Usinf your periodic table, Indicate whether each other following substances could act as an oxidizing agent (OA), a reducing agent (RA) or both (OA/RA):
(A.) Ba2+ (aq)
So I think it should be reduction because it gained 2 electrons?
(B.) Co2+ (aq) : RA
(C.) Se(s) :
(D.) Cs(s):
I don't know the last two and I don't know how to use the periodic table to answer these questions. I know that the metals are on the left and they give electrons whereas Nonmetals are on the right side of the periodic table and they accept electrons. So knowing that reduction uses oxidizing agents to gain electrons does that mean oxidizing agents would only imply to nonmetals since they accept electrons? How do I know if the substances are both?
A. You're right; Ba^2+ is reduced because it gains electrons. That makes it an oxidizing agent.
B. So Co^2+ + 2e = Co and that's the same as A.
C. Se. You have the choice of
Se --> Se^4+ + 4e with a loss of electrons and that is oxidation or reducing agent.
Or. Se + 2e ==> Se^2-
Technically you need to know what it is reacting with.
Since it can go either way (both gain and loss of electrons) is is an OA/RA.
D. Cs can do only
Cs ==> Cs^+ + e and means oxidation and reducing agent.
The metals in group I, II, III are reducing agents.
The non-metals in VII (or 17) etc are oxidizing agents.
For example, Cl2 + 2I^- ==> 2Cl^- + I2. That means Cl2 is an OA and I^- is a RA
To determine whether a substance can act as an oxidizing agent (OA), reducing agent (RA), or both (OA/RA), you can use the periodic table to analyze the oxidation states of the elements involved.
For (A) Ba2+(aq), you correctly identified that it gained 2 electrons. This means that it has reduced, making it a reducing agent (RA).
For (B) Co2+(aq), you also correctly identified it as a reducing agent. However, it's important to note that the periodic table alone doesn't provide direct information about oxidation states. In this case, you can infer the oxidation state from the charge of the ion (+2). Since it has a positive charge, it means that cobalt (Co) lost some electrons, making it a reducing agent.
Moving on to (C) Se(s), solid selenium. In this case, the substance is not in an aqueous solution, so oxidation state cannot be determined just by looking at the periodic table. However, we know that as a nonmetal, selenium tends to gain electrons, making it a potential candidate for being an oxidizing agent (OA). Consequently, we can conclude that it can function as an OA.
For (D) Cs(s), solid cesium, we encounter a similar situation as in (C). Since cesium is a metal located on the left side of the periodic table, it tends to lose electrons. Therefore, it is more likely to be a reducing agent (RA) rather than an oxidizing agent (OA).
In summary:
(A) Ba2+(aq): Reducing agent (RA)
(B) Co2+(aq): Reducing agent (RA)
(C) Se(s): Oxidizing agent (OA)
(D) Cs(s): Reducing agent (RA)
Remember, this is a general guide, and there may be exceptions based on the specific reaction conditions. However, understanding the electronegativity and behavior of elements in gaining or losing electrons is crucial in determining their potential role as oxidizing or reducing agents.