Given the following information, which of
the following shows the acids in order from
strongest to weakest? The order of atomic
radii is I > Br > Cl, the order of bond
strengths is HOI > HOBr > HOCl, and the
order of electronegativities is Cl > Br > I.
1. HOI > HOBr > HOCl
2. HOCl > HOBr > HOI
3. HOBr > HOCl > HOI
4. None of these
5. HOI > HOCl > HOBr
#2 should be right.
Ka for HOCl = about 3E-8
Ka for HOBr = about 3E-9
Ka for HOI = about 3E-11
Well, this question is starting to look like a chemistry circus! Time to bring in the clown car and have some fun with it!
Alright, ladies and gentlemen, get ready for the Acidic Spectacular Show! Introducing the stars of the show – the acids! Let's rank them from strongest to weakest, and remember, this is all in good chemical fun!
In the yellow corner, we have Cl - Chlorine! Watch out, folks, this electronegative acid knows how to pack a punch! It's got a bigger atomic radius than Br and I, making it more willing to let go of its acidic H+.
Next up, in the green corner, we have Br - Bromine! This acid may be a bit bigger than Cl, but it still knows how to hold its own. With a lower electronegativity than Cl, it's slightly less acidic, but don't underestimate it!
And finally, in the red corner, we have I - Iodine! This acid may have the biggest atomic radius, but it's also the least electronegative of the three. It's like the gentle giant of acids, not as willing to let go of its H+ as the others.
So, to recap, the acids in order from strongest to weakest are: Cl, Br, and I. Remember, folks, in the chemistry circus, the acids may be strong, but the humor is even stronger! Enjoy the show!
To determine the order of acidity from strongest to weakest, we need to consider the factors that affect acidity: the stability of the resulting ions and the strength of the bond between the hydrogen and the halogen.
Based on the given information:
1. Order of atomic radii: I > Br > Cl
2. Order of bond strengths: HOI > HOBr > HOCl
3. Order of electronegativities: Cl > Br > I
From the given information, we can deduce that larger atomic radii lead to weaker (more stable) anions and stronger bonds. Additionally, higher electronegativity indicates a stronger pull on the electrons, which results in a more stable anion.
Combining these factors, we can conclude the order of acidity from strongest to weakest as follows:
1. HOCl (Chlorine is the most electronegative element, creating a stable anion, and chlorine has a smaller atomic radius compared to bromine and iodine.)
2. HOBr (Bromine has a larger atomic radius than chlorine but a smaller atomic radius than iodine. It also has a higher electronegativity than iodine, making it more acidic.)
3. HOI (Iodine has the largest atomic radius and the lowest electronegativity. This leads to a less stable anion and a weaker acid.)
Therefore, the correct order of acidity from strongest to weakest is HOCl > HOBr > HOI.
To determine the order of acids from strongest to weakest, we need to consider the three factors given: atomic radii, bond strengths, and electronegativities.
1. Atomic Radii: The larger the atomic radius, the more spread out the negative charge of an acid will be when it dissociates in water. Therefore, acids with larger atomic radii tend to be weaker. Based on the given information, the order of atomic radii is I > Br > Cl, which means that HI (hydroiodic acid) has the largest atomic radius, followed by HBr (hydrobromic acid), and then HCl (hydrochloric acid).
2. Bond Strengths: The stronger the bond between the hydrogen atom and the rest of the acid molecule, the less likely it is to dissociate in water. Therefore, acids with stronger bond strengths are generally weaker acids. According to the given data, the order of bond strengths is HOI > HOBr > HOCl. This means that hydroiodic acid (HI) has the strongest bond, followed by hydrobromic acid (HBr), and then hydrochloric acid (HCl).
3. Electronegativities: The more electronegative an atom, the greater its ability to attract electrons towards itself. Therefore, the more electronegative an atom is, the more likely it is to donate a hydrogen ion (H+) and form an acid. According to the information, the order of electronegativities is Cl > Br > I. This means that chlorine (Cl) is the most electronegative, followed by bromine (Br), and then iodine (I).
Now let's combine all the information to determine the order of the acids from strongest to weakest:
Based on the given information:
- Hydroiodic acid (HI) has the largest atomic radius, the strongest bond strength (HOI), and the least electronegative atom (I). Therefore, HI is the strongest acid.
- Hydrobromic acid (HBr) has a smaller atomic radius than HI, a weaker bond strength (HOBr), and a more electronegative atom (Br). Therefore, HBr is the second-strongest acid.
- Hydrochloric acid (HCl) has the smallest atomic radius, the weakest bond strength (HOCl), and the most electronegative atom (Cl). Therefore, HCl is the weakest acid.
So, the correct order of the acids from strongest to weakest is: Hydroiodic acid (HI) > Hydrobromic acid (HBr) > Hydrochloric acid (HCl).