is an ion that carries a negative two charge.

00:37 So calcium would have a positive two charge.

00:42 That's because we know that this molecule has to add up to a zero oxidation state.

00:47 Okay, so now let's move to the other side where we have calcium as well.

00:52 Oxygen is a negative two oxidation state and therefore calcium is positive two.

01:00 So this equals zero and this equals zero.

01:04 So if we look at calcium, did it change from one side to the next? and the answer is no.

01:12 The oxidation state did not change from plus two to plus two.

01:16 So for a, the answer is no, this is not a redox reaction for calcium.

01:23 Let's go to the next one, which is calcium oxide plus so2.

01:35 Give this calcium three.

01:41 Okay, so let's do the same thing here.

01:43 Let's first look at the oxidation state over here.

01:46 We don't see any charges associated with this molecule, which means that the oxidation states of these elements must add up to zero.

01:55 We know that oxygen is a negative 2, so calcium is also a plus 2.

02:00 These add up to 0.

02:02 Let's look on the right -hand side of the equation.

02:05 We have the s .o3.

02:07 S .o .3 in its ionic form carries a negative to charge, okay, which means calcium, again, is plus two.

02:17 And these add up to zero...

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