What is the oxidation state of Cl in each ion? a. ClO - b. ClO 2 - c. ClO 3 - d. ClO 4 -

All right. Hi, everyone. So this question says given the oxo Aids of Bromine, Hbrohbro two, HBRO three and HBRO four identify the Oxo aid where Bromine exhibits a plus five or positive five oxidation number. Additionally determine which oxo aid among the given possesses the highest acidic strength. So here we've got four different answer. Choices. Each proposing a different one whose bromate has an oxidation number of positive five as well as a different one for who is the strongest acid of the four or which is the strongest acid. So recall that in this case, the oxidation number of bromine is unknown, but we can solve for it by using the oxidation numbers of the other atoms in these molecules. Because recall that when you add up the oxidation numbers of each atom multiplied by the number of each atom in the molecule itself, that total should equal the charge of your molecule. Now, in this case, it just so happens that all of these oxo acids are neutral, which means that I'm going to make all of my equations equal to zero, right. Starting off with HBO, starting off with HBRO by remembering the oxidation states of hydrogen and oxygen we can use them to solve for bromine. In this case, right, recall it, hydrogen can have an oxidation state of either positive one or negative one depending on what it is connected to. When hydrogen is combined with non metals, it has an oxidation state of positive one. However, when it's combined with either metals or boron, it's going to have an oxidation state of negative one. So hydrogen is going to be a positive one. Whereas oxygen, if you recall is generally going to have an oxidation state of negative two. Now exceptions do apply if the compound is a peroxide or a superoxide, but those exceptions do not apply in this case. So our oxidation state for oxygen is negative too. So now to set up the equation right X is going to be the oxidation state of bromine and I can add that to the oxidation state of hydrogen which is positive one multiplied by the number of hydrogens in the given compound. And then I add that by the oxidation state of oxygen which is negative two multiplied by the number of oxygen atoms. And so this entire expression is going to be equal to zero because that is the charge of my compound overall. So in this case, I can make some substitutions because it just so happened that I have one hydrogen atom as well as one oxygen atom. So here when I solve for X, it just so happens that X is going to be equal to positive one, which means that the oxidation state of bromine and HBO is positive one. But in this case, we're looking for an oxidation state of positive five. So here's where I proceed to the next one, which is HBRO two. So here I'm going to use the same equation as last time. But now it just so happens that I have two oxygens instead of one. However, I still have one hydrogen. So the second term is going to stay the same and it's still equal to zero. So when I solve for this expression, I get that X is equal to positive three, which is still not quite what I'm looking for. So I can proceed on to the next Oxo aid, which is H bro 03. And I'm also going to scroll down briefly, right? So once again, the second term is not going to change because I still have only one hydrogen in this compound. However, my third term where oxygen is going to change because now I have three oxygens. And after I solve for this, I do actually get that X meaning the oxidation state of bromine is equal to positive five. So HBRO three is the correct Oxo aid because it has bromine with an oxidation state of positive five. But regardless, I still want to show the calculation for our fourth and final Oxo aid, that's HBRO four. So here is my expression. And now I have four oxygens. Therefore, when I solve for eggs, I get positive seven. So again, right? HBRO three is the Oxo aid that we're looking for. But I just wanted to show all four calculations regardless, however we're not quite done. And because we still have to discuss which of the Oxo Aids listed is the strongest one. So recall that there is actually a general trend that we can follow for Oxo Aids that contain halogens, right? Because generally speaking, as the number of oxygen atoms increases, so does the strength of the given acid, right? Because recall that the term oxo in oxo aid refers to the presence of doubly bonded oxygen atoms. So when it comes to halogen oxo aids, right, as the number of oxo groups increases. So does the strength of the acid? Why? Because oxygen being electron is going to pull electron density away from the bond between oxygen and hydrogen, which makes that proton easier to be removed, therefore more acidic. So of the four Oxo aids discussed in this question, HBRO four is the strongest because it has the highest number of oxo groups. So our answer if I scroll up once more is going to be option c in the multiple choice because bromine in H bro three exhibits an oxidation number of positive five and HB four is the strongest acid because it has the highest number of oxo groups. So with that being said, if you stuck around to the end. Thank you so very much for watching and I hope you found this helpful.

Ch.5 - Introduction to Solutions and Aqueous Solutions

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Ch.5 - Introduction to Solutions and Aqueous Solutions

Problem 64

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Chapter 5, Problem 64

What is the oxidation state of Cl in each ion? a. ClO^- b. ClO₂^- c. ClO₃^- d. ClO₄^-

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insert step 1> Identify the general rule for oxidation states: The sum of the oxidation states in a neutral compound is zero, and in an ion, it is equal to the charge of the ion.

insert step 2> Assign the oxidation state of oxygen as -2, which is common in most compounds.

insert step 3> For each ion, set up an equation where the sum of the oxidation states of Cl and O equals the charge of the ion.

insert step 4> Solve the equation for the oxidation state of Cl in each ion.

insert step 5> Verify that the calculated oxidation state of Cl satisfies the charge balance for each ion.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Oxidation State

The oxidation state, or oxidation number, is a measure of the degree of oxidation of an atom in a chemical compound. It indicates the number of electrons that an atom can gain, lose, or share when forming chemical bonds. Oxidation states are assigned based on a set of rules, including the assumption that compounds are neutral and that certain elements have fixed oxidation states.

Rules for Assigning Oxidation States

There are specific rules for determining oxidation states, such as the fact that the oxidation state of an element in its elemental form is zero, and the oxidation state of oxygen is typically -2. In polyatomic ions, the sum of the oxidation states must equal the overall charge of the ion. These rules help in systematically determining the oxidation states of elements in various compounds.

Chlorine Compounds and Oxidation States

Chlorine can exhibit multiple oxidation states, ranging from -1 to +7, depending on the compound it forms. In oxyanions like ClO-, ClO2-, ClO3-, and ClO4-, chlorine's oxidation state increases with the number of oxygen atoms bonded to it. Understanding the relationship between chlorine's oxidation state and the number of oxygen atoms is crucial for determining the oxidation state in these specific ions.